Adding more electrons that need to occupy higher energy orbitals
decrese as you move down the group 1A elements
shielding of the outer electrons by inner electrons.
The atomic radius decreases along the elements across a period. Along a group, there is an increment in the atomic radius of corresponding elements.
Shielding.
In a group the ionization energy decrease when the atomic radius increase; in a period this relation is not generally valid.
Noble gases have the smallest atomic radius.
Comparing d-block elements with s & p-block elements, it does have smaller atomic radii because of the richness in electrons & protons.
As we descend down the group, the atomic radii increases. This is because the number of shells increases.
group 1 elements
I think that the ionic radii decrease
The atomic radius decreases along the elements across a period. Along a group, there is an increment in the atomic radius of corresponding elements.
Shielding.
Shielding.
Within a group, the number of shells (or energy level) increases (as we go from top to bottom of a group) and hence the size of the atom or the atomic radii increases.
The atomic radii of members of the Group 1A (Alkali metals), increases down the group. Therefore Francium has the largest atomic radius of the Alkali metals. However Fr has no stable isotopes, thus is not naturally occurring. So Cs-133 is the largest you can find.
The ionic radii of metallic elements is smaller than its atomic radii, because the ion has less electrons. This gives it a smaller electron cloud and makes the atom smaller.
In a group the ionization energy decrease when the atomic radius increase; in a period this relation is not generally valid.
Look for a reference chart in a book or online. Look for a Periodic Table of the Elements that has the atomic radii on it.
Seventeen