Chemistry Quiz: Oxidation States and Bonding

The energy required to remove an electron from an atom in its gaseous state. This energy is a measure of how tightly the electron is held by the atom.

The process of losing an electron from an atom or molecule, resulting in the formation of a positively charged ion (cation).

The energy required to remove the first electron from an atom in its gaseous state.

The energy required to remove the second electron from an atom in its gaseous state, after the first electron has already been removed.

The process where an atom gains an electron resulting in the formation of a negatively charged ion (anion).

The ability of an atom to attract a bonding pair of electrons. It is a measure of the atom's electronegativity.

The size of an ion. This is determined by the number of electron shells and the number of protons in the nucleus.

Two opposite symmetry orbitals in a molecule cannot overlap. This occurs because of the different spatial arrangements of electrons in the orbitals.

The presence of unpaired electrons in a molecule makes it paramagnetic, meaning it is attracted to a magnetic field.

A molecule with all paired electrons is diamagnetic and is not attracted to a magnetic field.

The strength of the attraction between oppositely charged ions in an ionic compound influences its melting point. Higher ionic character leads to stronger attraction and a higher melting point.

Fajan's rule describes the extent of covalent character in an ionic bond. This character increases with the size of the cation and the charge of the anion.

The tendency of an element to lose electrons and form positive ions.

Elements in the periodic table that have the tendency to lose electrons easily.

The tendency of an element to gain electrons and form negative ions.

Metals typically have low ionization energies and high electropositivity.

Second ionization energy is always greater than the first ionization energy.

Elements in the second period (Li to Ne) cannot expand their octet beyond 8 electrons.

Elements in the third period (Na to Ar) and beyond can form more than four bonds due to the presence of vacant d-orbitals.

The formal charge on an atom in a molecule is the difference between the number of valence electrons in a free atom and the number of electrons assigned to that atom in the Lewis structure.

A central atom surrounded by ligands. The central atom can be a metal or a non-metal.

The atoms or molecules that are directly bonded to the central atom in a coordination complex.

The number of bonds that a central atom forms with its ligands in a coordination complex.

The overall charge of a coordination complex.

In a coordination complex, the geometry is determined by the spatial arrangement of ligands around the central atom.

The central metal atom in a coordination complex is the atom to which the ligands are attached.

The central atom in a coordination complex can have a specific oxidation state, which indicates its charge.

Ligands can be classified based on their ability to donate one or more electron pairs to the central metal atom. Monodentate ligands donate one electron pair, and bidentate ligands donate two.

The theory that explains how ligands form coordinate covalent bonds with the central atom.

A complex in which the central metal atom is surrounded by only one type of ligand.