group 2

Question 1

Explain the trend for atomic / ionic radius / 1st IE / electronegativity

Answer 1

Down the group, the nuclear charge increases as the number of protons increases

However, the increasing nuclear charge is cancelled out by the number of inner shell electrons increases which results in an increased shielding effect

The number of quantum shells increases. The distance between the nucleus and the outermost electrons increases

Hence, electrostatic forces of attraction between the nucleus and the valence electrons decreases

Atomic radius: resulting in an increase in atomic radius.

Ionic radius: The ionic radius increases down the group

First ionisation energy: Less energy is required to remove the electron and first ionisation energy decreases

Electronegativity: Ability of the atom to attract shared electrons in a covalent bond towards itself decreases and electronegativity decreases