AP Chemistry Name : Worksheet : Ch 10-1

AP Chemistry
Worksheet : Ch 10-1-2
Name :
Date :
_____ 1. Held together by London Dispersion forces
For questions 1-5
_____ 2. Lattice of positive and negative ions held together by
electrostatic forces
_____ 3. Closely packed lattice with delocalized electrons
a. Mg
b. graphite(C)
c. CaF2
d. Xe
e. HF
_____ 4. Held together by network covalent bonds
_____ 5. Has strong hydrogen bonding
For questions 6-11
_____ 6. diamond
a. ionic solid
b. network atomic solid
c. metallic solid
d. molecular solid
e. Group 8A solid
_____ 7. Si
_____ 8. SiO2
_____ 9. AlF3
_____ 10. Solid Kr
_____ 11. Mg
_____ 12. Which of the following molecules will not exhibit dipole interactions?
a. H2O
b. CO2
c. CO
d. SO2
e. HF
_____ 13. Which of the following would have the highest boiling point?
a. F2
b. Cl2
c. Br2
d. I2
_____ 14. Which of the following would have the lowest freezing point?
a. CH3OH
b. C2H5OH
c. C3H7OH
d. C4H9OH
e. C6H11OH
d. P4O10
e. C8H18
_____ 15. Which of the following has the highest melting point?
a. S8
b. Br2
c. SiO2
16. Identify the most important types of interparticle forces present in the solids of each of the following
a. BaSO4
b. Xe
c. CsI
d. H2O
17. For which molecule in each of the following pairs would you expect greater intermolecular forces?
b. CH3CH3 or H2CO
c. CH3OH or H2CO
d. HF or HBr
18. In each of the following groups of substances, pick the one that has the given property. Justify your answer.
a. Highest boiling point: HC1, Ar, or F2
b. Highest freezing point: H2O, NaCl, or HF
c. Lowest vapor pressure at 25°C: C12, Br2, or I2
d. Lowest freezing point: N2, CO, or CO2
e. Lowest boiling point: CH4, CH3CH3, or CH3CH2CH3
f. Highest boiling point: HF, HC1, or HBr
g. Lowest vapor pressure at 25°C: CH3CH2CH3, CH3CCH3, or CH3CH2CH2OH
19. The meniscus in of water in a glass tube is different from the meniscus of mercury in a glass tube. Why?
What would be the shape of the meniscus of water in a polyethylene tube? [Polyethylene can be represented as
CH3(CH2)nCH3, where n is a large number on the order of 1000.]
20. Carbon diselenide (CSe2) is a liquid at room temperature. The normal boiling point is 125°C, and the melting
point is -45.5°C. Carbon disulfide (CS2) is also a liquid at room temperature with normal boiling and melting
points of 46.5°C and -111,6°C, respectively. How do the strengths of the interparticle forces vary from CO2 to
CS2 to CSe2? Explain.
21. How can an n-type semiconductor be produced from pure germanium?
22. How can a p-type semiconductor be produced from pure germanium?
23. Selenium is a semiconductor used in photocopying machines. What type of semiconductor would be
formed if a small amount of indium impurity is added to pure selenium?
24. What type of solid will each of the following substances form?
a. KBr
b. H2O
c. NaOH
d. U
e. CaCO3
f. PH3
25. Arrange the following hydrogen bonds (---) according to increasing strength.
a. N---H—O
b. O---H—F
c. O---H—O
d. N----H—N
Answers : 216a. ionic 16b. LD only 16c. ionic 16d. H-bonding, LD
17a. H2NCH2CH2NH2 –
more extensive H-bonding 17b. H2CO – polar 17c. CH3OH – more polar, stronger H-bonding 17d. HF –
more polar 18a. HCl – polar 18b. NaCl – ionic
18c. I2 – all nonpolar – I2 is largest – greatest LD
N2 – nonpolar and smallest – weakest LD 18e. CH4 – smallest, weakest LD 18f. HF – polar, H-bonding
18g. CH3CH2CH2OH – H-bonding 19. Glass is polar and has a stronger bond with H2O than it does for itself.
Hg-Hg bonds are stronger than Hg-glass bonds (Hg is nonpolar).
20. CO2 is a gas at room temp. As mp and
bp increase, the strength of intermolecular forces must increase. – All are linear and nonpolar, so LD forces are
dominant giving CO2<CS2<CSe2.
21. n-type semiconductors are doped with elements with more valence
electrons – so you must add something with more than 4 valence electrons. A group 5A element such as P, or As.
322. Group 3A element – Ga or In. 23. p-type
24a. ionic
24b. molecular 24c. ionic 24d. atomic,
metallic 24e. ionic 24f. molecular 25. H-bonding increases with increasing electronegativity of the
electronegativity of the element bonded to hydrogen. : weakest N···H—N < N···H—O < O···H—O < O···H—F