Seventeen
Because the trend is the same. Atomic radius decreases from left to right across a period.
Across a period the atomic size decreases. Hence elements in the right side of the periodic table have small size / radii.
As we descend down the group, the atomic radii increases. This is because the number of shells increases.
Noble gases have larger atomic radii than alkali metals in the same period.
I think that the ionic radii decrease
Because the trend is the same. Atomic radius decreases from left to right across a period.
Because the trend is the same. Atomic radius decreases from left to right across a period.
The atomic radius decreases along the elements across a period. Along a group, there is an increment in the atomic radius of corresponding elements.
Across a period the atomic size decreases. Hence elements in the right side of the periodic table have small size / radii.
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.
As we descend down the group, the atomic radii increases. This is because the number of shells increases.
Noble gases have the smallest atomic radius.
Noble gases have larger atomic radii than alkali metals in the same period.
Comparing d-block elements with s & p-block elements, it does have smaller atomic radii because of the richness in electrons & protons.
I think that the ionic radii decrease