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As we descend down the group, the atomic radii increases. This is because the number of shells increases.
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.
Atomic radius increases down the group due to increase in no.of orbits around the nucleus.
the atomic radii increases down the group.
As we go down the group, nuclear charge deceases and atomic radii increases. So the element can easily lose electron and hence react.
Radii generally decrease from left to right along each period (row) of the table, from the alkali metals to the noble gases; radii increase down each group (column). The radius increases sharply between the noble gas at the end of each period and the alkali metal at the beginning of the next period
Atomic radii increases moving down a group in the Periodic Table due to the increasing energy levels in the electron configuration and electrons filling in energy levels further away from the nucleus.
Ionic radius (or radii) increases as you move down a group and across a period.
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 trend of atomic radius increases down a group on the periodic table. This occurs because each successive element down a group has another energy level. As more electrons are added, more energy levels are needed to hold the electrons.
As we move down the group ,the electrons in the valence shell remains constant but the number of shells increases by one.size of the element increases down the group .elements are more electro-positive as we move down the group so elements at the bottom are more electro-positive than those at the top.as the size of the elements increases the nuclear charge on the elements decreases.due to less nuclear charge shielding effect decreases down the group.
Reactivity in group 1 of elements increases as we go down the group (to francium) because in the alkali metals as we go down the group number of atomic shells increases so the elements with most shells will easily release their electrons in the outer most shell.