Question

A group of elements in the periodic table are given below (\[Boron\] is the first member of the group and $Thallium$ is the last)
$Boron,Aluminium,Gallium,Indium,Thallium$
Answer the following question in relation to the above group of elements:
Will the elements in the group to the right of this \[Boron\] group be more metallic or less metallic in character? Justify your answer.

Answer 1

Hint:As we move down the group in periodic table, the metallic character of the elements increases but as we move from left to right in a period the non-metallic character increases or the metallic character decreases.

Complete answer:
Metallic character is the general property of elements in the periodic table. It is the tendency of a metal to lose electrons during the course of chemical reactions. They always exist in positive oxidation states.
As the size of elements increases the ionization enthalpy decreases because the effective nuclear attraction on the last shell in bigger size elements will be poor. Thus the electrons will be free to move and readily participate in chemical reactions.
The oxides of metals are considered to be basic.
Also metals have very poor electronegativity as compared to the elements of p-block.
In the periodic table the groups on the left side are considered to consist of metals and the groups to the right side contain non-metals with very poor metallic nature.
Group-$13$ have the following elements- $Boron,Aluminium,Gallium,Indium,Thallium$
They are from the p-block family. The groups to the right side of this group are Carbon family, Oxygen family, Nitrogen family,Halogen group and the inert gas group. They consist of nonmetals and metalloids. Their oxides are acidic and amphoteric in nature. These elements also show negative oxidation states which contradicts the metallic nature.
Fluorine And Oxygen Considered as the most electronegative atoms of the periodic table with very high ionization energy indicating their smaller atomic size.
These groups, thus have very low metallic character and are known as non-metals. But on moving down along these groups the metallic character increases. For e.g. $Bismuth$ from $Nitrogen$ family has very good metallic nature.
Hence the elements in the group to the right of this Boron group are less metallic in nature.

Note:
Metalloids are the elements which have properties of both metals and nonmetals. For e.g. $Arsenic,Antimony$ from $Nitrogen$ family, $Silicon$ from $Carbon$ family etc.
Electronegativity is the tendency of an electron to attract the shared pair of electrons towards itself. Being most electronegative Fluorine and Oxygen do not want to lose their electrons and show only negative oxidation states.