Atomic Radius, Forces of Attraction, and Ionization Energy

Front

What is Atomic Radius?

Back

The atomic radius is the distance from the nucleus of an atom to the outermost shell of electrons. It generally increases down a group and decreases across a period.

Front

What is Ionization Energy?

Back

Ionization energy is the energy required to remove an electron from an atom in its gaseous state. It generally increases across a period and decreases down a group.

Front

What is the trend of Ionization Energy across a period?

Back

Ionization energy increases as you move from left to right across a period due to increasing nuclear charge.

Front

What is the trend of Ionization Energy down a group?

Back

Ionization energy decreases as you move down a group due to increased distance between the nucleus and the outermost electrons.

Front

What is the Force of Attraction in atoms?

Back

The force of attraction refers to the electrostatic force between the positively charged nucleus and the negatively charged electrons.

Front

How does Atomic Radius change down a group?

Back

Atomic radius increases down a group because additional electron shells are added, increasing the distance between the nucleus and the outermost electrons.

Front

How does Atomic Radius change across a period?

Back

Atomic radius decreases across a period due to increased nuclear charge pulling the electrons closer to the nucleus.

Front

Which atom has the highest Ionization Energy: O, Se, S, or Te?

Back

O (Oxygen) has the highest ionization energy among these options.

Front

Which atom has the largest Force of Attraction: Li, Na, K, or Rb?

Back

Li (Lithium) has the largest force of attraction due to its smaller atomic radius.

Front

What happens to the Force of Attraction as you move down a group?

Back

The force of attraction decreases as you move down a group due to increased atomic radius.