Chapter 5 and 6 electrons and bonding, shapes of molecules and intermolecular forces

orbital

a region around the nucleus that can hold up to two electrons, with opposite spins.

ionic bonding

the electrostatic attraction between positively and negatively charged ions

dative bond

a shared pair of electrons in which the bonded pair has been provided by one of the bonding atoms only

average bond enthalpy

the average energy required to break one mole of a bond in a gaseous molecule.

compound

a substance formed when two or more different elements chemically bond together.

molecule

a group of atoms chemically bonded together

covalent bond

the strong electrostatic attraction between a shared pair of electrons and the nuclei of the bonded atoms

intermolecular forces

weak interactions between dipoles of different molecules

simple molecular substances

made up of discrete molecules containing a specific number of atoms and have a constant molecular formula

hydrogen bond

a special type of dipole-dipole interaction that occurs between molecules containing a hydrogen atom bonded to a highly electronegative atom with a lone pair, such as nitrogen, oxygen, or fluorine.

electronegativity

a measure of the ability of an atom in a molecule to attract a pair of electrons in a covalent bond to itself

polar bond

a type of covalent bond where electrons are shared unequally between two atoms, resulting in a molecule with a positive and a negative end.