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Chemistry > Chapter 9 Review > Flashcards

Chapter 9 Review Flashcards

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1
Q

What parts of a molecule define the shape and size of the molecule?

A

The bond angles and bond lengths

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2
Q

What determines the properties of a substance?

A

The shape of the molecule, the size of the molecule, the strength of its bonds, and the polarity of the bonds

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3
Q

Electron domains are . . .

A

regions where electrons are likely to be found around an atom

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4
Q

What is considered as ONE electron domain?

A

a single bond, a double bond, a triple bond, and a lone pair

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5
Q

The BEST arrangement of a given number of electron domains is the one that . . .

A

minimizes the repulsions among them

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6
Q

Molecular Geometry is . . .

A

the arrangement of only the bonded atoms in a molecule or ion

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7
Q

Molecular Geometry describes . . .

A

the shape of only those electron domains that contain bonding electrons

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8
Q

Determine Molecular Geometry by . . .

A

counting the number of bonding domains

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9
Q

2 electron domains, 0 nonbonding domains

A

linear

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10
Q

3 electron domains, 0 nonbonding domains

A

Trigonal Planar

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11
Q

3 electron domains, 1 nonbonding domain

A

Bent

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12
Q

4 electron domains, 0 nonbonding domains

A

Tetrahedral

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13
Q

4 electron domains, 1 nonbonding domain

A

Trigonal Pyramidal

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14
Q

4 electron domains, 2 nonbonding domains

A

Bent

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15
Q

5 electron domains, 0 nonbinding domains

A

Trigonal Bipyramidal

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16
Q

5 electron domains, 1 nonbonding domain

A

Seesaw

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17
Q

5 electron domains, 2 nonbonding domains

A

T-Shaped

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18
Q

5 electron domains, 3 nonbonding domains

A

Linear

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19
Q

6 electron domains, 0 nonbonding domains

A

Octahedral

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20
Q

6 electron domains, 1 nonbinding domain

A

Square Pyramidal

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21
Q

6 electron domains, 2 nonbonding domains

A

Square Planar

22
Q

Nonbonding electron pairs are . . . than bonding pairs

A

physically larger

23
Q

Because nonbonding electron pairs are physically larger than bonding pairs, they . . .

A

have greater repulsions

24
Q

Nonbonding pairs tend to . . .

A

decrease angles in a molecule

25
Q

Double and triple bonds place . . . than do single bonds

A

greater electron density on one side of the central atom

26
Q

Linear EDG molecules have a predicted angle of . . .

A

180 degrees

27
Q

Trigonal Planar EDG molecules have a predicted angle of . . .

A

120 degrees

28
Q

Tetrahedral EDG molecules have a predicted angle of . . .

A

109.5 degrees

29
Q

Trigonal Bipyramidal EDG molecules have a predicted angle of . . .

A

90 degrees (from vertical bonds to horizontal bonds) and 120 degrees (between horizontal bonds)

30
Q

In a Trigonal Bypyramidal EDG, lone electron pairs prefer to be in . . .

A

equatorial positions rather than axial positions

31
Q

Octahedral EDG molecules have a predicted angle of . . .

A

90 degrees and (between lone electron pairs) 180 degrees

32
Q

In Octahedral EDG molecules, lone electron pairs are placed . . .

A

opposite of each other

33
Q

In larger molecules, there is more than one . . .

A

central atom

34
Q

If electrons are shared unequally, bonds become . . .

A

polar

35
Q

A molecule is polar (or nonpolar) depending on whether or not . . .

A

the dipoles “combine” or “cancel each other”

36
Q

To determine if a molecule is polar or not, you must consider these two things

A
  1. the polarity of each bond
  2. Geometry of the molecule
37
Q

Polar molecules result from . . .

A

a distribution of charge from polar bonds that is not symmetrical

38
Q

The dipoles of polar molecules . . .

A

combine

39
Q

The dipoles of nonpolar molecules . . .

A

cancel each other

40
Q

First step to determine molecule polarity

A

Draw Lewis structure

41
Q

Second step to determine molecule polarity

A

Determine if the bonds are polar or nonpolar

42
Q

Third step to determine molecule polarity

A

Identify EDG

43
Q

Fourth step to determine molecule polarity

A

Identify MG

44
Q

Final step to determine molecule polarity

A

Determine if there is an asymmetry to the molecule

45
Q

Valence Bond (VB) Theory assumes . . .

A

a covalent bond is formed between two atoms by the overlap of half-filled valence atomic orbitals

46
Q

When atomic orbitals mix to form new orbitals, what are these orbitals called?

A

Hybrid orbitals

47
Q

Hybrid orbitals are degenerate. In other words, they are . . .

A

equivalent in energy

48
Q

The number of hybrid orbitals is equal to the number of . . .

A

atomic orbitals

49
Q

An atomic s + p orbital results in . . .

A

2 sp hybrid orbitals

50
Q

An atomic s + p + p orbital results in . . .

A

3 sp^2 hybrid orbitals

51
Q

An atomic s + p + p + p orbital results in . . .

A

4 sp^3 hybrid orbitals

52
Q

The number of hybrid orbitals is . . . the number of electron domains around a central atom

A

equal to

Chemistry (17 decks)

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