QBManager

CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE

313712 In which of the following sets, all the species are diamagnetic in nature?

1

[O_{2}^{2 -}, O_{2}^{2 +}, N_{2}^{2 -}]

2

[C_{2}, O_{2}^{2 -}, N_{2}^{2 +}]

3

[O_{2}^{2 -}, O_{2}^{+}, O_{2}^{2 +}]

4

[N_{2}^{+}, O_{2}^{2 +}, B_{2}]

Explanation:

$C_{2} - 12 e^{-}, O_{2}^{- 2} - 18 e^{-}, N_{2}^{+ 2} \to 12 e^{-} \to$ all are diamagnetic
$O_{2}^{- 2} - 18 e^{-}, O_{2}^{+ 2} - 14 e^{-} (Dia) &$
$N_{2}^{- 2} (16 e^{-})$ paramagnetic
$O_{2}^{- 2} - 18 e^{-}, O_{2}^{+ 2} - 14 e^{-} ($ Dia $) &$
$O_{2}^{+} (15 e^{-})$ paramagnetic
$O_{2}^{+ 2} - 14 e^{-}$ ,diamagnetic,
$B_{2} \to 10 e^{-}, N_{2}^{+} \to 13 e^{-} \Rightarrow$ paramagnetic
Hint: All odd no. $e^{-}, 10, 16 \to$ paramagnetic
All even no. of $e^{-}$ (except 10,16) $\to$
Diamagnetic

CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE

313713 The molecular electronic configuration of $H_{2}^{-}$ ion is

1

(σ ls)^{2}

2

(σ 1 s)^{2} {(σ^{*} 1 s)}^{2}

3

(σ 1 s)^{2} {(σ^{*} 1 s)}^{1}

4

(σ 1 s)^{3}

Explanation:

$H_{2}^{-}$ ionn has 3 electrons so $σ 1 s^{2} \overset{*}{σ} 1 s^{1}$

CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE

313723 The number of antibonding electron pairs in $O_{2}^{2 -}$ molecular ion on the basis of molecular orbital theory is (Atomic number of O is 8)

1 5

2 4

3 3

4 2

Explanation:

$O_{2}^{2 -}$ , no. of antibonding electron pairs = 4 pairs.
supporting img
Molecular orbital diagram of $O_{2}^{2 -}$ (peroxide ion)

CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE

313714 Molecular orbital electronic configuration for ' $X$ ' anion is $KK$ $σ^{*} 2 s^{2} σ^{*} 2 s^{2} π 2 p_{x}^{2} 2 p_{y}^{2} σ 2 p_{z}^{2} π^{*} 2 p_{x}^{1}$ , the anion ' $X$ ' is

1

N_{2}^{-}

2

O_{2}^{-}

3

N_{2}^{2 -}

4

O_{2}^{2 -}

Explanation:

In the given configuration, total number of electrons of anion $X = 15$
Hence; the anion $X$ is $N_{2}^{-}$ (15 electrons)
$[O_{2}^{-} (17 e^{-}), N_{2}^{- 2} (16 e^{-}), O_{2}^{- 2} (18 e^{-})]$

CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE

313712 In which of the following sets, all the species are diamagnetic in nature?

1

[O_{2}^{2 -}, O_{2}^{2 +}, N_{2}^{2 -}]

2

[C_{2}, O_{2}^{2 -}, N_{2}^{2 +}]

3

[O_{2}^{2 -}, O_{2}^{+}, O_{2}^{2 +}]

4

[N_{2}^{+}, O_{2}^{2 +}, B_{2}]

Explanation:

$C_{2} - 12 e^{-}, O_{2}^{- 2} - 18 e^{-}, N_{2}^{+ 2} \to 12 e^{-} \to$ all are diamagnetic
$O_{2}^{- 2} - 18 e^{-}, O_{2}^{+ 2} - 14 e^{-} (Dia) &$
$N_{2}^{- 2} (16 e^{-})$ paramagnetic
$O_{2}^{- 2} - 18 e^{-}, O_{2}^{+ 2} - 14 e^{-} ($ Dia $) &$
$O_{2}^{+} (15 e^{-})$ paramagnetic
$O_{2}^{+ 2} - 14 e^{-}$ ,diamagnetic,
$B_{2} \to 10 e^{-}, N_{2}^{+} \to 13 e^{-} \Rightarrow$ paramagnetic
Hint: All odd no. $e^{-}, 10, 16 \to$ paramagnetic
All even no. of $e^{-}$ (except 10,16) $\to$
Diamagnetic

CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE

313713 The molecular electronic configuration of $H_{2}^{-}$ ion is

1

(σ ls)^{2}

2

(σ 1 s)^{2} {(σ^{*} 1 s)}^{2}

3

(σ 1 s)^{2} {(σ^{*} 1 s)}^{1}

4

(σ 1 s)^{3}

Explanation:

$H_{2}^{-}$ ionn has 3 electrons so $σ 1 s^{2} \overset{*}{σ} 1 s^{1}$

CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE

313723 The number of antibonding electron pairs in $O_{2}^{2 -}$ molecular ion on the basis of molecular orbital theory is (Atomic number of O is 8)

1 5

2 4

3 3

4 2

Explanation:

$O_{2}^{2 -}$ , no. of antibonding electron pairs = 4 pairs.
supporting img
Molecular orbital diagram of $O_{2}^{2 -}$ (peroxide ion)

CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE

313714 Molecular orbital electronic configuration for ' $X$ ' anion is $KK$ $σ^{*} 2 s^{2} σ^{*} 2 s^{2} π 2 p_{x}^{2} 2 p_{y}^{2} σ 2 p_{z}^{2} π^{*} 2 p_{x}^{1}$ , the anion ' $X$ ' is

1

N_{2}^{-}

2

O_{2}^{-}

3

N_{2}^{2 -}

4

O_{2}^{2 -}

Explanation:

In the given configuration, total number of electrons of anion $X = 15$
Hence; the anion $X$ is $N_{2}^{-}$ (15 electrons)
$[O_{2}^{-} (17 e^{-}), N_{2}^{- 2} (16 e^{-}), O_{2}^{- 2} (18 e^{-})]$

CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE

313712 In which of the following sets, all the species are diamagnetic in nature?

1

[O_{2}^{2 -}, O_{2}^{2 +}, N_{2}^{2 -}]

2

[C_{2}, O_{2}^{2 -}, N_{2}^{2 +}]

3

[O_{2}^{2 -}, O_{2}^{+}, O_{2}^{2 +}]

4

[N_{2}^{+}, O_{2}^{2 +}, B_{2}]

Explanation:

$C_{2} - 12 e^{-}, O_{2}^{- 2} - 18 e^{-}, N_{2}^{+ 2} \to 12 e^{-} \to$ all are diamagnetic
$O_{2}^{- 2} - 18 e^{-}, O_{2}^{+ 2} - 14 e^{-} (Dia) &$
$N_{2}^{- 2} (16 e^{-})$ paramagnetic
$O_{2}^{- 2} - 18 e^{-}, O_{2}^{+ 2} - 14 e^{-} ($ Dia $) &$
$O_{2}^{+} (15 e^{-})$ paramagnetic
$O_{2}^{+ 2} - 14 e^{-}$ ,diamagnetic,
$B_{2} \to 10 e^{-}, N_{2}^{+} \to 13 e^{-} \Rightarrow$ paramagnetic
Hint: All odd no. $e^{-}, 10, 16 \to$ paramagnetic
All even no. of $e^{-}$ (except 10,16) $\to$
Diamagnetic

CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE

313713 The molecular electronic configuration of $H_{2}^{-}$ ion is

1

(σ ls)^{2}

2

(σ 1 s)^{2} {(σ^{*} 1 s)}^{2}

3

(σ 1 s)^{2} {(σ^{*} 1 s)}^{1}

4

(σ 1 s)^{3}

Explanation:

$H_{2}^{-}$ ionn has 3 electrons so $σ 1 s^{2} \overset{*}{σ} 1 s^{1}$

CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE

313723 The number of antibonding electron pairs in $O_{2}^{2 -}$ molecular ion on the basis of molecular orbital theory is (Atomic number of O is 8)

1 5

2 4

3 3

4 2

Explanation:

$O_{2}^{2 -}$ , no. of antibonding electron pairs = 4 pairs.
supporting img
Molecular orbital diagram of $O_{2}^{2 -}$ (peroxide ion)

CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE

313714 Molecular orbital electronic configuration for ' $X$ ' anion is $KK$ $σ^{*} 2 s^{2} σ^{*} 2 s^{2} π 2 p_{x}^{2} 2 p_{y}^{2} σ 2 p_{z}^{2} π^{*} 2 p_{x}^{1}$ , the anion ' $X$ ' is

1

N_{2}^{-}

2

O_{2}^{-}

3

N_{2}^{2 -}

4

O_{2}^{2 -}

Explanation:

In the given configuration, total number of electrons of anion $X = 15$
Hence; the anion $X$ is $N_{2}^{-}$ (15 electrons)
$[O_{2}^{-} (17 e^{-}), N_{2}^{- 2} (16 e^{-}), O_{2}^{- 2} (18 e^{-})]$

CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE

313712 In which of the following sets, all the species are diamagnetic in nature?

1

[O_{2}^{2 -}, O_{2}^{2 +}, N_{2}^{2 -}]

2

[C_{2}, O_{2}^{2 -}, N_{2}^{2 +}]

3

[O_{2}^{2 -}, O_{2}^{+}, O_{2}^{2 +}]

4

[N_{2}^{+}, O_{2}^{2 +}, B_{2}]

Explanation:

$C_{2} - 12 e^{-}, O_{2}^{- 2} - 18 e^{-}, N_{2}^{+ 2} \to 12 e^{-} \to$ all are diamagnetic
$O_{2}^{- 2} - 18 e^{-}, O_{2}^{+ 2} - 14 e^{-} (Dia) &$
$N_{2}^{- 2} (16 e^{-})$ paramagnetic
$O_{2}^{- 2} - 18 e^{-}, O_{2}^{+ 2} - 14 e^{-} ($ Dia $) &$
$O_{2}^{+} (15 e^{-})$ paramagnetic
$O_{2}^{+ 2} - 14 e^{-}$ ,diamagnetic,
$B_{2} \to 10 e^{-}, N_{2}^{+} \to 13 e^{-} \Rightarrow$ paramagnetic
Hint: All odd no. $e^{-}, 10, 16 \to$ paramagnetic
All even no. of $e^{-}$ (except 10,16) $\to$
Diamagnetic

CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE

313713 The molecular electronic configuration of $H_{2}^{-}$ ion is

1

(σ ls)^{2}

2

(σ 1 s)^{2} {(σ^{*} 1 s)}^{2}

3

(σ 1 s)^{2} {(σ^{*} 1 s)}^{1}

4

(σ 1 s)^{3}

Explanation:

$H_{2}^{-}$ ionn has 3 electrons so $σ 1 s^{2} \overset{*}{σ} 1 s^{1}$

CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE

313723 The number of antibonding electron pairs in $O_{2}^{2 -}$ molecular ion on the basis of molecular orbital theory is (Atomic number of O is 8)

1 5

2 4

3 3

4 2

Explanation:

$O_{2}^{2 -}$ , no. of antibonding electron pairs = 4 pairs.
supporting img
Molecular orbital diagram of $O_{2}^{2 -}$ (peroxide ion)

CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE

313714 Molecular orbital electronic configuration for ' $X$ ' anion is $KK$ $σ^{*} 2 s^{2} σ^{*} 2 s^{2} π 2 p_{x}^{2} 2 p_{y}^{2} σ 2 p_{z}^{2} π^{*} 2 p_{x}^{1}$ , the anion ' $X$ ' is

1

N_{2}^{-}

2

O_{2}^{-}

3

N_{2}^{2 -}

4

O_{2}^{2 -}

Explanation:

In the given configuration, total number of electrons of anion $X = 15$
Hence; the anion $X$ is $N_{2}^{-}$ (15 electrons)
$[O_{2}^{-} (17 e^{-}), N_{2}^{- 2} (16 e^{-}), O_{2}^{- 2} (18 e^{-})]$

Explanation:

Explanation:

Explanation:

Explanation:

Explanation:

Explanation:

Explanation:

Explanation:

Question Bank Series

Explanation:

Explanation:

Explanation:

Explanation:

Explanation:

Explanation:

Explanation:

Explanation: