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Electronegativity Difference
(ΔEN) Bond Classification
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Zero (0.0) Pure Covalent
Small (0.1 – 0.4) Nonpolar Covalent
Intermediate (0.4 – 1.7) Polar Covalent
Large (Greater than 1.7) Ionic
• ↑ higher electronegativity difference → more ionic
• ↓ lower electronegativity difference → more covalent
Calculate the electronegativity difference and determine their bond classification:
*the electronegativity value for each element can be found in books or the internet
*negative differences can be ignored since we are only looking at the value
a) B-F < C-F
• B–F
ΔEN = 2.0 – 4.0
ΔEN = 2.0
• C–F
ΔEN = 2.5 – 4.0
ΔEN = 1.5
C-F < B-F
b) Cl-S < Cl-Br
• Cl–S
ΔEN = 3.0 – 2.5
ΔEN = 0.5
• Cl–Br
ΔEN = 3.0 – 2.8
ΔEN = 0.2
Cl-Br < Cl-S
c) F-O < O-O
• F–O
ΔEN = 4.0 – 3.5
ΔEN = 0.5
• O–O
ΔEN = 3.5 – 3.5
ΔEN = 0.0
O-O < F-O
d) Al-O < P-O
• Al–O
ΔEN = 1.5 – 3.5
ΔEN = 2.0
• P–O
ΔEN = 2.1 – 3.5
ΔEN = 1.4
P-O < Al-O
Which of the following is correctly ranked in order of increasing bond polarity?
a) B-F < C-F
b) Cl-S < Cl-Br
c) F-O < O-O
d) Al-O < P-O
e) Li-F < C-O
f) H-H < N-N
g) O-O < O-F
Frequently Asked Questions
What scientific concept do you need to know in order to solve this problem?
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