The position of three elements X, Y and Z in the periodic table is shown below.
Group 1 Group 2
$-$ $-$
X $-$
$-$ $-$
Y Z
(i) Which type of ion- cation or anion, will be formed by an element X?
(ii) Which element Y or Z, has the atom of comparatively larger size? Give reasons for each case.

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Solution

Part 1: Formation of ion by X
Element X is in group 1 period 2.
Element X is an alkali metal, and hence has 1 valence electron in its outermost shell.
After losing the electron element X would form a cation.
Part 2: Comparison of larger size
Element Y is in group 1 period 4 and element Z is in group 2 period 4.
Hence number of electrons in Z is greater than in Y.
We know that atomic size decreases as we go from left to right across a period.
Also due to more number of electrons, element Z has a greater nuclear force of attraction between the nucleus and electrons, rather than element Y
Therefore Y atom has a larger size than Z atom.
Final Answer:- (i) Element X being metal will form cation
(ii) Due to greater nuclear force of attraction Z is comparatively smaller than Y.

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The position of three elements X, Y and Z in the periodic table is shown below.Group 1Group 2--X---YZ(i) Which type of ion- cation or anion, will be formed by an element X?(ii) Which element Y or Z, has the atom of comparatively larger size? Give reasons for each case.

The position of three elements X, Y and Z in the periodic table is shown below.
Group 1 Group 2
$-$ $-$
X $-$
$-$ $-$
Y Z
(i) Which type of ion- cation or anion, will be formed by an element X?
(ii) Which element Y or Z, has the atom of comparatively larger size? Give reasons for each case.