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Chapter 22: Problem 70

Write the formulas for the following compounds, and indicate the oxidation state of the group 4 A element or of boron in each: (a) silicon dioxide, (b) germanium tetra chloride, (c) sodium borohydride, (d) stannous chloride, (e) diborane, (f) boron trichloride.

Short Answer

Expert verified
(a) Silicon dioxide formula is SiO_2, and the oxidation state of Si is +4. (b) Germanium tetra chloride formula is GeCl_4, and the oxidation state of Ge is +4. (c) Sodium borohydride formula is NaBH_4, and the oxidation state of B is -3. (d) Stannous chloride formula is SnCl_2, and the oxidation state of Sn is +2. (e) Diborane formula is B_2H_6, and the oxidation state of both B atoms is +3. (f) Boron trichloride formula is BCl_3, and the oxidation state of B is +3.

Step by step solution

01

(a) Silicon dioxide formula and oxidation state

Silicon (Si) is from Group 4A, and oxygen (O) is in Group 6A. The formula for silicon dioxide can be determined by finding the lowest common multiple of their valence electrons to form a neutral compound. Since silicon has 4 valence electrons and oxygen has 6, the compound formula is SiO_2. In this case, the oxidation state of Si is +4 because each oxygen is taking two electrons from silicon.
02

(b) Germanium tetra chloride formula and oxidation state

Germanium (Ge) is from Group 4A, and chlorine (Cl) is in Group 7A. We can determine the compound formula similarly by finding the lowest common number of valence electrons needed to form a neutral compound. Since germanium has 4 valence electrons and chlorine has 7, the compound formula is GeCl_4. The oxidation state of germanium in this compound is +4 because each chlorine contributes a -1 charge.
03

(c) Sodium borohydride formula and oxidation state

Sodium (Na) is from Group 1A, boron (B) is from Group 3A, and hydrogen (H) is in Group 1A. In this case, the negative hydrogen acts as a hydride ion (H^-). Because sodium has a +1 charge and boron requires three electrons from hydrogen to get the lowest common multiple of their valence electrons, the compound forms NaBH_4. The oxidation state of boron in this compound is -3 because it gains three electrons from hydrogen.
04

(d) Stannous chloride formula and oxidation state

"Stannous" indicates that this is a tin(II) compound, which means tin (Sn) has an oxidation state of +2. Chlorine (Cl) has a -1 charge value in the compound. To create a neutral compound, we need two chlorine atoms for each tin atom, resulting in a formula of SnCl_2. The oxidation state of tin is +2, as already mentioned.
05

(e) Diborane formula and oxidation state

Diborane refers to a compound with two boron atoms (B) and six hydrogen atoms (H), therefore the formula is B_2H_6. As it's a unusual compound, both boron atoms have an oxidation state of +3 in diborane. Note, in this case, we need to know the structure of the compound instead of using valence electrons.
06

(f) Boron trichloride formula and oxidation state

Boron (B) is from Group 3A, and chlorine (Cl) is in Group 7A. The lowest common multiple of their valence electrons needed to form a neutral compound is three for boron and one for chlorine. Thus, the compound formula is BCl_3. The oxidation state of boron in this compound is +3 because it loses three electrons to the three chlorine atoms.

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Most popular questions from this chapter

Predict whether each of the following oxides is acidic, basic, amphoteric, or neutral: (a) \(\mathrm{NO}_{2},(\mathbf{b}) \mathrm{CO}_{2},(\mathbf{c}) \mathrm{Al}_{2} \mathrm{O}_{3},(\mathbf{d}) \mathrm{CaO}\)

Name the following compounds and assign oxidation states to the halogens in them: (a) \(\mathrm{Fe}\left(\mathrm{ClO}_{3}\right)_{3},(\mathbf{b}) \mathrm{HClO}_{2}\) (c) \(\mathrm{XeF}_{6},(\mathbf{d}) \mathrm{BrF}_{5},(\mathbf{e}) \mathrm{XeOF}_{4},(\mathbf{f}) \mathrm{HIO}_{3}\)

Ultrapure germanium, like silicon, is used in semiconductors. Germanium of "ordinary" purity is prepared by the high-temperature reduction of \(\mathrm{GeO}_{2}\) with carbon. The Ge is converted to GeCl_ by treatment with \(\mathrm{Cl}_{2}\) and then purified by distillation; GeCl_ is then hydrolyzed in water to GeO \(_{2}\) and reduced to the elemental form with \(\mathrm{H}_{2}\) . The element is then zone refined. Write a balanced chemical equation for each of the chemical transformations in the course of forming ultrapure Ge from GeO \(_{2} .\)

Give the chemical formula for (a) hydrocyanic acid, (b) nickel tetracarbonyl, (c) barium bicarbonate, (d) calcium acetylide, (e) potassium carbonate.

A sulfuric acid plant produces a considerable amount of heat. This heat is used to generate electricity, which helps reduce operating costs. The synthesis of \(\mathrm{H}_{2} \mathrm{SO}_{4}\) consists of three main chemical processes: (a) oxidation of S to SO, (b) oxidation of \(\mathrm{SO}_{2}\) to \(\mathrm{SO}_{3},\) (c) the dissolving of \(\mathrm{SO}_{3}\) in \(\mathrm{H}_{2} \mathrm{SO}_{4}\) and the subsequent reaction with water to form \(\mathrm{H}_{2} \mathrm{SO}_{4}\) . If the third process produces \(130 \mathrm{kJ} / \mathrm{mol},\) how much heat is produced in preparing a mole of \(\mathrm{H}_{2} \mathrm{SO}_{4}\) from a mole of S? How much heat is produced in preparing 5000 pounds of \(\mathrm{H}_{2} \mathrm{SO}_{4} ?\)
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