Question

Explain giving reason why although the nuclear charge in atoms increases in moving from left to right in a period as well as in moving from top to bottom in a group in the Modern periodic table, but the size of the atoms does not vary similarly in both situations.

Answer 1

The distance between the centre of the nucleus and the outermost shell of an isolated atom is known as its atomic size. Radius of an atom is referred to as atomic size. As we advance along the group, the elements' atomic sizes grow. This is due to the fact that as we move along the group, additional shells are being added. This lengthens the gap between the outermost shell and the nucleus, increasing atomic size despite an increase in nuclear charge.

Additionally, as you move across a period from left to right, the atomic radius of the elements decreases. This occurs as a result of an increase in nuclear charge, which tends to draw electrons closer to the nucleus and cause an atom's size to decrease.