Explain how the electronegativity of carbon atoms is related to their state of hybridization in an organic compound.

(N/A) The electronegativity of a carbon atom depends on the percentage of '$s$' character in its hybrid orbitals. The '$s$' orbital is spherical and closer to the nucleus,making it more strongly attracted to the nucleus than the '$p$' orbital.
As the percentage of '$s$' character increases,the hybrid orbital becomes more electronegative. The relationship is summarized in the following table:
| Hybridization | $s : p$ ratio | $\% \ s$ character | Electronegativity |
| :--- | :--- | :--- | :--- |
| $sp$ | $1:1$ | $50\%$ | Highest |
| $sp^2$ | $1:2$ | $33.3\%$ | Intermediate |
| $sp^3$ | $1:3$ | $25\%$ | Lowest |
Thus,the electronegativity of carbon follows the order: $sp > sp^2 > sp^3$.