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A tabular arrangement of the chemical elements, organized by their atomic number, electron configuration, and recurring chemical properties.

A type of chemical bonding that involves the electrostatic attraction between oppositely charged ions.

A chemical bond that involves the sharing of electron pairs between atoms.

A bond formed by the attraction between positively charged metal ions and the electrons around them.

A number that represents the total number of electrons that an atom either gains or loses in order to form a chemical bond with another atom.

A compound that contains one or more coordinate bonds, where a central metal atom is bonded to a number of anions or neutral molecules.

An ion or molecule that binds to a central metal atom to form a coordination complex.

A model that describes the electronic structure of transition metal compounds, where d-orbital degeneracy is broken due to ligand interactions.

A theory that describes the electron structure of molecules in terms of molecular orbitals, which are formed from the combination of atomic orbitals.

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

A Lewis acid is an electron pair acceptor, while a Lewis base is an electron pair donor.

A chemical reaction in which the oxidation states of atoms are changed.

A reaction where an acid reacts with a base to produce water and a salt.

A type of bonding in which a ligand forms multiple bonds with a single central atom within a complex.

A group of 15 metallic elements from lanthanum through lutetium in the periodic table, known for their f-electron configurations and magnetic properties.

A group of 15 metallic elements from actinium through lawrencium in the periodic table, most of which are radioactive.

A group of elements on the periodic table from groups 3 to 12 which have d-electrons and exhibit unique properties such as variable oxidation states and colored compounds.

A mixture composed of two or more elements, at least one of which is a metal, often having enhanced strength or other properties compared to the pure elements.

A reaction that occurs when two soluble salts in aqueous solution combine to form an insoluble solid, known as a precipitate.