a bond formed by the sharing of electrons between atoms.
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Molecule
a neutral group of atoms joined together by covalent bonds.
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Diatomic molecule
a molecule consisting of two atoms.
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Molecular compound
a compound that is composed of molecules.
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Molecular formula
a chemical formula of a molecular compound that shows the kinds/numbers of atoms present in a molecule of a compound.
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Single covalent bond
a bond formed when two atoms share a pair of electrons
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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 e-.
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Unshared pair
a pair of valence e- that is not shared between atoms.
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Double covalent bond
a bond in which two atoms share two pairs of e-
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Triple covalent bond
a covalent bond in which 3 pairs of e- are shared by two atoms
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Coordinate covalent bond
a covalent bond in which one atom contributes both bonding e-.
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Bond dissociation energy
the energy required to break the bond between 2 covalently bonded atoms; expressed in kJ per mol of substance.
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Resonance structure
one of the two or more equally valid e- dot structures of a molecule or polyatomic ion.
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Molecular orbital
\: an orbital that applies to the entire molecule.
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Polyatomic ion:
a tightly bound group of atoms that behaves as a unit & has a positive or negative charge.
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Bonding orbital
a molecular orbital that can be occupied by 2 e- of a covalent bond
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Sigma bond
a bond formed when 2 atomic orbitals combine to form a molecular orbital that is symmetrical around the axis connecting the 2 atomic nuclei
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Pi bond
a covalent bond in which the bonding e- are most likely to be found in sausage shaped regions above & below the bond axis of the bonded atoms.
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Tetrahedral Angle
a bond angle of 109.5 that results when a central atom forms 4 bonds directed toward the center of a regular tetrahedron.
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VSEPR theory
valence-shell electron-pair repulsion theory; because e- pairs repel, molecules adjust their shapes so that valence e- pairs are as far apart as possible.
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Hybridization
the mixing of several atomic orbitals to form the same total number of equivalent hybrid orbitals.
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nonpolar covalent bond
\: a covalent bond in which the e- are shared equally by the 2 atoms
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Polar covalent bond
\: a covalent bond between atoms in which the e- are shared unequally.
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Polar molecule
\: a molecule in which one side of the molecule is slightly negative & the opposite side is slightly positive
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Dipole
\: a molecule that has two poles, or regions, with opposite charges
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Van der Waals forces
the two weakest intermolecular attractions-dispersion interactions & dipole forces.
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Dipole interaction
intermolecular forces resulting from the attraction of oppositely charged regions of polar molecules
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Dispersion force
\: attraction between molecules caused by the e- motion on one molecule affecting the e- motion on the other through electrical forces; weakest interactions between molecules.
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Hydrogen bond
attractive forces in which a H covalently bonded to a very electronegative atom is also weakly bonded to an unshared e- pair of another electronegative atom.
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Network solid
a solid in which all of the atoms are covalently bonded to each other.
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