Bonding and Percent
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WS E: Lewis Structure Worksheet: See me to see which ones you have to do.
 Draw the Lewis Structures
You may need to watch the bonding videos
 Determine the shape
in the Chem1 folder on the desk top.
 Determine the polarity of the molecule
1. HCl
9. OI2
2. Br2
10. CS2
3. SeBr2
11. SiBr4
4. CF4
12. F2
5. PI3
13. HCN
6. O2
14. NH4 +
7. N2
15. NO2 –
8. H2
16. SO3
Bonding and Percent
17. SO4
2-
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26. OCN-
18. NO3-
27. SCN-
19. PO33-
28. O3
20. CN-
For the following structures: You do NOT
have to determine the shapes
29. H3CCOOH
21. CO2
30.CH3CH2OH
22. CO
31.H3COCH3
23. I2
32.H3CCH3
24. CO32-
33.H2CCH2
25. SO2
34.HCCH
Bonding and Percent
35.
C2H4
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43. CH3NH2 (Explanation: 1st C has 3 H’s and one
N. The N has 2 H’s.)
36. CH2CCH2 (Explanation for CH2CCH2: The
notation here has organization to it. It is written
this way because the 1st C has 2 H’s attached the
second C as NO H’s attached and the third C has
2 H’s attached.)
44.
(CH2)5
45. As
37. HCN
38. CH3COCH3
39. Cl2
40. P2
41. PCl3
42. CCl3F
Bonding and Percent
WS F: Intermolecular Forces
Substance #1
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Predominant
Intermolecular Force
Substance #2
(a) HCl(g)
I2
(b) CH3F
CH3OH
(c) H2O
H2S
(d) SiO2
SO2
(e) Fe
Kr
(f) CH3OH
CuO
(g) NH3
CH4
(h) HCl(g)
NaCl
(i) SiC
Predominant
Intermolecular Force
Cu
2. Rank the following substances in order from lowest to highest melting point.
CO2, NaCl, Ag, H2O, He, HBr
3. Rank the following substances in order from lowest to highest freezing point.
H2O, Ca3(PO4)2, Cr, C2H6, OF2
4. Rank the following substances in order from highest to lowest boiling point.
Cl2, Ne, Ca, Cr(OH)3, CH3CH2OH, Diamond
Substance with Higher
Boiling Point
Bonding and Percent
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Molecular Shapes
“clouds”
2
Linear Diatomic
Polarity depends upon
electronegativity
difference
Polar if >0.5
Nonpolar if <0.5
Linear Triatomic, Usually nonpolar
CO2, HCN
3
Trigonal Planar: BF3, SO3, NO3120˚ Usually nonpolar
In molecules where
the outside
molecules are
different, shapes
that tend to be
nonpolar usually
become polar.
Remember to count
the number of
“clouds” of electrons,
not the actual number
of electrons. A
double or triple bond
counts as one
effective pair.
Bent, 12O˚ Usually polar
NO2-
Also: If there ever
is a two molecule
atom (diatomic) that
molecule’s polarity
depends upon the
electronegativity
difference of the
atoms
4
Tetrahedral; 109˚: Usually
nonpolar CH4, CF4
Pyrimidal: 107˚ Usually
polar: NH3, PCl3
Bent: 104.5˚
Usually polar: H2O, OF2
Bond
Ionic (85)
Covalent
Polar Molecules
Nonpolar Molecules
H-Bond (5)
Dipole Force (1)
LDF (0.1)
Metallic (65)
Network Solids (100)