4 bonded pairs, 0 lone pairs or 4 electron pairs. 109.5 degrees
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Octahedral
6 electron pairs. 90 degrees
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Trigonal planar
3 electron pairs. 120 degrees
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Pyramidal
3 bonded pairs, 1 lone pair. 107 degrees
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Linear
2 electron pairs. 180 degrees
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Non-linear
2 bonded pairs, 2 lone pairs. 104.5 degrees
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Electronegativity
A measure of the attraction of a bonded atom for the pair of electrons in a covalent bond
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London forces (induced dipole-dipole interactions)
Weak intermolecular forces that exist between all molecules. Relative strength increases as the number of electrons increase
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Permanent dipole-dipole interactions
An attractive force between permanent dipoles in neighbouring polar molecules
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Hydrogen bond
A strong dipole-dipole attraction between an electron-deficient hydrogen atom on one molecule and a lone pair of electrons on a highly electronegative atom on a different molecule
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