periodic trends -ionization energy

Front

What is ionization energy?

Back

The energy required to remove an electron from an atom in its gaseous state.

Front

How does atomic radius affect ionization energy?

Back

The smaller the atomic radius, the stronger the attraction between the nucleus and the electrons, resulting in higher ionization energy.

Front

What is the trend of ionization energy across a period?

Back

Ionization energy generally increases across a period from left to right due to increasing nuclear charge.

Front

What is the trend of ionization energy down a group?

Back

Ionization energy generally decreases down a group due to increased atomic radius and electron shielding.

Front

What is the second ionization energy?

Back

The energy required to remove the second electron from an atom after the first has been removed.

Front

Why does fluorine have a higher ionization energy than nitrogen?

Back

Fluorine has a higher ionization energy because it has a smaller atomic radius and a stronger effective nuclear charge.

Front

What is effective nuclear charge?

Back

The net positive charge experienced by an electron in a multi-electron atom, accounting for shielding by other electrons.

Front

What role does electron shielding play in ionization energy?

Back

Electron shielding reduces the effective nuclear charge felt by outer electrons, making them easier to remove.

Front

What is a valence electron?

Back

An electron in the outermost shell of an atom that can participate in chemical bonding.

Front

How does distance from the nucleus affect electron attraction?

Back

The greater the distance from the nucleus, the less the attraction experienced by the valence electrons.