Hybridization Flashcards

1
Q

What is the valence bond theory?

A

Bonding occurs when atomic orbitals overlap.

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2
Q

What does the Valence Bond Theory have problems with?

A

The shape and the bond angles.

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3
Q

What is the solution when The VBF and VSEPR theories disagree?

A

Hybrid orbitals!

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4
Q

How is the bond formation maximized?

A

Valence electrons are re-oriented and electrons clouds are reshaped. This allows optimum contact.

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5
Q

What can also occur to form as many bonds as possible from the available valence electrons?

A

The separation of electron pairs may also occur!

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6
Q

How are all 2 region species hybridized?

A

Sp hybridized.

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7
Q

How are all 3 region species hybridized?

A

sp2 hybridized

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8
Q

How are all 4 region species hybridized?

A

sp3 hybridized.

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9
Q

How do you know how many hybrid orbitals you’ll get?

A

By counting the valence electrons.

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10
Q

How are all 5 region species hybridized?

A

sp3d hybridized

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11
Q

How are all 6 region species hybridized?

A

sp3d2 hybridized

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12
Q

What is the hybridization of linear molecules?

A

sp

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13
Q

What is the hybridization of trigonal planar molecules?

A

sp2

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14
Q

What is the hybridization of tetrahedral molecules?

A

sp3

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15
Q

What is the hybridization of trigonal bipyramidal molecules?

A

sp3d

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16
Q

What is the hybridization of octahedral molecules?

A

spd2

17
Q

What can you tell about a species from the Lewis structure and the number of electronic regions?

A

The shape and the hybridization.