Why nitrogen shows catenation properties less than phosphorus?

Catenation power of nitrogen is less because N-N bond is weaker than the single P-P bond. N-N single bond is weaker than P-P bond is due to smaller size of nitrogen atom there is stronger inter electronic repulsion between nitrogen atoms hence it form strong pπ–pπ multiple bond and become diatomic molecule.

Related Questions:

Which is more basic N(CH3)3 or N(SiH3)3 , explain?

Are all the five bonds of PCl5 equivalent? Justify your answer.

Trisilyl amine, N(SiH3)3 is planar whereas trimethyl amines N(CH3)3 is pyramidal. Explain why?.

What are common structural features of oxides (P4O6 and P4O5) of phosphorous?

What are the structural difference between oxides ( P4O6 and P4O10) of phosphorous?

What are abnormal behaviour of Nitrogen atom as compared to other family members?

What is product obtained when N2O5 is treated with NaCl?

What is metaphophoric (HPO3)?

Phosphorus can form PCl5 but nitrogen can not form NCl5 why?

Why PCl3 hydrolysed while NCl3 can not be hydrolysed? 

Why bond angle of hydrides of group 15, decreases down the group?

What is "calgon" ? Give structure and its uses?

Why nitrogen shows catenation properties less than phosphorus?

Why Nitrogen is fairly inert gas?

Why Nitrogen (N2) is less reactive at room temperature?

Why Nitrogen dioxide (NO2) dimerises to form Dinitrogen tetraoxide (N2O4)?

Why Nitrogen dioxide (NO2) is coloured but Dinitrogen tetraoxide (N2O4) is colourless?

Hypophosphorous acid (H3PO2) and Phosphorous acid (H3PO3) act as as good reducing agents while H3PO4 does not.Why?

Which will have very fast tendency to dimerized ClO2 or NO and why?

In case of ClO₂ odd electron is delocalized over 3 atoms so extent of delocalization of odd electron is higher in comparison to NO. Hence tendency of demerisation of a NO is faster that of ClO₂.

Although electron affinity of chlorine is higher than fluorine, yet fluorine act as better oxidizing agent than chlorine? Explain.

Oxidizing character of elements calculated in aqueous medium while electron affinity is the term related to gaseous state.

Since fluorine possesses small size and high negative charge density thus undergoes more hydration as compared to chlorine as result of which its hydration energy increases than electron affinity and thus fluorine takes electron easily in aqueous medium and act as best oxidizing agent.The another reason of high oxidizing power of fluorine is its low bond dissociation energy as compare to chlorine.

Related Questions:

Although electron affinity of chlorine is higher than fluorine, yet fluorine act as better oxidizing agent than chlorine? Explain.

Why chlorine trifluoride (ClF3) exists but fluorine trichloride (FCl3) does not?

Why Chlorine (Cl2) bleaches a substance permanently but sulphuredioxide (SO2) does it temporarily?

What is the correct order of electronegativity of Cl atoms in HClO, HClO2, HClO3 and HClO4 ?

How does the thermal stability of oxy acids of chlorine increase with an increase in the oxidation state of chlorine atom ?

Which of the following is a strongest acid among oxy acids of chlorine and why? "HClO, HClO2, HClO3, HClO4"

Which will have very fast tendency to dimerized ClO2 or NO and why?