**Pulse Electroplating of Ultrafine Grained Tin Coating**

Ashutosh Sharma, Siddhartha Das and Karabi Das

Additional information is available at the end of the chapter

http://dx.doi.org/10.5772/61255

#### **Abstract**

In the electronic packaging industries, soldering materials are essential in joining various microelectronic networks. Solders assure the reliability of joints and protect the micro‐ electronic packaging devices. They provide electrical, thermal, and mechanical continuity among various interconnections in an electronic device. The service performance of all the electronic appliances depends on high strength and durable soldering materials. Lead-containing solders are in use for years, resulting in an extensive database for the re‐ liability of these materials. However, due to toxicity and legislations, lead-free solders are now being developed. As tin (Sn) is the major component of solders, this chapter presents the detailed results and discussion about the metallurgical overview of Sn, synthesis, and characterization of pulse electrodeposited pure tin finish from different aqueous solution baths. The experiments on pulse electrodeposition such as common tin plating baths em‐ ployed, their chemical compositions, rationale behind their selection and their characteri‐ zation by bath conductivity and cathodic current efficiency, microstructures, and tin whisker growth are discussed. Further, the effect of pulse electrodeposition parameters such as current density, additive concentration, pH, duty cycle, frequency, temperature, and stirring speed on microstructural characteristics of the coating obtained from sulfate bath and their effect on grain size distribution have been presented.

**Keywords:** Tin plating, pulse electrodeposition, morphology, plating baths, grain size

## **1. Introduction**

#### **1.1. Background**

Lead-bearing solders are in use till date due to their indispensable properties [1–3]. Firstly, it is very cheap, available in abundance and provides good physical and chemical bonding to the substrate without interfering with the substrate [4–5]. Secondly, lead (Pb) reduces the surface tension of pure tin, which is 550 mN/m at 232°C, and the lower surface tension of 63Sn-37Pb solder (470 mN/m at 280°C) facilitates wetting [4, 6, 7]. The presence of Pb also helps

© 2015 The Author(s). Licensee InTech. This chapter is distributed under the terms of the Creative Commons Attribution License (http://creativecommons.org/licenses/by/3.0), which permits unrestricted use, distribution, and reproduction in any medium, provided the original work is properly cited.

to prevent the white tin (*β*-Sn) to gray tin (*α*-Sn) allotropic phase transformation from occurring in high-Sn solders upon cooling below 13ºC [7]. This makes it a prime choice for soldering.

#### **1.2. Replacement of Pb**

There are many technology-based problems that can serve as reasons for the elimination of Sn-Pb solders. First, it has been already proved in the past that many lead-free candidate solders exhibit significantly better strength and fatigue life properties [4, 6]. Secondly, Pb and Pb compounds have been cited by the Environmental Protection Agency (EPA) as one of the top 17 chemicals posing the greatest threat to human life and the environment [7, 8]. In view of these reasons, elimination of Pb from electronics is necessary in electronics packaging [1, 6].

#### **1.3. The lead-free definition and regulations**

Legislations to restrict the use of Pb were first implemented in the USA in 1991 with the Lead Exposure Reduction Act of 1991 and the Lead Exposure Act of 1992, which bans Pb in some applications and limits Pb content in others to less than 0.1% [7, 8]. In the United States, the National Electronics Manufacturing Initiative (NEMI) program was developed to research on lead-free alternatives [9]. In Japan, this movement is connected to the Lead-free Soldering Research Council (1994 to 2000) within the Japan Institute of Electronic Packaging. Japan Electronics and Information Technology Industries Association (JEITA) has set guidelines for lead-free products, which was published in 1999 [10, 11]. These companies aimed to use leadfree solders in mass-produced consumer products and to implement lead-free soldering technologies in their products by 2003 [2]. In Europe, the EU directives (WEEE) and (RoHS) have issued a ban on the use of lead in consumer goods [12, 13].

## **2. Metallurgical overview of Sn**

Pure Sn has two allotropes, white tin (*β*-Sn, metallic) and gray tin (*α*-Sn, semiconductor). The most common form of Sn in real life is white tin, which transforms to gray tin at temperatures below 13ºC [14]. *β*-Sn possesses body-centered tetragonal crystal structure with lattice parameters *a* = *b* = 0.5820 nm and *c* = 0.3175 nm [15]. This *c/a* ratio of 0.546 gives rise to highly anisotropic behavior in Sn. The mechanical properties are very poor, the hardness being 11 Hv and tensile strength 44 MPa [16]. This is largely due to its lower melting point relative to common engineering metals such as aluminum (Al), copper (Cu), and steel [14–16].

#### **2.1. Pb-free Sn alloys**

A relatively large number of Pb-free solder alloys have thus been proposed so far, Sn being the primary or major constituent. The two other elements that are major constituents are indium (In) and bismuth (Bi). Other alloying elements are zinc (Zn), silver (Ag), antimo‐ ny (Sb), copper (Cu), and magnesium (Mg), and in one case, a minor amount of Pb [1–3]. The most popular Pb-free alloy system candidates are listed in a thorough review paper by Abtew and Selvaduray [1]. The most important characteristics that must be considered in selecting suitable Pb-free solder candidates are: nontoxic; availability; sufficient electri‐ cal as well as thermal conductivity; adequate mechanical properties compatible with metallic substrates such as Cu, nickel (Ni), Ag, or gold (Au); economically viable; acceptable melting and processing temperatures; and less temperature effects on substrates, printed circuit boards(PCBs), etc. [1–4, 6].

#### **2.2. Intermetallic compounds and whisker growth**

to prevent the white tin (*β*-Sn) to gray tin (*α*-Sn) allotropic phase transformation from occurring in high-Sn solders upon cooling below 13ºC [7]. This makes it a prime choice for soldering.

There are many technology-based problems that can serve as reasons for the elimination of Sn-Pb solders. First, it has been already proved in the past that many lead-free candidate solders exhibit significantly better strength and fatigue life properties [4, 6]. Secondly, Pb and Pb compounds have been cited by the Environmental Protection Agency (EPA) as one of the top 17 chemicals posing the greatest threat to human life and the environment [7, 8]. In view of these reasons, elimination of Pb from electronics is necessary in electronics packaging [1, 6].

Legislations to restrict the use of Pb were first implemented in the USA in 1991 with the Lead Exposure Reduction Act of 1991 and the Lead Exposure Act of 1992, which bans Pb in some applications and limits Pb content in others to less than 0.1% [7, 8]. In the United States, the National Electronics Manufacturing Initiative (NEMI) program was developed to research on lead-free alternatives [9]. In Japan, this movement is connected to the Lead-free Soldering Research Council (1994 to 2000) within the Japan Institute of Electronic Packaging. Japan Electronics and Information Technology Industries Association (JEITA) has set guidelines for lead-free products, which was published in 1999 [10, 11]. These companies aimed to use leadfree solders in mass-produced consumer products and to implement lead-free soldering technologies in their products by 2003 [2]. In Europe, the EU directives (WEEE) and (RoHS)

Pure Sn has two allotropes, white tin (*β*-Sn, metallic) and gray tin (*α*-Sn, semiconductor). The most common form of Sn in real life is white tin, which transforms to gray tin at temperatures below 13ºC [14]. *β*-Sn possesses body-centered tetragonal crystal structure with lattice parameters *a* = *b* = 0.5820 nm and *c* = 0.3175 nm [15]. This *c/a* ratio of 0.546 gives rise to highly anisotropic behavior in Sn. The mechanical properties are very poor, the hardness being 11 Hv and tensile strength 44 MPa [16]. This is largely due to its lower melting point relative to

A relatively large number of Pb-free solder alloys have thus been proposed so far, Sn being the primary or major constituent. The two other elements that are major constituents are indium (In) and bismuth (Bi). Other alloying elements are zinc (Zn), silver (Ag), antimo‐ ny (Sb), copper (Cu), and magnesium (Mg), and in one case, a minor amount of Pb [1–3]. The most popular Pb-free alloy system candidates are listed in a thorough review paper

common engineering metals such as aluminum (Al), copper (Cu), and steel [14–16].

**1.2. Replacement of Pb**

106 Electroplating of Nanostructures

**1.3. The lead-free definition and regulations**

**2. Metallurgical overview of Sn**

**2.1. Pb-free Sn alloys**

have issued a ban on the use of lead in consumer goods [12, 13].

Due to the Pb-free solder implementation, pure Sn and Sn-Cu, Sn-Ag are commonly used to replace eutectic Sn-Pb as the surface finish on the lead-frames and metal terminations of passive devices [17, 18, 19]. However, in Sn-rich lead-free finish, Sn whiskers have been found to form, which poses a serious threat for the reliability of passive devices. The Sn whisker formation was first reported in 1946 [20]. It is generally accepted that the driving forces of Sn whiskers mainly attribute to the internal stresses, the dissolution of the metal under-layer, and the interfacial compound formation. There are two intermetallic compounds of Cu and Sn below 300ºC, they are Cu6Sn5 and Cu3Sn. The Cu6Sn5 forms at room temperature while Cu3Sn forms after annealing at elevated temperatures [21, 22]. Some intermetallic compounds (IMCs), such as AuSn4 for Sn/Au couples, Cu6Sn5 for Sn/Cu couples, and Ni3Sn4 for Sn/Ni couples, even form at room temperature [23, 24].

Based on these three main root-causes of Sn whisker formation, three methods are devised by researchers to retard the Sn whiskers formation: (1) choosing optimal thickness of the finish layer, (2) alloying with other metal elements, and (3) adding a reaction barrier layer beneath the finish layer [25–27].

## **3. Synthesis routes and technologies for solder fabrication**

There are many synthesis routes for the fabrication of solders varying from solid state mechanical alloying, powder metallurgy, sol gel, melting and casting route, chemical routes, gaseous phase sputtering or evaporation methods, electrodeposition method, etc. [28-35]. Among all these methods, we will discuss techniques related to thin film pulse electrodepo‐ sition of solders. The other methods are not discussed here because they are out of the scope of this chapter.

#### **3.1. Electrodeposition**

Both evaporation and sputter deposition techniques require high vacuum and/or high temperature processing, which increases operation costs and cause inter-diffusion problems. Compared to these fabrication processes, electrodeposition is an economically viable process [36]. It can be used to plate either single layer or multilayer deposits with easy and precise control of the thickness and composition of each layer. Electrodeposition can be performed on substrates with varying sizes and complex shapes and the deposit can be very thin or very thick [37–38]. There are, however, safety and environmental concerns related with chemical treatment and safe disposal of wastes. Numerous metals and metal alloys have been success‐ fully electrodeposited from aqueous solutions. The most useful electrodeposited metals include Sn, Cr, Cu, Ni, Ag, Au, Zn, and alloys such as chromium-nickel (Cr-Ni), iron-cobalt (Fe-Co), and various Sn alloys [36–38].

#### **3.2. General aspects of electrodeposition**

In electrodeposition, metal ions present in a solution, the electrolyte, are reduced at the surface of an electrode to form a metal layer, as shown in Fig. 1.

**Figure 1.** A schematic for the electrodeposition process.

This process essentially consists of: (1) an anode (the positive electrode), (2) a cathode (the item to be electroplated, which is the negative electrode), (3) the electrolyte acts as a transport medium for the tin ions to be deposited at the cathode as a coating on the item to be electro‐ plated, (4) an electric current or voltage source for controlling the deposition, and (5) various peripherals for contacting the electrodes, stirring and heating the solution, etc. [36–37].

In electrodeposition, the metal is deposited over a conductive substrate by the application of electric current through the electrolytic bath. The current provides sufficient energy to proceed the oxidation-reduction reactions at anode and cathode, respectively. The metal ions in the electrolyte accept the electrons and get deposited on the substrate. The weight of the deposited material can be calculated from the relation given by Faraday's laws [37–39]:

$$\frac{\text{Thickness}}{\text{time}} = \frac{J(ECE)(CCE)}{\text{density}}\tag{1}$$

where thickness of the deposit is in mg, time in seconds, J = current density, ECE = electro‐ chemical equivalent, CCE = current efficiency (ratio of actual/theoretical weight deposited), and density of deposit is in g/cm3 .

#### **3.3. Cathodic and anodic reactions**

treatment and safe disposal of wastes. Numerous metals and metal alloys have been success‐ fully electrodeposited from aqueous solutions. The most useful electrodeposited metals include Sn, Cr, Cu, Ni, Ag, Au, Zn, and alloys such as chromium-nickel (Cr-Ni), iron-cobalt

In electrodeposition, metal ions present in a solution, the electrolyte, are reduced at the surface

This process essentially consists of: (1) an anode (the positive electrode), (2) a cathode (the item to be electroplated, which is the negative electrode), (3) the electrolyte acts as a transport medium for the tin ions to be deposited at the cathode as a coating on the item to be electro‐ plated, (4) an electric current or voltage source for controlling the deposition, and (5) various peripherals for contacting the electrodes, stirring and heating the solution, etc. [36–37].

In electrodeposition, the metal is deposited over a conductive substrate by the application of electric current through the electrolytic bath. The current provides sufficient energy to proceed the oxidation-reduction reactions at anode and cathode, respectively. The metal ions in the

(Fe-Co), and various Sn alloys [36–38].

108 Electroplating of Nanostructures

**3.2. General aspects of electrodeposition**

**Figure 1.** A schematic for the electrodeposition process.

of an electrode to form a metal layer, as shown in Fig. 1.

Electrochemical deposition of metals and alloys involves the reduction of metal ions from aqueous, organic, and fused-salt electrolytes. In this thesis, electrodeposition from aqueous solutions is being considered. The reduction of metal ions Mn+ in aqueous solution is repre‐ sented by [37–39]:

$$\text{M}^{n^+} + \text{ne}^+ \to \text{M} \tag{2}$$

Reaction (2) is often accompanied by hydrogen evolution. In acid solutions, we have:

$$\text{2H}^+ + 2\text{e}^\cdot \rightarrow \text{H}\_2\tag{3}$$

In neutral and basic solutions, hydrogen evolution follows the equation:

$$\text{2H}\_2\text{O} + 2\text{e}^\cdot \rightarrow \text{H}\_2 + 2\text{OH}^\cdot \tag{4}$$

At the anode, the anodic reactions are as follows. In an acidic solution, we have:

$$2\text{H}\_2\text{O} \rightarrow \text{O}\_2 + 4\text{H}^+ + 4\text{e}^- \tag{5}$$

In an alkaline solution, the anode reaction is:

$$\text{4OH}^{\cdot} \rightarrow \text{O}\_{2} + 2\text{H}\_{2}\text{O} + 4\text{e}^{\cdot} \tag{6}$$

For a soluble anode, oxidation reactions, which will dissolve the anode into solution:

$$\mathbf{M} \to \mathbf{M}^{n^\*} + \mathbf{ne}^\* \tag{7}$$

The equilibrium electrode potential between a metal and a solution of its ions is given by the Nernst equation:

$$E\_{M/M^{n^\*}} = E^\circ + \frac{RT}{nF} \text{Im} \, \mathcal{C}\_{M^{n^\*}} \tag{8}$$

where *Eo* is the standard electrode potential, *R* is the gas constant, *F* is the Faradaic constant, and *CM <sup>n</sup>*<sup>+</sup> is the metal ion concentration. It can be noticed that the value of *EM* /*<sup>M</sup> <sup>n</sup>*+ depends on the concentration of metal ions to be plated, addition of additives, current density, etc. [38, 39].

#### **3.4. Electrolyte conductivity**

The conductivity of an electrolyte depends on the degree of dissociation, the mobility of individual ions, temperature (and thus viscosity), and the electrolyte composition. In aqueous solutions, the ionic conduction depends on the degree of dissociation of dissolved species in the solution [38, 39]. In order to increase the conductivity of electrolytes, certain salts and acids or alkali are added; these are known as supporting electrolytes. For acid electrolytes, chlorides and acids are useful; for neutral electrolytes, chlorides are useful; and for alkaline electrolytes, sodium hydroxide or cyanides are useful [39]. Generally, a marked decrease in conductivity at higher concentration is due to the greater coulombic forces acting between the ever closer ions in solution. This leads to the loose association of opposite charged ions that are effectively neutral and thus no longer contribute to the overall conductivity [39].

#### **3.5. Polarization and overpotential**

The equilibrium potential of an electrode differs in an electrochemical cell after the application of current. Suppose the equilibrium potential of an electrode when there is no external current flowing is E. After the application of an external current (I), the potential of the electrode change by E(I), the overpotential (*η*) can be given as:

$$
\eta = \operatorname{E}(\mathbf{I}) - \operatorname{E} \tag{9}
$$

It can be also expressed as in terms of current and voltage by the Tafel equation:

$$
\mathfrak{h} = \mathsf{a} \nvdash \mathsf{b} \log \mathsf{I} \tag{10}
$$

where *a* and *b* are constants.

The overpotential *η* is required to overcome hindrance of the overall electrode reaction, which is usually composed of a sequence of partial reactions, charge transfer, diffusion, chemical reaction, and crystallization [36, 38]. The overpotential is generally used as a measure of the extent of polarization. Polarization demonstrates departure of the electrode potential from the equilibrium value upon passage of a Faradaic current [39]. Depending upon the nature and sites of the inhibition factors, there may be different kinds of overpotentials, such as charge transfer overpotential or activation overpotential, which is caused by inhibition of the charge transfer taking place across the close proximity of solution/cathode interface.

Thus, four different kinds of overpotential are distinguished and the total overpotential *η* can be considered to be composed of four components: where *η*ct, *ηd*, *ηr*, and *η<sup>c</sup>* are, as defined above, charge-transfer, diffusion, reaction, and crystallization overpotentials, respectively. The electrode reaction can then be represented by a resistance (RE), composed of a series of resistances (or more precisely, impedance), which represent the different steps: Rmt, Rct, and Rrxn. A fast reaction step is characterized by a small resistance, while a slow reaction step is represented by a high resistance. In other words, RE will be the sum of all the resistances Rmt, Rct, and Rrxn, as shown in Fig. 2 [38].

**Figure 2.** Processes in an electrode reaction represented as resistances (From A.J. Bard, and L.R. Faulkner, Chapter 1: Introduction and Overview of Electrode Processes, Page 24, Electrochemical Methods - Fundamentals and Applica‐ tions, 2nd Edition. Reprinted by permission of John Wiley & Sons, Inc. Copyright 2001 © John Wiley & Sons, Inc.

#### **3.6. Pulse current electrodeposition**

The equilibrium electrode potential between a metal and a solution of its ions is given by the

where *Eo* is the standard electrode potential, *R* is the gas constant, *F* is the Faradaic constant, and *CM <sup>n</sup>*<sup>+</sup> is the metal ion concentration. It can be noticed that the value of *EM* /*<sup>M</sup> <sup>n</sup>*+ depends on the concentration of metal ions to be plated, addition of additives, current density, etc. [38, 39].

The conductivity of an electrolyte depends on the degree of dissociation, the mobility of individual ions, temperature (and thus viscosity), and the electrolyte composition. In aqueous solutions, the ionic conduction depends on the degree of dissociation of dissolved species in the solution [38, 39]. In order to increase the conductivity of electrolytes, certain salts and acids or alkali are added; these are known as supporting electrolytes. For acid electrolytes, chlorides and acids are useful; for neutral electrolytes, chlorides are useful; and for alkaline electrolytes, sodium hydroxide or cyanides are useful [39]. Generally, a marked decrease in conductivity at higher concentration is due to the greater coulombic forces acting between the ever closer ions in solution. This leads to the loose association of opposite charged ions that are effectively

The equilibrium potential of an electrode differs in an electrochemical cell after the application of current. Suppose the equilibrium potential of an electrode when there is no external current flowing is E. After the application of an external current (I), the potential of the electrode change

The overpotential *η* is required to overcome hindrance of the overall electrode reaction, which is usually composed of a sequence of partial reactions, charge transfer, diffusion, chemical reaction, and crystallization [36, 38]. The overpotential is generally used as a measure of the extent of polarization. Polarization demonstrates departure of the electrode potential from the

neutral and thus no longer contribute to the overall conductivity [39].

h

h

It can be also expressed as in terms of current and voltage by the Tafel equation:

*nF* + + = + (8)

= E I – E ( ) (9)

= a +b log I (10)

/ *n n* ln *<sup>o</sup> M M M RT EE C*

Nernst equation:

110 Electroplating of Nanostructures

**3.4. Electrolyte conductivity**

**3.5. Polarization and overpotential**

where *a* and *b* are constants.

by E(I), the overpotential (*η*) can be given as:

In olden times, direct current (DC) electrodeposition had only one parameter, namely, current density that is variable. In modern times, pulsed current (PC) plating where the potential or current density alternates rapidly between two different values is used [36–39]. This is accomplished with a series of pulses of equal amplitude, duration, and polarity, separated by a period of zero current, and time (t) axis as shown in Fig. 3. Each pulse consists of an on-time (*Ton*), during which potential and current is applied, and an off-time (*Toff*), during which open circuit potential and zero current is applied.

The duty cycle is given by the equation:

$$\text{Duty Cycle (\%)} = \frac{T\_{\text{ou}}}{T\_{\text{on}} + T\_{\text{off}}} \tag{11}$$

The average current density is defined as:

$$J\_{\text{anyage}} = (J\_{\text{peak}}) \times \text{Duty Cycle} \tag{12}$$

**Figure 3.** Schematic diagram of pulsed current waveform.

*Javerage* is the average current density and *Jpeak* is the peak current density [35, 39, 40]. The average current density in PC plating is similar to the current density used in DC plating. For a given average current density, a number of combinations of different peak current densities and onoff times are available. This gives PC plating two important features. Firstly, a very high instantaneous current density, one to two orders in magnitude greater than the steady-state limiting current density as reported, can be used without depleting the metal ions at the electrode surface [40]. This favors the initiation of the nucleation process and greatly increases the number of grains per unit area, resulting in a finer grained deposit with better properties than conventional DC plating. Secondly, during the off-time period, adsorption and desorp‐ tion, as well as recrystallization of the deposit occurs, which can control the microstructure of the deposits [36, 40, 41].

#### **4. Electrodeposition of Sn**

Sn can be electrodeposited from both acidic and alkaline aqueous solutions [42, 43]. In acidic baths, Sn usually exists as Sn2+ ions, while in alkaline baths, Sn4+ is the more stable species. The various Sn plating baths available in literature are discussed below.

#### **4.1. Sodium stannate baths**

The alkaline stannate electrolytes usually contain sodium or potassium stannate and the corresponding alkali metal hydroxide. These electrolytes are environment friendly, as they are non-corrosive in nature and do not require other organic additives [42, 43]. The alkaline tin baths have a very high throwing power and can be operated over a wide current density range. The tin coatings electroplated from alkaline electrolytes possess improved solderability, since they do not require any organic additive agents [44, 45]. This leads to a great improvement in wettability. One major disadvantage of alkaline plating baths is that highly alkaline baths may dissolve the photoresist used to define areas on semiconductor wafers. Alkaline plating baths also usually require higher plating temperatures (60–70°C) as compared to acidic ones [46].

#### **4.2. Stannous sulfate baths**

Sulfate baths are primarily used for bright acid Sn plating. Organic agents are necessary if bright and dense films are to be obtained. Electroplating of tin from acidic stannous (divalent Sn) solutions consumes less electricity than alkali stannate solutions (tetravalent Sn) [42–45]. The major drawback of this system is Sn oxidation. At high current density, soluble Sn anodes are passivated due to the formation of SnO2. Irregular, dendritic, needle-like electrodeposits of tin are in general obtained from acidic electrolytes without organic additives [47–49]. To improve the surface finish, morphology, and adhesion during acidic tin plating, various organic chemicals as additives have been investigated in the past [50–52]. In the literature, we observe that sulfate baths have been used widely to plate pure Sn and various Sn alloys in electronics industries [53].

#### **4.3. Stannous chloride baths**

*Javerage* is the average current density and *Jpeak* is the peak current density [35, 39, 40]. The average current density in PC plating is similar to the current density used in DC plating. For a given average current density, a number of combinations of different peak current densities and onoff times are available. This gives PC plating two important features. Firstly, a very high instantaneous current density, one to two orders in magnitude greater than the steady-state limiting current density as reported, can be used without depleting the metal ions at the electrode surface [40]. This favors the initiation of the nucleation process and greatly increases the number of grains per unit area, resulting in a finer grained deposit with better properties than conventional DC plating. Secondly, during the off-time period, adsorption and desorp‐ tion, as well as recrystallization of the deposit occurs, which can control the microstructure of

Sn can be electrodeposited from both acidic and alkaline aqueous solutions [42, 43]. In acidic baths, Sn usually exists as Sn2+ ions, while in alkaline baths, Sn4+ is the more stable species. The

The alkaline stannate electrolytes usually contain sodium or potassium stannate and the corresponding alkali metal hydroxide. These electrolytes are environment friendly, as they are non-corrosive in nature and do not require other organic additives [42, 43]. The alkaline tin baths have a very high throwing power and can be operated over a wide current density range.

various Sn plating baths available in literature are discussed below.

the deposits [36, 40, 41].

112 Electroplating of Nanostructures

**4. Electrodeposition of Sn**

**Figure 3.** Schematic diagram of pulsed current waveform.

**4.1. Sodium stannate baths**

For tin electroplating, sulfate baths use a number of additives to produce a homogeneous deposit [47–53]. However, in-spite of these advantages, the use of additives is undesirable for health concerns. Moreover, adverse effects on plating efficiency and the working environment have been observed [54, 55]. In case of alkaline baths, the same is true as it requires heating the solution that causes bubble formation [44–46]. Also tin is tetravent in alkaline baths causing more power. In view of these disadvantages, recently, He *et al*. developed a bath containing citric acid or its salt and an ammonium salt [53]. In the same line, Sharma *et al*. produced bulk tin films from stannous chloride-citrate bath and found improved thermal and mechanical properties [56].

#### **4.4. Methanesulfonic acid baths**

The problem of oxidation of Sn2+ to Sn4+ can be minimized by using a reducing acid Methane‐ sulfonic acid (MSA) bath as compared to sulfate bath. MSA is much less corrosive to electronic materials than sulfuric acid [55]. It forms a clear solution, have high dissolving power and less sensitive to Sn oxidation at higher current densities [57]. Different combinations of methane‐ sulfonate baths have been developed to electrodeposit both pure Sn and various Sn alloys by adding different additives [58].

## **4.5. Pyrophosphate baths**

There are a number of pyrophosphate baths available in the literature [42]. These types of baths containing P2O2 2- is considered as one of the most stable systems and is widely used for Sn plating [59, 60]. However, its use is limited in literature due to one disadvantage, that it requires more control and maintenance than the other plating baths. The operational temperature should not exceed 43–60°C because the pyrophosphate complex hydrolyzes to orthophosphate at temperatures higher than 60°C, which degrades the solution [42, 61].

## **5. Electrodeposition of Sn alloys**

According to the electrochemical series of metals, we know that the reduction potential of two elements would be different [35]. For a solution containing two or more different metal ions at low overpotential, the metal with the most noble reduction potential will deposit at a faster rate [35, 36]. If the electrode potential difference is far apart, then metal alloy electrodeposition may be impossible. The difference can be eliminated in view of the Nernst equation by modifying the activity values and feasibility of the co-deposition can thus be determined [37, 39]. This can be achieved by inducing a considerable change in ionic concentrations via complex ion using certain complexing agents. In the past, thiourea has been utilized as a complexing agent for the electrodeposition of Sn-Ag and Sn-Ag-Cu alloys [62, 63]. The formation of complexes by bonding the metal ions with complexing agents will decrease the concentration of the free metal ions in the solution significantly and modify the reduction potential of the metal ions [64, 65]. With an increase in overpotential, the electrodeposition reaction will progress from the charge transfer region to the mix and then to the mass-transfer regime. Under mass transfer control at sufficiently higher overpotentials, the relative deposi‐ tion rates of two or more metals will be governed by the concentrations and the diffusion coefficients of the metal ions [38, 39]. For alloy deposition, the basic mechanism remains the same as the Sn deposition discussed in the previous section. The summary of the previous studies on different types of plating baths are given in Table 1.



**Table 1.** Summary of various studies on electrodeposition of Sn.

more control and maintenance than the other plating baths. The operational temperature should not exceed 43–60°C because the pyrophosphate complex hydrolyzes to orthophosphate

According to the electrochemical series of metals, we know that the reduction potential of two elements would be different [35]. For a solution containing two or more different metal ions at low overpotential, the metal with the most noble reduction potential will deposit at a faster rate [35, 36]. If the electrode potential difference is far apart, then metal alloy electrodeposition may be impossible. The difference can be eliminated in view of the Nernst equation by modifying the activity values and feasibility of the co-deposition can thus be determined [37, 39]. This can be achieved by inducing a considerable change in ionic concentrations via complex ion using certain complexing agents. In the past, thiourea has been utilized as a complexing agent for the electrodeposition of Sn-Ag and Sn-Ag-Cu alloys [62, 63]. The formation of complexes by bonding the metal ions with complexing agents will decrease the concentration of the free metal ions in the solution significantly and modify the reduction potential of the metal ions [64, 65]. With an increase in overpotential, the electrodeposition reaction will progress from the charge transfer region to the mix and then to the mass-transfer regime. Under mass transfer control at sufficiently higher overpotentials, the relative deposi‐ tion rates of two or more metals will be governed by the concentrations and the diffusion coefficients of the metal ions [38, 39]. For alloy deposition, the basic mechanism remains the same as the Sn deposition discussed in the previous section. The summary of the previous

at temperatures higher than 60°C, which degrades the solution [42, 61].

studies on different types of plating baths are given in Table 1.

*Sn* Electroplating

*Sn* Electroplating

*Sn-Co* Electroplating

*Sn* Electroplating

*Sn* Electroplating

**Coating Processing Methods Plating bath Applications Reference**

Lead-free Abdel Rahim *et.al*., 1986 [44]

Lead-free Rehim *et al*., 1996 [48]

Lead-free Nakamura *et al*., 1997 [50]

sorbitol Soldering Broggi *et al*., 2003 [45]

aldehydes Solder joints Tzeng *et al*., 1996 [49]

Sodium stannate bath + halides

Sodium stannate bath +

Stannous sulfate Gluconate bath

Stannous sulfate bath +

Stannous sulfate bath + Benzal acetone and N,Nbis(tetraoxyethylene)octad ecylamine

*Sn* Pulse electroplating Sodium stannate bath Lead-free Sharma *et al*., 2012 [46]

**5. Electrodeposition of Sn alloys**

114 Electroplating of Nanostructures

#### **6. Process parameters and nanostructure formation**

The electrodeposition method is dependent on several processing parameters involved in the electrodeposition process. Therefore, to obtain the desired properties, it is essential to optimize the operating parameters. The effect of these parameters on tin electrodeposition is discussed in the following sections.

#### **6.1. Current density**

The current density is the primary controlling parameter in pulse electrodeposition. The average current density *Javerage,* is given by peak current density *Jpeak* x Duty Cycle. This enables us to achieve a very high current density in pulse electrolysis without depleting the metal ions at the electrode surface [66]. A high overpotential associated with higher pulse current density raises the nucleation rate resulting in fine grained deposit and thus improved properties can be obtained [38–40]. For a stable growth, the critical radius of the electrodeposited nucleus varies inversely to the cathodic overpotential. The higher the cathodic overpotential, the higher the nucleation rate will be and vice versa [66, 67]. Thus, the grain size decrease with the increase in cathodic overpotential and finer grains are obtained. A higher current density also leads to the development of dendritic morphology of the deposits [49–54, 56]. The dendritic morphol‐ ogy can be suppressed by using additives. For alloy deposition, the change in alloy morphol‐ ogy has been noted by several researchers with increase in current densities [64, 65, 68].

The dendritic or irregular shaped morphology in response to the current density is due to the fact that if there is a significant increase in the current density, it increases the nucleation rate and is also associated with a higher rate of hydrogen evolution. Due to high overpotential at this state, the rate of diffusion of Sn2+ ions towards cathode becomes significant over its replenishment from the electrolyte [68, 69]. This phenomenon creates a concentration gradient in the vicinity of electrolyte/cathode interface. As a consequence, the deposition occurs preferentially on certain protrusions (heterogeneous active sites on the cathode in a random manner. This type of non-uniform growth kinetics has also been observed in copper plating [70]. The cathodic current efficiency at this stage is poor indicating a rapid hydrogen evolution which decreases the concentration of Sn2+ ions in the electrolyte.

#### **6.2. pH**

The effect of pH in tin plating has not been discussed in detail in the literature. The majority of the tin plating baths available in literature are acidic in nature. As a general statement the rate of deposition increases with pH [71]. Bath pH not only affects the deposition rate but modifies the crystal orientation. Some people have noted a pH induced texture in Sn grains from acidic electrolyte [72]. Ebrahimi *et al*. investigated the effect of pH on nickel deposits [73]. He found that the pH values of 4.5, 4.7, and 5.0 resulted in grain size of 79, 45, and 56 nm, respectively. The increasing pH value from 2.8 to 5.1 enhanced the nucleation rate of nickel crystals, which corresponded to decreasing grain size from 343 to 35 nm. For copper electro‐ deposition, Natter and Hempelmann reported the smallest copper grain size of 8 nm at pH 1.5–2.0 and a continuous increase of the grain size up to 100 nm at pH 11.5 [74]. The morphology of the deposited Sn coatings with different bath pH gets refined with an increase in pH. At a high value of pH around 2, irregular and porous deposits are observed due to the progressive increase in hydrogen evolution reaction. However, at a very high pH (=3), the deposits turn powdery due to severe hydrogen gas evolution [54].

#### **6.3. Temperature**

the operating parameters. The effect of these parameters on tin electrodeposition is discussed

The current density is the primary controlling parameter in pulse electrodeposition. The average current density *Javerage,* is given by peak current density *Jpeak* x Duty Cycle. This enables us to achieve a very high current density in pulse electrolysis without depleting the metal ions at the electrode surface [66]. A high overpotential associated with higher pulse current density raises the nucleation rate resulting in fine grained deposit and thus improved properties can be obtained [38–40]. For a stable growth, the critical radius of the electrodeposited nucleus varies inversely to the cathodic overpotential. The higher the cathodic overpotential, the higher the nucleation rate will be and vice versa [66, 67]. Thus, the grain size decrease with the increase in cathodic overpotential and finer grains are obtained. A higher current density also leads to the development of dendritic morphology of the deposits [49–54, 56]. The dendritic morphol‐ ogy can be suppressed by using additives. For alloy deposition, the change in alloy morphol‐ ogy has been noted by several researchers with increase in current densities [64, 65, 68].

The dendritic or irregular shaped morphology in response to the current density is due to the fact that if there is a significant increase in the current density, it increases the nucleation rate and is also associated with a higher rate of hydrogen evolution. Due to high overpotential at this state, the rate of diffusion of Sn2+ ions towards cathode becomes significant over its replenishment from the electrolyte [68, 69]. This phenomenon creates a concentration gradient in the vicinity of electrolyte/cathode interface. As a consequence, the deposition occurs preferentially on certain protrusions (heterogeneous active sites on the cathode in a random manner. This type of non-uniform growth kinetics has also been observed in copper plating [70]. The cathodic current efficiency at this stage is poor indicating a rapid hydrogen evolution

The effect of pH in tin plating has not been discussed in detail in the literature. The majority of the tin plating baths available in literature are acidic in nature. As a general statement the rate of deposition increases with pH [71]. Bath pH not only affects the deposition rate but modifies the crystal orientation. Some people have noted a pH induced texture in Sn grains from acidic electrolyte [72]. Ebrahimi *et al*. investigated the effect of pH on nickel deposits [73]. He found that the pH values of 4.5, 4.7, and 5.0 resulted in grain size of 79, 45, and 56 nm, respectively. The increasing pH value from 2.8 to 5.1 enhanced the nucleation rate of nickel crystals, which corresponded to decreasing grain size from 343 to 35 nm. For copper electro‐ deposition, Natter and Hempelmann reported the smallest copper grain size of 8 nm at pH 1.5–2.0 and a continuous increase of the grain size up to 100 nm at pH 11.5 [74]. The morphology of the deposited Sn coatings with different bath pH gets refined with an increase in pH. At a high value of pH around 2, irregular and porous deposits are observed due to the progressive increase in hydrogen evolution reaction. However, at a very high pH (=3), the deposits turn

which decreases the concentration of Sn2+ ions in the electrolyte.

powdery due to severe hydrogen gas evolution [54].

in the following sections.

**6.1. Current density**

116 Electroplating of Nanostructures

**6.2. pH**

The majority of acid type formulations operate at room temperature, while alkaline tin baths need to be heated at higher optimum temperatures. As the temperature increases, the rate of deposition also increases [41, 54, 74]. The velocity (diffusion and migration) of the metal ions and inhibitor molecules are functions of the temperature. The viscosity of the electrolyte decreases at high temperature, therefore, the diffusion rate and the velocity of metal ions and inhibitor molecules are increased. Sahaym *et al*. studied the effect of bath temperature in Sn electrodeposits and found the pyramid type morphology at elevated temperatures [75]. They varied the bath temperature from 35ºC to 85ºC and explained that at higher bath/substrate temperature, the cooling rate of the adatoms will be slower. This indicates that at higher plating temperatures, adatoms can travel to longer diffusion distances on the cathode. This shows that an increase in the bath temperature may lead to increased grain growth and a smooth coating surface. Similar results are shown by Sharma *et al*. [74]. Bath temperature has been also shown to affect the morphology of the whiskers that formed upon aging at room temperature [75]. The metal ions and the inhibiting species have a higher mobility at high temperatures. It results in an increase in the concentration of metal ions towards the cathode and a decreases in the cathodic overpotential is observed. This increases the energy barrier (ΔG) for the nucleation process according to the equation given by Glasstone in reference [74], resulting in coarser grain size at higher temperature:

$$
\Delta G \propto \left| \frac{1}{\left(\eta + \left[\frac{C}{C}\right]\right)^2} \right| \tag{13}
$$

where *C* ' is the activity of the Sn2+ on the electrode and C is the activity of Sn2+ in the bulk solution. The adsorption rate of inhibiting species decreases at high temperatures due to the decrease in viscosity causing an enhanced grain growth. It is reported in the past that in an acidic plating bath may decompose at high temperature [41, 42]. Therefore, the plating bath color may also change from light to dark yellow and get precipitated. This may be due to the decomposition of the sulfate entity or oxidation of Sn2+ to Sn4+, which affects the solution chemistry [41–42, 45, 46]. The plating bath decomposition at elevated temperatures will decrease the bath conductivity and hence the current efficiency decreases beyond 40°C, with a negligible change in deposit morphology.

#### **6.4. Additives**

Although literature review about composite films and nanocrystalline films contains infor‐ mation about additives, additives for conventional metal deposition are still important as those additives would provide another aspect of information about deposition mechanism and novel additives. Popular organic additives that have been used in electrodeposition are gelatin, thiourea, EDTA (Ethylenediaminetetracetic acid), citric acid, benzotriazole (BTA), and inorganic additives such as chloride, are covered in this chapter. Nakamura *et al*. used various organic additives such as benzalacetone (BA) and N, N-bis (tetraoxyethylene) octadecylamine [50]. They found that by increasing the concentration of BA, smaller grains are obtained and roughness increases. Further, when both are used with a high concentration of BA, fine-grained deposits are obtained due to a synergistic action of these adsorbed species. Tzeng *et al*. studied the behavior of aliphatic and aromatic aldehyde groups in tin electrodeposition. They found that as compared to formaldehayde and propionoaldehyde, benzaldehyde is hydrophobic in nature showing more overpotential and thus acts as the best grain refiner [49]. Surface active agents such as Triton X-100, aromatic carbonyl compounds, amine-aldehyde reaction prod‐ ucts, methane sulphonic acid and its derivatives, etc. [50, 52, 57, 58, 76, 77], are added to plating baths. The addition of excessive amounts of additives, high current density, and an increase in the concentration of metal ions in the electrolyte may affect the deposit solderability. It is mainly attributed to the oxidation of tin ions in the solution, as well as the aging of the deposit in the presence of organic brighteners [76–78]. Fine-grained and smooth deposits were obtained from acid stannous sulphate solutions containing some aromatic ketones [50]. It was found that these organic compounds were adsorbed on the cathode surface and enhanced the overpotential. In acidic solutions, many other chemicals, such as polyoxyethylene laurylether, triethanolamine, sorbitol, sodium gluconate, 1, 4- hydroxybenzene, Trion X-100, or polypro‐ pylene glycol may be added as complexing agents. The additives are necessary to improve solution stability and deposit morphology. However, an excessive amount of additives would make the coating less solderable [54, 57, 58, 78].

For alkaline stannate bath additives, few reports are available in literature. They usually do not require any additives since deposition occurs at a very negative potential and hydrogen evolution runs parallel with tin deposition acting as a leveler. However, the disadvantage is the diffusion of hydrogen inside the tin deposits [74–79]. In literature, the effect of additives has not been discussed in detail for chlorides electrolytes. Sekar *et al*. investigated the effect of additives in detail on pulse elctrodeposition of tin containing Gelatin, β-naphthol, polyethy‐ lene glycol, peptone, and histidine as additives [80]. They observed a grain refinement brought about by additives but a marked decrease in current efficiency and found that the bath containing peptone has the lowest crystallite size with better corrosion properties. The selection of organic additive(s) generally depends upon the nature of the metal ions, bath pH, as well as the temperature of the plating solution/substrate. For instance, semi-bright or bright nickel plating solution has different sets of additives as compared to the additives used in acidic zinc plating. Similarly, additives used in acid tin plating baths are different than those used in alkaline tin plating. However, the coating morphologies and properties obtained from acidic and alkaline solutions may or may not be similar to each other. In MSA baths, glycol type additives, PEG, PPG, and Phenolphthalein have been tried in literature [55]. Glycol-type additives are effective in minimizing hydrogen gas evolution at low overpotentials and refining the grain structure across a wide current density range. These additives are active in the presence of Phenolphthalein [57]. Low and Walsh used the perfluorinated surfactant in MSA bath and observed that the adsorption of the surfactant hindered hydrogen evolution and reduced the peak and limiting current densities [58]. There is little information on pyrophosphate baths in literature. Pyrophosphate baths include mostly glycol additives used in SnAg type solder bumps. These baths require more control of the electrodeposition parameters. Normally chelating agents and organic additives such as triethanolamine, sodium gluconate, 1, 4-hydroxybenzene, and Triton X-100 have been added in pyrophosphate baths [42, 59, 60, 61, 81, 82]. The additives are active only up to a certain concentration and have a beneficial effect on the microstructure of the deposits by increasing the cathodic polarization.

At higher concentration of additives, the progressive evolution of hydrogen gas leads to the development of non-uniform powdery deposits. The powdery deposits generally arise due to the adsorption and absorption of the hydrogen gases in the deposits according to the following reactions [54, 83]:

$$\text{2H}\_{\text{ads}} \text{--} \text{H}\_2 \tag{14}$$

$$\mathbf{H}^+ \mathbf{+e}^- \cdots \mathbf{H}\_{\text{ads}} \tag{15}$$

$$\text{CH}\_{\text{ads}} \text{---} \text{H}\_{\text{abs}} \tag{16}$$

The additive blocks the association of generated hydrogen atoms according to Equation (14). Consequently, the concentrations of Hads rises following Equation (15). The combined effect of these two phenomena (Equations 15 and 16) results in absorption of hydrogen atoms in the deposits according to Equation (16).

#### **6.5. Duty cycle and frequency**

thiourea, EDTA (Ethylenediaminetetracetic acid), citric acid, benzotriazole (BTA), and inorganic additives such as chloride, are covered in this chapter. Nakamura *et al*. used various organic additives such as benzalacetone (BA) and N, N-bis (tetraoxyethylene) octadecylamine [50]. They found that by increasing the concentration of BA, smaller grains are obtained and roughness increases. Further, when both are used with a high concentration of BA, fine-grained deposits are obtained due to a synergistic action of these adsorbed species. Tzeng *et al*. studied the behavior of aliphatic and aromatic aldehyde groups in tin electrodeposition. They found that as compared to formaldehayde and propionoaldehyde, benzaldehyde is hydrophobic in nature showing more overpotential and thus acts as the best grain refiner [49]. Surface active agents such as Triton X-100, aromatic carbonyl compounds, amine-aldehyde reaction prod‐ ucts, methane sulphonic acid and its derivatives, etc. [50, 52, 57, 58, 76, 77], are added to plating baths. The addition of excessive amounts of additives, high current density, and an increase in the concentration of metal ions in the electrolyte may affect the deposit solderability. It is mainly attributed to the oxidation of tin ions in the solution, as well as the aging of the deposit in the presence of organic brighteners [76–78]. Fine-grained and smooth deposits were obtained from acid stannous sulphate solutions containing some aromatic ketones [50]. It was found that these organic compounds were adsorbed on the cathode surface and enhanced the overpotential. In acidic solutions, many other chemicals, such as polyoxyethylene laurylether, triethanolamine, sorbitol, sodium gluconate, 1, 4- hydroxybenzene, Trion X-100, or polypro‐ pylene glycol may be added as complexing agents. The additives are necessary to improve solution stability and deposit morphology. However, an excessive amount of additives would

For alkaline stannate bath additives, few reports are available in literature. They usually do not require any additives since deposition occurs at a very negative potential and hydrogen evolution runs parallel with tin deposition acting as a leveler. However, the disadvantage is the diffusion of hydrogen inside the tin deposits [74–79]. In literature, the effect of additives has not been discussed in detail for chlorides electrolytes. Sekar *et al*. investigated the effect of additives in detail on pulse elctrodeposition of tin containing Gelatin, β-naphthol, polyethy‐ lene glycol, peptone, and histidine as additives [80]. They observed a grain refinement brought about by additives but a marked decrease in current efficiency and found that the bath containing peptone has the lowest crystallite size with better corrosion properties. The selection of organic additive(s) generally depends upon the nature of the metal ions, bath pH, as well as the temperature of the plating solution/substrate. For instance, semi-bright or bright nickel plating solution has different sets of additives as compared to the additives used in acidic zinc plating. Similarly, additives used in acid tin plating baths are different than those used in alkaline tin plating. However, the coating morphologies and properties obtained from acidic and alkaline solutions may or may not be similar to each other. In MSA baths, glycol type additives, PEG, PPG, and Phenolphthalein have been tried in literature [55]. Glycol-type additives are effective in minimizing hydrogen gas evolution at low overpotentials and refining the grain structure across a wide current density range. These additives are active in the presence of Phenolphthalein [57]. Low and Walsh used the perfluorinated surfactant in MSA bath and observed that the adsorption of the surfactant hindered hydrogen evolution and reduced the peak and limiting current densities [58]. There is little information on

make the coating less solderable [54, 57, 58, 78].

118 Electroplating of Nanostructures

The pulse deposition rate is given by the pulse current density and other parameters such as 'on' time (*Ton*) and 'off' (*Toff*) time. The pulse length *Ton* and *Toff* time have significant effect on grain size. An increase in pulse current density at constant length *Ton* and constant average current density with an increase in *Toff* time cause an increase in grain-size, because grain growth takes place during the *Toff* time. But an increase in pulsed current density at constant pulse charge and at constant *Toff* implies a decrease in grain-size. Therefore, a shor*t Ton* prevents grain growth and increases the nucleation rate [32].

The frequency of the pulse is the reciprocal of the total pulse duration consisting of *Ton* and *Toff*. The pulse length *Ton* and *Toff* time had significant effect on grain size. A higher pulse duration at lower pulse frequencies indicates enough time for the charging (*Ton* ) and discharging (*Toff*) ofthe double layer[36–38].In contrast, at a high pulse frequency the double layer does not have enough time for charging and discharging [39, 40]. Thus, lowerfrequencies cause bigger grains while higher frequencies results in a grain refinement of the electrodeposits [36–41, 84].

The deposition rate in the pulse technique is governed by the pulse current density (*Jpeak*), and on time (*Ton*) and off time (*Toff*). At a given peak current density, the duty cycle is given by:

$$\text{Duty Cycle (\%)} = \frac{T\_{\text{ou}}}{T\_{\text{on}} + T\_{\text{off}}} \tag{17}$$

As discussed already, the average current density (*Javerage*) in a pulse electrodeposition is given by:

$$J\_{\text{average}} = \text{Duty Cycle} \times J\_{\text{peak}} \tag{18}$$

where *Jpeak* is the peak current density. A 100% duty cycle means there is no pulse used. The effect of pulse parameters has been studied in a paper by Sharma *et al*. [54], where they used various combinations of pulse on and on time to produce several duty cycles as shown in Table 2. These combinations are not unique and can be varied according to the desired changes in deposit microstructures.


(Reprinted "With kind permission from Springer Science+Business Media: Journal of Metallurgical and Materials Transactions A, Volume 45, 2014, Issue 10, Page 4610-4622, A. Sharma, S. Bhattacharya, S. Das, K. Das, Table II. © The Minerals, Metals & Materials Society and ASM International 2014").

**Table 2.** Pulse parameters at various duty cycles.

However, at a duty cycle of 100%, the grain size observed is usually much coarser. Thus, it is inferred that the grain size of the deposits decreases with an increase in *Ton* (at constant *Toff* and *Jpeak*). An increase in *Ton* (longer current on times) results in an increased overpotential [84]. Youssef and his co-workers have also observed similar behavior in zinc electrodeposits [85]. It is reported that the deposit grain size decreases up to a duty cycle of 44%, and an increase in the grain size is noticed beyond duty cycle of 44%. This may be explained due to the fact that the pulse deposition gets transformed to the direct current deposition at this stage [85].

The pulse current (PC) with lower duty cycle (<20%) produces uniform and compact deposits. At higher duty cycles (>20%) and at direct current (DC) deposition, severe increase porosity is observed. This may be due to higher average current flow time *Ton*, which triggers hydrogen gas evolution [86]. This type of porous deposit morphology can be attributed to the dissolved hydrogen and oxygen gases in the plating bath. A higher solubility of hydrogen (1617 and 43.3 mg/L in water) compared to that of the oxygen in water (43.3 mg/L), at 25ºC and a 1 bar favors the dissolution of hydrogen gas and its incorporation over oxygen in the deposits [86]. Therefore, the morphology is rather porous and rough beyond a duty cycle of 20%.

A reduced porosity in case of PC deposition with lower duty cycles can be correlated to the two factors. (i) partial diffusion of the hydrogen and oxygen gas away from the substrate during off time (*Toff*) and hence a suppressed absorption of hydrogen gas in the deposit; (ii) the total amount of gas generated during the electrolysis of water in on time (*Ton*) is less compared to a continuous DC [54, 86]. Therefore, pulse current with lower duty cycle will result in a uniform and dense morphology as compared to high duty cycles or DC deposition.

The morphology of electrodeposits is also influenced by the pulse frequency in the electrode‐ position. The pulse frequency parameters varied according to Sharma *et al*. [54] and are shown in Table 3. These combinations are also not unique like the duty cycle and can be varied to obtain the optimum deposit microstructures.

Frequency (*f*) of the pulse is described as follows:

$$f = \frac{1}{\left(T\_{\rm ou} + T\_{\rm off}\right)}\tag{19}$$


(Reprinted "With kind permission from Springer Science+Business Media: Journal of Metallurgical and Materials Transactions A, Volume 45, 2014, Issue 10, Page 4610-4622, A. Sharma, S. Bhattacharya, S. Das, K. Das, Table III. © The Minerals, Metals & Materials Society and ASM International 2014").

**Table 3.** Pulse frequency parameters

Duty Cycle % ( ) *on*

by:

deposit microstructures.

120 Electroplating of Nanostructures

As discussed already, the average current density (*Javerage*) in a pulse electrodeposition is given

where *Jpeak* is the peak current density. A 100% duty cycle means there is no pulse used. The effect of pulse parameters has been studied in a paper by Sharma *et al*. [54], where they used various combinations of pulse on and on time to produce several duty cycles as shown in Table 2. These combinations are not unique and can be varied according to the desired changes in

(Reprinted "With kind permission from Springer Science+Business Media: Journal of Metallurgical and Materials Transactions A, Volume 45, 2014, Issue 10, Page 4610-4622, A. Sharma, S. Bhattacharya, S. Das, K. Das, Table II. © The

However, at a duty cycle of 100%, the grain size observed is usually much coarser. Thus, it is inferred that the grain size of the deposits decreases with an increase in *Ton* (at constant *Toff* and *Jpeak*). An increase in *Ton* (longer current on times) results in an increased overpotential [84]. Youssef and his co-workers have also observed similar behavior in zinc electrodeposits [85]. It is reported that the deposit grain size decreases up to a duty cycle of 44%, and an increase in the grain size is noticed beyond duty cycle of 44%. This may be explained due to the fact that the pulse deposition gets transformed to the direct current deposition at this stage [85].

The pulse current (PC) with lower duty cycle (<20%) produces uniform and compact deposits. At higher duty cycles (>20%) and at direct current (DC) deposition, severe increase porosity is observed. This may be due to higher average current flow time *Ton*, which triggers hydrogen gas evolution [86]. This type of porous deposit morphology can be attributed to the dissolved hydrogen and oxygen gases in the plating bath. A higher solubility of hydrogen (1617 and 43.3

**Duty Cycle (%)** *Ton (s) Toff (s)* 0.00042 0.01 0.0011 0.01 0.0025 0.01 0.0067 0.01 0.0150 0.01

Minerals, Metals & Materials Society and ASM International 2014").

**Table 2.** Pulse parameters at various duty cycles.

*on off T*

*T T* <sup>=</sup> <sup>+</sup> (17)

Duty Cycle *average peak J J* = ´ (18)

Lower pulse frequency (*f*) indicates a longer pulse period (*Ton*+*Toff*) at a constant duty cycle (D), as shown in Equation (19). The pulse duration is higher at lower frequencies providing sufficient time for the charging and discharging of the double layer.

The Sn atoms can migrate freely to the most stable position facilitating the grain growth. An increase in the pulse frequency shortens the pulse duration, i.e., both *Ton* and *Toff* are smaller as shown in Table 3. Shanthi *et al*. have noticed a severe grain refinement during pulse current plating of silver alloy with short pulse and high frequency [84]. As already discussed, at high pulse frequencies the charging an discharging action of double layer gets poor. These phe‐ nomena results in very thin diffusion layers that make the transportation of the migrating Sn ions towards cathode difficult. The nucleation rate improves as a consequence a dense microstructure is obtained [85, 66].

#### **6.6. Effect of agitation**

Agitation in the plating solution can be produced either by agitating the electrolyte or by moving the cathode. At low agitation rates, the effect of agitation on deposit composition is not visible, while the agitation rates may decrease the tin content in the coatings. Moreover, agitation may also increase the deposit roughness up to some extent [42, 54]. Agitation has beneficial effects of increasing the plating rate and permits the use of higher current densities by lowering polarization [36, 37, 38, 39]. Wen and Szpunar studied the nucleation and growth of tin and pointed out that agitation should not exceed beyond a certain limit where turbulent flow occurs that cause the difficulty of tin ions supply to the cathode even at high current densities [87]. Thus the cathode coverage is poor and the deposition rate decreases.

It is interesting to note that the stirring rate of the bath has a significant effect on the deposit morphology. The deposition parameters, except the stirring speed that controls the bath agitation, are kept constant. During still deposition, the cathode coverage is poor, and irregular and non-uniform deposits are obtained. This can be explained as when no agitation is provided, the depositing ions from the electrolyte get deposited preferentially on the cathode. Thus, a concentration gradient is established in the vicinity of electrolyte/cathode interface. The deposition is uneven at this stage and morphology is very poor. When the bath stirring is increased, the concentration gradient is decreased and deposition rate increases [87, 88]. Further stirring of the bath will cause fast transportation of metal ions towards cathode. At a sufficiently high stirring rates of the plating bath, the flow of the electrolyte will be turbulent and the metal ions may move away from the cathode vigorously and a lowering in the deposition rate is observed [88].

## **7. Sensitivity of the variables and grain size distribution**

The electrodeposition parameters considered in this investigation include current density, concentration of the additive, duty cycle, frequency, pH, temperature, and agitation. The obtained results in this work indicate that the pulsed current electrodeposition can be an efficient method for the electrosynthesis of tin deposits. The surface morphology evolution depends on the electrodeposition parameter that tries to modify the overpotential, in a direct or indirect way. The current density is the most sensitive of all the plating parameters which affects the deposit morphology severely. The nucleation rate and grain growth can be signif‐ icantly controlled by changing the duty cycle to lower values up 5 to 20%. At higher duty cycles, the porous deposits are produced.

Smaller pulse frequency gives large grained deposits. Thus, a combination of duty cycle and pulse frequency can be optimized for an ultrafine grained or an optimum grain morphology depending upon the application. The presence of additives in the plating bath improves the surface finish and morphology if it is added up to its optimum concentration. The current density is found to decrease with bath pH increase. The grain size decreases as pH value increases due to the increase in the cathodic polarization. It is also noteworthy point that powdery deposits are too developed at very high pH due to the precipitation of stannic hydroxides. An increase in bath temperature is noticed to raise the grain size of the deposits. However, a decrease in the electrolyte conductivity and current efficiency is noted at elevated temperatures due to the precipitation of metal ions in the plating bath. Bath stirring improves the availability of metal ions towards cathode and thus the deposition rate is enhanced before the flow of electrolyte turns turbulent where the metal ions move away from the cathode. The grain size is also increased due to the decrease in overpotential with bath stirring rate

## **Author details**

**6.6. Effect of agitation**

122 Electroplating of Nanostructures

deposition rate is observed [88].

cycles, the porous deposits are produced.

Agitation in the plating solution can be produced either by agitating the electrolyte or by moving the cathode. At low agitation rates, the effect of agitation on deposit composition is not visible, while the agitation rates may decrease the tin content in the coatings. Moreover, agitation may also increase the deposit roughness up to some extent [42, 54]. Agitation has beneficial effects of increasing the plating rate and permits the use of higher current densities by lowering polarization [36, 37, 38, 39]. Wen and Szpunar studied the nucleation and growth of tin and pointed out that agitation should not exceed beyond a certain limit where turbulent flow occurs that cause the difficulty of tin ions supply to the cathode even at high current

densities [87]. Thus the cathode coverage is poor and the deposition rate decreases.

**7. Sensitivity of the variables and grain size distribution**

It is interesting to note that the stirring rate of the bath has a significant effect on the deposit morphology. The deposition parameters, except the stirring speed that controls the bath agitation, are kept constant. During still deposition, the cathode coverage is poor, and irregular and non-uniform deposits are obtained. This can be explained as when no agitation is provided, the depositing ions from the electrolyte get deposited preferentially on the cathode. Thus, a concentration gradient is established in the vicinity of electrolyte/cathode interface. The deposition is uneven at this stage and morphology is very poor. When the bath stirring is increased, the concentration gradient is decreased and deposition rate increases [87, 88]. Further stirring of the bath will cause fast transportation of metal ions towards cathode. At a sufficiently high stirring rates of the plating bath, the flow of the electrolyte will be turbulent and the metal ions may move away from the cathode vigorously and a lowering in the

The electrodeposition parameters considered in this investigation include current density, concentration of the additive, duty cycle, frequency, pH, temperature, and agitation. The obtained results in this work indicate that the pulsed current electrodeposition can be an efficient method for the electrosynthesis of tin deposits. The surface morphology evolution depends on the electrodeposition parameter that tries to modify the overpotential, in a direct or indirect way. The current density is the most sensitive of all the plating parameters which affects the deposit morphology severely. The nucleation rate and grain growth can be signif‐ icantly controlled by changing the duty cycle to lower values up 5 to 20%. At higher duty

Smaller pulse frequency gives large grained deposits. Thus, a combination of duty cycle and pulse frequency can be optimized for an ultrafine grained or an optimum grain morphology depending upon the application. The presence of additives in the plating bath improves the surface finish and morphology if it is added up to its optimum concentration. The current density is found to decrease with bath pH increase. The grain size decreases as pH value increases due to the increase in the cathodic polarization. It is also noteworthy point that powdery deposits are too developed at very high pH due to the precipitation of stannic Ashutosh Sharma1\*, Siddhartha Das2 and Karabi Das2

1 Department of Materials Science and Engineering, University of Seoul, Seoul, Korea

2 Department of Metallurgical and Materials Engineering, Indian Institute of Technology Kharagpur, Kharagpur, India

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## **Chapter 6**
