Periodic Trends

Periodic trends refer to the patterns and variations in the properties of elements across different periods and groups in the periodic table, such as atomic radius, electronegativity, and ionization energy.

Electronegativity is the ability of an atom in a chemical compound to attract electrons towards itself. It is a key factor in determining how atoms bond with each other.

Fluorine has the highest electronegativity of all elements.

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.

Atomic radius decreases across a period from left to right due to increasing nuclear charge, which pulls electrons closer to the nucleus.

Atomic radius increases down a group because additional electron shells are added, which outweighs the increase in nuclear charge.

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.

Ionization energy increases across a period due to increasing nuclear charge, which makes it harder to remove an electron.

Ionization energy decreases down a group because the outer electrons are further from the nucleus and are shielded by inner electrons.

Electronegativity increases across a period and decreases down a group.