Question

Arrange the elements Nitrogen, Phosphorus, Oxygen and Sulphur in increasing order of first Ionization Enthalpy.

Answer 1

Phosphorus<Nitrogen<Sulphur<Oxygen 

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Answer 2

Answer: Increasing order of first ionization enthalpy is given by: $\text{Sulfur}<\text{Phosphorous}<\text{Oxygen}<\text{Nitrogen}$

Explanation:

Ionization energy is defined as the energy required by an isolated gaseous atom to remove the outermost electron.

$X(g)\rightarrow X^+(g)+e^-$

Ionization energy increases as we move from left to right in a period and decreases as we move from top to bottom in a group.

Nitrogen atom belongs to Group 15 and Period 2.

Phosphorous belongs to Group 15 and Period 3.

Oxygen atom belongs to Group 16 and Period 2.

Sulfur atom belongs to Group 16 and Period 3.

Nitrogen and Phosphorus have half filled electronic configuration (stable configuration) while oxygen and sulfur doesn't have.

Therefore, Nitrogen will require more energy than oxygen and Phosphorus will require more energy than sulfur.

Hence, the increasing order of first ionization enthalpy is given by: $\text{Sulfur}<\text{Phosphorous}<\text{Oxygen}<\text{Nitrogen}$