Two elements ‘X’ and ‘Y’ belong to 4th period of the modern periodic table and are in group I and group 2 respectively. Compare their following characteristics in tabular form:
(i) The number of electrons in their atoms.
(ii) The size of their atoms.
(iii) Their metallic character.
(iv) Their tendencies to lose electrons.
(v) The formula of their oxides.
(vi) The formula of their chlorides.
Answers
Answer:
Given: X and Y belong to same period, X belongs to group '1' and Y belongs to group '2'.
(i) Valence electrons in any atom = Group number
So, Valence electron in element X = 1
valence electrons in Y= group number-2.
(ii) Since valence electrons in element X=1
So, to get stable gas electronic configuration, no. of electrons required = 1
So, The valency of X = 1 whereas
The valence electrons in element Y = 2 and is already stable.
So, valency of Y is 2.
(iii) Since metallic character decreases on moving from left to right in a period and X lies in group1 and Y in group 2. So, X will have more metallic character than Y.
(iv) The size of the atom decreases when move from left to right in a period. So, the size of X will be larger than Y and is 4 more than the size of Y.
(v) The Oxide of element X and Y are: Oxide of X is X20 Oxide of Y is YO
(vi) Since valency of X is 1. So, Chloride of X = XCI
The valency of Y is 2, Chloride of Y = YCl2
hope it helps:)