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CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE

313469 In which of the following conversion, bond length increases?
(P) $NO \to {NO}^{+}$
(Q) $N_{2}^{+} \to N_{2}^{-}$
(R) $O_{2} \to O_{2}^{+}$
(S) $H_{2} \to H_{2}^{+}$

1 P and Q

2 Q and R

3 Q and S

4 P, Q and R

Explanation:

Bond length $\propto \frac{1}{Bond order}$ ,
if BO same, BL depends on no. of antibonding electrons
(P) $NO \to {NO}^{+}$ (B. O. increases 2.5 to 3 ).
(Q) $N_{2}^{+} \to N_{2}^{-}$ [B.O. is same (2.5) but no. of
antibonding electrons increase So, bond length increases.]
(R) $O_{2} \to O_{2}^{+}$ (Bond order increase, 2 to 2.5)
(S) $H_{2} \to H_{2}^{+}$ (Bond order decrease, 1 to 0.5 )

CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE

313470 The correct order of increasing bond length of C - H, C - O, C - C and C = C is

1 C - H < C - O < C - C < C = C

2 C - H < C = C < C - O < C - C

3 C - C < C = C < C - O < C - H

4 C - O < C - H < C - C < C = C

Explanation:

The bond lengths are:
$\underset{107 p m}{C - H} < \underset{134 p m}{C = C} < \underset{141 p m}{C - O} < \underset{154 p m}{C - C}$

CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE

313471 Bond length depends upon the size of atoms, hybridisation, resonance, bond order etc. In the following relations,
I. Bond length $\propto$ size of atoms
II. Bond length $\propto$ hybridisation (no. of hybrid
III. Bond length $\propto$ bond order
Choose the correct option.

1 I and II

2 Only I

3 I and III

4 I, II and III

Explanation:

Statements I and II are correct while the statement III is incorrect. It’s correct form is as follows:
Bond length is inversely proportional to bond order.
$B o n d l e n g t h \propto \frac{1}{b o n d o r d e r}$
So, the option (1) is correct.

CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE

313472 Match Column I and Column II
Column I
Column II
supporting img

1 A - S, B - R, C - Q, D - P

2 A - P, B - Q, C - R, D - S

3 A - Q, B - R, C - S, D - P

4 A - Q, B - S, C - R, D - P

Explanation:

Bond length $\propto$ radii of atom. order of radii of atom :
$C > O > F > H$
so, $H - C > H - O > F - H > H - H$ .
So, correct option is (3).

CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE

313473 Assertion :
Molecular nitrogen is less reactive than molecular oxygen.
Reason :
The bond length of $N_{2}$ is shorter than that of oxygen.

1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.

2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.

3 Assertion is correct but Reason is incorrect.

4 Assertion is incorrect but Reason is correct.

Explanation:

$\underset{Dinitrogen}{N \equiv N} \underset{Dioxygen}{O = O}$
Molecular nitrogen has a triple bond. Whereas, molecular oxygen has a double bond. Triple bond is shorter than the double bond. Shorter the bond , higher the bond dissociation energy, higher the stability and lesser the reactivity. So the option (1) is correct.

CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE

313469 In which of the following conversion, bond length increases?
(P) $NO \to {NO}^{+}$
(Q) $N_{2}^{+} \to N_{2}^{-}$
(R) $O_{2} \to O_{2}^{+}$
(S) $H_{2} \to H_{2}^{+}$

1 P and Q

2 Q and R

3 Q and S

4 P, Q and R

Explanation:

Bond length $\propto \frac{1}{Bond order}$ ,
if BO same, BL depends on no. of antibonding electrons
(P) $NO \to {NO}^{+}$ (B. O. increases 2.5 to 3 ).
(Q) $N_{2}^{+} \to N_{2}^{-}$ [B.O. is same (2.5) but no. of
antibonding electrons increase So, bond length increases.]
(R) $O_{2} \to O_{2}^{+}$ (Bond order increase, 2 to 2.5)
(S) $H_{2} \to H_{2}^{+}$ (Bond order decrease, 1 to 0.5 )

CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE

313470 The correct order of increasing bond length of C - H, C - O, C - C and C = C is

1 C - H < C - O < C - C < C = C

2 C - H < C = C < C - O < C - C

3 C - C < C = C < C - O < C - H

4 C - O < C - H < C - C < C = C

Explanation:

The bond lengths are:
$\underset{107 p m}{C - H} < \underset{134 p m}{C = C} < \underset{141 p m}{C - O} < \underset{154 p m}{C - C}$

CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE

313471 Bond length depends upon the size of atoms, hybridisation, resonance, bond order etc. In the following relations,
I. Bond length $\propto$ size of atoms
II. Bond length $\propto$ hybridisation (no. of hybrid
III. Bond length $\propto$ bond order
Choose the correct option.

1 I and II

2 Only I

3 I and III

4 I, II and III

Explanation:

Statements I and II are correct while the statement III is incorrect. It’s correct form is as follows:
Bond length is inversely proportional to bond order.
$B o n d l e n g t h \propto \frac{1}{b o n d o r d e r}$
So, the option (1) is correct.

CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE

313472 Match Column I and Column II
Column I
Column II
supporting img

1 A - S, B - R, C - Q, D - P

2 A - P, B - Q, C - R, D - S

3 A - Q, B - R, C - S, D - P

4 A - Q, B - S, C - R, D - P

Explanation:

Bond length $\propto$ radii of atom. order of radii of atom :
$C > O > F > H$
so, $H - C > H - O > F - H > H - H$ .
So, correct option is (3).

CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE

313473 Assertion :
Molecular nitrogen is less reactive than molecular oxygen.
Reason :
The bond length of $N_{2}$ is shorter than that of oxygen.

1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.

2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.

3 Assertion is correct but Reason is incorrect.

4 Assertion is incorrect but Reason is correct.

Explanation:

$\underset{Dinitrogen}{N \equiv N} \underset{Dioxygen}{O = O}$
Molecular nitrogen has a triple bond. Whereas, molecular oxygen has a double bond. Triple bond is shorter than the double bond. Shorter the bond , higher the bond dissociation energy, higher the stability and lesser the reactivity. So the option (1) is correct.

CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE

313469 In which of the following conversion, bond length increases?
(P) $NO \to {NO}^{+}$
(Q) $N_{2}^{+} \to N_{2}^{-}$
(R) $O_{2} \to O_{2}^{+}$
(S) $H_{2} \to H_{2}^{+}$

1 P and Q

2 Q and R

3 Q and S

4 P, Q and R

Explanation:

Bond length $\propto \frac{1}{Bond order}$ ,
if BO same, BL depends on no. of antibonding electrons
(P) $NO \to {NO}^{+}$ (B. O. increases 2.5 to 3 ).
(Q) $N_{2}^{+} \to N_{2}^{-}$ [B.O. is same (2.5) but no. of
antibonding electrons increase So, bond length increases.]
(R) $O_{2} \to O_{2}^{+}$ (Bond order increase, 2 to 2.5)
(S) $H_{2} \to H_{2}^{+}$ (Bond order decrease, 1 to 0.5 )

CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE

313470 The correct order of increasing bond length of C - H, C - O, C - C and C = C is

1 C - H < C - O < C - C < C = C

2 C - H < C = C < C - O < C - C

3 C - C < C = C < C - O < C - H

4 C - O < C - H < C - C < C = C

Explanation:

The bond lengths are:
$\underset{107 p m}{C - H} < \underset{134 p m}{C = C} < \underset{141 p m}{C - O} < \underset{154 p m}{C - C}$

CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE

313471 Bond length depends upon the size of atoms, hybridisation, resonance, bond order etc. In the following relations,
I. Bond length $\propto$ size of atoms
II. Bond length $\propto$ hybridisation (no. of hybrid
III. Bond length $\propto$ bond order
Choose the correct option.

1 I and II

2 Only I

3 I and III

4 I, II and III

Explanation:

Statements I and II are correct while the statement III is incorrect. It’s correct form is as follows:
Bond length is inversely proportional to bond order.
$B o n d l e n g t h \propto \frac{1}{b o n d o r d e r}$
So, the option (1) is correct.

CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE

313472 Match Column I and Column II
Column I
Column II
supporting img

1 A - S, B - R, C - Q, D - P

2 A - P, B - Q, C - R, D - S

3 A - Q, B - R, C - S, D - P

4 A - Q, B - S, C - R, D - P

Explanation:

Bond length $\propto$ radii of atom. order of radii of atom :
$C > O > F > H$
so, $H - C > H - O > F - H > H - H$ .
So, correct option is (3).

CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE

313473 Assertion :
Molecular nitrogen is less reactive than molecular oxygen.
Reason :
The bond length of $N_{2}$ is shorter than that of oxygen.

1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.

2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.

3 Assertion is correct but Reason is incorrect.

4 Assertion is incorrect but Reason is correct.

Explanation:

$\underset{Dinitrogen}{N \equiv N} \underset{Dioxygen}{O = O}$
Molecular nitrogen has a triple bond. Whereas, molecular oxygen has a double bond. Triple bond is shorter than the double bond. Shorter the bond , higher the bond dissociation energy, higher the stability and lesser the reactivity. So the option (1) is correct.

CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE

313469 In which of the following conversion, bond length increases?
(P) $NO \to {NO}^{+}$
(Q) $N_{2}^{+} \to N_{2}^{-}$
(R) $O_{2} \to O_{2}^{+}$
(S) $H_{2} \to H_{2}^{+}$

1 P and Q

2 Q and R

3 Q and S

4 P, Q and R

Explanation:

Bond length $\propto \frac{1}{Bond order}$ ,
if BO same, BL depends on no. of antibonding electrons
(P) $NO \to {NO}^{+}$ (B. O. increases 2.5 to 3 ).
(Q) $N_{2}^{+} \to N_{2}^{-}$ [B.O. is same (2.5) but no. of
antibonding electrons increase So, bond length increases.]
(R) $O_{2} \to O_{2}^{+}$ (Bond order increase, 2 to 2.5)
(S) $H_{2} \to H_{2}^{+}$ (Bond order decrease, 1 to 0.5 )

CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE

313470 The correct order of increasing bond length of C - H, C - O, C - C and C = C is

1 C - H < C - O < C - C < C = C

2 C - H < C = C < C - O < C - C

3 C - C < C = C < C - O < C - H

4 C - O < C - H < C - C < C = C

Explanation:

The bond lengths are:
$\underset{107 p m}{C - H} < \underset{134 p m}{C = C} < \underset{141 p m}{C - O} < \underset{154 p m}{C - C}$

CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE

313471 Bond length depends upon the size of atoms, hybridisation, resonance, bond order etc. In the following relations,
I. Bond length $\propto$ size of atoms
II. Bond length $\propto$ hybridisation (no. of hybrid
III. Bond length $\propto$ bond order
Choose the correct option.

1 I and II

2 Only I

3 I and III

4 I, II and III

Explanation:

Statements I and II are correct while the statement III is incorrect. It’s correct form is as follows:
Bond length is inversely proportional to bond order.
$B o n d l e n g t h \propto \frac{1}{b o n d o r d e r}$
So, the option (1) is correct.

CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE

313472 Match Column I and Column II
Column I
Column II
supporting img

1 A - S, B - R, C - Q, D - P

2 A - P, B - Q, C - R, D - S

3 A - Q, B - R, C - S, D - P

4 A - Q, B - S, C - R, D - P

Explanation:

Bond length $\propto$ radii of atom. order of radii of atom :
$C > O > F > H$
so, $H - C > H - O > F - H > H - H$ .
So, correct option is (3).

CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE

313473 Assertion :
Molecular nitrogen is less reactive than molecular oxygen.
Reason :
The bond length of $N_{2}$ is shorter than that of oxygen.

1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.

2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.

3 Assertion is correct but Reason is incorrect.

4 Assertion is incorrect but Reason is correct.

Explanation:

$\underset{Dinitrogen}{N \equiv N} \underset{Dioxygen}{O = O}$
Molecular nitrogen has a triple bond. Whereas, molecular oxygen has a double bond. Triple bond is shorter than the double bond. Shorter the bond , higher the bond dissociation energy, higher the stability and lesser the reactivity. So the option (1) is correct.

CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE

313469 In which of the following conversion, bond length increases?
(P) $NO \to {NO}^{+}$
(Q) $N_{2}^{+} \to N_{2}^{-}$
(R) $O_{2} \to O_{2}^{+}$
(S) $H_{2} \to H_{2}^{+}$

1 P and Q

2 Q and R

3 Q and S

4 P, Q and R

Explanation:

Bond length $\propto \frac{1}{Bond order}$ ,
if BO same, BL depends on no. of antibonding electrons
(P) $NO \to {NO}^{+}$ (B. O. increases 2.5 to 3 ).
(Q) $N_{2}^{+} \to N_{2}^{-}$ [B.O. is same (2.5) but no. of
antibonding electrons increase So, bond length increases.]
(R) $O_{2} \to O_{2}^{+}$ (Bond order increase, 2 to 2.5)
(S) $H_{2} \to H_{2}^{+}$ (Bond order decrease, 1 to 0.5 )

CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE

313470 The correct order of increasing bond length of C - H, C - O, C - C and C = C is

1 C - H < C - O < C - C < C = C

2 C - H < C = C < C - O < C - C

3 C - C < C = C < C - O < C - H

4 C - O < C - H < C - C < C = C

Explanation:

The bond lengths are:
$\underset{107 p m}{C - H} < \underset{134 p m}{C = C} < \underset{141 p m}{C - O} < \underset{154 p m}{C - C}$

CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE

313471 Bond length depends upon the size of atoms, hybridisation, resonance, bond order etc. In the following relations,
I. Bond length $\propto$ size of atoms
II. Bond length $\propto$ hybridisation (no. of hybrid
III. Bond length $\propto$ bond order
Choose the correct option.

1 I and II

2 Only I

3 I and III

4 I, II and III

Explanation:

Statements I and II are correct while the statement III is incorrect. It’s correct form is as follows:
Bond length is inversely proportional to bond order.
$B o n d l e n g t h \propto \frac{1}{b o n d o r d e r}$
So, the option (1) is correct.

CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE

313472 Match Column I and Column II
Column I
Column II
supporting img

1 A - S, B - R, C - Q, D - P

2 A - P, B - Q, C - R, D - S

3 A - Q, B - R, C - S, D - P

4 A - Q, B - S, C - R, D - P

Explanation:

Bond length $\propto$ radii of atom. order of radii of atom :
$C > O > F > H$
so, $H - C > H - O > F - H > H - H$ .
So, correct option is (3).

CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE

313473 Assertion :
Molecular nitrogen is less reactive than molecular oxygen.
Reason :
The bond length of $N_{2}$ is shorter than that of oxygen.

1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.

2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.

3 Assertion is correct but Reason is incorrect.

4 Assertion is incorrect but Reason is correct.

Explanation:

$\underset{Dinitrogen}{N \equiv N} \underset{Dioxygen}{O = O}$
Molecular nitrogen has a triple bond. Whereas, molecular oxygen has a double bond. Triple bond is shorter than the double bond. Shorter the bond , higher the bond dissociation energy, higher the stability and lesser the reactivity. So the option (1) is correct.

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