PERIODIC TRENDS

Front

What is ionization energy?

Back

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

Front

Why does ionization energy decrease down a group in the periodic table?

Back

As you move down a group, the atomic radius increases, and the valence electrons are farther from the nucleus, making them easier to remove.

Front

What trend is observed in ionization energy as you move across a period from left to right?

Back

Ionization energy generally increases due to the increasing nuclear charge, which attracts electrons more strongly.

Front

What is the atomic radius?

Back

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

Front

Why does atomic radius decrease across a period?

Back

The increasing number of protons pulls the electrons closer to the nucleus, reducing the atomic radius.

Front

What is electronegativity?

Back

A measure of the tendency of an atom to attract a bonding pair of electrons.

Front

How does electronegativity change across a period?

Back

Electronegativity increases across a period due to increasing nuclear charge.

Front

What is the relationship between atomic radius and ionization energy?

Back

Generally, as atomic radius decreases, ionization energy increases because electrons are held more tightly by the nucleus.

Front

What is the trend in ionization energy for alkali metals (Group 1)?

Back

Ionization energy decreases as you move down the group.

Front

Which element has the highest ionization energy in Period 6?

Back

Rn (Radon) has the highest ionization energy in Period 6.