Dipole interactions
intermolecular forces resulting from the attraction of oppositely charges regions of polar molecules
Dispersion forces
attraction between molecules caused by the electron motion on one molecule affecting the electron motion of the other through electrical forces; these are the weakest interactions between molecules
Hydrogen bonds
attractive forces in which hydrogen is added to a carbon-carbon double bond to give an alkane
Network solids
a solid in which all of the atoms are covalently bonded to each other
covalent bond
a bond formed by the sharing of electrons between atoms
molecule
a neutral group of atoms joined together by covalent bonds
diatomic molecule
molecule consisting of two atoms
Molecular formula
a chemical formula of a molecular compound that shows the kinds and numbers of atoms present in a molecule of a compound
Single covalent bond
a bond formed when two atoms share a pair of electrons
Structural formula
a chemical formula that shows the arrangement of atoms in a molecule or a polyatomic ion; each dash between a pair of atoms indicates a pair of shared electrons
Unshared pair
a pair of valence electron that is not shared between atoms
Double covalent bond
a bond in which two atoms share two pairs of electrons
Triple covalent bond
a covalent bond in which three pairs of electrons are shared by two atoms
Coordinate covalent bond
a covalent bond in which one atom contributes both bonding electrons
Polyatomic ion
a tightly bound group of atoms that behaves as a unit and has a positive or negative charge
Bond dissociation energy
the difference in temperature between the boiling point of a solution and the boiling point of the pure solvent
Resonance structure
one of the two or more equally valid electron dot structures of a molecule or polyatomic ion
Tetrahedral angle
a bond angle of 109.50 that results when a central atom forms four bonds directed toward the center of a regular tetrahedron
VSEPR theory
valence-shell electron-pair repulsion theory; because electron pairs repel, molecules adjust their shapes so that valence electron pairs are as far apart as possible
Polar molecule
a molecule in which one side of the molecule is slightly negative and the opposite side is slightly positive
Dipole
a molecule that has two poles, or regions, with opposite charges
Van der Waal forces
the two weakest intermolecular attractions- dispersion interactions and dipole forces