Atomic Radius and Ionization Energy Exam

Front

What is the trend of atomic radius as you move across a period in the periodic table?

Back

Atomic radius decreases.

Front

What happens to the number of energy levels or shells when you move down a group in the periodic table?

Back

There is an increase in the number of energy levels or shells.

Front

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

Back

Ionization energy increases.

Front

What type of electron is removed from an atom/ion that is isoelectronic with a noble gas?

Back

Inner (core) electron.

Front

Why does it require more ionization energy to remove a 2nd and 3rd electron?

Back

They are more attracted to a positive ion than to a neutral atom.

Front

Define atomic radius.

Back

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

Front

What is ionization energy?

Back

The energy required to remove an electron from an atom or ion.

Front

Explain the concept of effective nuclear charge.

Back

The net positive charge experienced by an electron in a multi-electron atom, accounting for shielding by inner electrons.

Front

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

Back

Atomic radius increases due to the addition of energy levels.

Front

What is the relationship between atomic radius and ionization energy?

Back

As atomic radius increases, ionization energy generally decreases.