In period 2, element X is to the right of element Y. Then, find which of the elements have:

(i) Low nuclear charge

(ii) Low atomic size

(iii) High ionization energy

(iv) High electro negativity

(v) More metallic character

i) Y has low nuclear charge

a) The nuclear charge increases from left to right in a period because the atomic number increases.

b) The outer electrons are added in the same valence shell.

c) As a result, the attraction on the electrons by the nucleus increases as we move from left to right.

d) Thus, Y has low nuclear charge.

ii) X has low atomic size.

a) Atomic radius goes on decreasing as we move from left to right.

b) This is due to increase in attraction by the nucleus on the electrons.

c) This tends to decrease the size with increase in atomic number.

d) Thus, X has low nuclear charge.

iii) X has higher ionization energy.

Ionization goes on increasing as we move from left to right due to increased nuclear charge. Thus, X has higher ionization energy.

Note: More is the nuclear charge; more is the ionization energy.

iv) X has higher electronegativity.

Electronegativity goes on increasing as we move from left to right due to increase in attraction between the outer electrons and the nucleus. Thus, X has higher electronegativity.

v) Y has more metallic character

Metallic character goes on decreasing while going from left to right in a period due to increased attraction by the nucleus. Thus, Y has ore metallic character.

Note: More easily an element loses electrons, higher will be its metallic character (electropositive character)