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Bonding
overlap or orbitals on 2 atoms to form a molecular orbital
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Orbital
Describes the region where electrons are likely to be (95%)
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Sigma bond
First bond, symmetrical with respect to rotation along bond axis
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Pi bond
Second and third bonds, not symmetrical with respect to rotation along bond axis
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MO Theory
Form molecular orbitals by making linear combination of atomic orbitals
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How many molecular orbitals per atomic orbital
1
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Bonding orbital
high electron density between nuclei
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Antibonding orbital
Low electron density between nuclei-contains node
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How many electrons per molecular orbital
2
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Bonding/antibonding higher or lower in energy than AO
Bonding-lower,antibonding-higher
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Pauli Exclusion principle only applies to
Molecular orbitals
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Bond order formula
Bonding-antibonding/2
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Li2-N2 order of molecular orbitals
σ2s, σ2s*, π2p, σ2p, π2p*, σ2p*
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O2, F2, beyond molecular orbitals
σ2s, σ2s*, σ2p, π2p, π2p*, σ2p
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Paramagnetic
Unpaired electron spins, attracted to magnetic field
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Diamagnetic
Paired spins, repelled by magnetic field
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Heteronuclear Diatomics
- Molecule consisting of 2 different atoms
- If molecule contains only 2nd period elements except O or F, use Li2-N2 filling order
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What orbitals contribute significantly to molecular orbitals
valence orbitals
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Delocalization
When you have a network of adjacent atoms with unhybridized p orbitals, the pi bond spreads over entire network
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