Question

How many of the following elements have first
ionisation energy greater than that of sulphur?
AI, Si, N, O, F, P, CI, Na, Ne​

Answer 1

Answer:

Explanation:

Either all unpaired or all paired makes it stable, so if phosphorus is all unpaired it take more energy to remove an electron than it would from sulfur in which one electron can be removed making it more stable. Because it takes more energy for phosphorus, it has a higher ionization energy.

The decreasing order of the ionization potential of the following elements is Ne>Cl>P>S>Mg>Al. First ionization potential of Mg is higher than that of AI.

Answer 2

From the following elements Ne, Cl, and P have their first ionization energy greater than that of sulfur.

• The first ionization energy of an element is the energy required to transfer the first valence electron of the element to the infinite shell.
• Elements that have a completely filled valence electronic configuration (Neon 2s²2p⁶) or have a stable half-filled configuration (Nitrogen 2s²2p³) show a higher ionization enthalpy than the expected value.
• The ionization enthalpy decreases down the periodic table and increases from Group 1 to Group 17.
• Hence the order of ionization enthalpy is Ne > Cl > P > S > Mg > Al.