Arrange the following in order of increasing atomic radii from smallest to largest.
Mg
Ra
Sr
Be
Ca
Ba
Be Mg Ca Sr Ba Rb
Generally atomic size decreases as we go from left to right and increases as we go top to bottom on the periodic table.
To arrange the elements in order of increasing atomic radii, we need to consider their positions on the periodic table. The atomic radius generally increases as you move down a group and decreases as you move across a period from left to right.
Let's start by organizing the elements given in the question in their respective groups in the periodic table:
Mg (Magnesium) - Group 2 (Alkaline Earth Metals)
Ra (Radium) - Group 2 (Alkaline Earth Metals)
Sr (Strontium) - Group 2 (Alkaline Earth Metals)
Be (Beryllium) - Group 2 (Alkaline Earth Metals)
Ca (Calcium) - Group 2 (Alkaline Earth Metals)
Ba (Barium) - Group 2 (Alkaline Earth Metals)
Since all elements given belong to the same group (Group 2), their atomic radii will increase as we move from the top of the group to the bottom.
Therefore, the elements arranged in order of increasing atomic radii from smallest to largest are as follows:
Be < Mg < Ca < Sr < Ba < Ra