Question

state more factors which affect or influence the atomic size of elements in a periodic table with reference to elements in period 2,also state which elements has the largest atomic size and which elements has the smallest atomic size?​

Answer 1

Answer:

Atomic size decreases across a Period from left to right as we face the Table, but INCREASES down a Group, a column of the Periodic Table. ... And thus across the Period nucular charge predominates, and draws the valence electrons towards the nuclear core, with the result of a marked decrease in atomic radius.

Helium has the smallest atomic radius because the stronger force between the two protons and two electrons pulls the electron shell in closer than the lone electron and lone proton in a Hydrogen atom

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Answer 2

Answer:

Explanation:

Atomic size or atomic radius is the distance between the centre of the nucleus and the outermost shell.There are two factors which determine atomic size.They are:

Number of shells- As number of shells increases, atomic size increases. Nuclear charge- Nuclear charge is equal to the number of protons in the nucleus of an atom. As nuclear charge increases, the attractive force of the nucleus on the valence electrons increases. Hence atomic size decreases. As we move from left to right in a period atomic size decreases.Along a period number of shells remain the same but nuclear charge increases.Hence attractive force of the nucleus on the valence electrons increases.Thus atomic size decreases along a period.