Periodic Trends

Front

What is ionization energy?

Back

Ionization energy is the amount of energy required to remove an electron from an atom in its gaseous state.

Front

Why does Francium (Fr) have the lowest ionization energy in Group 1?

Back

Its 1 valence electron is very far from the nucleus, so little energy is needed to remove it.

Front

Which atom has the largest atomic radius among potassium, rubidium, francium, and cesium?

Back

Francium has the largest atomic radius.

Front

What happens to atomic size as you move across a period in the periodic table?

Back

Atoms tend to get smaller because they have more protons.

Front

What causes atoms to get larger as you move down a group in the periodic table?

Back

Atoms get larger because they have more energy levels.

Front

Define atomic radius.

Back

Atomic radius is the distance from the nucleus of an atom to the outermost shell of electrons.

Front

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

Back

Ionization energy generally decreases as you move down a group.

Front

What is the trend of ionization energy as you move across a period in the periodic table?

Back

Ionization energy generally increases as you move across a period.

Front

Explain why Calcium (Ca) has a lower ionization energy than Scandium (Sc).

Back

Calcium has a lower ionization energy because it is located further down the group, meaning its outer electron is further from the nucleus.

Front

What is the relationship between atomic size and electronegativity?

Back

As atomic size increases, electronegativity generally decreases.