Question

Metallic nature and basic nature of the oxides ...... as we move along a period
(A) Increases
(B) Decreases
(C) First increases and then decreases
(D) Remains constant

Answer 1

Hint: Periodic table has $18$ groups and $7$periods. The left most side contains metals including group $1,2$(forming s block) and group $13$. The d block elements are called transition metals. Whereas the right most side of the periodic table are called non-metals.

Complete Step by Step Solution:
The oxides of metals are called metallic oxides. For example, $MgO,CaO$are metal oxides of group $2$. $L{i_2}0$is an example of metal oxide from group $1$.They react with water to form bases, hence metallic oxides are basic in nature. For example, magnesium oxide reacts with water to form magnesium oxide. The reaction is $MgO + {H_2}O \to Mg{(OH)_2}$.

The metallic character decreases as we move from left to right in a period. This is because size decreases and electronegative character increases. Thus, it becomes more difficult to lose an electron. And metals have a tendency to lose electrons and thus, acquire positive charge.

Moreover, as we move towards the right of the periodic table, the tendency to achieve noble gas configuration by accepting electrons increases. For example, fluorine has $7$electrons in its outermost shell and easily accepts one electron from metals to gain stability.
Thus, the metallic trend decreases along a period which decreases the basic nature of oxides. Thus, the correct answer is $2$.

Note: On moving along the group, the size increases due to addition of shells and thus, electronegativity decreases. So the metallic character and basic nature of oxides increases on moving top to bottom in a group.