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liberstina [14]
2 years ago
9

Balancing Chemical Equations & Identifying Chemical Reactions

Chemistry
1 answer:
Stells [14]2 years ago
3 0
The answer is 17 and a half
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Determine the electron geometry (eg) and molecular geometry (mg) of <img src="https://tex.z-dn.net/?f=CH_3%5E%2B" id="TexFormula
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Answer : The correct option is, (e) eg = trigonal planar, mg = trigonal planar

Explanation :

Formula used  :

\text{Number of electron pair}=\frac{1}{2}[V+N-C+A]

where,

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N = number of monovalent atoms bonded to central atom

C = charge of cation

A = charge of anion

The given molecule is, CH_3^+

\text{Number of electron pair}=\frac{1}{2}\times [4+3-1]=3

That means,

Bond pair = 3

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The number of electron pair are 3 that means the hybridization will be sp^2 and the electronic geometry of the molecule will be trigonal planar.

Hence, the electron geometry (eg) and molecular geometry (mg) of CH_3^+  is, trigonal planar and trigonal planar respectively.

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