Electronegativity Worksheet

Electronegativity: Answer key
For our purposes use the definitions in the chart. The
most polar bond determi nes the polarity of a mole cule (i.e.
if a compound contains one non-polar, and one polar
bond the molecule, as a whole, is considered to be polar)
% ionic character
ΔEN
polarity
0 – 10 0 – 0.5 non-polar
10 – 50 0.5 – 1.7 polar (covalent)
50 – 100 1.7 + ionic
A B C D E F G
Molecule Lewis structure
Draw shape.
Indicate bond
dipoles
ΔEN of
bonds
Polarity of
bonds (ignore
shape)
Symmetrical
molecule?
Polarity of
molecule
1. NH
3
3.1 – 2.1
= 1.0
polar No polar
2. N
2
No dipole
3.1 – 3.1
= 0
non-polar Yes non-polar
3. HBr
H Br
2.8 – 2.1
= 0.7
polar No polar
4. OCl
2
3.5 – 2.9
= 0.6
polar No polar
5. SF
6
All away from centre
4.1 – 2.4
= 1.7
polar / ionic Yes non-polar
H
6. SO
2
3.5 – 2.4
= 1.1
polar No polar
7. SiCl
4
All away from centre
2.9 – 1.8
= 1.1
polar Yes non-polar
8. CF
2
Cl
2
All away from centre
C-F: 4.1 –
2.5 = 1.6
C-Cl: 2.9 –
2.5 =0.4
polar
non-polar
No (yes if you
think just about
shape, but no
because Cl and
F are different)
polar
9. XeF
4
All away from centre
(4.1 – 2.6
= 1.5)
(polar) Yes non-polar
10. C
2
H
4
(small dipoles)
C-C: 2.5 –
2.5 = 0
C-H: 2.5 –
2.1 =0.4
non-polar
non-polar
Yes non-polar
Q1 – which binary (two element) compound would have the greatest ΔEN? FrF - ΔEN = 4.1 - 0.9 = 3.2 (ionic)
H
H N
N N
Br
H
F
S
F
F
F
F
F
S
O O
O
S
O
O Cl Cl
F
Xe
F
F
F
C
F
F
Cl
Cl
Si
Cl
Cl
Cl
Cl
H
C
C
H
H
H
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