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