Unit 2 Experience 3 - Periodic Trends

Front

Atomic Radius

Back

Distance between the outermost electrons and the nucleus.

Front

Does Atomic Radius increase or decrease down a group and why?

Back

Atomic Radius increases down a group because the valence electrons are moving further away from the nucleus as we add protons and energy levels.

Front

Does Atomic Radius increase or decrease left to right across a period and why?

Back

Atomic Radius decreases left to right across a period because the valence electrons are being pulled closer to the nucleus as effective nuclear charge increases.

Front

An atom of group of atoms that has a positive or negative charge.

Back

Ion

Front

Cation

Back

An atom that loses one or more electrons to form an ion with a net positive charge. Cations are always smaller than their parent atoms.

Front

An atom that gains one or more electrons to form an ion with a net negative charge. These are always bigger than their parent atoms.

Back

Anion

Front

Ionization Energy

Back

The energy required to remove the outermost electron from the ground state of a gaseous atom.

Front

Why do smaller atoms have higher ionization energy?

Back

Smaller atoms have valence electrons closer to the nucleus which means they feel a stronger charge. It will take more energy to remove those valence electrons.

Front

Does Ionization energy increase or decrease left to right across a period and why?

Back

Ionization energy increases left to right because the atomic radius decreases left to right which means the atoms are getting smaller.

Front

Does Ionization Energy increase or decrease down a group on the periodic table and why?

Back

Ionization energy decreases down a group because the atoms are getting bigger which means it doesn't take as much energy to remove the valence electrons.