**Electrochemical Characterisation to Study the Pitting Corrosion Behaviour of Beryllium**

J. S. Punni\* *AWE, Reading UK* 

### **1. Introduction**

Beryllium has widespread uses in aerospace industry as it has attractive mechanical properties, a high melting point (1289 °C), a low density (1.85 g/cc), high specific heat capacity and thermal conductivity. It has a hexagonal close packed (hcp) structure and due to its low neutron cross section it is widely used for nuclear applications. To achieve the required mechanical properties beryllium is produced by vacuum hot pressing in the temperature range 1000 to 1100°C, using a high purity and fine grained beryllium powder. To get stress relief, the material is subsequently heat treated at 800°C; this also serves to remove elemental aluminium at grain boundaries in material structure, by converting it to the intermetallic form AlFeBe4. A proper balance between Fe and Al is required to avoid 'hot shortness' due to the presence of elemental aluminium at the grain boundaries.

The principle contaminants within commercial beryllium are oxygen (as beryllium oxide), carbon, silicon, iron, aluminium and magnesium. Silicon, iron and aluminium principally come from the ore, although additional iron may be contributed from billet machining operations. Magnesium arises primarily from reduction of beryllium fluoride using magnesium to produce beryllium metal. Carbon arises principally from casting operations, which use graphite moulds. Oxygen is always present as an oxide film on powder particles. Other elements are also present but generally at very low levels.

Past studies have shown that beryllium is susceptible to pitting corrosion in the presence of chloride, fluoride and sulphate ions (Hill, et al., 1996, 1998; Stonehouse & Weaver, 1965). This is due to the breakdown of passive film at localised sites resulting in sporadic pits. The pitting is an insidious form of corrosion since it can proceed unnoticed and can lead to a catastrophic component failure. During the pitting process most of the metal surface remains passive and acts as the cathodic site for a small anodic area inside the pit which leads to accelerated attack in this location.

Pitting corrosion is a localised form of corrosion by which cavities and holes are produced in the material, which are generally plugged with corrosion products. Corrosion, in general, is an electrochemical process in which electrons are generated and consumed at the corroding metal surface. This process consists of (i) an anodic site at the metal surface where metal is

<sup>\*</sup> © British Crown Owned Copyright 2011/MOD

Electrochemical Characterisation to Study the Pitting Corrosion Behaviour of Beryllium 3

Pitting corrosion of beryllium in moist air has been reviewed by several authors (Stonehouse & Weaver, 1965; Miller & Boyd, 1968). Beryllium has adequate corrosion resistance for use in many engineering applications due to the formation of a protective oxide film when exposed to air. The metal will normally remain bright for years upon exposure to the atmosphere. The oxide (BeO) formed on the surface of beryllium is resistant to cracking or spalling because it grows inward and it is in a state of compression (due to its volume being 1.68 times larger than the metal it occupies). However, two prime situations were described by Mueller and Adolphson (1979) under which beryllium was found susceptible to pitting corrosion. The first is when beryllium has carbide particles exposed to moist air which produce active sites for corrosion. This was evidenced by the white corrosion products developed at sites occupied by these inclusions on beryllium under storage conditions. The second is when the surface of beryllium is contaminated with chloride and sulphate ions which may be introduced from human contact, contaminated air, rain water, cleaning solvent or certain packaging materials. A study by Stonehouse and Beaver using humidity cabinet experiments evaluated that machined beryllium (having surface residue deposits)

An initial study on the corrosion of beryllium in water focused on reactor environments where beryllium was used as a neutron reflector, and is not available in the general literature. Although beryllium corrosion rates were high in some of the simulated environments, service life for beryllium reflectors exposed to high purity irradiated water was reported to be good. There was no major problem of coupling beryllium with aluminium and stainless steel (Miller & Boyd, 1968). Another study was conducted (Flitton et al., 2002) as part of nuclear waste disposal, to understand beryllium corrosion as a result of being placed underground. Beryllium (99% pure) coupons were buried 4 and 10 feet deep underground. The general loss of material was measured at the rate 2 µm and 7 µm per year respectively, and the maximum pit depth at 4 feet underground depth was recorded as 153 µm. In some other instances where beryllium components were stored in

uncontrolled moist environments, corrosion pits as deep as 250 µm were detected.

It has generally been recommended (Mueller & Adolphson, 1979; Stonehouse & Weaver, 1965) that for beryllium, the use of tap water should be minimised, metal surfaces should be as clean as possible, and excessive machine damage should be avoided. The storage of finished beryllium components should be maintained in polythene bags with a desiccant to maintain a dry atmosphere and in humidity controlled room. Where corrosion conditions are expected in service, the use of chromate coating and anodic films can be beneficial.

Electrochemical techniques were widely used in the past (Hill, et al., 1996, 1998; Punni & Cox, 2010; Lillard, 2000) to characterise pitting corrosion behaviour of beryllium in aggressive aqueous environments. In aqueous salt solutions beryllium develops a passive hydrated oxide film, either Be(OH)2 or its hydrate (BeO (H2O)x) (Vaidya et al. 1999) Electrochemical impedance spectroscopy (EIS) experiments had shown that the oxide growth rate on beryllium was 6.4 angstroms/V over the range of 0–4V. This barrier layer is quickly disrupted at

localised sites in the presence of aggressive ions in the environment (Hill et al., 1998).

**2. Review of beryllium corrosion** 

was susceptible to pitting corrosion.

**2.2 Effect of pH and chloride ion concentration** 

**2.1 Background** 

converted into metal ions by losing electrons. In the case of beryllium the anodic reaction is as follows:

$$\mathbf{B}\mathbf{e} = \mathbf{B}\mathbf{e}^{2\*} + \mathbf{2}\mathbf{e}^{\*}\tag{1}$$

Beryllium is a reactive metal having a standard potential of Eo = -1.85V and it lies between aluminium (-1.66V) and magnesium (-2.37V) in the reactive series (Kaye & Laby, 1978)

i. A cathodic site at the metal surface where a complementary reaction to consume excess electrons takes place which could be either

$$\rm O\_2 + 2H\_2O + 4e^- = 4OH^- \tag{2}$$

At Eo = +1.23V – 0.591 pH at 25°C or

$$2\mathbf{H}^\* + 2\mathbf{e}^\* = \mathbf{H}\_2 \tag{3}$$

In acidic conditions, at Eo = +0.0V – 0.591 pH at 25°C

ii. A conductor to conduct electrons between the anode and cathode and (iv) an electrolyte to provide a medium for transporting ionic products away from the metal surface.

The stability (potential-pH) diagram for beryllium in water at 25°C, as provided by Pourbaix (Pourbaix, 1966), is represented in Figure 1. This defines the regions of corrosion, passivation and immunity. The problem of pitting corrosion is mainly confined to the passivation region where insoluble beryllium hydroxide is a stable product. At low temperature, in high purity water, beryllium has little or no corrosion problem. However, the performance of beryllium in tap water can be seriously compromised by the presence of small concentrations of chloride and sulphate ions (Stonehouse & Weaver, 1965).

Fig. 1. Potential-pH diagram for the Be-water system at 25°C for the β-Be(OH)2 crystalline hydroxide and assuming a 10-6 M concentration of Be2+, after Pourbaix (1966)

### **2. Review of beryllium corrosion**

### **2.1 Background**

2 Pitting Corrosion

converted into metal ions by losing electrons. In the case of beryllium the anodic reaction is

Beryllium is a reactive metal having a standard potential of Eo = -1.85V and it lies between aluminium (-1.66V) and magnesium (-2.37V) in the reactive series (Kaye & Laby, 1978)

i. A cathodic site at the metal surface where a complementary reaction to consume excess

O2 + 2H2O + 4e- = 4OH- (2)

2H+ + 2e- = H2 (3)

ii. A conductor to conduct electrons between the anode and cathode and (iv) an electrolyte to provide a medium for transporting ionic products away from the metal surface. The stability (potential-pH) diagram for beryllium in water at 25°C, as provided by Pourbaix (Pourbaix, 1966), is represented in Figure 1. This defines the regions of corrosion, passivation and immunity. The problem of pitting corrosion is mainly confined to the passivation region where insoluble beryllium hydroxide is a stable product. At low temperature, in high purity water, beryllium has little or no corrosion problem. However, the performance of beryllium in tap water can be seriously compromised by the presence of

small concentrations of chloride and sulphate ions (Stonehouse & Weaver, 1965).

Fig. 1. Potential-pH diagram for the Be-water system at 25°C for the β-Be(OH)2 crystalline

hydroxide and assuming a 10-6 M concentration of Be2+, after Pourbaix (1966)

electrons takes place which could be either

In acidic conditions, at Eo = +0.0V – 0.591 pH at 25°C

At Eo = +1.23V – 0.591 pH at 25°C or

Be = Be2+ + 2e- (1)

as follows:

Pitting corrosion of beryllium in moist air has been reviewed by several authors (Stonehouse & Weaver, 1965; Miller & Boyd, 1968). Beryllium has adequate corrosion resistance for use in many engineering applications due to the formation of a protective oxide film when exposed to air. The metal will normally remain bright for years upon exposure to the atmosphere. The oxide (BeO) formed on the surface of beryllium is resistant to cracking or spalling because it grows inward and it is in a state of compression (due to its volume being 1.68 times larger than the metal it occupies). However, two prime situations were described by Mueller and Adolphson (1979) under which beryllium was found susceptible to pitting corrosion. The first is when beryllium has carbide particles exposed to moist air which produce active sites for corrosion. This was evidenced by the white corrosion products developed at sites occupied by these inclusions on beryllium under storage conditions. The second is when the surface of beryllium is contaminated with chloride and sulphate ions which may be introduced from human contact, contaminated air, rain water, cleaning solvent or certain packaging materials. A study by Stonehouse and Beaver using humidity cabinet experiments evaluated that machined beryllium (having surface residue deposits) was susceptible to pitting corrosion.

An initial study on the corrosion of beryllium in water focused on reactor environments where beryllium was used as a neutron reflector, and is not available in the general literature. Although beryllium corrosion rates were high in some of the simulated environments, service life for beryllium reflectors exposed to high purity irradiated water was reported to be good. There was no major problem of coupling beryllium with aluminium and stainless steel (Miller & Boyd, 1968). Another study was conducted (Flitton et al., 2002) as part of nuclear waste disposal, to understand beryllium corrosion as a result of being placed underground. Beryllium (99% pure) coupons were buried 4 and 10 feet deep underground. The general loss of material was measured at the rate 2 µm and 7 µm per year respectively, and the maximum pit depth at 4 feet underground depth was recorded as 153 µm. In some other instances where beryllium components were stored in uncontrolled moist environments, corrosion pits as deep as 250 µm were detected.

It has generally been recommended (Mueller & Adolphson, 1979; Stonehouse & Weaver, 1965) that for beryllium, the use of tap water should be minimised, metal surfaces should be as clean as possible, and excessive machine damage should be avoided. The storage of finished beryllium components should be maintained in polythene bags with a desiccant to maintain a dry atmosphere and in humidity controlled room. Where corrosion conditions are expected in service, the use of chromate coating and anodic films can be beneficial.

### **2.2 Effect of pH and chloride ion concentration**

Electrochemical techniques were widely used in the past (Hill, et al., 1996, 1998; Punni & Cox, 2010; Lillard, 2000) to characterise pitting corrosion behaviour of beryllium in aggressive aqueous environments. In aqueous salt solutions beryllium develops a passive hydrated oxide film, either Be(OH)2 or its hydrate (BeO (H2O)x) (Vaidya et al. 1999) Electrochemical impedance spectroscopy (EIS) experiments had shown that the oxide growth rate on beryllium was 6.4 angstroms/V over the range of 0–4V. This barrier layer is quickly disrupted at localised sites in the presence of aggressive ions in the environment (Hill et al., 1998).

Electrochemical Characterisation to Study the Pitting Corrosion Behaviour of Beryllium 5

found that chloride concentration in the range 0.001 to 0.1M NaCl did not have a significant effect on corrosion of beryllium. This conclusion was based on the observation that there was not much difference in passive range. It was stated that the size of the passive range, or the ability of a solution to break the oxide layer on the surface of the beryllium, appeared to be a function of pH, and not of chloride concentration. This result on chloride effect is not in agreement with the findings of Hill and co-workers (1996) and a recent investigation by

A minimum in both the passive and corrosion current densities was observed in the pH range of 4 to 11 (Hill et al., 1996, 1998). The relationship of both passive current density and corrosion current density with solution pH is represented in Figure 3. This agrees well with the Pourbaix diagram (Pourbaix, 1966) for the beryllium water system at 25°C, as represented in Figure 1. This shows that between pH 4 and 11, the formation of insoluble

The crystallographic orientation effect of commercial beryllium was described by Lillard (2000) and Friedman and Hanafee (2000). Pitting experiments indicated that once pit initiation has started, beryllium corrodes preferentially in certain orientations. Potentiodynamic polarisation studies for beryllium (0001), (1010) and (1120) surfaces were carried out in deaerated 0.01 M NaCl, as represented in Figure 4. The pitting potential (Epit) was found to decrease with crystal orientation in the order (0001) > (1010) > (1120). Repassivation potentials (Rrp) appeared to follow the same crystallographic trends as Epit. The potential region defined by Epit – Erp was large for (0001) and (1010) surfaces (>100mv) and appeared to be much smaller for the (1120) surface. There is a relationship between Epit and pit density on the surface such that for a higher Epit at a surface there is a smaller population density of pits and vice versa. The expression Epit – Erp represents the extent of pit growth. This implies that a surface orientation with large Epit and with large (Epit – Erp)

Fig. 3. Passive current density, ipass, and corrosion current density, icorr, as a function of solution

pH. A minimum in ipass and icorr exists between a pH of 4 and 11, after Hill et al. (1998)

Punni and Cox (2010).

species Be(OH)2 is thermodynamically favourable.

**2.3 Crystallographic orientation effect** 

would experience fewer, but deeper, pits.

`

The passivity and pitting of commercially produced beryllium has been studied extensively in chloride solutions. The key points for a typical cyclic polarisation curve from a recent polarisation study (Punni & Cox, 2010) for a commercial beryllium are displayed in Figure 2. It was observed that the anodic polarisation was characterised by a region of passivity followed by a logarithmic increase in the current density, which corresponded to the onset of pitting corrosion (Epit).

Fig. 2. Typical cyclic polarisation curve for beryllium metal in 0.0001M KCl solution, sweep rate of 20mV/min, after Punni & Cox (2010)

A previous electrochemical study (Hill et al., 1996, 1998) in sodium chloride (NaCl) solution of varying chloride ion concentrations (from 0.0001 to 1M) showed that on increasing the chloride concentration, both pitting potential and repassivation potential decreased progressively and at 1M NaCl, the pitting commenced at open circuit conditions. A logarithmic relationship between pitting potential (in mV) and chloride concentration (in morality) was presented as given below.

$$E\_{\rm piit} = -67 \log \left[ \rm Cl^{-1} \right] \cdot 1010 \tag{4}$$

The effect of pH on pitting corrosion behaviour of beryllium was studied by Hill and coworkers (1998). Beryllium was found to be passive in the pH range from 2 to 12.5 but it was susceptible to general attack below a pH of 2. The surface of samples exposed to pH 1 solutions were characterised by thick, black deposits over the entire surface. There was an increase in pitting potential with increase in pH. The total change in pitting potential over the pH range 2 to 12.5 was ~35 mV.

According to another investigation (Friedman and Hanafee, 2000) the change in pitting potential was rather greater ~90 mV over the same sort of pH range. This investigation also found that chloride concentration in the range 0.001 to 0.1M NaCl did not have a significant effect on corrosion of beryllium. This conclusion was based on the observation that there was not much difference in passive range. It was stated that the size of the passive range, or the ability of a solution to break the oxide layer on the surface of the beryllium, appeared to be a function of pH, and not of chloride concentration. This result on chloride effect is not in agreement with the findings of Hill and co-workers (1996) and a recent investigation by Punni and Cox (2010).

A minimum in both the passive and corrosion current densities was observed in the pH range of 4 to 11 (Hill et al., 1996, 1998). The relationship of both passive current density and corrosion current density with solution pH is represented in Figure 3. This agrees well with the Pourbaix diagram (Pourbaix, 1966) for the beryllium water system at 25°C, as represented in Figure 1. This shows that between pH 4 and 11, the formation of insoluble species Be(OH)2 is thermodynamically favourable.

### **2.3 Crystallographic orientation effect**

`

4 Pitting Corrosion

The passivity and pitting of commercially produced beryllium has been studied extensively in chloride solutions. The key points for a typical cyclic polarisation curve from a recent polarisation study (Punni & Cox, 2010) for a commercial beryllium are displayed in Figure 2. It was observed that the anodic polarisation was characterised by a region of passivity followed by a logarithmic increase in the current density, which corresponded to the onset

Fig. 2. Typical cyclic polarisation curve for beryllium metal in 0.0001M KCl solution, sweep

Pitting Potential (Epit) Repassivation Potential (Erepass)

0000000 **Current Density (mA/cm<sup>2</sup>**

10-7 10-6 10-4 10-3 10-2 10-1 10-5

Start Finish

**)**

Passivation Current (Ipass)

A previous electrochemical study (Hill et al., 1996, 1998) in sodium chloride (NaCl) solution of varying chloride ion concentrations (from 0.0001 to 1M) showed that on increasing the chloride concentration, both pitting potential and repassivation potential decreased progressively and at 1M NaCl, the pitting commenced at open circuit conditions. A logarithmic relationship between pitting potential (in mV) and chloride concentration (in

 Epit = - 67 log [Cl-1] -1010 (4) The effect of pH on pitting corrosion behaviour of beryllium was studied by Hill and coworkers (1998). Beryllium was found to be passive in the pH range from 2 to 12.5 but it was susceptible to general attack below a pH of 2. The surface of samples exposed to pH 1 solutions were characterised by thick, black deposits over the entire surface. There was an increase in pitting potential with increase in pH. The total change in pitting potential over

According to another investigation (Friedman and Hanafee, 2000) the change in pitting potential was rather greater ~90 mV over the same sort of pH range. This investigation also

of pitting corrosion (Epit).


**Potential (mV, SCE)**

rate of 20mV/min, after Punni & Cox (2010)

Open Circuit Potential (OCP)

morality) was presented as given below.

the pH range 2 to 12.5 was ~35 mV.

The crystallographic orientation effect of commercial beryllium was described by Lillard (2000) and Friedman and Hanafee (2000). Pitting experiments indicated that once pit initiation has started, beryllium corrodes preferentially in certain orientations. Potentiodynamic polarisation studies for beryllium (0001), (1010) and (1120) surfaces were carried out in deaerated 0.01 M NaCl, as represented in Figure 4. The pitting potential (Epit) was found to decrease with crystal orientation in the order (0001) > (1010) > (1120). Repassivation potentials (Rrp) appeared to follow the same crystallographic trends as Epit. The potential region defined by Epit – Erp was large for (0001) and (1010) surfaces (>100mv) and appeared to be much smaller for the (1120) surface. There is a relationship between Epit and pit density on the surface such that for a higher Epit at a surface there is a smaller population density of pits and vice versa. The expression Epit – Erp represents the extent of pit growth. This implies that a surface orientation with large Epit and with large (Epit – Erp) would experience fewer, but deeper, pits.

Fig. 3. Passive current density, ipass, and corrosion current density, icorr, as a function of solution pH. A minimum in ipass and icorr exists between a pH of 4 and 11, after Hill et al. (1998)

Electrochemical Characterisation to Study the Pitting Corrosion Behaviour of Beryllium 7

material, the small fibres of unattacked beryllium were also observed in the interior in the (0001) surface but the orientation of these fibres was normal to (0001) surface. Similar differences in pit morphologies between the basal plane (0001) and prism planes (1010) and

In a previous investigation (Vaidya et al., 1998) pitted beryllium samples were tested under 4-point bending stress. Beryllium samples were exposed to 0.01, 0.1 and 1 M NaCl solutions for 168 hours. The resultant bending stress results (displacement to failure plots) are shown in Figure 5. The material exhibited a typical elastoplastic response, with a small amount of strain hardening. Displacement to failure and failure strength of the samples were affected by exposure to the NaCl solutions, however, the displacement to failure was much lower in

Fig. 5. Bending stress vs displacement to failure plots for as received and corroded beryllium

This was attributed to difference in the sizes and distribution of the pits formed on the surface of the samples. The fewer but deeper pits which formed on the samples exposed to 0.01 and 0.1 M NaCl solutions act as stress concentration sites and degrade the mechanical properties of the material to a greater extent than those exposed to 1M NaCl solutions.

The pitting corrosion process for beryllium is considered to be common with other metals and alloys (aluminium, titanium and stainless steel) which develop a passive oxide film. Following the development of the passive oxide film there are four processes (Szklarska-Smialowska, 1999) which lead to the onset of corrosion pits as; (1) Interactions occurring at the surface of the passive film; (2) interactions occurring within the passive film; (3)

(1120) were also observed by Friedman and Hanafee (2000).

**2.5 Performance of pitted beryllium under stress** 

0.1 M and 0.01 M solutions than in a 1 M solution.

samples after Vaidya et al. (1998)

**2.6 Mechanism of pitting corrosion** 

Fig. 4. Typical polarisation curves for (0001), (1010) and (1120) single crystal Be surfaces in deaerated 0.01 M NaCl solution, after Lillard (2000)

Cyclic polarisation studies on beryllium single crystals in 0.01M NaCl solution with a pH of 7, were also conducted by Friedman and Hanafee (2000). The size of the passive range differed in all three planes, but the basal plane differed most compared to the two prism planes. Interestingly, Erp was identical for all three crystal orientations; -864mV. The difference in the results from the two investigations may be explained by variations in electrochemical conditions.

Orientation imaging microscopy maps of polycrystalline beryllium indicated no correlation between pit initiation sites and crystallographic orientation of specific grains. Therefore, altering the bulk texture of polycrystalline beryllium will not affect the pitting corrosion resistance of beryllium, although it may affect pit propagation (Lillard, 2000).

### **2.4 Morphology of electrochemical corrosion pits**

The morphology of corrosion pits in polycrystalline commercial beryllium on electrochemical polarisation in 0.01M KCl solution was described by Hill et al. (1998). It was observed that the corrosion pits in beryllium have the same size and shape as the beryllium grain morphology. The pits were not hemispherical and parallel plates of unattacked beryllium were found inside the pits.

In the case of the single crystal study reported by Lillard (2000) for (1010) and (1120) surfaces, the pit interiors were characterised by crystallographically oriented parallel plates of unattacked beryllium. At greater depth these beryllium lamellae were transformed to small 'wires' or fibres of uniform diameter. For the beryllium (1010) surface, the orientation of the fibres was parallel to the (0001) direction and normal to the (1010) surface. For the beryllium surface (1120), the lamellae were parallel to the (0001) direction and normal to the (1120) surface. In comparison to the (1010) and (1120) surfaces, the interior of corrosion pits formed in the (0001) surface lacked any crystallographic orientation; however, the propagation was often in the (1010) and (1120) directions. As in the case of polycrystalline material, the small fibres of unattacked beryllium were also observed in the interior in the (0001) surface but the orientation of these fibres was normal to (0001) surface. Similar differences in pit morphologies between the basal plane (0001) and prism planes (1010) and (1120) were also observed by Friedman and Hanafee (2000).

### **2.5 Performance of pitted beryllium under stress**

6 Pitting Corrosion

Fig. 4. Typical polarisation curves for (0001), (1010) and (1120) single crystal Be surfaces in

Cyclic polarisation studies on beryllium single crystals in 0.01M NaCl solution with a pH of 7, were also conducted by Friedman and Hanafee (2000). The size of the passive range differed in all three planes, but the basal plane differed most compared to the two prism planes. Interestingly, Erp was identical for all three crystal orientations; -864mV. The difference in the results from the two investigations may be explained by variations in

Orientation imaging microscopy maps of polycrystalline beryllium indicated no correlation between pit initiation sites and crystallographic orientation of specific grains. Therefore, altering the bulk texture of polycrystalline beryllium will not affect the pitting corrosion

The morphology of corrosion pits in polycrystalline commercial beryllium on electrochemical polarisation in 0.01M KCl solution was described by Hill et al. (1998). It was observed that the corrosion pits in beryllium have the same size and shape as the beryllium grain morphology. The pits were not hemispherical and parallel plates of unattacked

In the case of the single crystal study reported by Lillard (2000) for (1010) and (1120) surfaces, the pit interiors were characterised by crystallographically oriented parallel plates of unattacked beryllium. At greater depth these beryllium lamellae were transformed to small 'wires' or fibres of uniform diameter. For the beryllium (1010) surface, the orientation of the fibres was parallel to the (0001) direction and normal to the (1010) surface. For the beryllium surface (1120), the lamellae were parallel to the (0001) direction and normal to the (1120) surface. In comparison to the (1010) and (1120) surfaces, the interior of corrosion pits formed in the (0001) surface lacked any crystallographic orientation; however, the propagation was often in the (1010) and (1120) directions. As in the case of polycrystalline

resistance of beryllium, although it may affect pit propagation (Lillard, 2000).

deaerated 0.01 M NaCl solution, after Lillard (2000)

**2.4 Morphology of electrochemical corrosion pits** 

beryllium were found inside the pits.

electrochemical conditions.

In a previous investigation (Vaidya et al., 1998) pitted beryllium samples were tested under 4-point bending stress. Beryllium samples were exposed to 0.01, 0.1 and 1 M NaCl solutions for 168 hours. The resultant bending stress results (displacement to failure plots) are shown in Figure 5. The material exhibited a typical elastoplastic response, with a small amount of strain hardening. Displacement to failure and failure strength of the samples were affected by exposure to the NaCl solutions, however, the displacement to failure was much lower in 0.1 M and 0.01 M solutions than in a 1 M solution.

Fig. 5. Bending stress vs displacement to failure plots for as received and corroded beryllium samples after Vaidya et al. (1998)

This was attributed to difference in the sizes and distribution of the pits formed on the surface of the samples. The fewer but deeper pits which formed on the samples exposed to 0.01 and 0.1 M NaCl solutions act as stress concentration sites and degrade the mechanical properties of the material to a greater extent than those exposed to 1M NaCl solutions.

### **2.6 Mechanism of pitting corrosion**

The pitting corrosion process for beryllium is considered to be common with other metals and alloys (aluminium, titanium and stainless steel) which develop a passive oxide film. Following the development of the passive oxide film there are four processes (Szklarska-Smialowska, 1999) which lead to the onset of corrosion pits as; (1) Interactions occurring at the surface of the passive film; (2) interactions occurring within the passive film; (3)

Electrochemical Characterisation to Study the Pitting Corrosion Behaviour of Beryllium 9

It may be noted that once carbide particles have been consumed no further corrosion should be observed. However, in the presence of corrosive ions in moist environments the above corrosion reaction may disrupt the continuity of the passivating film and provide a crevice

Earlier studies (Gulbrandsen & Johansen, 1994; Venugopal et al., 2000) have indicated that corrosion pits in beryllium may be associated with sites previously occupied by inclusions. Beryllium components for structural applications are generally produced by a powder metallurgy route and contain a number of impurities as a result of the powder production process, from which the pressed component is manufactured, and as a result of the powder pressing process itself. The major impurities found in such structural material include, beryllium oxide (> 0.5 wt. %), carbides (carbon up to 0.015 wt. %), silicon (~ 0.025 wt. %),

The purpose of the study at AWE was to understand the role these inclusions play in the initiation of localised corrosion attack. To accomplish this, the electrochemical characteristics of beryllium material containing differing impurity contents and distribution were assessed and the resulting localised corrosion sites evaluated. Earlier results of this investigation were published in a previous paper (Punni & Cox, 2010) and a brief account of this work

Samples measuring 12.5 mm in diameter and 2 mm thick were machined from three different beryllium pressings, i.e. a small vacuum hot pressed bar produced from Brush Wellman S65 specification power (S65-Bar), a large vacuum hot pressed billet also produced from S65 specification power (S65-Billet), and a small vacuum hot pressed bar produced from Kawecki Berylco P10 specification powder (P10-Bar). All pressings had been consolidated using graphite dies under a pressure of ~7 MN/m2 and at a temperature of 1000 to 1100 ºC, followed by a heat treatment at 800 ºC. The metallic impurity content for each pressing was determined by Emission Spectroscopy via Direct Coupled Plasma, BeO by Inert Gas Fusion (LECO method), and carbon by combustion (LECO method). The

To understand the pit initiation sites it is important to know the microstructure for all the three beryllium grades. For this task, samples were progressively polished down to 0.25 µm diamond finish. Polished samples were examined in a Hitachi SEM with the impurity inclusions being analysed using the associated EDS system (Oxford Instruments). Secondary

For pit initiation treatment the same polished samples were subjected to an electrochemical polarisation treatment to initiate tiny corrosion pits at the polished surface. This was done in 0.001 M KCl solution at a fast sweep rate of 600 mV/min. Polarisation started at -1100 mV SCE and ended at -500 mV SCE and the time during which the sample stayed in the pitting range (-800mV SCE to -500mV SCE) was ~30 seconds; referred to as the exposure time for

electron (SE) images and EDS spectra showing elemental analysis were recorded.

site for further reaction.

and the intermetallic compounds.

**3.2 Experimental procedure** 

**3.2.1 Material** 

with updated information is described here.

chemical composition of these grades is given in Table 1.

**3.2.2 SEM examination and pit initiation treatment** 

formation of metastable pits which soon repassivate; and (4) stable pit growth, above certain potential termed the critical pitting potential.

The first two stages are concerned with the breakdown of film by the interaction of chloride ions, with very little being known about the interaction mechanism. This is certainly dependent upon the composition and structure of the oxide film and the underlying material. The structural characteristics of the oxide are dependent on the material composition and hence the presence and distribution of micro-defects (vacancies, voids, etc.) as well as macro-defects (inclusions, second phase particles and their size and shape), crystal structure and the degree of noncrytalinity of the oxide. It also depends on the electrolyte, its composition, pH value and temperature (Szklarska-Smialowska, 1999).

Metastable pits form sometimes just before the pitting potential is reached. When these occur first the current increases as the pit nucleate and grow, then decreasing after a short delay. It was found that metastable pits are covered by a remnant hard oxide film. It is well established that metastable pits sometimes form several hundred milli volts below the pitting potential and during the induction time for stable pit formation. There are a number of studies for metastable pits on steel and aluminium (Blanc & Mankowski, 1997; Pride et al., 1994) but few on beryllium (Lillard, 2000).

According to a previously suggested mechanism (West, 1970) a filmed metal may begin to dissolve at sensitive points. These sensitive points may be crystallographic defects, cavities or scratches in metal, or a rift in surface film due to high internal stresses during oxide growth. Some of these sensitive points are associated with the localised chemical deficiencies in the film where there are underlying inclusions. As the dissolution proceeds at localised points where the film is impaired, the remaining intact surface film acts as a cathodic area. At this stage, two other important processes are taking place inside the pore (a shallow pit). Firstly the attempt by the film to repair itself at the pore consumes hydroxyl ions so the acidity within the pore is increased. Secondly the pore being an anodic site, causes various aggressive ions such as Cl-1 to accumulate within the pore. Being highly deformable, chloride ions are surface active, so they displace water molecules from the double layer. The film in the pore therefore is prevented from repairing itself. At the same time, depletion of aggressive ions from the immediate vicinity of the pore makes it more difficult for the anodic reaction to spread sideways. This action together with a large surface area acting as cathode makes an accelerated dissolution at the localised area of pore, thus promoting it to become a narrow deep pit.

### **3. Investigation on the effect of inclusions on pitting corrosion behaviour of beryllium**

### **3.1 Introduction**

Mueller & Adolphson concluded that pitting corrosion is associated with beryllium carbide particles. Carbon arises as one of the primary impurities in historic grades of beryllium to 0.2 wt% or more, which results in formation of second-phase particles (Be2C). In the presence of moisture these particles quickly react to form BeO and methane.

$$\text{Be} \text{C} + 2 \text{ H} \text{MgO} \rightarrow 2 \text{ BeO} + \text{CH}\_4 \tag{5}$$

It may be noted that once carbide particles have been consumed no further corrosion should be observed. However, in the presence of corrosive ions in moist environments the above corrosion reaction may disrupt the continuity of the passivating film and provide a crevice site for further reaction.

Earlier studies (Gulbrandsen & Johansen, 1994; Venugopal et al., 2000) have indicated that corrosion pits in beryllium may be associated with sites previously occupied by inclusions. Beryllium components for structural applications are generally produced by a powder metallurgy route and contain a number of impurities as a result of the powder production process, from which the pressed component is manufactured, and as a result of the powder pressing process itself. The major impurities found in such structural material include, beryllium oxide (> 0.5 wt. %), carbides (carbon up to 0.015 wt. %), silicon (~ 0.025 wt. %), and the intermetallic compounds.

The purpose of the study at AWE was to understand the role these inclusions play in the initiation of localised corrosion attack. To accomplish this, the electrochemical characteristics of beryllium material containing differing impurity contents and distribution were assessed and the resulting localised corrosion sites evaluated. Earlier results of this investigation were published in a previous paper (Punni & Cox, 2010) and a brief account of this work with updated information is described here.

### **3.2 Experimental procedure**

### **3.2.1 Material**

8 Pitting Corrosion

formation of metastable pits which soon repassivate; and (4) stable pit growth, above certain

The first two stages are concerned with the breakdown of film by the interaction of chloride ions, with very little being known about the interaction mechanism. This is certainly dependent upon the composition and structure of the oxide film and the underlying material. The structural characteristics of the oxide are dependent on the material composition and hence the presence and distribution of micro-defects (vacancies, voids, etc.) as well as macro-defects (inclusions, second phase particles and their size and shape), crystal structure and the degree of noncrytalinity of the oxide. It also depends on the electrolyte, its

Metastable pits form sometimes just before the pitting potential is reached. When these occur first the current increases as the pit nucleate and grow, then decreasing after a short delay. It was found that metastable pits are covered by a remnant hard oxide film. It is well established that metastable pits sometimes form several hundred milli volts below the pitting potential and during the induction time for stable pit formation. There are a number of studies for metastable pits on steel and aluminium (Blanc & Mankowski, 1997; Pride et

According to a previously suggested mechanism (West, 1970) a filmed metal may begin to dissolve at sensitive points. These sensitive points may be crystallographic defects, cavities or scratches in metal, or a rift in surface film due to high internal stresses during oxide growth. Some of these sensitive points are associated with the localised chemical deficiencies in the film where there are underlying inclusions. As the dissolution proceeds at localised points where the film is impaired, the remaining intact surface film acts as a cathodic area. At this stage, two other important processes are taking place inside the pore (a shallow pit). Firstly the attempt by the film to repair itself at the pore consumes hydroxyl ions so the acidity within the pore is increased. Secondly the pore being an anodic site, causes various aggressive ions such as Cl-1 to accumulate within the pore. Being highly deformable, chloride ions are surface active, so they displace water molecules from the double layer. The film in the pore therefore is prevented from repairing itself. At the same time, depletion of aggressive ions from the immediate vicinity of the pore makes it more difficult for the anodic reaction to spread sideways. This action together with a large surface area acting as cathode makes an accelerated dissolution at the localised area of pore, thus

**3. Investigation on the effect of inclusions on pitting corrosion behaviour of** 

Mueller & Adolphson concluded that pitting corrosion is associated with beryllium carbide particles. Carbon arises as one of the primary impurities in historic grades of beryllium to 0.2 wt% or more, which results in formation of second-phase particles (Be2C). In the

Be2C + 2 H2O → 2 BeO + CH4 (5)

presence of moisture these particles quickly react to form BeO and methane.

composition, pH value and temperature (Szklarska-Smialowska, 1999).

potential termed the critical pitting potential.

al., 1994) but few on beryllium (Lillard, 2000).

promoting it to become a narrow deep pit.

**beryllium** 

**3.1 Introduction** 

Samples measuring 12.5 mm in diameter and 2 mm thick were machined from three different beryllium pressings, i.e. a small vacuum hot pressed bar produced from Brush Wellman S65 specification power (S65-Bar), a large vacuum hot pressed billet also produced from S65 specification power (S65-Billet), and a small vacuum hot pressed bar produced from Kawecki Berylco P10 specification powder (P10-Bar). All pressings had been consolidated using graphite dies under a pressure of ~7 MN/m2 and at a temperature of 1000 to 1100 ºC, followed by a heat treatment at 800 ºC. The metallic impurity content for each pressing was determined by Emission Spectroscopy via Direct Coupled Plasma, BeO by Inert Gas Fusion (LECO method), and carbon by combustion (LECO method). The chemical composition of these grades is given in Table 1.

### **3.2.2 SEM examination and pit initiation treatment**

To understand the pit initiation sites it is important to know the microstructure for all the three beryllium grades. For this task, samples were progressively polished down to 0.25 µm diamond finish. Polished samples were examined in a Hitachi SEM with the impurity inclusions being analysed using the associated EDS system (Oxford Instruments). Secondary electron (SE) images and EDS spectra showing elemental analysis were recorded.

For pit initiation treatment the same polished samples were subjected to an electrochemical polarisation treatment to initiate tiny corrosion pits at the polished surface. This was done in 0.001 M KCl solution at a fast sweep rate of 600 mV/min. Polarisation started at -1100 mV SCE and ended at -500 mV SCE and the time during which the sample stayed in the pitting range (-800mV SCE to -500mV SCE) was ~30 seconds; referred to as the exposure time for

Electrochemical Characterisation to Study the Pitting Corrosion Behaviour of Beryllium 11

**Coarse Inclusions:** All beryllium grades showed some coarse inclusions, 5 to 18 µm in diameter. The population and size of these coarse inclusions were greater in P10-Bar than in the other two grades. These coarse inclusions along with the fine inclusions (< 5 µm in size) can be seen in SEM images shown in Figures 6 (a to c). Most of the coarse inclusions appeared to be partially broken or dissolved by the abrading and polishing operations. The EDS analysis identified the coarse inclusions to be mainly elemental silicon, and mixed beryllium carbides containing Al, Si, Fe and occasionally other elements such as Ti, Mg, Cr

**Inclusion Type S65-Bar S65-Billet P10-Bar** 

size)

Mainly detected as coarse (5-12 µm in

Detected as coarse type (5-10 µm in size )

Detected as a fine type (~2 to 4 µm)

Fine type (2 to 4 µm size), relatively larger size than other two

Mostly detected as a fine type (~3 to 5 µm)

Relatively coarser dispersion

(0.4 to 1 µm in size)

grades

Mainly detected as coarse type (8-15 µm in size), relatively high population than other two grades

Coarse particle size 5 to 18 µm, relatively high population than other two grades

Detected as a fine type (~2 to 4 µm)

Fine type (1 to 2 µm

Mostly detected as a fine type (~3 to 5 µm)

Relatively coarser dispersion

(0.4 to 1 µm in size)

size)

Mainly detected as coarse type (5-10 µm

type (5-10 µm in size )

Detected as a fine type (~2 to 4 µm)

Fine type (1 to 2 µm

Mostly detected as a fine type (~3 to 5 µm)

Fine dispersion (0.2 to 0.5 µm in size) but more densely

populated than other

Table 2. Composition and particle size for each type of inclusion in the three beryllium

**Fine Inclusions:** The fine inclusions (0.25 to 5 µm in size) can be seen in Figures 6 to 8. These inclusions were examined using EDS analysis, as shown in Figures 7 and 8 and recorded in Table 2. Broadly speaking the fine inclusions at grain boundaries can be classified as finely dispersed oxide and intermetallic phases. EDS identified the finely dispersed oxide to contain the elements Be and O and is therefore probably the hexagonal compound BeO. These oxide inclusions were relatively finer in size and more numerous in the S65-Bar than in the other two grades. The intermetallic phases Al/Fe/Be and occasionally Si/Ti or Si/Al

two grades

size)

in size )

**Elemental Silicon:** Detected as coarse

and U (Table 2).

**Mixed beryllium carbides: containing Si, Al, and Fe, sometimes had association of Ti,** 

**Beryllium carbides: (possibly Be2C)** 

**Intermetallic, Al/Fe/Be: possibly AlFeBe4** 

**Intermetallic, Si/Ti and Si/Al (with possible association of Be)** 

**Beryllium Oxide:**

specifications

**(BeO)** 

**Cr, Mg or U** 


pit initiation treatment. After the pit initiation treatment the samples were rinsed in distilled water and wiped with ethanol soaked tissues. Samples were then examined again in the Hitachi SEM to locate any pit initiation sites and to perform elemental analysis on those sites.

Table 1. The compositions (wt %) of three different beryllium specifications studied in this investigation

### **3.2.3 Polarisation technique**

This technique is described in greater detail in a previous investigation (Punni & Cox, 2010). Samples for polarisation tests were ground down to a 600 grit silicon carbide paper finish. A custom designed glass electrochemical cell, equipped with a platinum counter electrode, noise electrode and a saturated calomel reference electrode (SCE) through a Luggin probe, was used in this study.

The potentiodynamic polarisation tests were carried out at room temperature (20 ± 2 ºC) at a sweep rate of 20 mV/min using a Gill AC Potentiostat. Some polarisation tests were carried out at a sweep rate of 10 mV/min. Tests were performed in a deaerated 600 ml potassium chloride (KCl) solution of 0.0001, 0.001, 0.01 or 0.1 M chloride concentrations with pH adjusted to 7, by adding a few drops of dilute potassium hydroxide solution. To ensure dynamic equilibrium, samples were left at their open circuit potential for 1 hour before each polarisation test was run. Some electrochemically polarised samples were also examined in a Hitachi SEM model S3400N to characterise the extent and nature of the corrosion pits.

### **3.3 Results and discussion**

### **3.3.1 Microstructures of the three beryllium grades**

SEM examination revealed that inclusions, varying in size and composition, were situated at the grain boundaries, as summarised in Table 2.

pit initiation treatment. After the pit initiation treatment the samples were rinsed in distilled water and wiped with ethanol soaked tissues. Samples were then examined again in the Hitachi SEM to locate any pit initiation sites and to perform elemental analysis on those sites.

Element/Compound S65-Bar S65-Billet P10-Bar Uncertainty of

Table 1. The compositions (wt %) of three different beryllium specifications studied in this

This technique is described in greater detail in a previous investigation (Punni & Cox, 2010). Samples for polarisation tests were ground down to a 600 grit silicon carbide paper finish. A custom designed glass electrochemical cell, equipped with a platinum counter electrode, noise electrode and a saturated calomel reference electrode (SCE) through a Luggin probe,

The potentiodynamic polarisation tests were carried out at room temperature (20 ± 2 ºC) at a sweep rate of 20 mV/min using a Gill AC Potentiostat. Some polarisation tests were carried out at a sweep rate of 10 mV/min. Tests were performed in a deaerated 600 ml potassium chloride (KCl) solution of 0.0001, 0.001, 0.01 or 0.1 M chloride concentrations with pH adjusted to 7, by adding a few drops of dilute potassium hydroxide solution. To ensure dynamic equilibrium, samples were left at their open circuit potential for 1 hour before each polarisation test was run. Some electrochemically polarised samples were also examined in a Hitachi SEM model S3400N to characterise the extent and nature of the corrosion pits.

SEM examination revealed that inclusions, varying in size and composition, were situated at

investigation

**3.2.3 Polarisation technique** 

was used in this study.

**3.3 Results and discussion** 

**3.3.1 Microstructures of the three beryllium grades** 

the grain boundaries, as summarised in Table 2.

Be 99.3 99.23 98.46 Balance BeO 0.56 0.6 1.18 ± 0.04 C 0.03 0.015 0.08 ± 0.009 Si 0.025 0.028 0.028 ±0.0024 Al 0.02 0.033 0.045 ± 0.0020 Fe 0.056 0.075 0.133 ±0.0032 Mg 0.0005 <0.0005 0.013 ± 0.0023 U 0.004 <0.0030 0.027 ± 0.0043 Co 0.001 0.0007 0.0012 ± 0.0003 Cr 0.0025 0.0025 0.0135 ± 0.0005 Cu 0.0025 0.0065 0.007 ± 0.00016 Ti 0.0045 0.011 0.011 ± 0.0003

Measurements

**Coarse Inclusions:** All beryllium grades showed some coarse inclusions, 5 to 18 µm in diameter. The population and size of these coarse inclusions were greater in P10-Bar than in the other two grades. These coarse inclusions along with the fine inclusions (< 5 µm in size) can be seen in SEM images shown in Figures 6 (a to c). Most of the coarse inclusions appeared to be partially broken or dissolved by the abrading and polishing operations. The EDS analysis identified the coarse inclusions to be mainly elemental silicon, and mixed beryllium carbides containing Al, Si, Fe and occasionally other elements such as Ti, Mg, Cr and U (Table 2).


Table 2. Composition and particle size for each type of inclusion in the three beryllium specifications

**Fine Inclusions:** The fine inclusions (0.25 to 5 µm in size) can be seen in Figures 6 to 8. These inclusions were examined using EDS analysis, as shown in Figures 7 and 8 and recorded in Table 2. Broadly speaking the fine inclusions at grain boundaries can be classified as finely dispersed oxide and intermetallic phases. EDS identified the finely dispersed oxide to contain the elements Be and O and is therefore probably the hexagonal compound BeO. These oxide inclusions were relatively finer in size and more numerous in the S65-Bar than in the other two grades. The intermetallic phases Al/Fe/Be and occasionally Si/Ti or Si/Al

Electrochemical Characterisation to Study the Pitting Corrosion Behaviour of Beryllium 13

was unable to be quantified with this technique. From previous findings it is anticipated this intermetallic will be either AlFeBe4 (Carrabine, 1963) or AlFeBe5 (Rooksby, 1962). These inclusions were relatively bigger in size and more numerous in the S65-Billet material compared to the other two grades. Small sized (~3 µm) particles containing only Be and C which are most probably the compound Be2C were identified in all the three grades. In general, the shapes of the inclusions varied; the Al/Fe/Be inclusions were either L-shaped or elongated while all other inclusions were either round or in some cases

3

2 4

**Spectrum 1 Spectrum 2**

**Spectrum 3 Spectrum 4** 

2

Fig. 7. EDS Spectra from inclusions in beryllium (a) S65-Bar and (b) P10-Bar (a number on

an inclusion relates it to the correspondingly numbered typical EDS spectrum)

(a) SE Image for Be S65-Bar (b) SE Image for Be P10-Bar

Si

2

elongated.

1

Fig. 6. SEM Images of polished beryllium surfaces from thee beryllium grades

with or without association of Be, were also detected. EDS analysis of the Al/Fe/Be inclusions, showed that the atomic percentage of Fe and Al to be equal, however the Be

**Fine Oxide Dispersion** 

(a) S65-Bar

(b) S65-Billet

(c) P10-Bar

Fig. 6. SEM Images of polished beryllium surfaces from thee beryllium grades

**Coarse Carbide** 

> **Fine Carbide**

**Coarse Carbide** 

**Fine Al/Fe/Be** 

**Fine Al/Fe/Be Ili**

**Inclusion Coarse elemental** 

**Silicon**

**Fine Oxide Dispersion** 

with or without association of Be, were also detected. EDS analysis of the Al/Fe/Be inclusions, showed that the atomic percentage of Fe and Al to be equal, however the Be

**Fine Al/Fe/Be**  was unable to be quantified with this technique. From previous findings it is anticipated this intermetallic will be either AlFeBe4 (Carrabine, 1963) or AlFeBe5 (Rooksby, 1962). These inclusions were relatively bigger in size and more numerous in the S65-Billet material compared to the other two grades. Small sized (~3 µm) particles containing only Be and C which are most probably the compound Be2C were identified in all the three grades. In general, the shapes of the inclusions varied; the Al/Fe/Be inclusions were either L-shaped or elongated while all other inclusions were either round or in some cases elongated.

Fig. 7. EDS Spectra from inclusions in beryllium (a) S65-Bar and (b) P10-Bar (a number on an inclusion relates it to the correspondingly numbered typical EDS spectrum)

particles).

30s exposure in 0.001M KCl

.

Electrochemical Characterisation to Study the Pitting Corrosion Behaviour of Beryllium 15

shown in Figure 9 (b) had initiated at the Al/Fe/Be inclusions and one had initiated at elemental silicon. There was some evidence of pits initiating at mixed beryllium carbide inclusions, and in such cases the inclusions themselves had corroded. This agrees with the pitting mechanism proposed by Mueller and Adolphson that pits initiate at beryllium carbide inclusions. In the case of intermetallic Al/Fe/Be or elemental silicon inclusions, pits had initiated at the interface between the inclusion and the surrounding metal (inclusions being intact at the edge of the pit as seen in Figure 9), indicating that these inclusions are nobler than the beryllium matrix. Work by Vaidya and co-workers (Vaidya et al., 1999) has suggested that BeO particles can also provide pit initiation sites due to their inhomogeneity with the metal matrix. Although a few isolated corrosion pits had initiated without any sign of Al/Fe/Be, elemental silicon or carbide inclusions, there was no conclusive evidence to support the above suggestion that BeO can provide pit initiation sites. Furthermore, no pits were detected at any other type of intermetallic inclusions (i.e. Si/Ti or Si/Al intermetallic

Fig. 9. Comparison of beryllium S65-Bar surfaces before and after pit initiation treatment for

(b) Same surface (as above) after pit initiation

(a) Polished surface of beryllium S65-Bar

Fig. 8. Elemental images of inclusions in beryllium P10-Bar

### **3.3.2 Pit initiation sites and pit morphology**

Surface morphologies before and after pit initiation polarisation treatment for grade S65-Bar are shown in Figures 9 (a and b). The initiation sites for corrosion pits before and after polarisation are indicated by arrows. From these figures it is clear that corrosion pits nearly always initiated at inclusions in the grain boundaries. In very rare cases the corrosion pits had initiated without any sign of inclusions. As detected by EDS the majority of the pits

Fig. 8. Elemental images of inclusions in beryllium P10-Bar

Fe Al

Surface morphologies before and after pit initiation polarisation treatment for grade S65-Bar are shown in Figures 9 (a and b). The initiation sites for corrosion pits before and after polarisation are indicated by arrows. From these figures it is clear that corrosion pits nearly always initiated at inclusions in the grain boundaries. In very rare cases the corrosion pits had initiated without any sign of inclusions. As detected by EDS the majority of the pits

**3.3.2 Pit initiation sites and pit morphology** 

SE Image O

C Si

shown in Figure 9 (b) had initiated at the Al/Fe/Be inclusions and one had initiated at elemental silicon. There was some evidence of pits initiating at mixed beryllium carbide inclusions, and in such cases the inclusions themselves had corroded. This agrees with the pitting mechanism proposed by Mueller and Adolphson that pits initiate at beryllium carbide inclusions. In the case of intermetallic Al/Fe/Be or elemental silicon inclusions, pits had initiated at the interface between the inclusion and the surrounding metal (inclusions being intact at the edge of the pit as seen in Figure 9), indicating that these inclusions are nobler than the beryllium matrix. Work by Vaidya and co-workers (Vaidya et al., 1999) has suggested that BeO particles can also provide pit initiation sites due to their inhomogeneity with the metal matrix. Although a few isolated corrosion pits had initiated without any sign of Al/Fe/Be, elemental silicon or carbide inclusions, there was no conclusive evidence to support the above suggestion that BeO can provide pit initiation sites. Furthermore, no pits were detected at any other type of intermetallic inclusions (i.e. Si/Ti or Si/Al intermetallic particles).

(a) Polished surface of beryllium S65-Bar

(b) Same surface (as above) after pit initiation

Fig. 9. Comparison of beryllium S65-Bar surfaces before and after pit initiation treatment for 30s exposure in 0.001M KCl

Electrochemical Characterisation to Study the Pitting Corrosion Behaviour of Beryllium 17

(a) Typical topography of an electrochemically produced pit after 30 s exposure in 0.001M KCl

Fig. 11. Typical morphology of corrosion pit produced by electrochemical polarisation and

(b) Typical morphology of a pit developed after ageing for 120 days at 75°C in a relative humidity

In the case of S65-Billet, the samples were subjected to two pit initiation treatments, the results of which are shown in Figures 10 (a to c). The results of the first initiation treatment are shown in Figures 10 (a) and (b) where the corrosion pit locations are marked by red arrows. The result of the second initiation treatment is shown in Figures 10 (b) and (c) where the new additional pit locations are marked by orange coloured arrows. It was found that the majority of existing corrosion pits did not grow any further; however, some isolated pits had grown up to 50% of their original size. Apart from the growth of some of the existing corrosion pits, many new pits had initiated, varying in size from 1 to 30 µm. The majority of these new pits had initiated at Al/Fe/Be inclusions as was the case after the first pit

Another investigation is underway at AWE to study growth kinetics of the corrosion pits on beryllium grade S65-Bar. In this study the corrosion pits were initiated using electrochemical polarisation and subsequently the samples were aged at 55°C, 65°C and 75°C in ovens at 12% to 16% relative humidity. This work is out of the scope for this chapter;

its comparison with that developed during ageing

of 16%.

initiation treatment.

(c) After 2nd pit initiation

Fig. 10. Comparison of beryllium S65-Billet surfaces before and after pit initiation treatment for 30s exposure in 0.001M KCl

(a) Polished Be surface

(b) After 1st pit initiation

(c) After 2nd pit initiation

Fig. 10. Comparison of beryllium S65-Billet surfaces before and after pit initiation treatment

for 30s exposure in 0.001M KCl

(a) Typical topography of an electrochemically produced pit after 30 s exposure in 0.001M KCl

(b) Typical morphology of a pit developed after ageing for 120 days at 75°C in a relative humidity of 16%.

Fig. 11. Typical morphology of corrosion pit produced by electrochemical polarisation and its comparison with that developed during ageing

In the case of S65-Billet, the samples were subjected to two pit initiation treatments, the results of which are shown in Figures 10 (a to c). The results of the first initiation treatment are shown in Figures 10 (a) and (b) where the corrosion pit locations are marked by red arrows. The result of the second initiation treatment is shown in Figures 10 (b) and (c) where the new additional pit locations are marked by orange coloured arrows. It was found that the majority of existing corrosion pits did not grow any further; however, some isolated pits had grown up to 50% of their original size. Apart from the growth of some of the existing corrosion pits, many new pits had initiated, varying in size from 1 to 30 µm. The majority of these new pits had initiated at Al/Fe/Be inclusions as was the case after the first pit initiation treatment.

Another investigation is underway at AWE to study growth kinetics of the corrosion pits on beryllium grade S65-Bar. In this study the corrosion pits were initiated using electrochemical polarisation and subsequently the samples were aged at 55°C, 65°C and 75°C in ovens at 12% to 16% relative humidity. This work is out of the scope for this chapter;

Electrochemical Characterisation to Study the Pitting Corrosion Behaviour of Beryllium 19

There is a similar evidence of pit initiation at the intermetallic inclusions in other passive metals i.e. sigma phase in duplex steels (Mathiesen & Hansen, 2010) and Al3Fe, Al/Cu/Mg, Al/Cu/Fe and Al2Cu in aluminium (Szklarska-Smialowska, 1999). All these inclusions are suggested to act as the cathode to initiate the corrosion reaction in the adjacent matrix. There could be other Al/Mg/Mn, Al/Mn/Cr and Al/Mn/Si inclusions in aluminium which are anodic to matrix and are harmless but pits may nucleate at these sites due to dissolution of these particles themselves (Szklarska-Smialowska, 1999). The geometry of inclusions may also affect the pitting behaviour. The difference in the pitting behaviour of 6056 and 2024 aluminium alloys was explained by the difference in behaviour of coarse particles in these

Fig. 13. Morphologies of typical corrosion pits initiated at Al/Fe/Be or silicon inclusions after ageing of pre-pitted surfaces at 55°C for 120 days in an environment with RH 16%

Corrosion pit initiated at Al/Fe/Be inclusion Another example of pit initiation at Al/Fe/Be

inclusion

Al/Fe/Be Inclusion

Silicon Inclusion

> Silicon Oxide

As discussed in section 2.6, the mechanism of film breakdown by inclusions is not clear at this stage, however, it is anticipated that composition or structure of passive film is altered at the site of underlying inclusions. The effected oxide at these localised sites could be more reactive to the chloride ions and result in film breakdown there (Blanc & Mankowski, 1997;

Corrosion pit initiated at elemental silicon inclusion Another example of pit initiation at elemental silicon

inclusion

alloys (Blanc & Mankowski, 1997).

Electrochemically produced corrosion pit

> Silicon Inclusion

Al/Fe/Be Inclusion

however, some relevant features of corrosion pit formation are described here. This work provided a good comparison between morphologies of electrochemically produced pits with those produced by humidity controlled experiments as shown in Figure 11 (a and b)). Pits produced by electrochemical polarisation showed pit walls and parallel plates of unattacked beryllium lamella left behind after pit propagation, similar to the one observed by Hill et al. (1996). On the other hand pits produced by ageing were covered with corrosion products containing oxygen (main element), silicon, aluminium and trace amount of chlorine. Examination of aged surfaces revealed there was no further growth of large (up to 50 µm) electrochemically produced corrosion pits. In addition to these large pits, there were very small corrosion or etch pits (<3 µm) which had initiated at the intermetallic Al/Fe/Be or elemental silicon inclusions and these grew further on ageing, as illustrated in Figures 12. Figure 13 shows morphologies of some other corrosion pits formed at the inclusion particles, this confirms that even under the controlled humidity conditions, Al/Fe/Be and elemental silicon inclusions are the preferential sites for pit initiation.

(b) Same surface (as above) after ageing, showing a pit growth at an inclusion

Fig. 12. Secondary electron images showing pit growth (at a site marked by arrows) on ageing at 55°C for 60 days in an environment with RH 16%

There is a similar evidence of pit initiation at the intermetallic inclusions in other passive metals i.e. sigma phase in duplex steels (Mathiesen & Hansen, 2010) and Al3Fe, Al/Cu/Mg, Al/Cu/Fe and Al2Cu in aluminium (Szklarska-Smialowska, 1999). All these inclusions are suggested to act as the cathode to initiate the corrosion reaction in the adjacent matrix. There could be other Al/Mg/Mn, Al/Mn/Cr and Al/Mn/Si inclusions in aluminium which are anodic to matrix and are harmless but pits may nucleate at these sites due to dissolution of these particles themselves (Szklarska-Smialowska, 1999). The geometry of inclusions may also affect the pitting behaviour. The difference in the pitting behaviour of 6056 and 2024 aluminium alloys was explained by the difference in behaviour of coarse particles in these alloys (Blanc & Mankowski, 1997).

18 Pitting Corrosion

however, some relevant features of corrosion pit formation are described here. This work provided a good comparison between morphologies of electrochemically produced pits with those produced by humidity controlled experiments as shown in Figure 11 (a and b)). Pits produced by electrochemical polarisation showed pit walls and parallel plates of unattacked beryllium lamella left behind after pit propagation, similar to the one observed by Hill et al. (1996). On the other hand pits produced by ageing were covered with corrosion products containing oxygen (main element), silicon, aluminium and trace amount of chlorine. Examination of aged surfaces revealed there was no further growth of large (up to 50 µm) electrochemically produced corrosion pits. In addition to these large pits, there were very small corrosion or etch pits (<3 µm) which had initiated at the intermetallic Al/Fe/Be or elemental silicon inclusions and these grew further on ageing, as illustrated in Figures 12. Figure 13 shows morphologies of some other corrosion pits formed at the inclusion particles, this confirms that even under the controlled humidity conditions,

Al/Fe/Be and elemental silicon inclusions are the preferential sites for pit initiation.

(a) Pre-pitted (using electrochemical polarisation)

Fig. 12. Secondary electron images showing pit growth (at a site marked by arrows) on

(b) Same surface (as above) after ageing, showing

ageing at 55°C for 60 days in an environment with RH 16%

a pit growth at an inclusion

surface before ageing

Corrosion pit initiated at Al/Fe/Be inclusion Another example of pit initiation at Al/Fe/Be inclusion

Corrosion pit initiated at elemental silicon inclusion Another example of pit initiation at elemental silicon inclusion

Fig. 13. Morphologies of typical corrosion pits initiated at Al/Fe/Be or silicon inclusions after ageing of pre-pitted surfaces at 55°C for 120 days in an environment with RH 16%

As discussed in section 2.6, the mechanism of film breakdown by inclusions is not clear at this stage, however, it is anticipated that composition or structure of passive film is altered at the site of underlying inclusions. The effected oxide at these localised sites could be more reactive to the chloride ions and result in film breakdown there (Blanc & Mankowski, 1997;

Electrochemical Characterisation to Study the Pitting Corrosion Behaviour of Beryllium 21

observed that polarisation at the slower sweep rate results in a denser population of

Pitting Potential, mV SCE

S65-Bar -1068 ± 67 -750 ± 7 -802 ± 10 0.51 ± 0.08 318

S65-Billet -1032 ± 22 -754 ± 16 -811 ± 17 0.46 ± 0.16 278

P10-Bar -1033 ±81 -773 ± 25 -831 ± 1 0.34 ± 0.03 260

S65-Bar -974 ± 66 -816 ± 21 -922 ± 26 0.31 ± 0.21 158

S65-Billet -934 ± 30 -835 ± 22 -926 ± 22 0.38 ± 0.22 99

P10-Bar -937 ± 17 -838 ± 25 -930 ± 16 0.28 ±0.20 99

S65-Bar -1029 ± 36 -898 ± 21 -977 ± 7 0.36 ± 0.25 131

S65-Billet -1028 ± 17 -919 ± 2 -975 ± 9 0.40 ± 0.14 109

P10-Bar -1020 ± 28 -909 ±16 -962 ± 11 0.34 ± 0.11 111

0.1M KCl S65-Bar -1022 ± 42 -978 ± 4 -1000 ± 4 0.69 ± 0.35 44

Figure 15 shows graphically how the pitting potentials (as listed in Table 3) for the three beryllium grades vary with chloride concentration. In all the three cases the onset of pitting potential (Epit) was found to decrease logarithmically with increasing chloride

The overall relationship for pitting potential variation with chloride concentration is

 Epit = - 72 log [Cl-1] -1044 (6) Where Epit is in mV vs SCE and [Cl-1] is the chloride concentration in molarity. This relationship is very close to that observed by Hill et al. (1998) for beryllium grade S200D (see

Table 3. Pitting corrosion data from potentiodynamic polarisation curves in deaerated

Repassivation Potential, mV SCE

Passive Current Density, µA/cm2

Passive Range, mV

corrosion pits.

0.0001M KCl

0.001M KCl

0.01M KCL

concentration.

Equation 4).

Solution Beryllium

Specification

potassium chloride solution at pH 7.0

represented by the relationship:

Open Circuit Potential, mV SCE

West 1970). It is also evident from this investigation that certain inclusions cause galvanic action with the matrix to initiate pitting, as the corrosion pit sites had the presence of intermetallic Al/Fe/Be and elemental silicon inclusions (Figure 13) suggesting that these act as cathode to promote corrosion of the surrounding metal . Other inclusions like carbides or any less noble inclusions may also result in pit initiation by dissolving themselves preferentially to the matrix.

### **3.3.3 Electrochemical polarisation of the three beryllium grades**

Potentiodynamic polarisation was performed for the three beryllium grades in various chloride concentrations, from 0.0001 M to 0.1 M KCl solutions. Typical polarisation curves for all the beryllium grades are shown in Figure 14. This figure shows that the pitting potential of S65-Bar at -745mV SCE is higher than those for P10-Bar (-790 mV SCE) and S65- Billet (-765 mV SCE) in a 0.0001 M KCl solution. Similar differences in polarisation behaviour were observed for all the grades in 0.001M and 0.01 M KCl solution. The results from the polarisation curves for all the three grades are summarised in Table 3. This table displays the average values of open circuit potential (OCP), pitting potential (Epit), repassivation potential (Erepass), passive current density (ipassive) and passive range (Epit - OCP).

Fig. 14. Typical polarisation curves for 3 beryllium grades in 0.0001M KCl solution, sweep rate of 20mV/min

The surface condition of samples (from three beryllium grades) after polarisation in 0.001M KCl solutions was visualised. It was observed that the extent of pitting corrosion correlated well with the pitting potentials in the corresponding polarisation curves i.e. the higher the pitting potential, the lower the amount of corrosion pitting occurring. It was generally

West 1970). It is also evident from this investigation that certain inclusions cause galvanic action with the matrix to initiate pitting, as the corrosion pit sites had the presence of intermetallic Al/Fe/Be and elemental silicon inclusions (Figure 13) suggesting that these act as cathode to promote corrosion of the surrounding metal . Other inclusions like carbides or any less noble inclusions may also result in pit initiation by dissolving themselves

Potentiodynamic polarisation was performed for the three beryllium grades in various chloride concentrations, from 0.0001 M to 0.1 M KCl solutions. Typical polarisation curves for all the beryllium grades are shown in Figure 14. This figure shows that the pitting potential of S65-Bar at -745mV SCE is higher than those for P10-Bar (-790 mV SCE) and S65- Billet (-765 mV SCE) in a 0.0001 M KCl solution. Similar differences in polarisation behaviour were observed for all the grades in 0.001M and 0.01 M KCl solution. The results from the polarisation curves for all the three grades are summarised in Table 3. This table displays the average values of open circuit potential (OCP), pitting potential (Epit), repassivation potential (Erepass), passive current density (ipassive) and passive range (Epit -

Fig. 14. Typical polarisation curves for 3 beryllium grades in 0.0001M KCl solution, sweep

0000000 **Current Density (mA/cm<sup>2</sup>**

10-7 10-6 10-5 10-4 10-3 10-2 10-1

**)** 

S38, S65-Bar S79, P10-Bar S97, S65-Billet

The surface condition of samples (from three beryllium grades) after polarisation in 0.001M KCl solutions was visualised. It was observed that the extent of pitting corrosion correlated well with the pitting potentials in the corresponding polarisation curves i.e. the higher the pitting potential, the lower the amount of corrosion pitting occurring. It was generally

**3.3.3 Electrochemical polarisation of the three beryllium grades** 

Epit (S65-Bar)=-745mV Epit (P10-Bar)=-790mV Epit (S65-Billet)=-765mV

preferentially to the matrix.

OCP).

**Potential (mV, SCE)**

rate of 20mV/min



observed that polarisation at the slower sweep rate results in a denser population of corrosion pits.

Table 3. Pitting corrosion data from potentiodynamic polarisation curves in deaerated potassium chloride solution at pH 7.0

Figure 15 shows graphically how the pitting potentials (as listed in Table 3) for the three beryllium grades vary with chloride concentration. In all the three cases the onset of pitting potential (Epit) was found to decrease logarithmically with increasing chloride concentration.

The overall relationship for pitting potential variation with chloride concentration is represented by the relationship:

$$E\_{\rm piit} = -72 \log \left[ \rm Cl^{-1} \right] \cdot 1044 \tag{6}$$

Where Epit is in mV vs SCE and [Cl-1] is the chloride concentration in molarity. This relationship is very close to that observed by Hill et al. (1998) for beryllium grade S200D (see Equation 4).

Electrochemical Characterisation to Study the Pitting Corrosion Behaviour of Beryllium 23

the three grades (as listed in Table 3) at various chloride concentrations also confirms that

There is no precise way to relate the pitting corrosion response to the extent of Al/Fe/Be inclusions in beryllium, however, as can be seen in Table 1, the level of iron and aluminium content is progressively higher in S65-Billet and P10-Bar, which can enhance the extent of Al/Fe/Be inclusions. The passive ranges, as determined in 0.0001M KCl solution, of the three beryllium grades were plotted against their aluminium content (wt%), as shown in Figure 16. This presents a tentative correlation of the pitting corrosion response to the

Fig. 16. Variation of pitting corrosion response in relation to aluminium content (hence the

0.01 0.015 0.02 0.025 0.03 0.035 0.04 0.045 0.05 **Aluminium content in beryllium, wt%**

S65-Bar S65-Billet P10-Bar

**Prior to the present experimental work being carried out, a brief review of past work on pitting corrosion of beryllium was conducted and the following conclusions were** 

1. Beryllium readily forms an adherent protective oxide film on its surface and the metal presents no corrosion problems in dry air or in high purity water at low temperature. However, it has been known that beryllium is susceptible to pitting corrosion in the presence of chloride, fluoride and sulphate ions. This is due to the breakdown of

2. Electrochemical studies in NaCl solution of varying chloride ion concentrations (from 0.0001 to 1M) and pH values (2 to 12.5 pH), showed that on increasing the chloride concentration, the pitting potential decreased and at 1M NaCl, it underwent pitting corrosion at open circuit conditions. On the other hand there was an increase in pitting

S65-Bar is more resistant to pitting corrosion than the other two grades.

extent of Al/Fe/Be inclusions in beryllium metal.

extent of Al/Fe/Be inclusion) in beryllium metal

passive film at localised sites resulting in sporadic pits.

**4. Conclusions** 

200

220

240

260

280

**Passive range, mV (increasing resistance to** 

**pitting corrosion)**

300

320

340

360

**made:** 

Moreover, the graph (Figure 15) shows that the pitting potential for S65-Bar is higher at all chloride concentrations i.e. the pitting potential decreases in the order S65-Bar > P10-Bar ≥ S65-Billet. These results suggest that S65-Bar is relatively more resistant to pitting corrosion. This work revealed that various inclusions in beryllium metal, such as intermetallic Al/Fe/Be, elemental silicon and some carbide phases act as pit initiation sites. It is also evident that there is a higher level of the coarse inclusions present in P10-Bar grade material (especially the mixed carbide and elemental silicon); and a larger sized Al/Fe/Be inclusions in the S65-Billet grade than in the S65-Bar grade. In P10 this is undoubtedly due to the significantly higher levels of C, Fe, Al, Mg and Ti impurities present (see Table 1). In the S65- Billet grade this may partly be due to the relatively higher levels of Fe and Al impurities (Table 1), and partly due to the prolonged heat treatment this material underwent during fabrication, leading to the diffusion and coalescence of impurities to form relatively large sized Al/Fe/Be inclusions at the grain boundaries. This difference in impurity content between the grades tends to explain the observed lower pitting potentials and hence the increased propensity for pitting corrosion in P10-Bar and S65-Billet grades compared to the S65-Bar grade.

Fig. 15. Comparison of pitting potential for 3 beryllium grades at varying chloride concentration

Both pitting potential and open circuit potential can be influenced by slight variations in surface finish, solution temperature and pH value. An alternative approach was adopted by Corlett (Corlett, 2008) that the gap between the pitting potential and the open circuit potential (i.e. passive range) can be a better measure, such that the larger the passive range, the greater the resistance to pitting corrosion. Comparison of the passive ranges among all the three grades (as listed in Table 3) at various chloride concentrations also confirms that S65-Bar is more resistant to pitting corrosion than the other two grades.

There is no precise way to relate the pitting corrosion response to the extent of Al/Fe/Be inclusions in beryllium, however, as can be seen in Table 1, the level of iron and aluminium content is progressively higher in S65-Billet and P10-Bar, which can enhance the extent of Al/Fe/Be inclusions. The passive ranges, as determined in 0.0001M KCl solution, of the three beryllium grades were plotted against their aluminium content (wt%), as shown in Figure 16. This presents a tentative correlation of the pitting corrosion response to the extent of Al/Fe/Be inclusions in beryllium metal.

Fig. 16. Variation of pitting corrosion response in relation to aluminium content (hence the extent of Al/Fe/Be inclusion) in beryllium metal

### **4. Conclusions**

22 Pitting Corrosion

Moreover, the graph (Figure 15) shows that the pitting potential for S65-Bar is higher at all chloride concentrations i.e. the pitting potential decreases in the order S65-Bar > P10-Bar ≥ S65-Billet. These results suggest that S65-Bar is relatively more resistant to pitting corrosion. This work revealed that various inclusions in beryllium metal, such as intermetallic Al/Fe/Be, elemental silicon and some carbide phases act as pit initiation sites. It is also evident that there is a higher level of the coarse inclusions present in P10-Bar grade material (especially the mixed carbide and elemental silicon); and a larger sized Al/Fe/Be inclusions in the S65-Billet grade than in the S65-Bar grade. In P10 this is undoubtedly due to the significantly higher levels of C, Fe, Al, Mg and Ti impurities present (see Table 1). In the S65- Billet grade this may partly be due to the relatively higher levels of Fe and Al impurities (Table 1), and partly due to the prolonged heat treatment this material underwent during fabrication, leading to the diffusion and coalescence of impurities to form relatively large sized Al/Fe/Be inclusions at the grain boundaries. This difference in impurity content between the grades tends to explain the observed lower pitting potentials and hence the increased propensity for pitting corrosion in P10-Bar and S65-Billet grades compared to the

Fig. 15. Comparison of pitting potential for 3 beryllium grades at varying chloride

Both pitting potential and open circuit potential can be influenced by slight variations in surface finish, solution temperature and pH value. An alternative approach was adopted by Corlett (Corlett, 2008) that the gap between the pitting potential and the open circuit potential (i.e. passive range) can be a better measure, such that the larger the passive range, the greater the resistance to pitting corrosion. Comparison of the passive ranges among all

0.00001 0.0001 0.001 0.01 0.1 **Chloride Concentration (Mole/L)**

S65-Bar P10-Bar S65-Billet

S65-Bar grade.

concentration


**Pitting Potential (mV, SCE)**

### **Prior to the present experimental work being carried out, a brief review of past work on pitting corrosion of beryllium was conducted and the following conclusions were made:**


Electrochemical Characterisation to Study the Pitting Corrosion Behaviour of Beryllium 25

The author would like to thank Ms. Jennifer Copeland of Brush Wellman Industries for the chemical analysis. The author also wish to acknowledge Mr Mike Cox, Dr Andrew

Blanc, C. & Mankowski, G. (1997). Susceptibility to Pitting Corrosion of 6056 Aluminium

Carrabine, J. A. (1963). Ternary AlMBe4 Phases in Commercially Pure Beryllium, J. Nuclear

Friedman, J. R. & Hanafee, J. E. (2000). Corrosion/Electrochemistry of Monocrystalline and Polycrystalline Beryllium in Aqueous Chloride Environment, UCRL-ID-137482 Flitton, M. K. A.; Mizia, R. E. & Bishop, C. W. (2002) Understanding Corrosion of Activated Metals in an Arid Vadose Zone Environment, INEEL/CON-01-01450, NACE Gulbrandsen, E. & Johansen, A. M. J. (1994), A Study of the Passive Behaviour of Beryllium

Hill, M. A.; Butt, D. P. & Lillard, R. S. (1996). The Corrosion/Electrochemistry of Beryllium

Hill, M. A.; Butt, D. P. & Lillard, R. S. (1998). The Passivity and Breakdown of Beryllium in

Kaye, G. W. C. & Laby T. H. (1978). Tables of Physicals and Chemical Constants, Longman

Lillard, R. S. (2000). Factors Influencing the Transition from Metastable to Stable Pitting in Single-Crystal Beryllium, J. Electrochemical Soc., Vol. 148, pp. B1-B11 Miller, P.D. & Boyd, W. K. (1968). Beryllium Deters Corrosion- some do's and don'ts,

Mueller, J. J. & Adolphson, D. R. (1979). Corrosion, Beryllium Science and Technology 2, D R Floyd and J N Lowe (eds), Plenum Press, New York 1979, pp. 417-432 Mathiesen, T. &. Hansen, J. V. (2010). Consequences of Sigma Phase on Pitting Corrosion

Pourbaix, M. (1966). Atlas of Electrochemical Equilibria in Aqueous Solutions, Pergamon

Pride, S. T.; Scully, J. R. & Hudson, J. L. (1994). Metastable Pitting of Aluminium and Criteria

Punni, J. S. & Cox, M. J. (2010). The Effect of Impurity Inclusions on the Pitting Corrosion

Rooksby, H. P. (1962). Intermetallic Phases in Commercial Beryllium, J. Nuclear Materials,

Stonehouse, A. J. & Weaver, W. W. (1965). Beryllium Corrosion, Materials Prot., Vol. 4, pp.

Behaviour of Beryllium, Corrosion Science, Vol. 52, pp. 2535-2546

Resistance of Duplex Stainless Steel, Duplex World Oct 2010 Conference, Beaune,

for the Transition to Stable Pit Growth, J. Electrochemical Soc., Vol. 141, pp. 3028-

and Beryllium Weldments in Aqueous Chloride Environments, Los Alamos

**5. Acknowledgements** 

**6. References** 

Wallwork and Dr S McCulloch of AWE for their support.

Materials, Vol. 8, pp. 278-280.

Press, New York 1978, p. 216

Press, New York, p. 135

Vol. 7, pp. 205-211

France

3040

24-36

Materials Engineering (July 1968) pp. 33-36

alloy, Corrosion Science, vol. 39, 1997, pp. 949-959

Corlett, N. (2008). Corrosion Checking, Materials World 2008, Vol. 16, pp. 27-29

in Aqueous Solutions, Corrosion Science, Vol. 36, pp. 1523-1536

National Laboratory New Mexico, Internet Report No. 87545.

Aqueous Solutions, J. Electrochemical Soc., Vol. 145, pp. 2799-2806

potential with increase in pH. Beryllium was found to be suffering from pitting corrosion in the pH range from 2 to 12.5 but was susceptible to general attack below a pH of 2.


### **The present experimental work was aimed at determining the effect of inclusions on pitting corrosion behaviour of beryllium. The following conclusions were drawn:**


### **5. Acknowledgements**

The author would like to thank Ms. Jennifer Copeland of Brush Wellman Industries for the chemical analysis. The author also wish to acknowledge Mr Mike Cox, Dr Andrew Wallwork and Dr S McCulloch of AWE for their support.

### **6. References**

24 Pitting Corrosion

3. Pitting experiments on single crystals have indicated that beryllium corrodes preferentially along certain orientations. The pitting potential, Epit, was found to decrease with surface orientation in the order (0001) > (1010) > (1120). In polycrystalline beryllium there was no correlation between pit initiation sites and crystallographic orientation of specific grains. Therefore, altering the bulk texture of polycrystalline beryllium will not affect the pitting corrosion resistance of beryllium, although it may

4. A relationship has been observed between failure strength and chloride ion concentration in terms of the type of corrosion pits generated in beryllium. Fewer but deeper pits degrade the mechanical properties of the material to a greater extent than

**The present experimental work was aimed at determining the effect of inclusions on** 

6. SEM examination of the polished samples of the three beryllium grades showed that there was a presence of fine inclusion particles (0.25 to 5 µm) and some relatively coarse particles (5 to 18 µm) located along the grain boundaries. In all cases, the majority of the fine inclusions were identified as BeO and intermetallic phases such as Al/Fe/Be (and in a few cases Si/Ti or Si/Al). The coarse inclusions were elemental silicon and mixed beryllium carbides. Other elements such as Mg, Ti, U and Cr were also associated with

7. SEM examination revealed that the number of coarse inclusions (and hence the overall inclusion population) was much greater in P10-Bar than that in the other two grades. In the case of S65-billet, although the overall inclusion content was approximately the same as in the S65-bar, the intermetallic Al/Fe/Be inclusion content was much higher

8. From the pit initiation study (using both electrochemical and ageing techniques), it was observed that corrosion pits were nearly always initiated at the metal grain boundaries. Although the intermetallic Al/Fe/Be and elemental silicon inclusions were the preferential sites for pit initiation, some corrosion pits had also initiated at carbide

9. Electrochemical polarisation of the three beryllium grades showed that the pitting potential of S65-Bar grade was relatively high compared to the other two grades. This is in agreement with the extent of corrosion pitting revealed on the coupons after polarisation. 10. The nature and extent of inclusions in each grade showed a strong relationship with its pitting potential. The lower overall inclusion content of the S65-Bar compared to the P10-Bar, and its lower Al/Fe/Be intermetallic inclusion content compared to the S65- Billet, resulted in it displaying a corresponding higher pitting potential and hence a

11. It is evident from the present work that the various inclusions in beryllium located at the grain boundaries, such as Al/Fe/Be, elemental silicon and carbides act as pit initiation sites and hence their presence is likely to enhance the propensity for pitting corrosion.

5. Previously suggested mechanisms for pitting corrosion have been reviewed.

**pitting corrosion behaviour of beryllium. The following conclusions were drawn:** 

pH of 2.

affect pit propagation

(i.e. larger particle size).

inclusions.

that by numerous but shallower pits.

some intermetallic and mixed carbide phases.

relatively greater resistance to pitting corrosion.

potential with increase in pH. Beryllium was found to be suffering from pitting corrosion in the pH range from 2 to 12.5 but was susceptible to general attack below a


**1. Introduction** 

potential.

deposited by PVD.

**2** 

G. Knörnschild

*Brazil* 

**Mechanism of Pit Growth** 

*Federal University of Rio Grande do Sul* 

**in Homogeneous Aluminum Alloys** 

Pitting corrosion is a process, which takes place on passive metals and alloys. A characteristic of this type of corrosion is that passivity breaks down at isolated points at the surface and the growth of pits is observed due to locally high rates of metal dissolution. In electrochemical experiments, the growth of pits leads to a rapid rise of the overall current density once a characteristic threshold potential, the pitting potential E(pit) is surpassed. Since the measured current density is composed of the passive current density at the passive surface area and the current density of fast metal dissolution at the pitted area conventional electrochemical tests are not useful for studying metal dissolution inside pits. Some authors tried to overcome this difficulty by working with small wire electrodes. The idea behind was to achieve an electrode state where the whole surface represents a pit and the measured current density becomes, therefore, identical to the real current density inside a pit. However, highly concentrated electrolytes and high potentials must usually be applied to achieve this electrode state [1-3]. Formation of salt films and mass transport control was usually observed under these conditions, which more likely represent the conditions of electropolishing rather than that of a metal suffering pitting corrosion at the corrosion

Other authors determined the current density during the initial stage of pit growth from the microscopic measurement of the dimensions of pits formed in short time experiments [4]. By measuring the time for perforation by pitting of thin metal foils Hunkeler [5] and Cheung [6] obtained average rates of pit growth, i.e., average current densities normal to the foil surface. Average rates of localized corrosion at grain boundaries of aged AlCu alloys have been determined by metallographic measurements of penetration depth and penetration time [7]. By the same method early stages of pit propagation were studied in 7075-T3 alloy [8]. Few studies have been made to measure in-situ metal dissolution inside pits. Edeleanu [9] examined the pit propagation in thin aluminum foils, glued to a glass foil which could be observed from the back side by a microscope. In this way pit propagation along the glass foil could be observed in situ. The technique was applied again for an intensive study of pit growth in pure aluminum by Baumgärtner [10-12], and for the study of homogeneous aluminum alloys by Knörnschild and Kaesche [13,14]. Later, Frankel [15] used a similar technique to study pit growth in thin aluminum films

