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JECA Chemistry Ch 16

JECA Chemistry Chapter 16 Vocabulary

molecular orbital with an enery that is higher than that of the atomic orbitals from which it is formed Antibonding orbital
the amount of energy required to break a covalent bond between atoms; this value is usually expressed in kJ per mol of substance Bond dissociation energy
molecular orbital whose energy is lower than that of the atomic orbitals from which it is formed Bonding orbital
a covalent bond formed when one atom contributes both bonding electrons Coordinate covalent bond
a substance that is weakly repelled by a magnetic field Diamagnetic
a molecule that has two elecrically charged regions or poles Dipole
a weak intermolecular force resulting from the attraction of oppositely charged regions of polar molecules Dipole interaction
the weakest kind of intermolecular attraction; this attraction is thought to be caused by the motion of electrons Dispersion force
a covalent bond is which two pairs of electrons are shared by two atoms Double covalent bond
process in which several atomic orbitals mix to form the same number of equivalent hybrid orbitals Hybridization
relatively strong intermolecular force in which a hydrogen atom that is covalently bonded to a very electronegative atom is also weakly bonded to an unshared electron pair of another electronegative atom in the same molecule or one nearby Hydrogen bond
an orbit resulting from the overlapping of atomic orbitals when two atoms combine Molecular orbit
substance in which all of the atomes are covalently bonded to eachother Network solid
bond formed when the atoms in a molecule are alike and the bonding electrons are shared equally Nonpolar covalent bond
a term used to describe a substance that shows a relatively strong attraction to an external magnetic field; these substances have molecules containing one of more unpaired electrons Paramagnetic
a bond in which the bonding electrons are most likely to be found in the sausage-shaped regions above and below the nuclei of the bonded atoms Pi bond
a bond formed when two diffrent atoms are joined by a covalent bond and the bonding elecrons are shared unequally Polar bond
a bond formed when two diffrent atoms are joined by a covalent bond and the bonding elecrons are shared unequally Polar covalent bond
a molecule,like water, in which one or more atoms is slightly negative and one or more is slightly positive, unless molecular geometry causes the polarities to cancel each other out Polar molecule
one of two or more equally valid electron dot structures for a molecule or polyatomic ion; the actual bonding is a hybrid, or mixture of the resonance structures Resonance structure
a bond formed when two atomic orbitals combine to form a molecular orbital that is symmertrical along the axis connecting the two atomic nuclei Sigma bond
a bond formed when a pair of electrons is shared between two atoms Single covalent bond
chemical formula that shows the arrangement of atoms in a molecule or a polyatomic ion; each dash between two atoms indicates a pair of shared electrons Structural formula
a bond angle of 109.5 degrees created when a central atom forms four bonds directed toward the corners of a regular tetrahedron Tetrahedral angle
covalent bond in which three pairs of electrons are shared by two atoms Triple covalent bond
a pair of valence electrons that is not involved in bonding Unshared pair
a term used to describe the weakest intermolecular attractions; these include dispersion forces and dipole interactions Van der Waals force
valence-shell electron-pair repulsion theory: because electron pairs repel, molecules adjust thier shapes so that valence-electron pairs are as far apart as possible VSEPR theory
Created by: hcatalino