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Question

Explain the trends from metallic to non-metallic character of the different elements in the first three periods.

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Answer

On moving across a period, nuclear pull increases due to increase in atomic number and thus the atomic size decreases. Hence, the elements cannot lose electrons easily. Therefore, metallic nature decreases across a period moving from left to right and non-metallic character increases.
The alkali metals ( group 1 [IA]) and alkaline earth metals (group 2 [IIA]), placed on the left side of the table are most metallic in nature and the halogens (group 16 [VIA]) placed on the right side of the table are most non-metallic in nature.

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With reference to group 1 [IA] of the periodic table – fill in the blanks with the correct word:
The elements are …………… [light/heavy] …………… [metals/non metals] since their atomic size is …………… [large/small]. The energy binding the atoms is …………… [high/low] and hence the elements have …………… [high/low] melting points. The melting points of the elements …………… [increases/decreases] down the subgroup. The electropositive character …………… [increases/decreases] down the subgroup and the elements are strong …………… [reducing/oxidizing] agents. The element with electronic configuration 2, 8, 1 will have …………… [higher/lower] electron affinity and …………… [smaller/larger] atomic size than the element with electronic configuration 2, 1.

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In period 2, element ‘A’ is to the right of element ‘B’
(a) The element ‘A’ would probably have a …………… [smaller/larger] atomic size than ‘B’.
(b) The element ‘B’ would probably have …………… [lower/higher] ionization potential than ‘A’.
(c) The element ‘A’ would have …………… [lesser/higher] electron affinity than ‘B’.
(d) Nuclear charge of element ‘B’ would be …………… [less/more] than element ‘A’.
(e) If an element ‘C’ had a low electronegativity and ionization potential it would have more tendency to …………… [gain/lose] electrons.

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