Chapter 9 Review Flashcards

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
Double and triple bonds place . . . than do single bonds
greater electron density on one side of the central atom
26
Linear EDG molecules have a predicted angle of . . .
180 degrees
27
Trigonal Planar EDG molecules have a predicted angle of . . .
120 degrees
28
Tetrahedral EDG molecules have a predicted angle of . . .
109.5 degrees
29
Trigonal Bipyramidal EDG molecules have a predicted angle of . . .
90 degrees (from vertical bonds to horizontal bonds) and 120 degrees (between horizontal bonds)
30
In a Trigonal Bypyramidal EDG, lone electron pairs prefer to be in . . .
equatorial positions rather than axial positions
31
Octahedral EDG molecules have a predicted angle of . . .
90 degrees and (between lone electron pairs) 180 degrees
32
In Octahedral EDG molecules, lone electron pairs are placed . . .
opposite of each other
33
In larger molecules, there is more than one . . .
central atom
34
If electrons are shared unequally, bonds become . . .
polar
35
A molecule is polar (or nonpolar) depending on whether or not . . .
the dipoles "combine" or "cancel each other"
36
To determine if a molecule is polar or not, you must consider these two things
1. the polarity of each bond 2. Geometry of the molecule
37
Polar molecules result from . . .
a distribution of charge from polar bonds that is not symmetrical
38
The dipoles of polar molecules . . .
combine
39
The dipoles of nonpolar molecules . . .
cancel each other
40
First step to determine molecule polarity
Draw Lewis structure
41
Second step to determine molecule polarity
Determine if the bonds are polar or nonpolar
42
Third step to determine molecule polarity
Identify EDG
43
Fourth step to determine molecule polarity
Identify MG
44
Final step to determine molecule polarity
Determine if there is an asymmetry to the molecule
45
Valence Bond (VB) Theory assumes . . .
a covalent bond is formed between two atoms by the overlap of half-filled valence atomic orbitals
46
When atomic orbitals mix to form new orbitals, what are these orbitals called?
Hybrid orbitals
47
Hybrid orbitals are degenerate. In other words, they are . . .
equivalent in energy
48
The number of hybrid orbitals is equal to the number of . . .
atomic orbitals
49
An atomic s + p orbital results in . . .
2 sp hybrid orbitals
50
An atomic s + p + p orbital results in . . .
3 sp^2 hybrid orbitals
51
An atomic s + p + p + p orbital results in . . .
4 sp^3 hybrid orbitals
52
The number of hybrid orbitals is . . . the number of electron domains around a central atom
equal to