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Chapter 8 vocab

VSEPR theory valence-shell electron-pair repulsion theory; molecules adjust their shapes so that valence electron pairs are as far apart as possible
Tetrahedral angle a bond angle of 109.5 that results when a central atom forms four bonds directed toward the center of a regular tetrahedron
Nonpolar covalent bond a covalent bond in which the electrons are shared equally by the two atoms
Polar covalent bond a covalent bond between atoms in which the electrons are shared unequally
Dipole a molecule that has two poles, or regions with opposite charges
Polar molecule a molecule in which one side of the molecule is slightly negative and the opposite side is slightly positive
Dipole interactions intermolecular forces resulting from the attraction of oppositely charged regions of polar molecules
Dispersion forces attractions between molecules caused by the electron motion on one molecule affecting the electron motion on the other through electrical forces
Hydrogen bonds attractive forces in which a hydrogen covalently bonded to a very electronegative atom
Network solids a solid in which all of the atoms are covalently bonded to each other
Molecular orbitals an orbital that applies to the entire molecule
Bonding orbital a molecular orbital that can be occupied by two electrons of a covalent bond
Sigma bond a bond formed when two atomic orbitals combined for form a molecular orbital that is symmetrical around the axis connecting the two atomic nuclei
Pi bond a covalent bond in which the bonding electrons are most likely to be found in sausage-shaped regions above and below the bond axis of the bonded atoms
Hybridization the mixing of several atomic orbitals to form the same total number of equivalent hybrid orbitals
Van der Waals forces the two weakest intermolecular attractions- dispersion interactions and dipole forces
Created by: VKimbrell718