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In N(2)O(5) valence of nitrogen is...

In `N_(2)O_(5)` valence of nitrogen is

A

2

B

3

C

4

D

5

Text Solution

Verified by Experts

The correct Answer is:
B
`N_(2)O_(5)`has the structure
`{:(" O O"),(" \\ /"),(" N - O - N"),(" / \\"),(" O O"):}`
In `N_(2)O_(5)`,N has a covalency of 3.
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Why valency of nitrogen is 3?

Nitrogen forms the largest number of oxides as it is capable of forming stable multiple bonds with oxygen. They range of N_(2)O (O.S of nitrogen +1) through NO, N_(2)O_(3),NO_(2),N_(2)O_(4) "to" N_(2)O_(5) (O.S of nitrogen +5). Following points are improtant regarding the study of oxides of nitrogen. (a) All oxides of nitrogen expect N_(2)O_(5) are endothermic as a large amount of energy is required to dissociate the stable molecule of oxygen and nitrogen. (b) The small electronegativity difference between oxygen and nitrogen make N-O bond easily breakle to give oxygen and hence oxides of nitrogen are said to be better oxidising agents. (c) Expect N_(2)O_(5) , all are gases at ordinary temperature. N_(2)O_(3) is stable only at lower temperature (253K). (d) Expect N_(2)O and NO which are neutal oxides, all are acidic oxides which dissolve in water forming coresponding oxy acids. (e) They are also good example for illustrating the concept of resonance. The gas which is acidic in nature is :

Knowledge Check

  • Nitrogen forms the largest number of oxides as it is capable of forming stable multiple bonds with oxygen. They range from N_(2)O (O.S of nitrogen +1) through NO, N_(2)O_(3), NO_(2), N_(2)O_(4), " to " N_(2)O_(5) (O.S of nitrogen +5). Following points are important regarding the study of oxides of nitrogen (a) All oxides of nitrogen except N_(2)O_(5) are endothermic as a large amount of energy is required to dissociate the stable molecule of oxygen and nitrogen. (b) The small electronegativity difference between oxygen and nitrogen make N - O bond easily breakble to give oxygen and hence oxides of nitrogen are said to be better oxidising agents. (c) Except N_(2)O_(5) , all are gases at ordinary temperature N_(2)O_(3) is stable only at lower temperature (253 K). (d) Except N_(2)O and NO which are neutral oxides, all are acidic oxides which dissolve in water forming corresponding oxy acids. (e) They are also good example for illustrating the concept of resonance Which of the following statements is correct for the oxides of nitrogen ?

    A
    Dinitrogen trioxide dissolves in potassium hydroxide forming potassium nitrate
    B
    Aqueous solution of nitrogen dioxide behaves both as a reducing agent and as an oxidising agent
    C
    Nitrous oxide is fairly soluble in cold water and turns blue litmus red
    D
    Nitrogen dioxide is not acidic oxide

  • Nitrogen forms the largest number of oxides as it is capable of forming stable multiple bonds with oxygen. They range of N_(2)O (O.S of nitrogen +1) through NO, N_(2)O_(3),NO_(2),N_(2)O_(4) to N_(2)O_(5) (O.S of nitrogen +5). Following points are improtant regarding the study of oxides of nitrogen. (a) All oxides of nitrogen expect N_(2)O_(5) are endothermic as a large amount of energy is required to dissociate the stable molecule of oxygen and nitrogen. (b) The small electronegativity difference between oxygen and nitrogen make N-O bond easily breakle to give oxygen and hence oxides of nitrogen are said to be better oxidising agents. (c) Expect N_(2)O_(5) , all are gases at ordinary temperature. N_(2)O_(3) is stable only at lower temperature (253K). (d) Expect N_(2)O and NO which are neutal oxides, all are acidic oxides which dissolve in water forming coresponding oxy acids. (e) They are also good example for illustrating the concept of resonance. Which of the following statements is corect for the oxides of nitrogen?

    A
    Dinitrogen trioxide dissolves in potassium hydroxide forming potassium nitrate.
    B
    Aqueuous slution of nitrogen dixide behaves both as a reducing agent and as a oxidising agent.
    C
    Nitrogen oxide is fairly soluble in cold water and turns blue litmus red.
    D
    Nitrogen dioxide is not acidic oxide.

  • In N_2O_4 oxidation state of nitrogen is

    A
    `-4`
    B
    `+4`
    C
    `-3`
    D
    `+3`

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    If density of a gaseous mixture of dinitrogen tetroxide (N_(2)O_(4)) and nitrogen dioxide (NO)_(2) is 2.5 gm/L at 127^(@)C and 1 atm pressure. [R=0.08 atm lit/mole-k] K_(p) for N_(2)O_(4)(g)hArr2NO_(2) is:

    If density of a gaseous mixture of dinitrogen tetroxide (N_(2)O_(4)) and nitrogen dioxide (NO)_(2) is 2.5 gm/L at 127^(@)C and 1 atm pressure. [R=0.08 atm lit/mole-k] Partial pressure of N_(2)O_(4) is:

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    NO_(2) and N_(2)O_(4) are two forms of nitrogen dioxide. One exists in gaseous state while other in liquid state. The nature of NO_(2) and N_(2)O_(4) forms are

    Assertion : The covalence of nitrogen in N_(2)O_(5) is 5 Reason : Nitrogen can expand its covalence beyond 4.

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