Ch.22 - Chemistry of the Nonmetals
Back
- Complete the exercises below. Write a balanced equation for each of the following reactions: a. Burning magnesium metal in a carbon dioxide atmosphere reduces the CO₂ to carbon. b. In photosynthesis, solar energy is used to produce glucose (C₆H₁₂O₆) and O₂ from carbon dioxide and water.
Problem 68
- Complete the exercises below. Write the formulas for the following compounds and indicate the oxidation state of the group 4A element or boron in each: a. boric acid, b. silicon tetrabromide, c. lead(II) chloride.
Problem 69
- Complete the exercises below. Select the member of group 4A that best fits each description: a. has the lowest first ionization energy, b. is found in oxidation states ranging from -4 to +4, c. is most abundant in Earth’s crust.
Problem 71
- Complete the exercises below. Select the member of group 4A that best fits each description: a. forms chains to the greatest extent, b. forms the most basic oxide, c. is a metalloid that can form an oxide.
Problem 72
- Speculate on why carbon forms carbonate rather than silicate analogs.
Problem 74
- Complete the exercises below. b. Determine the number of hydroxide ions in the chemical formula of the mineral pyrophyllite, Al₂(Si₂O₅)₂(OH)ₓ.
Problem 75
- Complete the exercises below. a. Determine the number of sodium ions in the chemical formula of albite, NaₓAlSi₃O₈ b. Determine the number of hydroxide ions in the chemical formula of tremolite, Ca₂Mg₅(Si₄O₁₁)₂(OH)ₓ.
Problem 76
- What is the significance of the statement that the hydrogen atoms in diborane are described as “hydridic”?
Problem 77
Problem 78a
Write a balanced equation for each of the following reactions:
a. Diborane reacts with water to form boric acid and molecular hydrogen.
Problem 78b
Write a balanced equation for each of the following reactions:
b. Upon heating, boric acid undergoes a condensation reaction to form tetraboric acid.
Problem 78c
Write a balanced equation for each of the following reactions:
c. Boron oxide dissolves in water to give a solution of boric acid.
- Complete the exercises below. Indicate whether each of the following statements is true or false. 2SO₂ (g) + O₂ (g) → 2SO₃ (g) is an example of a disproportionation reaction.
Problem 79
- Complete the exercises below. Write a balanced equation for the reaction of each of the following compounds with water: b. Cl₂O₇ (g).
Problem 81
- Complete the exercises below. Write a balanced equation for the reaction of the following compound with water: Na₂O₂ (s).
Problem 81
- Complete the exercises below. Write a balanced equation for the reaction of each of the following compounds with water: f. Mg₃N₂ (s).
Problem 81
- Complete the exercises below. What is the anhydride for each of the following acids: a. H₂SO₄, b. HClO₃, c. HNO₂, d. H₂CO₃, e. H₃PO₄?
Problem 82
- Complete the exercises below. Hydrogen peroxide is capable of oxidizing: a. hydrazine to N₂ and H₂O. Write a balanced net ionic equation for this redox reaction. b. SO₂ to SO₄²⁻. Write a balanced net ionic equation for this redox reaction. c. NO₂⁻ to NO₃⁻. Write a balanced net ionic equation for this redox reaction. d. H₂S (g) to S (s). Write a balanced net ionic equation for this redox reaction.
Problem 83
- Complete the exercises below. 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 H₂SO₄ consists of three main chemical processes: a. oxidation of S to SO₂, b. oxidation of SO₂ to SO₃, c. the dissolving of SO₃ in H₂SO₄ and the subsequent reaction with water to form H₂SO₄. If the third process produces 130 kJ/mol, how much heat is produced in preparing a mole of H₂SO₄ from a mole of S? How much heat is produced in preparing 5000 pounds of H₂SO₄?
Problem 84
- Complete the exercises below. a. What is the oxidation state of P in PO₄³⁻ and N in NO₃⁻? b. Why doesn't N form a stable NO₄³⁻ ion analogous to P?
Problem 85
- Complete the exercises below. Write a balanced chemical reaction for the condensation reaction between H₃PO₄ molecules to form H₅P₃O₁₀.
Problem 87
- Complete the exercises below. Ultrapure germanium, like silicon, is used in semiconductors. Germanium of “ordinary” purity is prepared by the high-temperature reduction of GeO₂ with carbon. The Ge is converted to GeCl₄ by treatment with Cl₂ and then purified by distillation; GeCl₄ is then hydrolyzed in water to GeO₂ and reduced to the elemental form with H₂. 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 GeO₂.
Problem 88
- Complete the exercises below. When aluminum replaces up to half of the silicon atoms in SiO₂, a mineral class called feldspars results. The feldspars are the most abundant rock-forming minerals, comprising about 50% of the minerals in Earth’s crust. Orthoclase is a feldspar in which Al replaces one-fourth of the Si atoms of SiO₂, and charge balance is completed by K⁺ ions. Determine the chemical formula for orthoclase.
Problem 89