Ionic Radius

Front

What is ionic radius?

Back

The ionic radius is the measure of an ion's size, typically defined as the distance from the nucleus to the outermost electron shell.

Front

What is the trend for ionic radius across a period for anions?

Back

The ionic radius of anions decreases across a period due to increasing nuclear charge, which pulls the electrons closer to the nucleus.

Front

Which is smaller: Mg or Mg²⁺?

Back

Mg²⁺ is smaller than Mg because it loses two electrons, resulting in a decrease in electron-electron repulsion and a loss of an energy level.

Front

Which ion has the smallest radius: O²⁻, S²⁻, Se²⁻, or Te²⁻?

Back

O²⁻ has the smallest radius among these ions due to its higher effective nuclear charge relative to the number of electrons.

Front

What is effective nuclear charge (Z_eff)?

Back

Effective nuclear charge (Z_eff) is the net positive charge experienced by an electron in a multi-electron atom, accounting for shielding by other electrons.

Front

How does the effective nuclear charge compare between Cl and Cl⁻?

Back

The effective nuclear charge (Z_eff) for Cl and Cl⁻ is the same because both have the same number of protons, but Cl has one less electron.

Front

What happens to the size of Cl compared to Cl⁻?

Back

Cl is smaller than Cl⁻ because Cl has a stronger nuclear attraction towards its valence electrons.

Front

What is the trend for ionic radius down a group?

Back

The ionic radius increases down a group due to the addition of electron shells, which outweighs the increase in nuclear charge.

Front

Why do cations have a smaller radius than their neutral atoms?

Back

Cations are smaller than their neutral atoms because they lose electrons, resulting in reduced electron-electron repulsion and a stronger pull from the nucleus.

Front

What is the relationship between ionic radius and charge?

Back

Generally, as the charge of an ion increases (more positive), the ionic radius decreases due to increased nuclear attraction.