Explain the structures and HCH bond angle of the
following molecules / species in the light of hybridization
CH4, CH3^- and Ch3^+)
Theory
Answers
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2
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Explanation:
The correct order of the bond angle is CH
3
+
>CH
4
>CH
3
−
In CH
3
+
, three bond pairs and zero lone pairs are present which result in sp
2
hybridization of C atom with bond angle of 120
0
.
In methane, sp
3
hybridization results in tetrahedral geometry with bond angle of 109
0
.
In CH
3
−
, the lone pair of elections repels the bond pair of electrons.
Hence, the bond angle is smaller than the tetrahedral angle.
Answered by
1
1. According to the theory of hybridization, CH₄ has sp³ hybridization.
It has a tetrahedral geometry with a bond angle of 109.5°.
It has four bond pairs and no lone pair.
2. According to the theory of hybridization, CH₃⁻( Methyl carbanion) has sp³ hybridization.
It likely has pyramidal geometry with a bond angle of approximately 107.3°
It has three bond pairs and one lone pair.
3. According to the theory of hybridization, CH₃₊ ( Methyl cation) has sp² hybridization.
It has trigonal planar-shaped geometry with a bond angle of 120⁰.
It has three bond pairs and no lone pair.
The order of bond angle among them would be CH₃₊ > CH₄>CH₃⁻.
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