AP Chemistry                                                               Unit 10-11

Chapter 10-11                                                             Liquids and Solids

Daily

 

  1. If water and carbon dioxide molecules interact, what intermolecular forces will exist

a. hydrogen bonding      b. London dispersion      c. ion-dipole      d. dipole-dipole

 

 

 

  1. Arrange the following in terms of decreasing intermolecular interactions
    1. CH3OH>CH3NH2>SO2>Cl2
    2. Cl2>SO2>CH3OH>CH3NH2
    3. SO2>CH3NH2>CH3OH>Cl2
    4. CH3NH2>CH3OH>SO2>Cl2

 

 

 

  1. Which of the following molecules interact primarily through London dispersion forces only
    1. SO2            b. CCl4            c. CH2Cl2            d. H2S

 

  1. Surface tension is a result of
    1. Liquid molecules being more cohesive than adhesive
    2. Liquid molecules being more adhesive than cohesive
    3. Liquid molecules being very weakly adhesive or cohesive
    4. Liquid molecules being both strongly adhesive and cohesive

 

  1. The smallest repeated unit of a lattice is called

a. unit cell       b. unit lattice         c. cell       d. unit crystal

 

  1. The difference between interstitial and substitutional alloys are that in substitutional alloys:
    1. some atoms of an element are replaced by another
    2. atoms of one type may be inserted into the spaces between another type
    3. atoms of 1 type fuse with another type
    4. there are 3 types of atoms present instead of 2

 

  1. A n-type semiconductor substance is produced by
    1. increasing the number of atoms of the semiconductor
    2. increasing the number of valence electrons of the semiconductors present
    3. decreasing the number of valence electrons of the semiconductors present
    4. chemically combining semiconductors to form new semiconductor types

 

  1. The change in state from solid to gas is called

a. sublimation      b. evaporation           c. special case melting      d. gas state melting

 

 

 

 

9. CCl2F2 is a liquid that cools by evaporation. How many kilograms of CCl2F2 must be evaporated to freeze a tray of water (1050 g. of water) at 273.15 K to ice at the same temperature? Heat of evaporation of CCl2F2 is 17.4 kJ/mol.                               a.2.44 kg  b.1.22 kg  c.10.3 kg  d.12.2 kg

 

10. How much heat is necessary to melt 175.32 g of NaCl at 801˚ C? (Heat of fusion NaCl = 28.16 kJ/mol)                                                                                     a.22.5 kJ   b.9.39 kJ   c.30.2 kJ   d.84.5 kJ

 

11. The heat of crystallization for substance A = -65.0 J/g. The heat of fusion of water is 335 J/g. If 2000.0 grams of liquid A is added to an excess of ice, how many grams of ice will melt, assuming no temperature change?

      a.388 g      .      b.200.0 g.   c.10.3 g.      d.10300

 

12. Arrange the following liquids, A, B, C, with vapor pressures, at room temperature, of 88, 680, and 155, respectively, in order of decreasing boiling points.

      a. B>C>A      b. A>B>C      c. A>C>B      d. C>A>B

 

13. The melting point of ice will change in what direction as pressure decreases?

      a. No change      b. Decreases      c. Increases      d. Depends on the pressure

 

14. Define the terms in your own words:

a. dipole-dipole forces               b. hydrogen bonding                        c. London dispersion

                        forces

 

15. Of HF, HCl, and HBr, which has the highest boiling point? Why? Which is the lowest boiling point.

 

16. Which would you expect to have a lower melting point, C3H8 or CH3OH? Why?

 

17. Arrange the following in order of increasing boiling points and justify your assignments: CH3F, CH3Cl, CH3Br, CH3I and CH3F, CH2F2, CHF3, CF4

 

18. Would mercury bead more on a waxed or unwaxed car?

 

19. Which would have a greater surface tension N2(l) or Br2(l)

 

20. Classify each as either ionic, molecular, network or metallic solids

a. CaF2(s)    b. graphite    c. diamond    d. pure copper  e. H2O(s)

 

21. Tungsten crystallizes in a body-centered cubic structure with a unit cell edge length of 315.83 pm. The density of tungsten metal is 19.3 g/cm3 and it’s atomic weight is 183.85 g/mol. Calculate the value of Avogadro’s number by this method.

 

22. From the diagram on page 509 (#22) what are the approximate range of conditions necessary to create a monoclinic solid Sulfur structure?

 

23. Why is iron relatively soft, ductile, and malleable, while high carbon steels are much harder, stronger and less malleable?

 

24. What accounts for the lubricating effect of graphite?

 

25. Explain why graphite conducts electricity parallel to the layers much better than it conducts electricity perpendicular to the layers.

 

 

26. What quantity of heat is required to vaporize (at 100°C) 1kg of ice (at 0°C)

 

27. What is the final temperature if 10 grams of water at 0°c is added to 100 g of water at 75°C

 

28. What is the final temperature if 10 grams of ice at 0°C is added to 100 g of water at 75°C

 

29. Calculate the amount of energy in Joules required to change 10 g of solid mercury at its melting point to mercury vapor at its boiling point.

Mp=-39°C

Bp=375°C

C=0.033cal/gram

ΔHf = 11.4 j/g

ΔHv = 59100j/mol