Unit 4 Exam Five Periodic Trends

Front

What is ionization energy?

Back

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

Front

What factors lead to a low value for first ionization energy?

Back

1. Large atomic radius 2. High number of core (shielding) electrons.

Front

Which element has the highest first ionization energy among sodium, aluminium, calcium, and phosphorus?

Back

Phosphorus.

Front

What is the correct order of increasing ionization energy for Li, Na, and K?

Back

K, Na, Li.

Front

Why does ionization energy generally increase across a period?

Back

Due to increased nuclear charge.

Front

What is the first ionization energy process for magnesium?

Back

Mg(g) → Mg⁺(g) + e⁻.

Front

How does atomic radius affect ionization energy?

Back

A larger atomic radius generally leads to lower ionization energy.

Front

What is the trend of ionization energy down a group in the periodic table?

Back

Ionization energy decreases down a group.

Front

What is the relationship between nuclear charge and ionization energy?

Back

Higher nuclear charge increases ionization energy.

Front

Define shielding effect in the context of ionization energy.

Back

The reduction in effective nuclear charge on the electron cloud due to the presence of other electrons.