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Chapter 22: Problem 57

Write a molecular formula for each compound, and indicate the oxidation state of the group 15 element in each formula: (a) hexafluoroantimonate(V) ion, (b) calcium phosphate, (c) potassium dihydrogen phosphate, (d) arsenic trioxide, (e) tetraphosphorus hexaoxide, (f) arsenic trifluoride.

Short Answer

Expert verified
(a) \(SbF_6^-\), oxidation state of antimony: +5 (b) \(Ca_3(PO_4)_2\), oxidation state of phosphorus: +5 (c) \(KH_2PO_4\), oxidation state of phosphorus: +5 (d) \(As_2O_3\), oxidation state of arsenic: +3 (e) \(P_4O_6\), oxidation state of phosphorus: +3 (f) \(AsF_3\), oxidation state of arsenic: +3

Step by step solution

01

(a) hexafluoroantimonate(V) ion formula and oxidation state of antimony

In hexafluoroantimonate(V) ion, the antimony (Sb) belongs to group 15 and has an oxidation state of +5. This compound is an ionic compound where antimony is bonded with six fluorine (F) atoms. Since Fluorine has an oxidation state of -1, six fluorine atoms will have the total oxidation state of -6. To form a complete ion, the formula will be \(SbF_6^-\), and the oxidation state of antimony is +5.
02

(b) Calcium phosphate formula and oxidation state of phosphorus

Calcium phosphate is an ionic compound with calcium (Ca) cations and phosphate (PO_4) anions. Calcium has a valency of +2, and phosphate has a valency of -3. To form a neutral compound, the ratio of calcium and phosphate ions would be 3:2. The molecular formula of calcium phosphate is \(Ca_3(PO_4)_2\). Phosphorus in the phosphate ion has an oxidation state of +5.
03

(c) Potassium dihydrogen phosphate formula and oxidation state of phosphorus

Potassium dihydrogen phosphate is an ionic compound with potassium (K) cations and dihydrogen phosphate (H_2PO_4) anions. Potassium has a valency of +1, and dihydrogen phosphate has a valency of -1. So, the ratio of potassium and dihydrogen phosphate ions would be 1:1. The molecular formula of potassium dihydrogen phosphate is \(KH_2PO_4\). In this compound, the oxidation state of phosphorus remains +5.
04

(d) Arsenic trioxide formula and oxidation state of arsenic

Arsenic trioxide is a covalent compound formed by the combination of arsenic (As) and oxygen (O). Arsenic belongs to group 15, and its oxidation state in this compound is +3. Oxygen has an oxidation state of -2. The molecular formula of arsenic trioxide is \(As_2O_3\). The oxidation state of arsenic is +3.
05

(e) Tetraphosphorus hexaoxide formula and oxidation state of phosphorus

Tetraphosphorus hexaoxide is a covalent compound formed by the combination of four phosphorus (P) atoms and six oxygen (O) atoms. The molecular formula of tetraphosphorus hexaoxide is \(P_4O_6\). In this compound, the oxidation state of phosphorus is not directly given, but it can be calculated as follows: Let x be the oxidation state of phosphorus. Oxidation state of oxygen = -2 Since there are four phosphorus atoms and six oxygen atoms, \(4x + 6(-2) = 0\) Solving for x, we get the oxidation state of phosphorus as +3.
06

(f) Arsenic trifluoride formula and oxidation state of arsenic

Arsenic trifluoride is a covalent compound formed by the combination of arsenic (As) and fluorine (F). In this compound, the arsenic has an oxidation state of +3. The molecular formula of arsenic trifluoride is \(AsF_3\). The oxidation state of arsenic is +3.

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Most popular questions from this chapter

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 \(\mathrm{GeCl}_{4}\) by treatment with \(\mathrm{Cl}_{2}\) and then purified by distillation; \(\mathrm{GeCl}_{4}\) is then hydrolyzed in water to \(\mathrm{GeO}_{2}\) 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 \(\mathrm{GeO}_{2}\).

Write a balanced chemical reaction for the condensation reaction between \(\mathrm{H}_{3} \mathrm{PO}_{4}\), molecules to form $\mathrm{H}_{6} \mathrm{P}_{4} \mathrm{O}_{13}$.

Consider the elements $\mathrm{Ba}, \mathrm{Na}, \mathrm{O}, \mathrm{B}, \mathrm{P},\( and \)\mathrm{Kr}$. From this list, select the element that (a) is most electronegative, (b) has the greatest metallic character, \((\mathbf{c})\) most readily forms a positive ion, \((\mathbf{d})\) exhibits a maximum oxidation sate of +5 , (e) exists as monoatomic gas at room temperature, (f) has multiple allotropes.

Complete and balance the following equations: (a) \(\mathrm{NaH}(s)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow\) (b) \(\mathrm{Fe}(s)+\mathrm{H}_{2} \mathrm{SO}_{4}(a q) \longrightarrow\) (c) \(\mathrm{H}_{2}(g)+\mathrm{Br}_{2}(g) \longrightarrow\) (d) \(\mathrm{Na}(l)+\mathrm{H}_{2}(g) \longrightarrow\) (e) \(\mathrm{PbO}(s)+\mathrm{H}_{2}(g) \longrightarrow\)

Write a balanced equation for each of the following reactions: (a) hydrolysis of \(\mathrm{PCl}_{5},(\mathbf{b})\) dehydration of phosphoric acid (also called orthophosphoric acid) to form pyrophosphoric acid, \((\mathbf{c})\) reaction of \(\mathrm{P}_{4} \mathrm{O}_{10}\) with water.
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