Bond Energy/Length
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Last updated 10:16 PM on 4/30/23
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14 Terms
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Single Bond
1 line/1 sigma bond
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Double Bond
2 lines/1 sigma & 1 pi bond
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Triple Bond
3 lines/1 sigma & 2 pi bonds
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Increasing Bond Length
Triple<Double<Single
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Increasing Bond Strength
Single<Double<Triple
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Bond Order (general)
total # of individual bonds/# of bond areas
* the closer to 0 the better the structure
* the closer to 0 the better the structure
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Formal Charge
group #-dots-sticks
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Bond Energy
deltaHrxn= sum of reactants - sum of products
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Lattice Energy
* increases as atoms get smaller
* ion1 charge \* ion2 charge
* high LE means high melting and boiling point
* ion1 charge \* ion2 charge
* high LE means high melting and boiling point
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Valence Bond Theory
* # of e- groups = # of hybrid orbitals
* look at partially filled/empty orbitals to determine overlap
* double/triple bonds are 1 e- group
* look at partially filled/empty orbitals to determine overlap
* double/triple bonds are 1 e- group
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Sigma Bond
end to end, lowers overall energy, allows free rotation
* stronger than pi bonds
* stronger than pi bonds
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Pi bond
side by side, restricts rotation
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Molecular Orbital Theory
Treats a molecule as a collection of atomic nuclei with orbitals that are delocalized over the entire molecule, thereby eliminating the need for resonance structures to depict molecules with fractional bond orders.
pi = 2 boxes
sigma = 1 box
pi = 2 boxes
sigma = 1 box
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Bond Order (Molecular Orbital ONLY)
Bond Order = 1/2(bonding-antibonding\*)
* the greater it is the more stable
* the greater it is the more stable