Question

How does hybridization affect electronegativity?

Answer 1

The inclination of a molecule to pull in holding electrons towards itself is called its electronegativity.
The more noteworthy the s-character of the half and half orbitals, the more prominent is the electronegativity on the grounds that a s orbital holds electrons all the more firmly to the core
Regarding Electronegativity: $sp{\text{ }} > {\text{ }}s{p^2} > {\text{ }}s{p^3}$

Complete step by step answer:
Electronegativity increments with the s-character of the half and half orbital utilized for making covalent bond.
It could be clarified by taking a straightforward illustration of three least difficult hydrocarbons
Ethane ${C_2}{H_6}$→ where $C$ uses- $s{p^3}$ hybrid orbital with $25\%$ s-Character
Ethene ${C_2}{H_4}$→ where $C$ uses-$s{p^2}$ hybrid orbital with $33.33\%$ s-Character
Ethyne ${C_2}{H_2}$→ where $C$ uses-$sp$ hybrid orbital with half s-Character
S orbital being the orbital nearer to the $C$-atom the electron pair of the bond shaped by the orbital having higher s-character is pulled in addition towards $C$-particle indicating higher electronegativity .
Along these lines the request for EN of Carbon
$Ethyne > Ethene > Ethane$
The electronegativity of carbon relies upon its hybridization state. Carbons that are $s{p^2}$ - hybridized are fairly more electronegative than $s{p^3}$ - hybridized carbons; sp-hybridized carbons are much more electronegative by another $0.2$ units. This implies that $s{p^3}-{\text{ }}s{p^2}$ carbon–carbon bonds have a slight bond dipole.
Bond-strength impacts and electronegativity impacts. The request can't be a bond-strength impact, since bond qualities increment with expanding s character. That is, the strength of a $C\left( {sp} \right)--{\text{ }}H$ bond is more prominent than that of a $C\left( {s{p^2}} \right)--{\text{ }}H$ bond, which is more noteworthy than that of a $\;C\left( {s{p^3}} \right)--{\text{ }}H$ bond. Hence, this should be an electronegativity impact. This corrosiveness request, at that point, is reliable with expanding electronegativity of carbons with expanding s character in their hybridizations.

Note:
Three kinds of hybridisation − $sp$, $s{p^2}$ and $s{p^3}$, are found in carbon particles relying on the number of atoms connected to the carbon.
A $sp$ hybrid orbital has half s-character and half p-character; a $s{p^2}$ hybrid orbital has $33.33\%$s-character and $66.66\%$ p-character; a $s{p^3}$ hybrid orbital has $25\%$ s-character and $75\%$ p-character.