Elements are arranged in groups by similar atomic structure on the periodic table. this allows for an element's properties to be predicted based on general periodic trends. one of these trends, atomic radius, increases down a group and to the left along a period and can be defined as

The number of energy levels increases as you move down a group as the number of electrons increases

Explanation:

The determination of distance of separation between the two nuclei of likely atoms connected together called atomic radius. This in a group usually increases from top to bottom. With the increase in the atomic number in the group, the positive nuclear charge increases again. However, the amount of principle energy is also increasing.

High principle energy levels made up of orbits of higher size than low energy levels. The impact of this exceeds the increased nuclear charge, and thus the atomic radius gets increased when going down a group in the periodic tables.

Atomic radius gradually decreases from the side left to the right during the elemental period. This is because all electrons of the same size are added over time or in a family of elements.

Literally, the Atomic radius of a chemical element is a term used to describe the size of an atom.

Atomic radius can be regarded as a measure of the size of its atoms. This is often characterized by the mean or typical distance of the chemical element from the center of the nucleus to the boundary of the surrounding shells of electrons.

In general, the size of an atom will decrease as you move from left to the right of a certain period

Periodic Trends of Atomic Radius. An atom gets larger as the number of electronic shells increase; therefore the radius of atoms increases as you go down a certain group in the periodic table of elements.

option number c is the right answer.

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