Study the part of the Periodic Table given below and answer the questions that follow: (Do not identify the elements)
| 1 | 2 | 13 | 14 | 15 | 16 | 17 | 18 |
|---|---|---|---|---|---|---|---|
| J | Q | ||||||
| L | |||||||
| M | O | P | |||||
| N | G |
(a) Draw the dot (.) and cross (×) structure of the compound formed between elements L and P.
(b) Which element has the highest ionization potential?
(c) Element N is more reactive than M. Justify.
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(a) L belongs to Group 2 (valency 2, forms L2+) and P belongs to Group 17 (valency 1, forms P-). One atom of L transfers one electron each to two atoms of P, forming the electrovalent compound LP2.
(b) Q — It is a noble gas placed at the top of Group 18 (rightmost and highest in the table), where the atomic size is smallest and the outermost electrons are most tightly held, giving it the highest ionization potential.
(c) Both M and N belong to Group 1. Going down the group, the atomic size increases and the outermost electron is held less tightly by the nucleus, so it is lost more easily. Since N lies below M in the group, N loses its valence electron more readily and is therefore more reactive than M.