Electronegativity and Hybridisation

Q. How many of following have at least one bond angle less than ${109}^{\circ }{28}^{{}^{\prime }}$ ?
$C{H}_4$ , $N{H}_4^{+}$ , $N{H}_3$ , $H_{2}O$, $F_{2}O$, $C{l}_{2}O$, $Cl{O}_2$ , $N{F}_3$ , $C{F}_4$ , $PC{l}_5$ , $N{O}_2$ , $S{O}_4^{2-}$ , $C{H}_2{F}_2$ , $S{F}_6$ , $B{F}_4^{-}$ , $C{F}_{3}Cl$, $H_{2}S$, $P{H}_3$ , $SO{F}_4$ , $P{F}_{2}C{l}_3$

Q. Element $B$ forms ccp structure and $A$ occupies half of the octahedral voids, while oxygen atoms occupy all the tetrahedral voids. The formula of bimetallic oxide is:
(JEE Main 2019)

Q. The correct order of increasing percentage s character in the hybrid orbitals in the given molecules/ions is: (assume all hybrid orbitals are equivalent)
$\begin{array}{ccccc}C{O}_3^{2-}& Xe{F}_4& I_3^{-}& NC{l}_3& BeC{l}_2\\ \left(I\right)& \left(II\right)& \left(III\right)& \left(IV\right)& \left(V\right)\end{array}$

1. II < III < IV < I < V
2. II < IV < III < V < I
3. III < II < I < V < IV
4. II < IV < III < I < V

Q. The correct order of increasing percentage s character in the hybrid orbitals in the given molecules/ions is: (assume all hybrid orbitals are equivalent)
$\begin{array}{ccccc}C{O}_3^{2-}& Xe{F}_4& I_3^{-}& NC{l}_3& BeC{l}_2\\ \left(I\right)& \left(II\right)& \left(III\right)& \left(IV\right)& \left(V\right)\end{array}$

1. II < III < IV < I < V
2. II < IV < III < V < I
3. III < II < I < V < IV
4. II < IV < III < I < V

Q. The relative Lewis acid strengths of boron trihalides are in the order:

1. $BB{r}_3>BC{l}_3>B{F}_3$
2. $BC{l}_3>B{F}_3>BB{r}_3$
3. $B{F}_3>BC{l}_3>BB{r}_3$
4. $B{F}_3>BB{r}_3>BC{l}_3$

Q. The relative Lewis acid strengths of boron trihalides are in the order:

1. $BB{r}_3>BC{l}_3>B{F}_3$
2. $BC{l}_3>B{F}_3>BB{r}_3$
3. $B{F}_3>BC{l}_3>BB{r}_3$
4. $B{F}_3>BB{r}_3>BC{l}_3$

Q. The electronegativity of $H,X$ and $O$ are $2.1,0.8$ and $3.5$ respectively on Pauling scale. The nature of compound $HOX$ is:

1. Acidic
2. Basic
3. Neutral
4. Amphoteric

Q. The hybridizations of atomic orbitals of nitrogen in $N{O}_2^{+},N{O}_3^{-}$ and $N{H}_4^{+}$ respectively are

1. $sp,s{p}^2$ and $s{p}^3$
2. $s{p}^2,sp$ and $s{p}^3$
3. $sp,s{p}^3$ and $s{p}^2$
4. $s{p}^2,s{p}^3$ and $sp$

Q. Find the number of molecules having two lone pair of electrons on central atom.
$I_3^{-},Xe{F}_2,Xe{F}_4,H_{2}O,N{H}_2^{-}{H}_{2}S,H_{2}S{O}_4,N{F}_3$