Periodic Trends Practice

Atomic mass is the weighted average mass of an atom's isotopes, measured in atomic mass units (amu). It reflects the number of protons and neutrons in the nucleus.

Gallium (Ga) has the largest atomic mass.

The atomic radius decreases as you move from left to right across a period due to increased nuclear charge attracting electrons more strongly.

The atomic radius increases as you move down a group because additional energy levels (shells) are added.

Ionization energy is the energy required to remove an electron from an atom in its gaseous state.

Neon (Ne) has a higher ionization energy than Arsenic (As).

Generally, as atomic radius increases, ionization energy decreases because the outer electrons are further from the nucleus and experience less attraction.

Increasing the number of protons in the nucleus pulls electrons closer, resulting in a smaller atomic radius.

The order of increasing radius is K⁺¹, Kr, F^-1, N^-3.

K⁺¹ is smaller than K because it has lost an electron, resulting in less electron-electron repulsion and a stronger pull from the nucleus.