Ch.22 - Chemistry of the Nonmetals
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- Complete the exercises below. The H₂/O₂ fuel cell converts elemental hydrogen and oxygen into water, producing, theoretically, 1.23 V. What is the most sustainable way to obtain hydrogen to run a large number of fuel cells? Explain.
Problem 28
- Complete the exercises below: Why does xenon form stable compounds with fluorine, whereas argon does not?
Problem 29
- Complete the exercises below. Write the chemical formula for each of the following, and indicate the oxidation state of the halogen or noble-gas atom in each: a. calcium hypobromite, b. bromic acid, c. xenon trioxide, d. perchlorate ion, e. iodous acid, f. iodine pentafluoride.
Problem 31
- Complete the exercises below. Write the chemical formula for each of the following compounds, and indicate the oxidation state of the halogen or noble-gas atom in each: a. chlorate ion, b. hydroiodic acid, c. iodine trichloride, d. sodium hypochlorite, e. perchloric acid, f. xenon tetrafluoride.
Problem 32
- Complete the exercises below. Name the following compounds and assign oxidation states to the halogens in them: a. Fe(ClO₃)₃
Problem 33
- Complete the exercises below. Name the following compounds and assign oxidation states to the halogens in them: a. KClO₃, b. Ca(IO₃)₂.
Problem 34
- Complete the exercises below. Explain each of the following observations: a. At room temperature, I₂ is a solid, Br₂ is a liquid, and Cl₂ and F₂ are both gases. b. F₂ cannot be prepared by electrolytic oxidation of aqueous F⁻ solutions. c. The halogens decrease in oxidizing power in the order F₂ > Cl₂ > Br₂ > I₂.
Problem 35
Problem 35c
Explain each of the following observations:
c. The boiling point of HF is much higher than those of the other hydrogen halides.
- Complete the exercises below. Explain the following observations: a. For a given oxidation state, the acid strength of the oxyacid in aqueous solution decreases in the order chlorine > bromine > iodine. b. Hydrofluoric acid cannot be stored in glass bottles. c. HI cannot be prepared by treating NaI with sulfuric acid. d. The interhalogen ICl₃ is known, but BrCl₃ is not.
Problem 36
Problem 37b,e
Write balanced equations for each of the following reactions.
b. When copper(II) nitrate is heated strongly, it decomposes to form copper(II) oxide, nitrogen dioxide, and oxygen.
e. Potassium peroxide reacts with CO2(g) to give potassium carbonate and O2.
- Complete the exercises below. Complete and balance the following equations: b. Al₂O₃ (s) + H⁺ (aq) →
Problem 38
- Complete the exercises below. Complete and balance the following equation: c. Na₂O₂ (s) + H₂O (l) →
Problem 38
- Complete the exercises below. Predict whether each of the following oxides is acidic, basic, amphoteric, or neutral: a. NO₂, b. CO₂, c. Al₂O₃, d. CaO.
Problem 39
- Complete the exercises below. Write the chemical formula for each of the following compounds, and indicate the oxidation state of the group 6A element in each: a. selenous acid, b. potassium hydrogen sulfite, c. hydrogen telluride, d. carbon disulfide, e. calcium sulfate, f. cadmium sulfide, g. zinc telluride.
Problem 41
- Complete the exercises below. Write the chemical formula for each of the following compounds, and indicate the oxidation state of the group 6A element in each: a. sulfur tetrachloride, b. selenium trioxide, c. sodium thiosulfate, d. hydrogen sulfide, e. sulfuric acid, f. sulfur dioxide, g. mercury telluride.
Problem 42
- Complete the exercises below. In aqueous solution, hydrogen sulfide reduces dilute HNO₃ to NO₂. In all cases, under appropriate conditions, the product is elemental sulfur. Write a balanced net ionic equation for each reaction.
Problem 43
- Complete the exercises below. An aqueous solution of SO₂ reduces a. aqueous KMnO₄ to MnSO₄ (aq) b. acidic aqueous K₂Cr₂O₇ to aqueous Cr⁵⁺, c. aqueous Hg₂(NO₃)₂ to mercury metal. Write balanced equations for these reactions.
Problem 44
- Complete the exercises below. Write the Lewis structure for each of the following species, and indicate the structure of each: a. SeO₃²⁻; b. S₂Cl₂; c. chlorosulfonic acid, HSO₃Cl (chlorine is bonded to sulfur).
Problem 45
- Complete the exercises below. The SF₅⁻ ion is formed when SF₄ (g) reacts with fluoride salts containing large cations, such as CsF(s). Draw the Lewis structures for SF₄ and SF₅⁻, and predict the molecular structure of each.
Problem 46
- Complete the exercises below. Write a balanced equation for each of the following reactions: a. Sulfur dioxide reacts with water. b. Solid zinc sulfide reacts with hydrochloric acid. c. Elemental sulfur reacts with sulfite ion to form thiosulfate. d. Sulfur trioxide is dissolved in sulfuric acid.
Problem 47
- Complete the exercises below. Write a balanced equation for each of the following reactions. a. Hydrogen selenide can be prepared by the reaction of an aqueous acid solution on aluminum selenide. b. Sodium thiosulfate is used to remove excess Cl₂ from chlorine-bleached fabrics. The thiosulfate ion forms SO₄²⁻ and elemental sulfur, while Cl₂ is reduced to Cl⁻.
Problem 48
- Complete the exercises below. Write the chemical formula for each of the following compounds, and indicate the oxidation state of nitrogen in each: a. sodium nitrite, b. ammonia, c. nitrous oxide, d. sodium cyanide, e. nitric acid, f. nitrogen dioxide, g. nitrogen, h. boron nitride.
Problem 49
- Complete the exercises below. Write the Lewis structure for each of the following species, describe its geometry, and indicate the oxidation state of the nitrogen: a. HNO₂, b. N₃⁻, c. N₂H₅⁺, d. NO₃⁻.
Problem 51
- Complete the exercises below. Write the Lewis structure for each of the following species, describe its geometry, and indicate the oxidation state of the nitrogen: a. NH₄⁺, b. NO₂⁻, c. N₂O, d. NO₂.
Problem 52
- Complete the exercises below. Complete and balance the following equations: a. Mg₃N₂ (s) + H₂O (l) → Which ones of these are redox reactions?
Problem 53
- Complete the exercises below. Write a balanced net ionic equation for each of the following reactions: a. Dilute nitric acid reacts with zinc metal with formation of nitrous oxide. b. Concentrated nitric acid reacts with sulfur with formation of nitrogen dioxide. c. Concentrated nitric acid oxidizes sulfur dioxide with formation of nitric oxide. d. Hydrazine is burned in excess fluorine gas, forming NF₃. e. Hydrazine reduces CrO₄²⁻ to Cr(OH)₄⁻ in base (hydrazine is oxidized to N₂).
Problem 54
- Complete the exercises below. Write complete balanced half-reactions for: a. oxidation of nitrous acid to nitrate ion in acidic solution, b. oxidation of N₂ to N₂O in acidic solution.
Problem 55
- Complete the exercises below. Write complete balanced half-reactions for: a. reduction of nitrate ion to NO in acidic solution, b. oxidation of HNO₂ to NO₂ in acidic solution.
Problem 56
- Complete the exercises below. Write a molecular formula for each compound, and indicate the oxidation state of the group 5A element in each formula: a. phosphorous acid, b. pyrophosphoric acid, c. antimony trichloride, d. magnesium arsenide, e. diphosphorus pentoxide, f. sodium phosphate.
Problem 57
- Complete the exercises below. Write a chemical formula for each compound or ion, and indicate the oxidation state of the group 5A element in each formula: a. phosphate ion, b. arsenous acid, c. antimony(III) sulfide.
Problem 58