Question

Which carbon is the most electronegative?
A. $s{p^3}$ hybridized carbon
B. $sp$ hybridized carbon
C. $s{p^2}$ hybridized carbon
D. The electron attracting power of $C$ is always the same irrespective of its hybrid state.

Answer 1

Hint- In order to deal with this question first we will understand the term electronegativity further we will discuss about the factor which define the electronegativity in $s{p^3}$, $s{p^2}$ and $sp$ and according to it we will find our required answer.

Complete step-by-step answer:
Electronegativity is a function of an atom's ability to draw a pair of bonding electrons.
So, electronegativity is the ability to attract electrons. $s$ orbitals are small and tightly held to the nucleus due to maximum shielding. $s$ orbitals are also spherical so it’s multidirectional. That is, it can attract in all directions unlike $p$ or $d$ orbitals which have 2 lobes and attract in that direction only. More probability of electrons being attracted.
So $s$ orbital character is chosen as criterion for electronegativity. $s$ character decreases from
$sp > s{p^2} > s{p^3}$
$sp = 50\% $
$s{p^2} = 33\% $
$s{p^3} = 25\% $
Above mentioned percentage is $s$ character respectively.
So electronegativity order will be $sp > s{p^2} > s{p^3}$
Hence, the most electronegative carbon is $sp$ hybridized carbon
So, the correct answer is option B.

Additional information:
In chemistry, valence bond theory is one of two fundamental theories, along with molecular orbital theory, which were developed to describe chemical bonding using the methods of quantum mechanics.

Note- In chemistry, orbital hybridization (or hybridization) is the process of merging atomic orbitals into new hybrid orbitals (with various energies, sizes, etc.) suitable for combining electrons to form chemical bonds in the theory of valence bonds.