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CHXI08:REDOX REACTIONS

315172 Oxidation state of $N^{1}, N^{2} a n d N^{3}$ in the compound $H N_{3}$ (hydrazoic acid), shown in below figure, are:
supporting img

1

0, 0, 3

2

0, 0, - 1

3

1, 1, - 3

4

- 3, - 3, - 3

Explanation:

supporting img
$N^{1}$ and $N^{2}$ has oxidation state zero because they
are linked to each other.
For $N^{3}, X + 0 + 0 + 1 = 0$
$X = - 1$

CHXI08:REDOX REACTIONS

315173 The oxidation numbers of manganese in ${KMnO}_{4}$ , ${MnSO}_{4}$ and $K_{2} {MnO}_{4}$ are

1

+ 7, + 2, + 6

respectively

2

+ 6, + 5, + 4

respectively

3

+ 2, + 3, + 4

respectively

4

+ 7, + 6, + 4

respectively

CHXI08:REDOX REACTIONS

315174 Oxidation state of nitrogen is correctly given for
$Compound Oxidation state$

1

{Mg}_{3} N_{2} - 3

2

N H_{2} OH + 1

3

{(N_{2} H_{5})}_{2} S O_{4} + 2

4

[Co {(N H_{3})}_{5} Cl] C l_{2} 0

Explanation:

The oxidation number of nitrogen in different compounds area.
$a . {Mg}_{3} N_{2} (- 3)$
$b . N H_{2} OH (- 1)$
$c . {(N_{2} H_{5})}_{2} S O_{4} (- 2)$
$d . [Co {(N H_{3})}_{5} Cl] C l_{2} (- 3)$

CHXI08:REDOX REACTIONS

315175 Oxidation number of $N$ in ${HNO}_{3}$ is

1 -3.5

2 +3.5

3

- 3, + 5

4 +5

Explanation:

Let the oxidation state of N in
$H N O_{3} = x$
$+ 1 + x + (- 2 \times 3) = 0$
$o r \underset{(+ 2)}{x} + 1 - 6 = 0 \Rightarrow x = + 5$

CHXI08:REDOX REACTIONS

315176 In which of the following metal atom has negative oxidation state.
$\begin{array}{ccc} CuH, & [Fe (CO)]^{2 -}, & Na - Hg \\ I & II & III \end{array}$

1 I, II and III

2 II

3 I and III

4 II and III

Explanation:

$Fe$ in $[Fe (CO)]^{2 -}$ has $- 2$ oxidation state.

CHXI08:REDOX REACTIONS

315172 Oxidation state of $N^{1}, N^{2} a n d N^{3}$ in the compound $H N_{3}$ (hydrazoic acid), shown in below figure, are:
supporting img

1

0, 0, 3

2

0, 0, - 1

3

1, 1, - 3

4

- 3, - 3, - 3

Explanation:

supporting img
$N^{1}$ and $N^{2}$ has oxidation state zero because they
are linked to each other.
For $N^{3}, X + 0 + 0 + 1 = 0$
$X = - 1$

CHXI08:REDOX REACTIONS

315173 The oxidation numbers of manganese in ${KMnO}_{4}$ , ${MnSO}_{4}$ and $K_{2} {MnO}_{4}$ are

1

+ 7, + 2, + 6

respectively

2

+ 6, + 5, + 4

respectively

3

+ 2, + 3, + 4

respectively

4

+ 7, + 6, + 4

respectively

CHXI08:REDOX REACTIONS

315174 Oxidation state of nitrogen is correctly given for
$Compound Oxidation state$

1

{Mg}_{3} N_{2} - 3

2

N H_{2} OH + 1

3

{(N_{2} H_{5})}_{2} S O_{4} + 2

4

[Co {(N H_{3})}_{5} Cl] C l_{2} 0

Explanation:

The oxidation number of nitrogen in different compounds area.
$a . {Mg}_{3} N_{2} (- 3)$
$b . N H_{2} OH (- 1)$
$c . {(N_{2} H_{5})}_{2} S O_{4} (- 2)$
$d . [Co {(N H_{3})}_{5} Cl] C l_{2} (- 3)$

CHXI08:REDOX REACTIONS

315175 Oxidation number of $N$ in ${HNO}_{3}$ is

1 -3.5

2 +3.5

3

- 3, + 5

4 +5

Explanation:

Let the oxidation state of N in
$H N O_{3} = x$
$+ 1 + x + (- 2 \times 3) = 0$
$o r \underset{(+ 2)}{x} + 1 - 6 = 0 \Rightarrow x = + 5$

CHXI08:REDOX REACTIONS

315176 In which of the following metal atom has negative oxidation state.
$\begin{array}{ccc} CuH, & [Fe (CO)]^{2 -}, & Na - Hg \\ I & II & III \end{array}$

1 I, II and III

2 II

3 I and III

4 II and III

Explanation:

$Fe$ in $[Fe (CO)]^{2 -}$ has $- 2$ oxidation state.

CHXI08:REDOX REACTIONS

315172 Oxidation state of $N^{1}, N^{2} a n d N^{3}$ in the compound $H N_{3}$ (hydrazoic acid), shown in below figure, are:
supporting img

1

0, 0, 3

2

0, 0, - 1

3

1, 1, - 3

4

- 3, - 3, - 3

Explanation:

supporting img
$N^{1}$ and $N^{2}$ has oxidation state zero because they
are linked to each other.
For $N^{3}, X + 0 + 0 + 1 = 0$
$X = - 1$

CHXI08:REDOX REACTIONS

315173 The oxidation numbers of manganese in ${KMnO}_{4}$ , ${MnSO}_{4}$ and $K_{2} {MnO}_{4}$ are

1

+ 7, + 2, + 6

respectively

2

+ 6, + 5, + 4

respectively

3

+ 2, + 3, + 4

respectively

4

+ 7, + 6, + 4

respectively

CHXI08:REDOX REACTIONS

315174 Oxidation state of nitrogen is correctly given for
$Compound Oxidation state$

1

{Mg}_{3} N_{2} - 3

2

N H_{2} OH + 1

3

{(N_{2} H_{5})}_{2} S O_{4} + 2

4

[Co {(N H_{3})}_{5} Cl] C l_{2} 0

Explanation:

The oxidation number of nitrogen in different compounds area.
$a . {Mg}_{3} N_{2} (- 3)$
$b . N H_{2} OH (- 1)$
$c . {(N_{2} H_{5})}_{2} S O_{4} (- 2)$
$d . [Co {(N H_{3})}_{5} Cl] C l_{2} (- 3)$

CHXI08:REDOX REACTIONS

315175 Oxidation number of $N$ in ${HNO}_{3}$ is

1 -3.5

2 +3.5

3

- 3, + 5

4 +5

Explanation:

Let the oxidation state of N in
$H N O_{3} = x$
$+ 1 + x + (- 2 \times 3) = 0$
$o r \underset{(+ 2)}{x} + 1 - 6 = 0 \Rightarrow x = + 5$

CHXI08:REDOX REACTIONS

315176 In which of the following metal atom has negative oxidation state.
$\begin{array}{ccc} CuH, & [Fe (CO)]^{2 -}, & Na - Hg \\ I & II & III \end{array}$

1 I, II and III

2 II

3 I and III

4 II and III

Explanation:

$Fe$ in $[Fe (CO)]^{2 -}$ has $- 2$ oxidation state.

CHXI08:REDOX REACTIONS

315172 Oxidation state of $N^{1}, N^{2} a n d N^{3}$ in the compound $H N_{3}$ (hydrazoic acid), shown in below figure, are:
supporting img

1

0, 0, 3

2

0, 0, - 1

3

1, 1, - 3

4

- 3, - 3, - 3

Explanation:

supporting img
$N^{1}$ and $N^{2}$ has oxidation state zero because they
are linked to each other.
For $N^{3}, X + 0 + 0 + 1 = 0$
$X = - 1$

CHXI08:REDOX REACTIONS

315173 The oxidation numbers of manganese in ${KMnO}_{4}$ , ${MnSO}_{4}$ and $K_{2} {MnO}_{4}$ are

1

+ 7, + 2, + 6

respectively

2

+ 6, + 5, + 4

respectively

3

+ 2, + 3, + 4

respectively

4

+ 7, + 6, + 4

respectively

CHXI08:REDOX REACTIONS

315174 Oxidation state of nitrogen is correctly given for
$Compound Oxidation state$

1

{Mg}_{3} N_{2} - 3

2

N H_{2} OH + 1

3

{(N_{2} H_{5})}_{2} S O_{4} + 2

4

[Co {(N H_{3})}_{5} Cl] C l_{2} 0

Explanation:

The oxidation number of nitrogen in different compounds area.
$a . {Mg}_{3} N_{2} (- 3)$
$b . N H_{2} OH (- 1)$
$c . {(N_{2} H_{5})}_{2} S O_{4} (- 2)$
$d . [Co {(N H_{3})}_{5} Cl] C l_{2} (- 3)$

CHXI08:REDOX REACTIONS

315175 Oxidation number of $N$ in ${HNO}_{3}$ is

1 -3.5

2 +3.5

3

- 3, + 5

4 +5

Explanation:

Let the oxidation state of N in
$H N O_{3} = x$
$+ 1 + x + (- 2 \times 3) = 0$
$o r \underset{(+ 2)}{x} + 1 - 6 = 0 \Rightarrow x = + 5$

CHXI08:REDOX REACTIONS

315176 In which of the following metal atom has negative oxidation state.
$\begin{array}{ccc} CuH, & [Fe (CO)]^{2 -}, & Na - Hg \\ I & II & III \end{array}$

1 I, II and III

2 II

3 I and III

4 II and III

Explanation:

$Fe$ in $[Fe (CO)]^{2 -}$ has $- 2$ oxidation state.

CHXI08:REDOX REACTIONS

315172 Oxidation state of $N^{1}, N^{2} a n d N^{3}$ in the compound $H N_{3}$ (hydrazoic acid), shown in below figure, are:
supporting img

1

0, 0, 3

2

0, 0, - 1

3

1, 1, - 3

4

- 3, - 3, - 3

Explanation:

supporting img
$N^{1}$ and $N^{2}$ has oxidation state zero because they
are linked to each other.
For $N^{3}, X + 0 + 0 + 1 = 0$
$X = - 1$

CHXI08:REDOX REACTIONS

315173 The oxidation numbers of manganese in ${KMnO}_{4}$ , ${MnSO}_{4}$ and $K_{2} {MnO}_{4}$ are

1

+ 7, + 2, + 6

respectively

2

+ 6, + 5, + 4

respectively

3

+ 2, + 3, + 4

respectively

4

+ 7, + 6, + 4

respectively

CHXI08:REDOX REACTIONS

315174 Oxidation state of nitrogen is correctly given for
$Compound Oxidation state$

1

{Mg}_{3} N_{2} - 3

2

N H_{2} OH + 1

3

{(N_{2} H_{5})}_{2} S O_{4} + 2

4

[Co {(N H_{3})}_{5} Cl] C l_{2} 0

Explanation:

The oxidation number of nitrogen in different compounds area.
$a . {Mg}_{3} N_{2} (- 3)$
$b . N H_{2} OH (- 1)$
$c . {(N_{2} H_{5})}_{2} S O_{4} (- 2)$
$d . [Co {(N H_{3})}_{5} Cl] C l_{2} (- 3)$

CHXI08:REDOX REACTIONS

315175 Oxidation number of $N$ in ${HNO}_{3}$ is

1 -3.5

2 +3.5

3

- 3, + 5

4 +5

Explanation:

Let the oxidation state of N in
$H N O_{3} = x$
$+ 1 + x + (- 2 \times 3) = 0$
$o r \underset{(+ 2)}{x} + 1 - 6 = 0 \Rightarrow x = + 5$

CHXI08:REDOX REACTIONS

315176 In which of the following metal atom has negative oxidation state.
$\begin{array}{ccc} CuH, & [Fe (CO)]^{2 -}, & Na - Hg \\ I & II & III \end{array}$

1 I, II and III

2 II

3 I and III

4 II and III

Explanation:

$Fe$ in $[Fe (CO)]^{2 -}$ has $- 2$ oxidation state.