Which of the following elements will have the lowest electron affinity Nitrogen Phosphorus Chlorine Flourine

To answer this question, we need to understand what electron affinity is. Electron affinity is the amount of energy released when an electron is added to a neutral atom to form a negative ion.

In the periodic table, electron affinity generally increases from left to right and decreases from top to bottom. This is due to the increase in nuclear charge from left to right and the increase in atomic radius from top to bottom.

Given the elements Nitrogen, Phosphorus, Chlorine, and Fluorine:

1. Nitrogen is in period 2, group 15 of the periodic table.
2. Phosphorus is in period 3, group 15 of the periodic table.
3. Chlorine is in period 3, group 17 of the periodic table.
4. Fluorine is in period 2, group 17 of the periodic table.

From this information, we can see that Nitrogen and Fluorine are in the same period (period 2), but Fluorine is more to the right, so it will have a higher electron affinity.

Phosphorus and Chlorine are in the same period (period 3), but Chlorine is more to the right, so it will have a higher electron affinity.

Comparing Nitrogen and Phosphorus, which are in the same group (group 15), Phosphorus is lower, so it will have a lower electron affinity.

Therefore, out of Nitrogen, Phosphorus, Chlorine, and Fluorine, Phosphorus will have the lowest electron affinity.