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The solid oxide of nitrogen is N2 O....

The solid oxide of nitrogen is `N_2 O`.

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To determine whether the statement "The solid oxide of nitrogen is N2O" is true or false, we can follow these steps: ### Step 1: Identify the compound N2O - N2O is known as nitrous oxide. ### Step 2: Determine the physical state of N2O - Nitrous oxide (N2O) is commonly recognized as a gas at room temperature and pressure. ### Step 3: Identify the solid oxide of nitrogen - The solid oxide of nitrogen is actually dinitrogen pentoxide (N2O5), which is a white solid. ### Step 4: Compare the two compounds - Since N2O is a gas and not a solid, while N2O5 is a solid, we can conclude that the statement is false. ### Conclusion - The statement "The solid oxide of nitrogen is N2O" is **false**. The correct solid oxide of nitrogen is N2O5. ---
To determine whether the statement "The solid oxide of nitrogen is N2O" is true or false, we can follow these steps: ### Step 1: Identify the compound N2O - N2O is known as nitrous oxide. ### Step 2: Determine the physical state of N2O - Nitrous oxide (N2O) is commonly recognized as a gas at room temperature and pressure. ...
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Which of the following oxides of Nitrogen is Neutral

The enthalpy changes of formation of the gaseous oxides of nitrogen (N_(2)O and NO) are positive because of :

Which oxide of nitrogen is neutral ?

Out of the following oxides of nitrogen how many of them are neutral oxides? N_(2)O, NO, N_(2)O_(3), NO_(2),N_(2)O_(4), N_(2)O_(5)

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 :

Among the oxides of nitrogen N_(2)O, NO and NO_(2) , molecules with unpaired electrons are:

Among the oxides of nitrogen N_(2)O, NO and NO_(2) , molecules with unpaired electrons are:

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The oxidation number of nitrogen in NH_(2)OH is :