Courses
Courses for Kids
Free study material
Offline Centres
More

How does hybridization affect electronegativity?

seo-qna
Last updated date: 26th Feb 2024
Total views: 338.4k
Views today: 6.38k
IVSAT 2024
Answer
VerifiedVerified
338.4k+ views
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: \[sp{\text{ }} > {\text{ }}s{p^2} > {\text{ }}s{p^3}\]

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.
Recently Updated Pages