Which of the following bonds is the most acid | vedclass

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(C) The acidity of a $C-H$ bond depends on the $s$-character of the carbon atom involved in the bond.As the $s$-character increases,the electronegativ

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$sp C - H$

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(C) The acidity of a $C-H$ bond depends on the $s$-character of the carbon atom involved in the bond.As the $s$-character increases,the electronegativity of the carbon atom increases,which stabilizes the resulting carbanion after the removal of a proton.The $s$-character in different hybridizations is as follows:$sp^3$ (alkane): $25\% \ s$-character$sp^2$ (alkene): $33.3\% \ s$-character$sp$ (alkyne): $50\% \ s$-characterSince the $sp$ hybridized carbon has the highest $s$-character,the $sp C-H$ bond is the most acidic.

Which of the following bonds is the most acidic?

Similar Questions

Number of $sp$ hybridised carbon atoms in the given compound is:
$CH_2 = CH - C \equiv C - CH_2 - CN$

The total number of $\pi-$bond electrons in the following structure is

What is the type of hybridisation of each carbon atom in the following compounds?
$(a)$ $CH_{3}Cl$
$(b)$ $(CH_{3})_{2}CO$
$(c)$ $CH_{3}CN$
$(d)$ $HCONH_{2}$
$(e)$ $CH_{3}CH=CHCN$

The ascending acidity order of the following $H$ atoms is:
$A: HC \equiv C-H$
$B: H_2C=CH-H$
$C: (CH_3)_3C-H$
$D: CH_3-CH_2-H$

$CH_3-CH_2-CH=CH_2$ has hybridisation

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