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Valence Bond Theory
Theory explaining bond formation via orbital interaction.
Hybridization
Mixing of atomic orbitals to form new orbitals.
Sigma Bond
Bond formed by head-on orbital overlap.
Pi Bond
Bond formed by sidewise orbital overlap.
sp3 Hybridization
Combination of one s and three p orbitals.
sp2 Hybridization
Combination of one s and two p orbitals.
sp Hybridization
Combination of one s and one p orbital.
Bond Order
Half the difference between bonding and antibonding electrons.
Paramagnetic
Substance with unpaired electrons, attracted to magnets.
Diamagnetic
Substance with all paired electrons, repelled by magnets.
LCAO Method
Linear combination of atomic orbitals to form MOs.
Molecular Orbital Theory
Theory using wave functions to describe molecular bonding.
Constructive Interference
Wave functions combine to lower energy, forming bonding MOs.
Destructive Interference
Wave functions combine to raise energy, forming antibonding MOs.
Bonding Molecular Orbital
Lower energy orbital formed by constructive interference.
Antibonding Molecular Orbital
Higher energy orbital formed by destructive interference.
Tetrahedral Geometry
Geometry with 109.5° bond angles and four groups.
Trigonal Planar Geometry
Geometry with 120° bond angles and three groups.
Octahedral Geometry
Geometry with 90° bond angles and six groups.
Bond Length
Distance between nuclei of bonded atoms.
Bond Strength
Energy required to break a bond.
Resonance
Delocalization of electrons across multiple structures.
Magnetic Behavior
Response of a substance to a magnetic field.
Quantum Mechanical Orbitals
Regions where electrons are likely found.
Electron Spin Pairing
Electrons must have opposite spins in orbitals.
Geometry of Molecules
Shape determined by orbital interactions and hybridization.
Delocalization
Electrons shared across multiple atoms in a molecule.
Note 
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