1.1-1.2

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SBI4U
1.1, 1.2 Polarity and Bonding Practice
1. Highlight all of the polar bonds in the following molecules. Bonds are
considered polar when the difference in electronegativity between the two
atoms is between 0.5 and 1.5.
2. Properly label the dipoles (use the “arrow method”
).
3. Determine whether the molecule as a whole is polar or not.
F
4.0
O
3.5
Cl
3.0
N
3.0
C
2.5
S
2.5
H
2.1
SBI4U
4. Draw approx. 5 dashed lines to show where hydrogen bonding would occur amongst
the following methanol molecules.
5. Draw a diagram showing how methanol dissolves in water.
6. Draw a diagram showing how sodium bromide (NaBr: a salt!) dissolves in water.
SBI4U
1.1, 1.2 Polarity and Bonding Practice
1. Highlight all of the polar bonds in the following molecules. Bonds are
considered polar when the difference in electronegativity between the two
atoms is between 0.5 and 1.5.
2. Properly label the dipoles (use the “arrow method”
).
3. Determine whether the molecule as a whole is polar or not.
POLAR
POLAR
NON-POLAR
non-POLAR
POLAR
POLAR
POLAR
non-POLAR
non-POLAR (because the non-polar region far
outweighs the polar region)
POLAR
F
4.0
O
3.5
Cl
3.0
N
3.0
C
2.5
S
2.5
H
2.1
SBI4U
4. Draw approx. 5 dashed lines to show where hydrogen bonding would occur amongst
the following methanol molecules.
5. Draw a diagram showing how methanol dissolves in water.
6. Draw a diagram showing how sodium bromide (NaBr: a salt!) dissolves in water.
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