Question

Arrange N, S, O and F in order of decreasing electron gain enthalpy​

Answer 1

Answer:

Electron affinity increases as you add more valence electron. That puts oxygen (O) as having more electron affinity than (N). So, O>N

Electron affinity would typically decrease as you move down the periodic table.

But there is a factor in the second period of elements due to the close distance or the orbital from the nucleus so that repulsion of an electron from each other reduce electron affinity.

So, S>O>N 

Answer 2

The arrangement of N, S, O, and F in order of decreasing electron gain enthalpy​ would be F>S>O>N.

• Electron gain enthalpy can be defined as the amount of energy that is released or absorbed when a neutral isolated gaseous atom accepts an electron to form a negatively charged anion.
• The energy in this reaction can either be released or absorbed when the electron combines with the isolated gaseous atom.
• The more energy released during the combining process, the greater the electron gain enthalpy which is denoted by
• In the periodic table on moving left to right in a period electron affinity increases due to an increase in electronegativity (tendency to attract electrons)
• In the periodic table on moving down, as the atomic radii increase, therefore electron affinity decreases.
• The electron gain enthalpy of sulfur is more than oxygen due to the small size of oxygen.
• Extra added electron in oxygen has more interelectronic repulsion than sulfur which has a large size.
• F>S>O>N is the order of decreasing electron gain enthalpy​ from Fluorine(F) to Nitrogen(N)

Hence, The arrangement of N, S, O, and F in order of decreasing electron gain enthalpy​ would be F>S>O>N.

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