Question

Atomic size seems to play an important role in explaining some differences between the first element in a group and the subsequent group elements. Explain.

Short answer

The elements have the smallest size compared to the next element of the same group. Hence they are said to polarize bonds with non-metal (greater covalent nature).

In Groups 4A-6A, the main difference between the first and second members of the group is the tendency of elements to form a bond of n.

In Group 7A, F has the smallest size causing the highest electronegativity and lesser electron affinity.

Step-by-step solution

Define Elements

An element is a pure material made up entirely of atoms with the same protons in their nuclei. Chemical elements cannot be broken down into smaller substances by chemical reactions.

Explanation of the question

$\mathrm{\pi }$TheGroups 1A-3A, the small sizes of H (is denoted as Li), Be (is denoted as Mg), and B (is denoted as AI) seem to be the reason why these elements have non-metallic properties.

While others in Groups 1A-3A are strictly metallic.

The atomic size affects the chemical and physical properties of the elements, such as the oxidation state, chemical reactivity, etc.

The small sizes of H, Be, and B also causes these species to polarize the electron cloud in the non-metals, which forces a sharing of electrons when the bonding occurs.

In Groups 4A-6A, a major difference between the group's first and second members is the elements' tendency to form a$\mathrm{\pi }$ bond.

The smaller elements form stable bonds, while the larger elements are not capable of good overlap between parallel p orbitals and, in turn, do not form a strong n bond.

Group 7A, the small size of F as compared to Cl, is used to explain the low electron affinity of F and the weakness of the F-F bond.

Therefore, the elements have the smallest size as compared to the next element of the same group. Hence they are said to polarize bonds with non-metal (greater covalent nature).

In Groups 4A-6A, the main difference between the first and second members of the group is the tendency of elements to form a bond of n.

Group 7A, F has the smallest size causing the highest electronegativity and lesser electron affinity.