Bond Pairs and Lone Pairs

Q.

The central oxygen atom in ether is_______

Q. Match the following:
$$\begin{array}{cc}\text{List- I}& \text{List - II}\\ \text{(Molecule)}& \text{(number of lone pairs on central atom)}\\ \left(A\right)N{H}_3& \text{(i) Two}\\ \left(B\right)H_{2}O& \text{(ii) three}\\ \left(C\right)Xe{F}_2& \text{(iii) zero}\\ \left(D\right)C{H}_4& \text{(iv) Four}\\ & \text{(v) One}\end{array}$$

1. $$\begin{array}{cccc}\left(A\right)& \left(B\right)& \left(C\right)& \left(D\right)\\ \left(v\right)& \left(i\right)& \left(iii\right)& \left(ii\right)\end{array}$$
2. $$\begin{array}{cccc}\left(A\right)& \left(B\right)& \left(C\right)& \left(D\right)\\ \left(iii\right)& \left(i\right)& \left(ii\right)& \left(v\right)\end{array}$$
3. $$\begin{array}{cccc}\left(A\right)& \left(B\right)& \left(C\right)& \left(D\right)\\ \left(v\right)& \left(i\right)& \left(ii\right)& \left(iii\right)\end{array}$$
4. $$\begin{array}{cccc}\left(A\right)& \left(B\right)& \left(C\right)& \left(D\right)\\ \left(i\right)& \left(v\right)& \left(iii\right)& \left(iv\right)\end{array}$$

Q. Which of the following does not contain any coordinate bond?

1. $H_3{O}^{+}$
2. $B{F}_4^{-}$
3. $H{F}_2^{-}$
4. $N{H}_4^{+}$

Q.

Total number of lone pairs in $XeO{F}_4$ is:

1. 1

2. 2

3. 3

4. None of these

Q. Calculate the sum of lone pairs of electrons in the central atoms of the molecules $XeO{F}_4,[Xe{O}_6{]}^{4-}$ and $Cl{F}_3$.

Q. Calculate the sum of lone pairs of electrons in the central atoms of the molecules $XeO{F}_4,[Xe{O}_6{]}^{4-}$ and $Cl{F}_3$.

Q.

The shape of covalent molecule $M{X}_3$ is

1. Triangular

2. T - shaped

3. Pyramidal

4. Either of these depending on the number of lone pairs of electrons on M

Q.

Total number of lone pairs in $XeO{F}_4$ is:

1. 1

2. 2

3. 3

4. None of these

Q. The geometry of electron pairs around $I$ in $I{F}_5$ is:

1. Octahedral
2. Trigonal bipyramidal
3. Square pyramidal
4. Pentagonal planar

Q.

Calculate % ionic character in HCl.

$Bondlength=1.275\stackrel{\circ }{A},{\mu }_{observed}=1.03D$

1. $17\%$

2. $20\%$

3. $30\%$

4. $50\%$

Q.

The number of electron pairs in $OS{F}_4$ is

1. 4

2. 5

3. 5.5

4. 6

Q.

The shape of covalent molecule $M{X}_3$ is

1. Triangular

2. T - shaped

3. Pyramidal

4. Either of these depending on the number of lone pairs of electrons on M

Q. Assume that in $CH{X}_3$, only the CX bond is polar and it has $20\%$ ionic character. Also, $CH{X}_3$ is a perfect tetrahedral i.e. $\angle HCX=\angle XCX={109}^{\circ }{28}^{{}^{\prime }}$. If the C-H bond length is 150 pm, then find dipole moment (in Debye) of $CH{X}_3$.(Given:$cos(180-{109}^{\circ }{28}^{{}^{\prime }})=\frac{1}{3}$) .