Ch.22 - Chemistry of the Nonmetals
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Problem 8
Which property of the third-row nonmetallic elements might be the one depicted below:
a. first ionization energy,
b. atomic radius,
c. electronegativity,
d. melting point,
e. X―X single-bond enthalpy? [Find more in Sections 22.3, 22.4, 22.6, 22.8, and 22.10]
- Complete the exercises below. Identify each of the following elements as a metal, nonmetal, or metalloid: a. phosphorus, b. strontium, c. manganese, d. selenium, e. sodium, f. krypton.
Problem 11
- Complete the exercises below. Identify each of the following elements as a metal, nonmetal, or metalloid: a. gallium, b. molybdenum, c. tellurium, d. arsenic, e. xenon, f. ruthenium.
Problem 12
- Complete the exercises below. Consider the elements O, Ba, Co, Be, Br, and Se. From this list, select the element that: a. is most electronegative, b. exhibits a maximum oxidation state of +7, c. loses an electron most readily, d. forms π bonds most readily, e. is a transition metal, f. is a liquid at room temperature and pressure.
Problem 13
- Complete the exercises below. Consider the elements Li, K, Cl, C, Ne, and Ar. From this list, select the element that a. is most electronegative, b. has the greatest metallic character, c. most readily forms a positive ion, d. has the smallest atomic radius, e. forms π bonds most readily, f. has multiple allotropes.
Problem 14
- Complete the exercises below. Which of the following statements are true? a. Both nitrogen and phosphorus can form a pentafluoride compound. b. Although CO is a well-known compound, SiO does not exist under ordinary conditions. c. Cl₂ is easier to oxidize than I₂. d. At room temperature, the stable form of oxygen is O₂, whereas that of sulfur is S₈.
Problem 15
- Complete the exercises below. Which of the following statements are true? a. Si can form an ion with six fluorine atoms, SiF₆²⁻, whereas carbon cannot. b. Si can form three stable compounds containing two Si atoms each, Si₂H₂, Si₂H₄, and Si₂H₆. c. In HNO₃ and H₃PO₄, the central atoms, N and P, have different oxidation states. d. S is more electronegative than Se.
Problem 16
- Complete the exercises below. Complete and balance the following equations: a. NaOCH₃ (s) + H₂O (l) →
Problem 17
- Complete the exercises below. Complete and balance the following equation: a. Mg₃N₂ (s) + H₂O (l) →
Problem 18
- Complete the exercises below. a. Give the names and chemical symbols for the three isotopes of hydrogen. b. List the isotopes in order of decreasing natural abundance. c. Which hydrogen isotope is radioactive? d. Write the nuclear equation for the radioactive decay of this isotope.
Problem 19
- Complete the exercises below. Complete and balance the following equation: b. Fe (s) + H₂SO₄ (aq) →
Problem 23
- Complete the exercises below. Write balanced equations for each of the following reactions: a. Aluminum metal reacts with acids to form hydrogen gas. b. Steam reacts with magnesium metal to give magnesium oxide and hydrogen. c. Manganese(IV) oxide is reduced to manganese(II) oxide by hydrogen gas. d. Calcium hydride reacts with water to generate hydrogen gas.
Problem 24
- Complete the exercises below. Identify the following hydrides as ionic, metallic, or molecular: a. BaH₂, b. H₂Te, c. TiH₁.₇.
Problem 25
- Complete the exercises below. Identify the following hydrides as ionic, metallic, or molecular: a. B₂H₆, b. RbH, c. Th₄H₁.₅.
Problem 26
- 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
Problem 35c
Explain each of the following observations:
c. The boiling point of HF is much higher than those of the other hydrogen halides.
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. 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