Valence and MO Theories Flashcards

1
Q

Valence Bond Theory

A

A covalent bond forms when orbital of two atoms overlap, and a pair of electrons is localized in the region between the atoms

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2
Q

3 Principles of Valence Bond Theory

A
  1. The pair of electrons has opposite spins
  2. Good, in-phase overlap leads to strong bonding interactions
  3. Orbitals can hybridize to more appropriate shapes and orientations, to maximize overlap.
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3
Q

Molecular Orbital Theory and basic principle

A

A bonding approach in which quantum mechanics is applied to molecules

The Schrödinger equation is solved for electrons in a molecule, resulting in molecular orbitals

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4
Q

Molecular Orbitals Similarities to Atomic Orbitals

A

They can each hold two electrons w/ opposite spins
The square of the molecular orbital wave function gives the probability function

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5
Q

Features of MO diagrams

A
  • Number of MOs = AOs
  • Combining 2 AOs gives a bonding MO and an antibonding MO
  • In ground state configurations, electrons occupy lowest energy MO upwards
  • Bond strength can be measured by the calculated bond order
  • Bond order = 1/2(no. of bonding es - no. of non-bonding es)
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6
Q

How do you calculate Bond Order?

A

Calculate from Molecular Order Theory
BO = 1/2(MO-MO*)
= 1/2 (bonding e - antibonding e)

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7
Q

Sigma Bond

A

End-to-end overlap of orbitals with electron density along axis of bond from MO Theory

single bonds and first overlap in multi-bonds

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8
Q

Pi bond

A

side-to-side overlap of orbitals, with electron density above and below axis of bond in MO theory

extra overlaps in multiple bonds

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9
Q

Limitations of Hybridization Schemes

A
  • VBT does not always match experimental data
  • Don’t work for d-orbitals
  • Misleading when molecules have resonance
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10
Q

Hybridization

A

A hypothetical process so tetrahedral geometry can be modified to create hybrid orbitals when bonding occurs

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11
Q

MO Triangle shape and Nonmetals

A

Sigma
Pi pi
Sigma
Pi pi

B2 C2 N2

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12
Q

MO oval shape and Nonmetals

A

Sigma
Pi pi
Pi pi
Sigma

O2 F2

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13
Q

Hybridization Rules

A

Number of hybrid orbitals = number of orbitals mixed

Type of hybrid orbitals varies on the types of atomic orbitals mixed (s + p = sp)

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14
Q

Bond Order Trend

A

Positive ion = low bond order
Negative ion = high bond order

Fewest antibonding electrons

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15
Q

Bond Length Trend

A

Reverse of bond order trend

positive ion = longest bond length

negative ion = shortest bond length

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