1. Which one of the following has an enthalpy change that is equal to the lattice energy of? A) B) C) D) E)

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1 PRACTICE FINAL CHEM 162 Chapter 14: Equilibrium WILL appear on the final. However, we have recently tested on it and I ve already given you practice MC test on equilibrium. I have not included any Ch 14 practice questions Chapter 9: Bonding 1. Which one of the following has an enthalpy change that is equal to the lattice energy of? A) B) C) D) E) 2. Which of the following processes is not exothermic? A) B) C) D) E) 3. Which of the following compounds would be expected to have the lowest melting point? A) AlF3 B) RbF C) NaF D) MgF2 E) CaF2 4. What is the ground-state electron configuration of? A) B) C) D) E) 5. All of the following species are isoelectronic except A) Ar. B) Ca 2+. C) Mg 2+. D) Cl.

2 E) S A bond in which both electrons of the bond are donated by one atom is called. A) a coordinate covalent bond B) a polar covalent bond C) an ionic bond D) a double bond E) a triple bond 7. An atom of which of the following elements has the highest electronegativity? A) K B) As C) Ba D) Si E) Br 8. The Lewis structure for each of the following species except contains a triple bond. A) N3 B) N2 C) HCCH D) NO + E) O For each of the following species except, the electronic structure may be adequately described by two resonance formulas. A) O3 B) SO3 2 C) NO2 D) C6H6 E) SO2 10. Which of the following is/are true concerning formal charge? 1. The formal charge of each individual atom in a molecule or ion is an actual atomic charge that can be experimentally determined. 2. The formal charge of each individual atom is always the same for each possible resonance form. 3. The sum of the formal charges of each atom in a molecule or ion equal the overall charge of the molecule or ion. A) 1 only B) 2 only C) 3 only D) 1 and 2 E) none Ch 10: VSEPR

3 11. Which molecule or ion has the same molecular geometry for its central atom as the carbonate ion? A) H2CO B) AsCl3 C) PF3 D) CH3 E) BrO3 12. The approximate CCO angle in acetone,, is A) 180. B) 90. C) 109. D) 60. E) What is the molecular geometry around carbon atom C1? A) tetrahedral B) trigonal planar C) linear D) trigonal pyramidal E) bent 14. Which of the following molecules has a permanent dipole moment? A) SF6 B) CCl4 C) NF3 D) SiCl4 E) BF3 15. What hybrid orbitals of sulfur are involved in the bonding in sulfur trioxide? A) sp 2 B) sp 2 d C) sp 3 D) sp 3 d 2 E) sp 16. Which of the following statements is true? A) A bond is twice as strong as a single bond. B) A bond results from the sideways overlap of hybridized orbitals. C) A double bond consists of a bond and a bond.

4 D) A bond has cylindrical symmetry about the bonding axis. E) A bond is twice as strong as a bond. 17. According to valence-bond theory, the bonding in ketene, H2CCO, is best described as A) five bonds. B) three bonds and two bonds. C) four bonds and two bonds. D) four bonds and one bond. E) five bonds. Chapter 11: Solids, Liquids and Gases 18. Which of the following processes is endothermic? A) melting of ice B) condensation of water C) deposition of carbon dioxide D) freezing of water E) condensation of ammonia 19. Enough of a volatile liquid is placed in a closed container to achieve a liquid-vapor equilibrium at a fixed temperature. Which of the following statements regarding this system is/are correct once equilibrium is established? 1. Liquid molecules are no longer evaporating. 2. The number of vapor molecules remains essentially constant. 3. The partial pressure exerted by the vapor molecules is called the vapor pressure of the liquid. A) 1 only B) 2 only C) 3 only D) 1 and 2 E) 2 and Choose the correct statement about the diagram below. A) The diagram shows the triple point above 1 atm pressure. B) The diagram is qualitatively correct for water. C) The diagram shows that the melting point of the solid increases with increasing pressure.

5 D) The diagram could represent the phase diagram of CO2. E) None of the above statements is correct. 21. Which of the following compounds has the highest vapor pressure at 25 C? A) CH3CH2OH B) CH3CH2CH2CH3 C) CH3OCH3 D) CH3CH2CH3 E) CH3CH2CH2Cl 22. Why does hydrogen fluoride have an unusually high normal boiling point compared to the other hydrogen halides? A) The H-F bond in hydrogen fluoride is very strong. B) Hydrogen fluoride has very strong London dispersion forces. C) Hydrogen fluoride is capable of forming hydrogen bonds. D) Hydrogen fluoride is ionic. E) Hydrogen fluoride is covalent. 23. Which of the following concerning intermolecular forces is/are correct? 1. Intermolecular forces depend in part on the shape of a molecule. 2. London forces contribute to the net forces of attraction found in all molecular solids and liquids. 3. Hydrogen bonding is a special category of dipole-dipole attractions. A) 1 only B) 2 only C) 3 only D) 1 and 2 E) 1, 2, and Which pure substance exhibits hydrogen bonding? A) HNF2 B) B2H6 C) HBr D) H2S E) CaH2 25. A solid has a very high melting point, is hard, and in the molten state is a non-conductor. The solid is most likely A) a covalent network solid. B) a metallic solid. C) an amorphous solid. D) a molecular solid. E) an ionic solid. 26. The unit cell in a certain lattice consists of a cube formed by an anion at each corner, an anion in the center, and a cation at the center of each face. The unit cell contains a net: A) 2 anions and 3 cations.

6 B) 2 anions and 2 cations. C) 5 anions and 3 cations. D) 3 anions and 4 cations. E) 5 anions and 6 cations. 27. How many atoms are there in a body-centered cubic unit cell of vanadium? A) 4 B) 8 C) 6 D) 2 E) 1 Ch 12: Solutions 28. Which of the following gases is least soluble in water? A) CO2 B) SO3 C) NH3 D) N2 E) HCl 29. Which of the following concerning the effects of temperature and pressure on solubility is/are correct? 1. All gases become more soluble in a liquid at a fixed pressure when the temperature of the liquid is increased. 2. The dissolution of an ionic compound in water may be exothermic or endothermic, depending on the initial temperature of the solution. 3. The solubility of a liquid in water generally is significantly effected by pressure changes of the system. A) 1 only B) 2 only C) 3 only D) 1 and 2 E) none 30. A concentrated perchloric acid solution has a density of 1.67 g/ml at 25 C and is 11.7 M. What is the percent by mass of HClO4 in the solution? A) 70.4% HClO4 by mass B) 0.702% HClO4 by mass C) 1.42% HClO4 by mass D) 0.699% HClO4 by mass E) 60.2% HClO4 by mass 31. What is the molality of ethanol, C2H5OH, in an aqueous solution that is 51.0% ethanol by mass? A) 1.04 m B) m

7 C) 22.6 m D) m E) 53.4 m 32. What is the vapor pressure at 75 C of an aqueous solution prepared by the addition of 64.3 g of the nonvolatile solute urea, CO(NH2)2, to 174 g of water? The vapor pressure of pure water at 75 C is 290. mmhg. A) 133 mmhg B) 28.9 mmhg C) 167 mmhg D) 261 mmhg E) 212 mmhg 33. What is the molar mass of an aromatic hydrocarbon if 0.85 g of the compound depresses the freezing point of 128 g of benzene by 0.37 C? (Kf for benzene is 5.12 C/m.) A) 35 g/mol B) 150 g/mol C) 93 g/mol 92 D) 2100 g/mol E) 140 g/mol 34. A 2.4-g sample of a small protein having a molecular weight of 62,000 g/mol is dissolved in 59.6 ml of water at 29 C. What is the osmotic pressure of the solution? (R = L atm/(k mol)) A) 12 mmhg B) 760 mmhg C) 1.2 mmhg D) 47,000 mmhg E) mmhg 35. Which of the following solutes in aqueous solution would be expected to exhibit the smallest freezing-point lowering (assuming ideal behavior)? A) 0.1 m NaCl B) 0.2 m CH3COOH C) 0.05 m Al2(SO4)3 D) 0.1 m MgCl2 E) 0.25 m NH3 36. Which of the following solutes, dissolved in 1.0 kg of water, creates a solution that boils at the highest temperature? A) mol H3PO4 B) mol HClO4 C) mol H2SO4 D) mol HCl E) mol HF Ch 13: Kinetics

8 37. In the reaction 2H2O2(aq) 2H2O(l) + O2(g), the initial concentration of H2O2 is M and, 21.2 seconds later, the concentration of H2O2 is M. What is the average rate of reaction over this time interval? A) M/s B) M/s C) M/s D) M/s E) M/s 38. The reaction 2H2(g) + 2NO(g) 2H2O(g) + N2(g) is first-order in H2 and second-order in NO at a particular temperature. What is the rate law? A) Rate = k[h2] 2 [NO] 2 B) Rate = k[h2][no] 2 C) Rate = k[h2][no] D) Rate = k[h2o] 2 [N2] E) Rate = k[h2] 2 [NO] 39. Nitrosyl chloride is produced from the reaction of nitrogen monoxide and chlorine: 2NO(g) + Cl2(g) 2NOCl(g) The following initial rates at a given temperature were obtained for the concentrations listed below. Experiment Initial Rate (mol L 1 h 1 ) [NO]0 (mol L 1 ) [Cl2]0 (mol L 1 ) From the data, what is the experimental rate law? A) Rate = k[cl2] B) Rate = k[no] C) Rate = k[no][cl2] 2 D) Rate = k[no] 2 [Cl2] E) Rate = k[no][cl2] 1/2 40. A chemical reaction that is first-order in X is observed to have a rate constant of s 1. If the initial concentration of X is 1.0 M, what is the concentration of X after 186 s? A) 0.20 M B) M C) 64 M D) 0.59 M E) 0.98 M 41. For a certain reaction of the general form aa products, the experimental data plotted as 1/[A] versus time is linear. The slope of this plot must equal A) 1. B) the rate constant.

9 C) one over the rate constant. D) the negative of the rate constant. E) For the hypothetical reaction aa products, the concentration of A was monitored with time. Given the following graph of the experimental data, what is the rate constant for the loss of reactant A? A) 2.42 min B) min C) min D) -400 min E) 24.2 min 43. For the following reaction producing 1 mol of oxygen gas at a particular temperature, H = 200 kj. NO(g) + O3(g) NO2(g) + O2(g) The activation energy is 11 kj/mol. What is the activation energy for the reverse reaction? A) 11 kj/mol B) 200 kj/mol C) 222 kj/mol D) 188 kj/mol E) 211 kj/mol 44. The Arrhenius equation, expresses the dependence of the rate constant on the reaction temperature. The slope of a plot of ln(k) versus 1/T is equal to A) B) C) D) E) 45. A suggested mechanism for the decomposition of ozone is as follows:

10 O3 O2 + O fast equilibrium O + O3 2O2 slow step What is the rate law predicted by this mechanism? A) Rate = B) Rate = k2[o] [O3] C) Rate = D) Rate = E) Rate = Special topics: Organic and Complex Ions 46. What is the coordination number of cobalt in [Co(en)2Cl2]Br? (ALSO be able to give oxidation number, cordination number, identity of ligands, and identiy of counter ions) en = A) 6 B) 3 C) 4 D) 5 E) Which of the following liquids could best act as a bidentate ligand for a metal ion? A) NH2Cl B) NH3 C) ClCH2CH2NH2 D) N2H5 + E) H2NCH2CH2NH2 48. What is the molecular formula of a cyclic alkane with 6 carbon atoms? A) C6 H14 B) C6 H10 C) C6 H16 D) C6 H12 E) C6 H6

11 49. What category of hydrocarbons contains a carbon carbon triple bond? A) alkane B) aromatic C) alkyne D) alkene E) cycloalkane 50. What is the IUPAC name for the following structural formula? A) 1,1-dimethyl-2-ethylpropane B) isoheptane C) 2-ethyl-3-methylbutane D) 2-methyl-3-ethylbutane E) 2,3-dimethylpentane 51. The functional group is characteristic of A) aldehydes. B) esters. C) ketones. D) alcohols. E) acids.

12 PRACTICE FINAL CHEM 162 Answer Section 1. ANS: E PTS: 1 DIF: easy REF: 9.1 OBJ: Define lattice energy. TOP: bonding ionic bonding KEY: Born-Haber cycle 2. ANS: E PTS: 1 DIF: moderate REF: 9.1 OBJ: Describe the Born-Haber cycle to obtain a lattice energy from thermodynamic data. TOP: bonding ionic bonding KEY: Born-Haber cycle 3. ANS: B PTS: 1 DIF: easy REF: 9.1 OBJ: Describe some general properties of ionic substances. TOP: bonding ionic bonding KEY: properties of ionic substance 4. ANS: C PTS: 1 DIF: easy REF: 9.2 OBJ: Write electron configurations of transition-metal ions. (Example 9.3) TOP: bonding ionic bonding KEY: electron configurations of ions transition-metal ions 5. ANS: C PTS: 1 DIF: easy REF: 9.3 OBJ: Define isoelectronic ions. TOP: bonding ionic bonding KEY: ionic radii 6. ANS: A PTS: 1 DIF: moderate REF: 9.4 OBJ: Define coordinate covalent bond. 7. ANS: E PTS: 1 DIF: easy REF: 9.5 OBJ: State the general periodic trends in the electronegativity. TOP: bonding covalent bonding KEY: electronegativity 8. ANS: A PTS: 1 DIF: easy REF: 9.6 OBJ: Write Lewis formulas having including multiple bonds. (Example 9.7) TOP: bonding covalent bonding KEY: multiple bonds 9. ANS: B PTS: 1 DIF: easy REF: 9.7 OBJ: Write resonance formulas. (Example 9.9) TOP: bonding covalent bonding KEY: resonance delocalization 10. ANS: C PTS: 1 DIF: easy REF: 9.9 OBJ: State the rules for obtaining formal charge. TOP: bonding covalent bonding 11. ANS: A PTS: 1 DIF: moderate REF: 10.1 OBJ: Predict the molecular geometry (two, three, or four electron pairs). (Example 10.1) TOP: bonding molecular geometry KEY: the valence-shell electron-pair repulsion model trigonal planar arrangement 12. ANS: E PTS: 1 DIF: easy REF: 10.1 OBJ: Predict the molecular geometry (two, three, or four electron pairs). (Example 10.1) TOP: bonding molecular geometry KEY: bond angle

13 13. ANS: B PTS: 1 DIF: moderate REF: 10.1 OBJ: Predict the molecular geometry in a molecule. TOP: bonding molecular geometry 14. ANS: C PTS: 1 DIF: easy REF: 10.2 OBJ: Explain the relationship between dipole moment and molecular geometry. (Example 10.3) TOP: bonding molecular geometry KEY: dipole moment 15. ANS: A PTS: 1 DIF: moderate REF: 10.3 OBJ: Apply valence bond theory (two, three, or four electron pairs). (Example 10.4) TOP: bonding bonding theories KEY: hybridization 16. ANS: C PTS: 1 DIF: moderate REF: 10.4 OBJ: Define pi bond. TOP: bonding bonding theories KEY: multiple bonding 17. ANS: C PTS: 1 DIF: moderate REF: 10.4 OBJ: Apply valence bond theory (multiple bonding). (Example 10.6) TOP: bonding bonding theories KEY: multiple bonding 18. ANS: A PTS: 1 DIF: moderate REF: 11.2 OBJ: Define melting, freezing, vaporization, sublimation, and condensation. TOP: phases phase transitions 19. ANS: E PTS: 1 DIF: moderate REF: 11.2 OBJ: Define vapor pressure. TOP: phases phase transitions 20. ANS: C PTS: 1 DIF: moderate REF: 11.3 OBJ: Define phase diagram. TOP: phases phase transitions KEY: phase diagram 21. ANS: D PTS: 1 DIF: easy REF: 11.5 OBJ: Relate the properties of liquids to the intermolecular forces involved. TOP: phases liquid KEY: intermolecular forces 22. ANS: C PTS: 1 DIF: easy REF: 11.5 OBJ: Relate the properties of liquids to the intermolecular forces involved. TOP: phases liquid KEY: intermolecular forces hydrogen bonding 23. ANS: E PTS: 1 DIF: moderate REF: 11.5 OBJ: Relate the properties of liquids to the intermolecular forces involved. TOP: phases liquid 24. ANS: A PTS: 1 DIF: easy REF: 11.5 OBJ: Define hydrogen bonding. TOP: phases liquid KEY: intermolecular forces hydrogen bonding 25. ANS: A PTS: 1 DIF: easy REF: 11.6 OBJ: Define molecular solid, metallic solid, ionic solid, and covalent network solid. TOP: phases solid 26. ANS: A PTS: 1 DIF: easy REF: 11.7 OBJ: Determine the number of atoms in a unit cell. (Example 11.9)

14 TOP: phases solid KEY: crystalline solids cubic unit cell 27. ANS: D PTS: 1 DIF: easy REF: 11.7 OBJ: Determine the number of atoms in a unit cell. (Example 11.9) TOP: phases solid KEY: structures of crystalline solids metallic solid 28. ANS: D PTS: 1 DIF: easy REF: 12.2 OBJ: Determine when a molecular solution will form when substances are mixed. TOP: solutions solution formation KEY: solubility molecular solution 29. ANS: E PTS: 1 DIF: easy REF: 12.3 OBJ: State the general trends of the solubility of gases and solids with temperature. TOP: solutions solution formation 30. ANS: A PTS: 1 DIF: easy REF: 12.4 OBJ: Calculate mass percentage of solute. (Example 12.2) TOP: solutions colligative properties 31. ANS: C PTS: 1 DIF: moderate REF: 12.4 OBJ: Calculate the molality of solute. (Example 12.3) TOP: solutions colligative properties KEY: expressing concentration conversion of concentration units 32. ANS: D PTS: 1 DIF: easy REF: 12.5 OBJ: Calculate vapor-pressure lowering. (Example 12.9) TOP: solutions colligative properties KEY: vapor pressure of a solution vapor pressure lowering 33. ANS: C PTS: 1 DIF: moderate REF: 12.6 OBJ: Calculate the molecular mass from freezing-point depression. (Example 12.12) TOP: solutions colligative properties KEY: freezing point depression 34. ANS: A PTS: 1 DIF: easy REF: 12.7 OBJ: Calculate osmotic pressure. (Example 12.13) TOP: solutions colligative properties KEY: osmotic pressure colligative properties 35. ANS: A PTS: 1 DIF: easy to moderate REF: 12.8 OBJ: Determine the colligative properties of ionic solutions. (Example 12.14) TOP: solutions colligative properties 36. ANS: C PTS: 1 DIF: moderate REF: 12.8 OBJ: Determine the colligative properties of ionic solutions. (Example 12.14) TOP: solutions colligative properties KEY: freezing point depression 37. ANS: D PTS: 1 DIF: easy REF: 13.1 OBJ: Calculate average reaction rate. (Example 13.2) TOP: rates of reaction reaction rate KEY: change of concentration with time

15 38. ANS: B PTS: 1 DIF: easy REF: 13.3 OBJ: Determine the order of reaction from the rate law. (Example 13.3) TOP: rates of reaction reaction rate KEY: dependence of rate on concentration reaction order 39. ANS: D PTS: 1 DIF: easy REF: 13.3 OBJ: Determine the rate law from initial rates. (Example 13.4) TOP: rates of reaction reaction rate KEY: dependence of rate on concentration determining the rate law 40. ANS: B PTS: 1 DIF: easy REF: 13.4 OBJ: Use an integrated rate law. (Example 13.5) TOP: rates of reaction reaction rate KEY: integrated rate laws first-order reaction 41. ANS: B PTS: 1 DIF: easy REF: 13.4 OBJ: Plot kinetic data to determine the order of a reaction. TOP: rates of reaction reaction rate 42. ANS: A PTS: 1 DIF: moderate REF: 13.4 OBJ: Plot kinetic data to determine the order of a reaction. TOP: rates of reaction reaction rate 43. ANS: E PTS: 1 DIF: moderate REF: 13.5 OBJ: Describe and interpret potential-energy curves for endothermic and exothermic reactions. TOP: rates of reaction reaction rate KEY: collision theory activation energy 44. ANS: E PTS: 1 DIF: easy REF: 13.6 OBJ: Use the Arrhenius equation. (Example 13.7) TOP: rates of reaction reaction rate 45. ANS: C PTS: 1 DIF: moderate REF: 13.8 OBJ: Determine the rate law from a mechanism with an initial fast, equilibrium step. (Example 13.12) TOP: rates of reaction reaction mechanism KEY: the rate law and the mechanism 46. ANS: A PTS: 1 DIF: moderate REF: 22.3 OBJ: Define complex ion, complex (coordination compound), ligand, and coordination number. TOP: transition elements complex ions and coordination compounds NOT: oxidation # is +3, coordination # is 6 (en is a bidentate ligand), ligands are en and Cl (the two inside the brackets), counter ion is Br 47. ANS: E PTS: 1 DIF: easy REF: 22.3 OBJ: Give examples of a monodentate ligand, bidentate ligand, and polydentate ligand. TOP: transition elements complex ions and coordination compounds KEY: structure of complex ligand 48. ANS: D PTS: 1 DIF: easy REF: 23.2 OBJ: Know the general formula of cyclic cycloalkanes. TOP: cycloalkane structural characteristic chemistry 49. ANS: C PTS: 1 DIF: easy REF: 23.3 OBJ: Know the general formula of alkynes. TOP: alkyne structural characteristic MSC: organic chemistry MSC: organic

16 50. ANS: E PTS: 1 DIF: moderate REF: 23.5 OBJ: Write the IUPAC name of an alkane given the structural formula. (Example 23.4) TOP: alkane nomenclature KEY: IUPAC nomenclature MSC: organic chemistry 51. ANS: C PTS: 1 DIF: easy REF: 23.6 OBJ: Recognize aldehydes and ketones by functional group. TOP: ketone structural characteristic MSC: organic chemistry

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