Atomic Radius, Forces of Attraction, and Ionization Energy

Front

What happens to the force of attraction between the nucleus and the valence electron as you move across a period from left to right?

Back

The force of attraction increases.

Front

Does an atom with more protons have a stronger or weaker force of attraction between the nucleus and the valence electrons compared to an atom with less protons?

Back

Stronger force of attraction.

Front

Which group of the periodic table does an atom with 2 valence electrons belong to?

Back

Group 2.

Front

What is the ionization energy required for loosely held electrons compared to tightly held electrons?

Back

Loosely held electrons require less ionization energy.

Front

Would you expect an atom with 2 valence electrons to form a cation or an anion?

Back

Cation.

Front

Define atomic radius.

Back

The distance from the nucleus of an atom to the outermost shell of electrons.

Front

How does atomic radius change as you move down a group in the periodic table?

Back

The atomic radius increases.

Front

What is ionization energy?

Back

The energy required to remove an electron from an atom.

Front

How does ionization energy change as you move across a period from left to right?

Back

Ionization energy generally increases.

Front

What is the trend of atomic radius as you move from left to right across a period?

Back

The atomic radius decreases.