The electronegativity increases across a period

The electronegativity stays the same across a period

The electronegativity is linked to radius size

The electronegativity reduces across a period

Ionisation energy stays the same downa group

The ionisation energy increases down a group

The ionisatisation energy relies on electronegativity

The ionisation energy decreases down a group

It is the increase in protons as you move across a period

It is the increase in number of positive charged protons and the increase in negative charged electrons across a period

It is the increase in size of the atom across a period

It is the increas in size of atomic radius across a group

the energy that a compound has to help it form a bond

the energy required to add electrons to another atom to make a compound

the energy that an atom has to break its bond in a gaseous state

the energy required to remove the most loosely bound electrons from a neutral gaseous atom in its ground state

When the electrons are excited and move to a higher energy level

When the electrons are removed and no more electrons exist in the atom

When the electrons are in the lowest possible energy level

When the electrons move to another atom by sharing electrons.

the power of attraction that an atom in a molecule has for a shared pair of electrons in a covalent bond

the charge that the atoms have when they form ions

it is the number of electrons that an atom has

It is the power of attraction that a molecule has to form ionic bonds

Using the ionisation energy table values

Using the atomic radius values

Using the electronegativity values

Using the deionisation values