Question

arrange the following as stated
1)N,O,F,Cl (increasing order of electron gain enthalpy)
2) F,O,N,Cl (increasing order of electronnegativity)
3)P,N,S,O (increasing orer of ionizationenthalpy)

Answer 1

Answer:

Electron gain enthalpy is the amount of energy required when one electron is added to the isolated gaseous atom.

1) Cl > F > O > N

This is because electron gain enthalpy decreases down the group and increases along the period.

Electronegativity is defined as tendency to attract pair of electrons.

2) F > O > N=Cl

Since electronegativity increase along the period.

Ionization enthalpy is defined as the minimum energy required to remove an electron from its atom in isolated state

3) O >N > P > S

Here, it is because it decreases moving down the group and increases along period.

Answer 2

Answer:

We know,Halogens have highest negative value of electron gain enthalpy. Here Cl and F both are halogens but electron gain enthalpy of Cl is more negative than F because of very small size of F which causes interelectronic repulsion among its electrons.