The Main Group Elements 987 Test Bank Chapter 20 - Chemistry Canada 4e | Complete Test Bank by John A. Olmsted. DOCX document preview.
CHAPTER 20
THE MAIN GROUP ELEMENTS
CHAPTER STUDY OBJECTIVES
1. Explain the chemistry of formation of adducts.
SKILLS TO MASTER: Identifying the Lewis acid and base in a reaction; drawing the Lewis structure of an adduct
KEY CONCEPTS: Any chemical species that acts as an electron-pair donor is a Lewis base. Any chemical species that acts as an electron-pair acceptor is a Lewis acid. An adduct is formed by the combination of a Lewis base with a Lewis acid.
2. Apply the concepts of hardness and softness to reactions.
SKILLS TO MASTER: Writing metathesis reactions
KEY CONCEPTS: A hard Lewis base has electron pairs of low polarizability. A soft Lewis base has a large donor atom of high polarizability and low electronegativity. A hard Lewis acid has an acceptor atom with low polarizability. A soft Lewis acid has relatively high polarizability. Hard Lewis acids tend to combine with hard Lewis bases. Soft Lewis acids tend to combine with soft Lewis bases.
3. Explain the production, reactions, and uses of the main group metals.
SKILLS TO MASTER: Explaining the Hall–Héroult process for making aluminum metal
4. Explain the production, reactions, and uses of the metalloids.
SKILLS TO MASTER: Explaining the bonding in boron compounds
5. Explain the production, reactions, and uses of phosphorus.
SKILLS TO MASTER: Describing the bonding in red and white phosphorus; explaining the processes for making phosphoric acid and phosphorus fertilizers; explaining phosphate condensation reactions
6. Explain the production, reactions, and uses of the other non-metals.
SKILLS TO MASTER: Describing the various allotropes of carbon; explaining the electrolytic chlor–alkali process; explaining the electrolytic production of fluorine gas
Multiple Choice QUESTIONS
1. In the reaction of trimethyl amine with trimethyl boron,
a) the product is [N(CH3)4+][B(CH3)2-].
b) trimethyl boron is the Lewis base.
c) the product is (CH3)3N–B(CH3)3.
d) trimethyl amine is the Lewis acid.
e) no reaction occurs.
Difficulty: Medium
Learning Objective: Explain the chemistry of formation of adducts.
Section Reference: 20.1 Lewis Acids and Bases
2. Which of the following are Lewis acids?
I. | II. | III. | IV. | V. |
Cl- | SO3 | CH4 | SnCl2 | Fe2+ |
a) I, II, and III
b) II, III, and IV
c) II, IV, and V
d) II and III
e) IV and V
Difficulty: Medium
Learning Objective: Explain the chemistry of formation of adducts.
Section Reference: 20.1 Lewis Acids and Bases
3. Which of the following are Lewis bases?
I. | II. | III. | IV. | V. |
Cl- | SO3 | NH3 | PCl5 | Cr2O3 |
a) I, II, and III
b) I, III, and V
c) II, IV, and V
d) I and III
e) II and IV
Difficulty: Medium
Learning Objective: Explain the chemistry of formation of adducts.
Section Reference: 20.1 Lewis Acids and Bases
4. What reactants likely lead to formation of the Lewis acid–base adduct shown below?
a) Pd2+ and Cl2
b) Pd and Cl-
c) Pd and SnCl4
d) Pd2+ and Cl-
e) PdCl2 and Sn
Difficulty: Medium
Learning Objective: Explain the chemistry of formation of adducts.
Section Reference: 20.1 Lewis Acids and Bases
5. Which statements are true about the following reaction?
PF5 + HF 🡪 H+ + PF6-
I) HF is a Brønsted acid and a Lewis acid.
II) PF5 is the Lewis acid.
III) The F- ion is the Lewis base.
IV) The orbital used in bonding is a dsp3 hybrid orbital.
V) PF6-is a Lewis acid.
a) I and V
b) II and III
c) I, III and IV
d) III and V
e) I and III
Difficulty: Hard
Learning Objective: Explain the chemistry of formation of adducts.
Section Reference: 20.1 Lewis Acids and Bases
6. Identify the Lewis acid and base in the reaction of trimethyl amine with trimethyl boron.
a) Base: trimethyl amine; acid trimethyl boron
b) Base: trimethyl boron; acid trimethyl amine
c) Neither acts as an acid nor a base.
Difficulty: Medium
Learning Objective: Explain the chemistry of formation of adducts.
Section Reference: 20.1 Lewis Acids and Bases
Feedback: Must first translate the names of compounds into structures and then apply concepts of Lewis acids and bases.
7. Which of the following groups of Lewis acids is in order of increasing hardness?
a) Cd2+, Zn2+, Ag+
b) Ag+, Zn2+ Cd2+
c) Ag+, Cd2+, Zn2+
d) Cd2+, Ag+, Zn2+
e) Zn2+, Ag+, Cd2+
Difficulty: Medium
Learning Objective: Apply the concepts of hardness and softness to reactions.
Section Reference: 20.2 Hard and Soft Lewis Acids and Bases
8. Which of the following groups of Lewis bases is in order of decreasing hardness?
a) N(CH3)3, NH3, P(CH3)3
b) NH3, P(CH3)3, N(CH3)3
c) P(CH3)3, N(CH3)3, NH3
d) NH3, N(CH3)3, P(CH3)3
e) N(CH3)3, P(CH3)3, NH3
Difficulty: Medium
Learning Objective: Apply the concepts of hardness and softness to reactions.
Section Reference: 20.2 Hard and Soft Lewis Acids and Bases
9. The reactions of Group 13 chlorides (BCl3, AlCl3, GaCl3, InCl3) with bases are predicted well by the HSAB principle. Which of the following is the predicted order of reactivity (completeness of adduct formation) of these compounds toward P(CH2CH3)3?
a) AlCl3 < InCl3 < BCl3 < GaCl3
b) BCl3< GaCl3 < AlCl3 < InCl3
c) BCl3 < AlCl3 < GaCl3 < InCl3
d) AlCl3 < BCl3 < GaCl3 < InCl3
e) InCl3 < GaCl3 < AlCl3 < BCl3
Difficulty: Medium
Learning Objective: Apply the concepts of hardness and softness to reactions.
Section Reference: 20.2 Hard and Soft Lewis Acids and Bases
10. Identify the following as Lewis acids or bases and rank from hardest to softest: Al3+, Tl3+, Tl+.
a) bases Al3+, Tl3+, Tl+
b) acids Al3+, Tl3+, Tl+
c) acids Tl+, Tl3+, Al3+
d) bases Tl+, Tl3+, Al3+
e) acids Al3+, Tl+, Tl3+
Difficulty: Medium
Learning Objective: Apply the concepts of hardness and softness to reactions.
Section Reference: 20.2 Hard and Soft Lewis Acids and Bases
Feedback: Metal cations act as Lewis acids, with hardest species being small and highly charged.
11. Identify the following as Lewis acids or bases and rank from hardest to softest: SbH3, PH3, PF3.
a) bases SbH3, PH3, PF3
b) acids PF3, PH3, SbH3
c) acids SbH3, PH3, PF3
d) bases PF3, PH3, SbH3
e) acids PH3, PF3, SbH3
Difficulty: Medium
Learning Objective: Apply the concepts of hardness and softness to reactions.
Section Reference: 20.2 Hard and Soft Lewis Acids and Bases
Feedback: All are Lewis bases, electron-pair donors with polarizability increasing with increased softness.
12. The substances below are main group compounds that follow the hard-soft acid–base principles quite reliably:
I. Al(CH3)3
II. MgCl2
III. AlCl3
IV. LiCl
V. LiCH3
VI. Mg(CH3)2
Referring to these compounds, which of the (unbalanced) equations below is expected to proceed?
a) Al(CH3)3 + MgCl2 🡪 AlCl3 + Mg(CH3)2
b) LiCl + Al(CH3)3🡪 LiCH3 + AlCl3
c) LiCH3 + MgCl2 🡪 LiCl + Mg(CH3)2
d) Mg(CH3)2 + LiCl 🡪 LiCH3 + MgCl2
Difficulty: Medium
Learning Objective: Apply the concepts of hardness and softness to reactions.
Section Reference: 20.2 Hard and Soft Lewis Acids and Bases
13. Potassium is found in nature most often as a chloride salt, whereas copper and mercury more often occur as the sulphides. The best explanation for this observation is
a) potassium is softer than copper or mercury.
b) the coinage metals are smaller than potassium.
c) the coinage metals prefer the +2 oxidation state.
d) potassium is less electronegative than copper.
e) the coinage metal ions are softer than potassium.
Difficulty: Medium
Learning Objective: Apply the concepts of hardness and softness to reactions.
Section Reference: 20.2 Hard and Soft Lewis Acids and Bases
14. Are the chlorides of Pb, Pb(II) chloride and Pb(IV) chloride solids, liquids, or gases at room temperature?
a) PbCl2: solid; PbCl4: solid
b) PbCl2: liquid; PbCl4: liquid
c) PbCl2: solid; PbCl4: liquid
d) PbCl2: liquid; PbCl4: solid
e) PbCl2: gas; PbCl4: liquid
Difficulty: Medium
Learning Objective: Explain the production, reactions, and uses of the main group metals.
Section Reference: 20.3 The Main Group Metals
Feedback: Typically one expects metal halide compounds to be ionic and solid at room temperature. Owing to the high charge density of Pb4+ species, PbCl4 is not an ionic compound, and therefore, is a liquid at room temperature.
15. What reasons are important for the use of Na3AlF6 in the production of aluminum?
I. The use of Na3AlF6 allows for electrolysis at lower temperature.
II. The fluoride will react with the electrodes.
III. The oxide ions combine with the fluoride ions.
IV. The fluoride is not readily oxidized.
V. The aluminum is more easily oxidized when bound to fluoride.
a) II and III
b) IV and V
c) I and V
d) I and IV
e) I, III, and V
Difficulty: Easy
Learning Objective: Explain the production, reactions, and uses of the main group metals.
Section Reference: 20.3 The Main Group Metals
16. Why are heavy metals such as lead(II) and cadmium(II) toxic?
a) They can replace oxygen atoms in proteins.
b) They can bind to sulphur atoms on proteins.
c) They are hard Lewis acids.
d) They are insoluble in aqueous solution and will precipitate.
e) They form ionic compounds.
Difficulty: Easy
Learning Objective: Explain the production, reactions, and uses of the main group metals.
Section Reference: 20.3 The Main Group Metals
17. Which of the following ionic species result when boric acid, H3BO3, is added to water:
H3O+, H2BO3-, HBO32-, BO33-, B(OH)4-, OH-?
a) H3O+, H2BO3-,
b) H3O+, H2BO3-, HBO32-
c) H3O+, H2BO3-, HBO32-, BO33
d) H3O+, B(OH)4-
e) H3O+, OH-
Difficulty: Medium
Learning Objective: Explain the production, reactions, and uses of the metalloids.
Section Reference: 20.4 The Metalloids
18. Which of the following boron halides has the most -bonding?
a) BI3
b) BBr3
c) BCl3
d) BF3
e) BF4-
Difficulty: Medium
Learning Objective: Explain the production, reactions, and uses of the metalloids.
Section Reference: 20.4 The Metalloids
19. What is the product of the reaction of silicon-copper alloy with chlorobutane?
a) 
b) 
c) 
d) 
e) Cu metal
Difficulty: Hard
Learning Objective: Explain the production, reactions, and uses of the metalloids.
Section Reference: 20.4 The Metalloids
20. Why is SiO2 a solid and CO2 a gas?
a) A Si atom is heavier than a C carbon.
b) Si has more electrons than C.
c) Intermolecular forces between SiO2 molecules are stronger than those between CO2 molecules.
d) It is preferable to form 4 Si – O single bonds rather than 2 Si – O double bonds.
e) SiO2 forms ionic bonds.
Difficulty: Hard
Learning Objective: Explain the production, reactions, and uses of the metalloids.
Section Reference: 20.4 The Metalloids
Feedback: a) this is true, but not the reason CO2 is a gas; b) is also true, but not the reason CO2 is a gas; c) SiO2 is a solid structure due to network covalent bonding and not as a result of strong intermolecular forces acting between discrete SiO2 molecules; d) correct answer – as a result each Si is bonded to 4 oxygen atoms and each O is bonded to 2 Si atoms; e) incorrect.
21. Silicon tetrachloride has Lewis acidic characteristics, whereas carbon tetrachloride does NOT. What orbital is used by SiCl4 in forming adducts that gives SiCl4 this property?
a) sp2
b) sp3
c) sp2d
d) sp3d
e) sp3d2
Difficulty: Medium
Learning Objective: Explain the production, reactions, and uses of the metalloids.
Section Reference: 20.4 The Metalloids
22. Arsenic oxide (As2O3) is used as a standard in oxidation-reduction titrations because it is stable and reacts very predictably. Reaction with MnO4- in acidic solution gives aqueous arsenic (H3AsO4) and Mn2+. If the coefficient of MnO4-is 4 in the balanced chemical equation of reaction, the coefficient of H3AsO4 is
a) 2.
b) 4.
c) 5.
d) 8.
e) 10.
Difficulty: Medium
Learning Objective: Explain the production, reactions, and uses of the metalloids.
Section Reference: 20.4 The Metalloids
23. Neutralization of 25 ml of 0.05 M H3PO4 requires what mass of solid sodium hydroxide, NaOH?
a) 0.05 g
b) 0.15 g
c) 0.02 g
d) 0.06 g
e) 2 g
Difficulty: Medium
Learning Objective: Explain the production, reactions, and uses of phosphorus.
Section Reference: 20.5 Phosphorus
Feedback: a) based on 1:1 NaOH:H3PO4; b) correct c) based on 1:1 and mass of OH-; d) based on mass of OH-; e) based on 0.05 moles of NaOH required
24. What is the oxidation state of chlorine in sodium hypochlorite?
a) 0
b) +1
c) –1
d) +2
e) –1/2
Difficulty: Easy
Learning Objective: Explain the production, reactions, and uses of the other non-metals.
Section Reference: 20.6 Other Non-Metals
Feedback: Halides are generally in oxidation state –1; in hypochlorite Cl is bound to more electronegative oxygen and has oxidation state +1.
25. Which allotrope of carbon is the most thermodynamically stable?
a) diamond
b) fullerene
c) graphite
d) coke
e) carbon nanotube
Difficulty: Easy
Learning Objective: Explain the production, reactions, and uses of the other non-metals.
Section Reference: 20.6 Other Non-Metals
26. CFCs, chlorofluorocarbons, are being phased out of use as refrigerants because
a) they highly reactive producing numerous pollutants in our atmosphere.
b) they are toxic.
c) they may remain in the atmosphere for hundreds of years, but react in the upper atmosphere.
d) they are gases and hard to contain.
e) hydrochlorfluorocarbons are cheaper and more effective refrigerants.
Difficulty: Easy
Learning Objective: Explain the production, reactions, and uses of the other non-metals.
Section Reference: 20.6 Other Non-Metals
Feedback: a) CFCs are unreactive in the lower atmosphere; b) CFCs are non-toxic – contributing to their early status as a “wonder-chemical”; c) correct answer; d) they are gases at low pressure and liquid at high pressure, this makes them good refrigerants; e) hydrochlofluorcarbons are not necessarily cheaper, but are somewhat shorter lived making them less of a hazard to the environment.
27. When SF4 acts as a Lewis base, it donates an F- ion and generates the SF3+ ion. The structure of SF3+ is
a) T-shaped.
b) trigonal planar.
c) trigonal pyramidal.
d) tetrahedral.
e) distorted trigonal bipyramidal.
Difficulty: Medium
Learning Objective: Explain the production, reactions, and uses of the other non-metals.
Section Reference: 20.6 Other Non-Metals
28. When SF4 acts as a Lewis acid, with trimethyl amine, it forms the adduct (CH3)3N-SF4. The structure of sulphur in (CH3)3N-SF4 is a(n)
a) distorted square planar.
b) tetrahedral.
c) octahedral.
d) square pyramidal.
e) trigonal bipyramidal.
Difficulty: Medium
Learning Objective: Explain the production, reactions, and uses of the other non-metals.
Section Reference: 20.6 Other Non-Metals
29. In the text, it is mentioned that sulphur compounds are poison for many catalysts. How, generally, would you expect that this is possible?
a) The sulphur coats the catalyst.
b) The sulphur reacts with the metal ions of the catalyst as a hard Lewis base.
c) The sulphur reacts with the other reactants.
d) The sulphur reacts with the metal ions of the catalyst as a soft Lewis base.
e) The sulphur changes the reaction products.
Difficulty: Medium
Learning Objective: Explain the production, reactions, and uses of the other non-metals.
Section Reference: 20.6 Other Non-Metals
30. Which polymer is fluoride found in?
a) CFC
b) Teflon
c) PVC
d) DDT
e) chlorofluorocarbons
Difficulty: Easy
Learning Objective: Explain the production, reactions, and uses of the other non-metals.
Section Reference: 20.6 Other Non-Metals
ESSAY QUESTIONS
31. Draw the three dimensional structure of BF3 and identify the orbital used for bonding in adduct formation. That is the orbital used in the pi bonding.
Difficulty: Medium
Learning Objective: Explain the chemistry of formation of adducts.
Section Reference: 20.1 Lewis Acids and Bases
32. One step in the synthesis of sulphuric acid from sulphur is the reaction of water with SO3. The first step may be the formation of a Lewis acid–base adduct between these two molecules. Draw the structure of this adduct.
Difficulty: Medium
Learning Objective: Explain the chemistry of formation of adducts.
Section Reference: 20.1 Lewis Acids and Bases
33. Ammonia is sometimes used as a solvent for reactions. Write a balanced equation showing how ammonia, NH3, can react with itself in an acid–base equilibrium.
Difficulty: Medium
Learning Objective: Explain the chemistry of formation of adducts.
Section Reference: 20.1 Lewis Acids and Bases
34. Identify the Lewis acid and base from among the reactants in each of the following, and explain briefly: (CH3)3N(g) + BF3(g) 🡨 🡪 (CH3)3NBF3(s)
Difficulty: Easy
Learning Objective: Explain the chemistry of formation of adducts.
Section Reference: 20.1 Lewis Acids and Bases
35. Write a balanced equation showing the acid–base reaction of antimony pentafluoride (SbF5) with itself.
Difficulty: Medium
Learning Objective: Explain the chemistry of formation of adducts.
Section Reference: 20.1 Lewis Acids and Bases
36. Arrange the following group of Lewis acids or bases in order of increasing hardness: Mn2+, Mn3+, Mo
Difficulty: Easy
Learning Objective: Apply the concepts of hardness and softness to reactions.
Section Reference: 20.2 Hard and Soft Lewis Acids and Bases
37. The reactions of Group 13 chlorides (BCl3, AlCl3, GaCl3, InCl3) with bases are predicted well by the HSAB principle. List them in the order of decreasing reactivity (completeness of adduct formation) of these compounds toward S(CH3)2)
Difficulty: Medium
Learning Objective: Apply the concepts of hardness and softness to reactions.
Section Reference: 20.2 Hard and Soft Lewis Acids and Bases
38. Write the equation for the reaction (if any) when methylmagnesium chloride is mixed with aluminumtrichloride.
Difficulty: Medium
Learning Objective: Apply the concepts of hardness and softness to reactions.
Section Reference: 20.2 Hard and Soft Lewis Acids and Bases
39. Would you expect to find lead as lead oxide or lead sulphide in rock formations and explain why?
Difficulty: Medium
Learning Objective: Apply the concepts of hardness and softness to reactions.
Section Reference: 20.2 Hard and Soft Lewis Acids and Bases
40. Arrange the following elements in order of hardness from softest to hardest:
Al+3, Li+, Fe+2, Fe+3, Pb+2
Difficulty: Hard
Learning Objective: Apply the concepts of hardness and softness to reactions.
Section Reference: 20.2 Hard and Soft Lewis Acids and Bases
41. Based on HSAB theory predict which of the following would be more stable and explain: Fe(CO)5 or Fe(NH3)5
Difficulty: Medium
Learning Objective: Apply the concepts of hardness and softness to reactions.
Section Reference: 20.2 Hard and Soft Lewis Acids and Bases
Feedback: Difficulty in this question is recognizing Fe is (0) and then relating low oxidation state to HSAB theory.
42. Based on the HSAB principle will the following reaction take place? Explain your reasoning.
Ni(CO)4 + 4NH3 🡪 Ni(NH3)4 + 4CO
Difficulty: Medium
Learning Objective: Apply the concepts of hardness and softness to reactions.
Section Reference: 20.2 Hard and Soft Lewis Acids and Bases
43. Based on hard-soft acid–base theory, would you expect lead chloride or lead iodide to be more soluble in water and explain why?
Difficulty: Medium
Learning Objective: Apply the concepts of hardness and softness to reactions.
Section Reference: 20.2 Hard and Soft Lewis Acids and Bases
44. Some modern bicycle frames utilize both aluminum and graphite in electrical contact for the structural components. However, both of these elements are (thermodynamically) easily oxidized to aluminum oxide (∆G°f = –1582.3 kJ/mole) and CO2 (∆G°f = –394.4 kJ/mole), respectively. Which of the two elements will be protected by anodic protection? Explain your reasoning.
Difficulty: Medium
Learning Objective: Explain the production, reactions, and uses of the main group metals.
Section Reference: 20.3 The Main Group Metals
45. Draw the Lewis structure of the soluble tetrahydoxyaluminate ion.
Difficulty: Medium
Learning Objective: Explain the production, reactions, and uses of the main group metals.
Section Reference: 20.3 The Main Group Metals
46. Identify the aluminum species present as acid is gradually added to an aqueous solution containing a bauxite Al(O)OH ore sample initially at pH 14.
Difficulty: Medium
Learning Objective: Explain the production, reactions, and uses of the main group metals.
Section Reference: 20.3 The Main Group Metals
Feedback: This question highlights the amphoteric nature of aluminum species and illustrates how speciation can be pH dependent.
47. Lewis acids are important in a wide range of industrial chemistry applications. Draw the Lewis structures of BF3 and that of its adduct with Cl-, BF3Cl-. What is the hybridization at the B atom in BF3 and BF3Cl-?
Difficulty: Medium
Learning Objective: Explain the production, reactions, and uses of the main group metals.
Section Reference: 20.3 The Main Group Metals
48. Bismuth is one of the main group metals. One of the more common ores it is found as is Bi2S3. How could this ore be converted to bismuth metal?
Difficulty: Easy
Learning Objective: Explain the production, reactions, and uses of the main group metals.
Section Reference: 20.3 The Main Group Metals
49. Please explain why lead sulphide is first roasted to make lead oxide before reacting with charcoal to make elemental lead and carbon monoxide based on hard-soft acid–base theory.
Difficulty: Easy
Learning Objective: Explain the production, reactions, and uses of the main group metals.
Section Reference: 20.3 The Main Group Metals
50. One reaction for the production of lead is the reaction of lead oxide with lead sulphide, forming sulphur dioxide as a by-product. What is the reducing agent in this reaction?
Difficulty: Medium
Learning Objective: Explain the production, reactions, and uses of the main group metals.
Section Reference: 20.3 The Main Group Metals
51. Boric acid has the formula B(OH)3. What is the conjugate base of boric acid in water?
Difficulty: Hard
Learning Objective: Explain the production, reactions, and uses of the metalloids.
Section Reference: 20.4 The Metalloids
52. Boron nitride has two crystalline forms, the second of which is formed at high temperatures and pressures and has a structure similar to diamond. The more common form produced at lower pressures is colourless and is an electrical insulator. These two observations suggest what about the energy of the band gap of the more common form?
Difficulty: Easy
Learning Objective: Explain the production, reactions, and uses of the metalloids.
Section Reference: 20.4 The Metalloids
53. Silicon-based life appears attractive when looking at the periodic chart. However, one of the main functional groups required for carbon-based life as we know it is the carbonyl (C=O) group. Analyze the following reaction considering bond strengths:
A Si-O single-bond energy is about 450 kJ/mole; the bond is expected to add about 100 kJ/mole, giving a double bond strength estimated to be about 550 kJ/mole. Is the enthalpy change for the forward reaction exothermic or endothermic and which side is favoured at equilibrium according to enthalpy?
Difficulty: Medium
Learning Objective: Explain the production, reactions, and uses of the metalloids.
Section Reference: 20.4 The Metalloids
54. High purity phosphoric acid is formed from the reaction of pure white phosphorus with molecular oxygen to form P4O10. What is the standard heat of formation for this reaction, and will the reaction occur spontaneously, and what is the oxidation state of phosphorus in this molecule?
Difficulty: Medium
Learning Objective: Explain the production, reactions, and uses of phosphorus.
Section Reference: 20.5 Phosphorus
Feedback: Requires application of concepts from Chapters 3 and 12.
55. If trisodium phosphate is added to water will the resulting solution be acidic, basic, or neutral? Support your answer with appropriate chemical reactions.
Difficulty: Medium
Learning Objective: Explain the production, reactions, and uses of phosphorus.
Section Reference: 20.5 Phosphorus
56. The dephosphorylation of ATP, below, is a major biochemical energy source:
ATP + H2O 🡪 ADP + H3PO4 ∆G° = –30.6 kJ/mole
If 50% of the energy released by ATP hydrolysis is converted to work, how many g of ATP (the disodiumsalt, MM = 551.1 g/mole) must be hydrolyzed for an 80 kg cyclist to climb 1000 m in elevation (approx 784 kJ)?
Difficulty: Hard
Learning Objective: Explain the production, reactions, and uses of phosphorus.
Section Reference: 20.5 Phosphorus
57. Tributyl phosphate is used as a ligand for coordinating rare earth metal ions. Write the reaction for its formation from n-butanol and phosphoric acid.
Difficulty: Medium
Learning Objective: Explain the production, reactions, and uses of phosphorus.
Section Reference: 20.5 Phosphorus
58. Write a reaction for the formation of PCl3 with the starting materials being the elemental forms.
Difficulty: Easy
Learning Objective: Explain the production, reactions, and uses of phosphorus.
Section Reference: 20.5 Phosphorus
59. Previously, pyrophosphate was added to detergents to remove metal ions from reacting with the soap. Draw a structure showing how one pyrophosphate ion, P2O74- coordinates a Mg2+ ion.
Difficulty: Hard
Learning Objective: Explain the production, reactions, and uses of phosphorus.
Section Reference: 20.5 Phosphorus
60. If 12,000 tons of phosphoric acid are produced from fluorapatite, Ca5F(PO4)3, each year, how many kg of fluorapatite must be mined to produce this amount of phosphoric acid if the reaction proceeds in 98% yield?
Difficulty: Medium
Learning Objective: Explain the production, reactions, and uses of phosphorus.
Section Reference: 20.5 Phosphorus
61. Draw the structure of H5P3O10 that is made from the condensation reaction of three phosphoric acid molecules.
Difficulty: Medium
Learning Objective: Explain the production, reactions, and uses of phosphorus.
Section Reference: 20.5 Phosphorus
62. The active ingredient in household bleach is sodium hypochlorite, NaClO. Hypochorite is produced by the reaction of Cl2 with water in alkaline solution. Write the balanced chemical equation for this reaction where another product is chloride.
Difficulty: Hard
Learning Objective: Explain the production, reactions, and uses of the other non-metals.
Section Reference: 20.6 Other Non-Metals
63. Write the equation for the reaction between NO2 and H2SO3 to give sulphuric acid.
Difficulty: Medium
Learning Objective: Explain the production, reactions, and uses of the other non-metals.
Section Reference: 20.6 Other Non-Metals
64. Write the equation for the production of HF from calcium fluoride and sulphuric acid.
Difficulty: Medium
Learning Objective: Explain the production, reactions, and uses of the other non-metals.
Section Reference: 20.6 Other Non-Metals
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