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BONDING REVIEW

1. Draw the shape diagram for CH3F(g), including arrows to represent bond dipoles. Is it a dipole?

2. Briefly explain in terms of intermolecular forces why iodine has a very low solubility in water but is quite

soluble in propanol (C3H7OH).

3. Explain why HF(g) has hydrogen bonding while HI (g) does not.

4. Draw Lewis Diagrams for each of the molecules below. Indicate the shape about each

central atom and tell if the molecule is polar or nonpolar.

a. H 2CO b. CH3Fc. H2O2

5. Define each of the following:

a. covalent bondj. hydrogen bond

b. nonpolar covalent bondk. Van der Waals forces

c. polar covalent bondl. macromolecule

d. bond dipolem. network covalent bonds

e. molecular dipolen. intermolecular forces

f. dipole-dipole forceo. intramolecular forces

g. London dispersion forceh. VSEPR Theory

6. Which substance in each pair below has the higher b.p.?EXPLAIN WHY.

a. Kr OR Hbrb. HF OR CF3Hc. H2S OR H2Te

d. BrCl OR C2H5Bre. NCl3 OR SCl2

7. Explain each of the following:

a. Glycerol (C3H5(OH)3) flows more slowly than waterb. CaCl2 has no molecules.

c. Silver can be bent to make chains.d. Graphite is a lubricant.

e. Diamonds are nonconductorsf. Molten ionic compounds conduct

g. Water expands on freezing.

8. Complete the following table:

Chemical / Lewis Dot Diagrams / Lone Pair Bonding Pair / Polarity
Yes/No / Intermolecular Forces
ClF 3
PBr3
CH3Cl
SO 3

9. Complete the following table:

Property of Substance / Type of Bonding
(i)Melts at 805oC, conducts electricity in the liquid state but not in solid state
(ii)Melts at -7.2oC, does not conduct electricity in either the solid or liquid state
(iii)Melts at 649oC, conducts electricity in both solid and liquid state.

10.Explain the difference between intramolecular bonding and intermolecular bonding.

11.Why glycerol, C3H5(OH)3, flows much more slowly than water.

12.Which substance in each pair has the higher boiling point? Give reason(s)

a)Kr or HBrb)HF or CF3H

c)PCl3 or PI3d)C5H12 or CF4

e)CO2 or SiO2f)K and KCl

13.Why does methanol completely mixes with ethanol

14.Why oil and water do not mix

15.Why hexane, C6H14(l), is a good solvent for I2(s) but water is not.

16.Why ice floats

17.Why diamonds do not conduct electricity

18.Why molten potassium chloride can conduct electricity but solid potassium chloride cannot.

19.Why a piece of sea salt shatters when a force is applied.

20.Why silver can be bent to make chains