Which of the following orders is incorrect :- | vedclass

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(B) . $BF_3$ is non-polar $(\mu = 0)$ while $PF_3$ has a dipole moment,so $BF_3 < PF_3$ is correct. $B$. $N_2$ has a triple bond with high bond energy

Vedclass · Accepted Answer

$N_2 < P_2$ (Bond strength)

Vedclass · Answer

(B) . $BF_3$ is non-polar $(\mu = 0)$ while $PF_3$ has a dipole moment,so $BF_3 $B$. $N_2$ has a triple bond with high bond energy,while $P_2$ is unstable and exists as $P_4$,so $N_2 > P_2$ in bond strength. Thus,$N_2 $C$. $NH_3$ forms hydrogen bonds with water,making it highly soluble,while $PH_3$ does not,so $PH_3  NH_3$ is incorrect. $D$. $Ne $ has a higher effective nuclear charge than $Ne$,so $I.P. (Ne) Note: Both $B$ and $C$ are technically incorrect statements based on standard chemical properties.

Column $I$ (Molecules)	Column $II$ (Number of lone pairs on central atom)
$A. \ NH_3$	$1. \ \text{Two}$
$B. \ H_2O$	$2. \ \text{Three}$
$C. \ XeF_2$	$3. \ \text{Zero}$
$D. \ CH_4$	$4. \ \text{Four}$
	$5. \ \text{One}$

Which of the following orders is incorrect $:-$

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