Question

How does hybridization affect electronegativity?

Answer 1

Hint: 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: $$sp>s{p}^2>s{p}^3$$

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 $$25\mathrm{\%}$$ s-Character
Ethene $$C_2{H}_4$$→ where $$C$$ uses-$$s{p}^2$$ hybrid orbital with $$33.33\mathrm{\%}$$ 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 $$s{p}^3-s{p}^2$$ 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 $$C\left(sp\right)--H$$ bond is more prominent than that of a $$C\left(s{p}^2\right)--H$$ bond, which is more noteworthy than that of a $$C\left(s{p}^3\right)--H$$ 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 $$33.33\mathrm{\%}$$s-character and $$66.66\mathrm{\%}$$ p-character; a $$s{p}^3$$ hybrid orbital has $$25\mathrm{\%}$$ s-character and $$75\mathrm{\%}$$ p-character.