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(C) Let us analyze the bond angles for each option:$A$: $CO_2$ $(180^\circ)$ > $BF_3$ $(120^\circ)$ > $CH_4$ $(109.5^\circ)$. This order is correct.$B

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$XeF_2 > XeF_4 > XeO_4$

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(C) Let us analyze the bond angles for each option:$A$: $CO_2$ $(180^\circ)$ > $BF_3$ $(120^\circ)$ > $CH_4$ $(109.5^\circ)$. This order is correct.$B$: $NO_2^+$ $(180^\circ)$ > $NO_3^-$ $(120^\circ)$ > $NO_2^-$ $($C$: $XeF_2$ $(180^\circ)$,$XeF_4$ $(90^\circ)$,and $XeO_4$ $(109.5^\circ)$. The correct order should be $XeF_2 > XeO_4 > XeF_4$. Thus,the given order $XeF_2 > XeF_4 > XeO_4$ is incorrect.$D$: According to Drago's rule,the bond angle decreases as the electronegativity of the central atom decreases. The bond angles are approximately $PH_3$ $(93.5^\circ)$,$AsH_3$ $(91.8^\circ)$,and $SbH_3$ $(91.3^\circ)$. Thus,the order $PH_3 > AsH_3 > SbH_3$ is correct.

Which of the following represents the incorrect order of adjacent bond angles?

Similar Questions

Arrange the following species in the increasing order of lone pairs of electrons:
$(A)$ $CO$
$(B)$ $NO_2^-$
$(C)$ $NF_3$
$(D)$ $CO_3^{2-}$

Observe the following molecules/ions: $NH_4^{+}, NH_3, BF_3, OH^{-}, CH_3^{+}, H^{+}, CO, C_2H_4$. The number of Lewis bases in the above list is:

Observe the following statements:
$i$. The dipole moment of $NH_3$ is higher than the dipole moment of $NF_3$.
$ii$. The dipole moment of chloroform $(CHCl_3)$ is zero.
$iii$. Covalent bond character in $NaCl$ is more compared to $CuCl$.

Which of the following is the correct decreasing order of bond length for $N_2$, $O_2$, and $Cl_2$?

Bonds present in $CuSO_4 \cdot 5H_2O$ are

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