Chemistry Chapter 11 States of Matter Liquids & Solids Part 1

Chem Chapter 11: States of Matter: Liquids & Solids 1. Calculate the amount of heat absorbed by 10.0 grams of ice at -15.0°C in converting it to liquid water at 50.0°C. (Sp. heat of H2O(s) = 2.09 J/g °C, Sp. heat of H2O(l) = 4.18 J/g °C, heat of fusion of H2O(s) = 333 J/g) a) 5.73 x 103 J b) 6.76 x 102 J c) 1.70 x 102 J d) 2.83 x 103 J e) 3.29 x 103 J 2. Some solids can be converted directly to the vapor phase by heating. The process is called: a) fusion b) sublimation c) vaporization d) condensation e) distillation 3. A sketch of the phase diagram (not to scale) of water is given below. Which statement is FALSE? a) Line AD is the sublimation curve - solid and vapor are in equilibrium. b) Point A is the triple point - solid, liquid, and vapor are at equilibrium. c) Line AC is the vapor pressure curve - liquid and gas (vapor) are in equilibrium. d) Line AB is the melting curve - solid and liquid are in equilibrium. e) The slope of line AB is negative showing that as the liquid is cooled, the molecules get closer and closer together as they solidify. 4. In a body-centered cubic lattice, how many atoms are present per in a unit cell? a) one b) two c) three d) four e) five 5. In any cubic lattice, an atom lying at the corner of a unit cell is shared equally by how many unit cells? a) one b) two c) eight d) four e) sixteen 6. Which one of the following statements is NOT applicable to COVALENT solids? a) The units that occupy the lattice points are atoms. b) The binding forces in covalent solids are shared electrons. c) Covalent solids have low melting points. d) Covalent solids are typically very hard. e) Covalent solids typically do not conduct electric current well. 7. Which one of the following substances is INCORRECTLY matched with the kind of solid it forms? Substance Kind of Solid a) sulfur dioxide molecular b) Graphite covalent c) calcium bromide ionic d) Lithium ionic e) Methane molecular 8. Substances have properties that are related to their structures. Which of the following statements regarding properties of solids is NOT expected to be CORRECT? a) Solid potassium should be a good conductor of electricity. b) Solid CaSO4 should sublime readily. c) Molten LiCl should be a good conductor of electricity. d) Graphite should have a high melting point. e) Solid CO2 should have a low melting point. 9. Arrange the following in order of increasing melting points: CsCl, BaCl2, diamond (c), H2, HF ----> Increasing Melting Points ----> a) H2 less than HF less than BaCl2 less than CsCl less than diamond b) HF less than H2 less than CsCl less than BaCl2 less than diamond c) H2 less than HF less than CsCl less than BaCl2 less than diamond d) H2 less than HF less than diamond less than CsCl less than BaCl2 e) HF less than H2 less than diamond less than CsCl less than BaCl2 10. In ideal close-packed structures of metallic solids, how many nearest neighbors does a metal ion have? a) 4 b) 3 c) 6 d) 8 e) 12 11. Metallic calcium crystallize in a face-centered cubic lattice, and the atomic radius of calcium is 1.97Å. Calculate the density of calcium. (1Å = 10-8 cm) a) 1.28 g/cm3 b) 1.42 g/cm3 c) 1.54 g/cm3 d) 1.84 g/cm3 e) 2.11 g/cm3 12. Which one of the following statements is NOT applicable to ionic solids? a) The binding forces in ionic solids are electrostatic attractions. b) Ionic solids have fairly high melting points. c) Most ionic solids are hard and brittle. d) The units that occupy the lattice points are ions. e) Ionic solids are usually excellent conductors of electric current. 13. How much heat is absorbed if 45 grams of sweat is evaporated from someone's skin? ΔHvap for water at body temperature is 2.41 kJ/g. a) 115,100 J b) 43,400 J c) 53.6 kJ d) 108,500 J e) 108.5 J 14. How much heat is released when 40.0 g of steam at 250.0°C cools and condenses to water at 30.0 °C? (Sp. heat of H2O(l) = 4.18 J/g °C, Sp. heat of H2O(g) = 2.03 J/g °C, heat of vap. of H2O(l) = 2.260 kJ/g) a) 32.9 kJ b) 122 kJ c) 114 kJ d) 24.0 kJ e) 23.0 J 15. A sketch of a phase diagram is given below. Which statement about this diagram is NOT TRUE? a) Increasing temperature at constant pressure can cause the solid to sublime. b) Increasing pressure at constant temperature can cause liquid to freeze. c) Increasing pressure at constant temperature can melt the solid. d) Increasing pressure at constant temperature can cause deposition of solid from gas. e) Increasing temperature at constant pressure can cause the liquid to vaporize. 16. Which substance would be expected to have the HIGHEST heat of vaporization? a) CH3OCH3 b) CCl4 c) CH2OHCH2OH d) C2H6 e) F2 17. Which response has the following substances arranged in order of INCREASING boiling point? Ar, NaClO3, H2O, H2Se a) NaClO3 less than H2O less than H2Se less than Ar b) Ar less than H2O less than H2Se less than NaClO3 c) Ar less than NaClO3 less than H2Se less than H2O d) NaClO3 less than H2Se less than H2O less than Ar e) Ar less than H2Se less than H2O less than NaClO3 18. In a body-centered cubic lattice, how many atoms are contained in a unit cell? a) one b) five c) three d) two e) four 19. Metallic calcium crystallized in a face-centered cubic lattice and the atomic radius of calcium is 1.97Å. Calculate the edge length, a, of a unit cell of calcium. a) 5.57Å b) 6.05Å c) 6.24Å d) 4.19Å e) 6.83Å 20. Which type of solid is expected for SO2? a) hypersaturated b) molecular c) covalent d) ionic e) metallic 21. Arrange the following ionic compounds in order of increasing melting points. NaF, MgF2, AlF3, NaBr, NaI a) MgF2 less than AlF3 less than NaF less than NaI less than NaBr b) NaF less than NaBr less than NaI less than MgF2 less than AlF3 c) AlF3 less than MgF2 less than NaF less than NaBr less than NaI d) NaBr less than NaI less than NaF less than AlF3 less than MgF2 e) NaI less than NaBr less than NaF less than MgF2 less than AlF3 22. Arrange the following in order of increasing melting points: KCl, He, H2O, HF. a) He less than HF less than H2O less than KCl b) KCl less than H2O less than HF less than He c) H2O less than He less than KCl less than HF d) He less than H2O less than HF less than KCl e) H2O less than HF less than He less than KCl KEY 1)a 2)b 3)e 4)b 5)c 6)c 7)d 8)b 9)c 10)e 11)c 12)e 13)d 14)c 15)b 16)c 17)e 18)d 19)a 20)b 21)e 22)a