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Molecular Models

Ionic Bond Transfer of electrons so that both have an octet EN greater than or equal to 1.67
Covalent Bond Share electrons so they both have an octet EN less than 1.67
Metallic Bond Dipole, polar, alloys, protons in sea of electrons, good conductors of heat and electricity
Dipole Polar, covalent bond, net pull
Vander Waals Forces Weak, intermolecular, attractive forces
London Dispersion Forces DD (strongest), DN (intermediate), or NN (weakest)
Molecule Two or more atoms
Lewis Structure Number of valence electrons for all atoms in a molecule, organized, complete octets
Sigma Bond End-to-end single, covalent bonds
Pi Bond Covalent, sideways/parallel bonds
Single Bond Covalent, 2 shared electrons (1 sigma)
Double Bond Covalent, 4 shared electrons (1 sigma, 1 pi)
Triple Bond Covalent, 3 shared electron pairs (1 sigma, 2 pi)
Resonance The average of all Lewis structures for a molecule
VSEPR Determines shape and angle from orbital position
Hybridized Orbital The blending of two or more orbitals
Molecular Orbitals New orbitals -> new molecule Bonding and anti-bonding
Bond Order Bond strength (B-A)/2
Paramagnetic 1 or more unpaired electrons Attracted to magnetic field
Diamagnetic No unpaired electrons Not attracted to magnetic field
Coordinate Covalent Bond Shared, come from the same atom
Bonding Orbital Molecular orbital, constructive interference, less energy, more stable
Anti-bonding Orbital Molecular orbital, destructive interference, more energy, less stable *
Created by: archergirl