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Chapter 22: Problem 69

Write the formulas for the following compounds, and indicate the oxidation state of the group 14 element or of boron in each: (a) silane, \((\mathbf{b})\) germanium dichloride, (c) \(\operatorname{tin}(\mathrm{II})\) sulfide, \((\mathbf{d})\) sodium borohydride, \((\mathbf{e})\) lead(IV) nitrate, \((\mathbf{f})\) tin dioxide.

Short Answer

Expert verified
(a) Silane: Formula - SiH4, Oxidation state of Si: 0 (b) Germanium dichloride: Formula - GeCl2, Oxidation state of Ge: +2 (c) Tin(II) sulfide: Formula - SnS, Oxidation state of Sn: +2 (d) Sodium borohydride: Formula - NaBH4, Oxidation state of B: +3 (e) Lead(IV) nitrate: Formula - Pb(NO3)4, Oxidation state of Pb: +4 (f) Tin dioxide: Formula - SnO2, Oxidation state of Sn: +4

Step by step solution

01

(a) Silane formula and oxidation state

Silane is a compound with the chemical formula SiH4. In this molecule, silicon (Si) is bonded to four hydrogen (H) atoms. Silicon's oxidation state in silane is 0, as it has gained no electrons.
02

(b) Germanium dichloride formula and oxidation state

Germanium dichloride has the chemical formula GeCl2. In this compound, germanium (Ge) is bonded to two chlorine atoms (Cl). To determine the oxidation state, we note that each chlorine atom has an oxidation state of -1, thus total oxidation state for the two chlorine atoms is -2. The germanium atom balances this by having an oxidation state of +2.
03

(c) Tin(II) sulfide formula and oxidation state

Tin(II) sulfide is a compound that includes tin in its +2 oxidation state. The chemical formula for tin(II) sulfide is SnS. The oxidation state of tin (Sn) in this compound is given as +2.
04

(d) Sodium borohydride formula and oxidation state

Sodium borohydride has the chemical formula NaBH4. In this compound, boron (B) is bonded to four hydrogen atoms in the form of hydride (H-) ions. Sodium (Na) is present as a cation with its +1 oxidation state, balancing the charges. Since the four hydride anions (H-) contribute a charge of -4, boron's oxidation state must be +3.
05

(e) Lead(IV) nitrate formula and oxidation state

Lead(IV) nitrate is a compound with lead in its +4 oxidation state. The chemical formula for lead(IV) nitrate is Pb(NO3)4. The oxidation state of lead (Pb) in this compound is given as +4.
06

(f) Tin dioxide formula and oxidation state

Tin dioxide has the chemical formula SnO2. In this compound, tin (Sn) is bonded to two oxygen atoms (O). To determine the oxidation state, we note that each oxygen atom has an oxidation state of -2, thus the total oxidation state for the two oxygen atoms is -4. The tin atom balances this by having an oxidation state of +4.

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Most popular questions from this chapter

Identify the following hydrides as ionic, metallic, or molecular: $(\mathbf{a}) \mathrm{H}_{2} \mathrm{~S},(\mathbf{b}) \mathrm{LiH},(\mathbf{c}) \mathrm{VH}_{0.56}$.

Give a reason why hydrogen might be placed along with the group 1 elements of the periodic table.

Write complete balanced half-reactions for (a) oxidation of nitrous acid to nitrate ion in acidic solution, (b) oxidation of \(\mathrm{N}_{2}\) to \(\mathrm{N}_{2} \mathrm{O}\) in acidic solution.

Although the \(\mathrm{ClO}_{4}^{-}\) and \(\mathrm{IO}_{4}^{-}\) ions have been known for a long time, \(\mathrm{BrO}_{4}^{-}\) was not synthesized until $1965 .$ The ion was synthesized by oxidizing the bromate ion with xenon difluoride, producing xenon, hydrofluoric acid, and the perbromate ion. (a) Write the balanced equation for this reaction. (b) What are the oxidation states of Br in the Br-containing species in this reaction?

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