Unit 7: bonding theories Flashcards

1
Q

VSEPR?

A

Valence-Shell electron pair repulsion theory

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2
Q

VBT?

A

Valence Bond Theory

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3
Q

What does VSEPR model do?

A
  • Structure around a given atom is determined by minimizing repulsions between electron pairs
  • Predicts geometry and bond angles
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4
Q

Charged clouds?

A

Can either be:
- Single bond
- Multiple bond
- Lone pair of electrons
- Single electrons

So if there is 3 bonding pairs and 1 lone e- pair, it’s 4 charged clouds!

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5
Q

The 5 VSEPR models?

A
  • Linear
    -Trigonal planar
  • Tetrahedral
  • Trigonal bipyramid
  • Octahedral
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6
Q

2 charged electrons?

A
  • Linear model
  • Bong angle of 180 degrees minimizes electron pair repulsion
  • Ex: CO2 and HCN
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7
Q

3 charged clouds?

A
  • Trigonal planar model
  • Bond angles of 120 degrees minimize electron pair repulsion
  • Can also have a bent structure
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7
Q

4 charged clouds?

A

-Tetrahedral model
- Bond angles of 110 degrees to minimize electron pair repulsion
- Can also be trigonal pyramid and bent structure

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8
Q

5 charged clouds?

A
  • Trigonal bipyramidal
  • Expanded octet with 5 electrons pairs
  • 3 equitorial (120) and 2 axial (90)
  • Can also be seasaw, T-shape or linear
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9
Q

6 charged clouds?

A
  • Octahedral
  • expanded octet with 6 electron pairs
  • can also be square pyramidal or square planar
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10
Q

Valence bond theory?

A
  • Describes how electrons are shared
  • Involves hybridizing orbitals
  • Predicts type of bonding and explains propreties!
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11
Q

Sigma bond?

A

When atoms form bonds, the atomic orbitals of their valence electrons involved with bonding overlap and combine to produce new combinations of orbitals.

  • SINGLE BOND mainly, but also present in double and triple bonds
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12
Q

How will F + F form F2?

A

-The 2 pz1 on each atom will bond together to form 2pz2 (full)

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13
Q

Ground state electron configuration?

A
  • Nothing is done to the electrons, not energized
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14
Q

Hybridization steps?
(Example for sp3)

A

1- An electron is promoted to a higher orbital (energizes it’s own electron)
2- Nonequivalent orbitals, so second hybridization so bonds are equivalent
3- Hybridized configuration (sp3 for tetrahedral structures)

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15
Q

Definition of hybridization?

A

Fusion of atomic orbitals to form bonding orbitals!

16
Q

Examples of sp3 hybridization and tetrahedral geometry?

A
  • Methane (tetrahedral)
  • Ammonia (trigonal pyramidal)
  • Water (Bent)
17
Q

sp2 hybridization?

A
  • In trigonal planar bonds (3 charged clouds)
  • In a double bond
  • Forms pi bonds and a sigma bond
18
Q

sp hybridization?

A
  • In linear bonds (2 charged clouds)
  • In a triple bond
  • Forms pi bonds and a sigma bond
19
Q

Short-cut to hybridization?

A

= (Sum of the attached atom) + (#lone pairs)