Periodic TRENDS REVIEW (plus more!)

Front

What property increases across the period (left to right)?

Back

Effective nuclear charge increases across the period due to the increasing number of protons in the nucleus, which pulls the electrons closer.

Front

Define first ionization energy.

Back

The energy required to remove an electron from a gaseous atom.

Front

Which species has the biggest ionic radius: Sr²⁺, Te²⁺, I⁻, Cs⁺?

Back

Cs⁺ has the biggest ionic radius because it has the least effective nuclear charge relative to its size.

Front

Why is potassium larger than sodium?

Back

Potassium has more energy levels than sodium, resulting in a larger atomic size.

Front

What does effective nuclear charge refer to?

Back

Effective nuclear charge refers to the net pull of the nucleus on the valence electrons, accounting for electron shielding.

Front

What is electron shielding?

Back

Electron shielding is the phenomenon where inner electrons repel outer electrons, reducing the effective nuclear charge felt by the outer electrons.

Front

How does atomic radius change down a group?

Back

Atomic radius increases down a group due to the addition of energy levels.

Front

What is the trend of ionization energy across a period?

Back

Ionization energy generally increases across a period due to increasing effective nuclear charge.

Front

What is the trend of electronegativity down a group?

Back

Electronegativity decreases down a group because the distance between the nucleus and valence electrons increases.

Front

What is the relationship between atomic radius and ionization energy?

Back

As atomic radius increases, ionization energy decreases because the outer electrons are further from the nucleus.