Periodic Table Trends

A pattern in the properties of elements as you move across a period or down a group

A random change in element properties

A trend that only occurs in metals

A trend that only occurs in nonmetals

Atomic Radius

Ionic Radius

Electronegativity

Melting Point

The distance between two atoms

Half the distance between nuclei of identical atoms

The size of the nucleus

The number of electrons in an atom

Atomic radius increases as you move down a group

Atomic radius decreases as you move across a period

Valence electrons are shielded from nuclear charge

Outermost orbital size increases down a group

More inner electrons shield the outer electron from the nucleus

The nucleus attracts the outer electron more strongly

Electrons are lost from the atom

Atoms gain protons

The radius becomes larger when an atom loses electrons

Electrostatic repulsion increases when an atom loses electrons

The loss of a valence electron can result in a smaller radius

Atoms gain electrons to form cations

The energy required to add an electron to an atom in the gas phase.

The energy required to remove an electron from an atom or ion in its ground state in the gas phase.

The energy released when an atom gains an electron.

The energy needed to break a chemical bond.

Ionization energy increases as you move across a period.

Ionization energy decreases as you move down a group.

Ionization energy remains constant across a period.

Ionization energy decreases as you move across a period.

Lithium (Li)

Beryllium (Be)

Boron (B)

Carbon (C)

Oxygen

Fluorine

Chlorine

Nitrogen

Fluorine

Oxygen

Nitrogen

Chlorine