Question

question 9 (mandatory) (1 point) using electronegativity, determine which of the following bonds is the most polar. a) c-c b) c-o c) c-n d) c-h e) c-cl

Explanation:

• For a bond to be polar, there must be a significant difference in electronegativity between the two atoms forming the bond.
• The electronegativity values (on the Pauling scale) are: \( C = 2.5 \), \( O=3.5 \), \( N = 3.0 \), \( H=2.1 \), \( Cl = 3.0 \).
• Calculate the electronegativity differences:
• For \( C - C \): \( |2.5 - 2.5|=0 \).
• For \( C - O \): \( |3.5 - 2.5| = 1.0 \).
• For \( C - N \): \( |3.0 - 2.5|=0.5 \).
• For \( C - H \): \( |2.5 - 2.1| = 0.4 \).
• For \( C - Cl \): \( |3.0 - 2.5|=0.5 \).

Answer:

B. \( C - O \)