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Chapter 7: Problem 104

We will see in Chapter 12 that semiconductors are materials that conduct electricity better than nonmetals but not as well as metals. The only two elements in the periodic table that are technologically useful semiconductors are silicon and germanium. Integrated circuits in computer chips today are based on silicon. Compound semiconductors are also used in the electronics industry. Examples are gallium arsenide, GaAs; gallium phosphide, GaP; cadmium sulfide, CdS; cadium selenide, CdSe. (a) What is the relationship between the compound semiconductors' compositions and the positions of their elements on the periodic table relative to \(\mathrm{Si}\) and Ge? (b) Workers in the semiconductor industry refer to \({ }^{4} \mathrm{II}-\mathrm{VI}^{m}\) and \({ }^{4} \mathrm{III}-\mathrm{V}^{n} \mathrm{ma}-\) terials, using Roman numerals; can you identify which compound semiconductors are II-VI and which are III-V? Suggest other compositions of compound semiconductors based on the positions of their elements in the periodic table.

Short Answer

Expert verified
(a) Compound semiconductors' compositions consist of one element from a group adjacent to Group IV, and one element from the opposite group adjacent to Group IV. For example, Ga is from Group III, and As is from Group V; Cd is from Group II, and S is from Group VI. (b) GaAs and GaP are \({}^{4}\mathrm{III}-\mathrm{V}^{n}\mathrm{ma}\) materials, while CdS and CdSe are \({}^{4}\mathrm{II}-\mathrm{VI}^{m}\) materials. Other possible compound semiconductor compositions include AlN, GaN, InP (Group III-V), and ZnS, ZnSe, MgTe (Group II-VI).

Step by step solution

01

1. Identify the positions of Si, Ge and compound semiconductors elements on the periodic table

Locate Silicon(Si) and Germanium(Ge) on the periodic table, which are both in Group IV. Then locate the elements of the compound semiconductors such as Gallium(Ga), Arsenic(As), Phosphorus(P), Cadmium(Cd), Sulfur(S), and Selenium(Se). Note that Gallium is in Group III, Arsenic is in Group V, Phosphorus is in Group V, Cadmium is in Group II, Sulfur is in Group VI, and Selenium is in Group VI.
02

2. Analyze the relationship between compound semiconductors and positions of their elements relative to Si and Ge

Observe the compositions of the compound semiconductors mentioned in the exercise: GaAs, GaP, CdS, and CdSe. Notice that they all consist of one element from Group II or Group III and one element from Group V or Group VI. Si and Ge are both in Group IV, and compound semiconductors are formed by combining elements from groups adjacent to Group IV. (a) Compound semiconductors' compositions consist of one element from a group adjacent to Group IV, and one element from the opposite group adjacent to Group IV. For example, Ga is from Group III, and As is from Group V; Cd is from Group II, and S is from Group VI.
03

3. Identify the compound semiconductors and determine their Roman numeral classifications

Consider the given compound semiconductors: GaAs, GaP, CdS, and CdSe. GaAs and GaP are composed of elements from Group III (Ga) and Group V (As and P, respectively). These compounds are III-V semiconductors. CdS and CdSe are composed of elements from Group II (Cd) and Group VI (S and Se, respectively). These compounds are II-VI semiconductors. (b) GaAs and GaP are \({}^{4}\mathrm{III}-\mathrm{V}^{n}\mathrm{ma}\) materials, while CdS and CdSe are \({}^{4}\mathrm{II}-\mathrm{VI}^{m}\) materials.
04

4. Suggest other compositions of compound semiconductors

Based on the positions of elements in the periodic table, we can suggest other possible compound semiconductor compositions involving elements adjacent to Group IV. Examples include: - Aluminum Nitride (AlN) - Group III and Group V - Gallium Nitride (GaN) - Group III and Group V - Indium Phosphide (InP) - Group III and Group V - Zinc Sulfide (ZnS) - Group II and Group VI - Zinc Selenide (ZnSe) - Group II and Group VI - Magnesium Telluride (MgTe) - Group II and Group VI

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Most popular questions from this chapter

Some ions do not have a corresponding neutral atom that has the same electron configuration. For each of the following ions, identify the neutral atom that has the same number of electrons and determine if this atom has the same electron configuration. If such an atom does not exist, explain why. (b) \(\mathrm{Sc}^{3+}\) (d) \(\mathrm{Zn}^{2+},(\mathrm{e}) \mathrm{Sn}^{4+}\) (a) \(\mathrm{Cl}\) (c) \(\mathrm{Fe}^{2+}\)

Make a simple sketch of the shape of the main part of the periodic table, as shown. (a) Ignoring \(\mathrm{H}\) and He, write a single straight arrow from the element with the smallest bonding atomic radius to the element with the largest. Ignoring \(\mathrm{H}\) and He, write a single straight arrow from the element with the smallest first ionization energy to the element with the largest. (c) What significant observation can you make from the arrows you drew in parts (a) and (b)? [Sections 7.3 and 7.4]

(a) Use orbital diagrams to illustrate what happens when an oxygen atom gains two electrons. (b) Why does \(\mathrm{O}^{3-}\) not exist?

When magnesium metal is burned in air (Figure 3.6 ), two products are produced. One is magnesium oxide, \(\mathrm{MgO}\). The other is the product of the reaction of \(\mathrm{Mg}\) with molecular nitrogen, magnesium nitride. When water is added to magnesium nitride, it reacts to form magnesium oxide and ammonia gas. (a) Based on the charge of the nitride ion (Table 2.5 ), predict the formula of magnesium nitride. (b) Write a balanced equation for the reaction of magnesium nitride with water. What is the driving force for this reaction? (c) In an experiment a piece of magnesium ribbon is burned in air in a crucible. The mass of the mixture of \(\mathrm{MgO}\) and magnesium nitride after burning is \(0.470 \mathrm{~g}\). Water is added to the crucible, further reaction occurs, and the crucible is heated to dryness until the final product is \(0.486 \mathrm{~g}\) of \(\mathrm{MgO}\). What was the mass percentage of magnesium nitride in the mixture obtained after the initial burning? (d) Magnesium nitride can also be formed by reaction of the metal with ammonia at high temperature. Write a balanced equation for this reaction. If a 6.3 -g Mg ribbon reacts with \(2.57 \mathrm{~g} \mathrm{NH}_{3}(g)\) and the reaction goes to completion, which component is the limiting reactant? What mass of \(\mathrm{H}_{2}(g)\) is formed in the reaction? (e) The standard enthalpy of formation of solid magnesium nitride is \(-461.08 \mathrm{~kJ} / \mathrm{mol} .\) Calculate the standard enthalpy change for the reaction between magnesium metal and ammonia gas.

Moseley established the concept of atomic number by studying X-rays emitted by the elements. The X-rays emitted by some of the elements have the following wavelengths: $$ \begin{array}{ll} \hline \text { Element } & \text { Wavelength }(\AA) \\\ \hline \mathrm{Ne} & 14.610 \\ \mathrm{Ca} & 3.358 \\ \mathrm{Zn} & 1.435 \\\ \mathrm{Zr} & 0.786 \\ \mathrm{Sn} & 0.491 \\ \hline \end{array} $$
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