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CHEM 140 > Midterm #1 > Flashcards

Midterm #1 Flashcards

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1
Q

What 2 characteristics of carbon are why carbon is important to life?

A

(1) versatility - to make single, double, triple bonds
(lots of molecules with different shapes)

(2) bond strength - not too strong and not too weak

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2
Q

What 2 things happen to a molecule during a reaction?

A

collision

covalent bonds break/form

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3
Q

Period

A

across periodic table

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4
Q

Group

A

down periodic table (columns)

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5
Q

constitutional isomers

A

same formula but different structure/arrangement (differ in the way they are connected)

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6
Q 
O
# of valence electrons
A

6

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7
Q 
He
# of valence electrons
A

2

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8
Q 
Li
# of valence electrons
A

1

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9
Q 
Be
# of valence electrons
A

2

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10
Q 
B
# of valence electrons
A

3

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11
Q 
C
# of valence electrons
A

4

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12
Q 
N
# of valence electrons
A

5

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13
Q 
F
# of valence electrons
A

7

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14
Q 
Na
# of valence electrons
A

1

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15
Q 
Mg
# of valence electrons
A

2

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16
Q 
K
# of valence electrons
A

1

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17
Q 
Al
# of valence electrons
A

3

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18
Q 
Si
# of valence electrons
A

4

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19
Q 
P
# of valence electrons
A

5

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20
Q 
S
# of valence electrons
A

6

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21
Q 
Cl
# of valence electrons
A

7

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22
Q 
Br
# of valence electrons
A

7

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23
Q 
I
# of valence electrons
A

7

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24
Q 
At
# of valence electrons
A

7

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25
Q

Electronegativity increases…

A

left to right across period (row)

bottom to top of group (column)

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26
Q

Electronegativity of Li

A

1.0

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27
Q

Electronegativity of Be

A

1.5

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28
Q

Electronegativity of C

A

2.5

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29
Q

Electronegativity of N

A

3.0

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30
Q

Electronegativity of O

A

3.5

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31
Q

Electronegativity of F

A

4.0

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32
Q

Electronegativity of Na

A

0.9

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33
Q

Electronegativity of Mg

A

1.2

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34
Q

Electronegativity of Al

A

1.5

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35
Q

Electronegativity of Si

A

1.8

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36
Q

Electronegativity of P

A

2.1

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37
Q

Electronegativity of S

A

2.5

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38
Q

Electronegativity of Cl

A

3.0

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39
Q

Electronegativity of K

A

0.8

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40
Q

Electronegativity of Br

A

2.8

41
Q

Covalent bonds

difference in EN?

A

<0.5

42
Q

Polar covalent bonds

difference in EN?

A

0.5< EN<1.7

43
Q

Ionic bonds

difference in EN?

A

> 1.7

44
Q

C-Br

what kind of bond?

A

polar covalent

45
Q

Induction

A

withdrawal of e toward EN atom

46
Q

4 sigma bonds - has what kind and how many hybridized orbitals?

A

4 sp3

47
Q

3 sigma bonds, 1 pi bond - has what kind and how many hybridized orbitals?

A

3 sp2 `

48
Q

2 sigma bonds, 2 pi bonds - what kind and how many hybridized orbitals?

A

2 sp

49
Q

steric number

A

total number of s bonds and lone pairs

50
Q

For any sp3 hybridized atom, the 4 valence e’s will form a ____ electorn group geometry

A

tetrahedral

51
Q

Steric number = 4

no lone pairs

A

sp3

tetrahedral

52
Q

Steric number = 4

1 lone pair

A

sp3

trigonal pyramidal

53
Q

Steric number = 4

2 lone pairs

A

sp3

bent

54
Q

Steric number = 3

one lone pair

A

sp2

bent

55
Q

Steric number = 3

no lone pairs

A

sp2

trigonal pyramidal

56
Q

Steric number = 2

A

sp

linear

57
Q

dipole moment

A

center of negative and positive charge are separated from each other by a certain distance

58
Q

molecular dipole moment

A

vector sum of individual dipole moments

-sum of magnitude and direction of each dipole moment

59
Q

carbocation

A

ion containing + charged carbon atom

60
Q

carbanion

A

ion containing - charged carbon atom

61
Q

delocalization of either a + or - charge __ a molecule

A

stabilizes

62
Q

curved arrows generally show?

A

electron movement for PAIRS

63
Q

curved arrows start where?

end where?

A

start where electrons are currently located

end where electrons will end up

64
Q

Bronsted-Lowry Acid

A

proton donor

65
Q

Bronsted-Lowry Base

A

proton acceptor

66
Q

conjugate acid is the product that results when ?

A

base is protonated

67
Q

conjugate base is the product that results when?

A

acid is deprotonated

68
Q

curved arrows are used to illustrate a ?

A

reaction mechanism - how a reaction occurs in terms of the motion of electrons

69
Q

value of Ka measures?

A

measures strength of acid

70
Q

strong acid has __ Ka and a ___ pKa

A

high Ka, low pKa

71
Q

weak acid has __ Ka and a ___ pKa

A

low Ka, high pKa

72
Q

4 factors affecting stability of (-) charge

A

1) type of atom that carries charge
2) resonance
3) induction
4) type of orbital where charge resides

73
Q

When two atoms are in the same row, which atom is better at stabilizing (-) charge?

A

ELECTRONEGATIVITY is dominant effect

more EN atom is better at stabilizing charge

74
Q

When two atoms are in the same group (column), which atom is better at stabilizing (-) charge?

A

SIZE is dominant effect

Larger atom can better stabilize the (-) charge

75
Q

How does RESONANCE affect stability of negative charge?

A

delocalized charge is more stable

resonance structures show electron delocalization

76
Q

How does INDUCTION affect stability of negative charge?

A

if atoms withdraw e density away from negatively charged region of compound, it stabilizes (-) charge

77
Q

How does TYPE OF ORBITAL affect stability of negative charge?

A

sp orbitals hold e’s closer to nucleus than sp2 or sp3

therefore sp is more stable

78
Q

Order of priority for stabilizing negative charge?

A 
ARIO 
atom (EN) 
resonance
induction
orbitals
79
Q

Steric hindrance occurs when…

A

the large size of groups within a molecule prevents chemical reactions that are observed in related molecules with smaller groups

80
Q

lewis acid

A

e pair acceptor

81
Q

lewis base

A

e pair donor

82
Q

Not all __ acid/bases can’t be classified as __ acid/bases

A

Lewis

BL

83
Q

Hydrocarbon

A

compounds comprised of JUST C and H

84
Q

Saturated Hydrocarbons or ALKANES

A

hydrocarbons that lack pi boinds

85
Q

Isopropyl

A

(1-methylethyl)

86
Q

sec-Butyl

A

(1-methylpropyl)

87
Q

Isobutyl

A

(2-methylpropyl)

88
Q

tert-Butyl

A

(1,1-dimethylethyl)

89
Q

Isopentyl or isoamyl

A

(3-methylbutyl)

90
Q

Neopentyl

A

(2,2-dimethylpropyl)

91
Q

dihedral angle or torsional angle

A

angle between two atoms on different carbons

92
Q

torsional strain

A

difference in energy b/w staggered and eclipsed conformations

93
Q

gauche interaction

A

steric interaction that results when two groups are seperated by 60

94
Q

anti conformation

A

staggered conformation with dihedral angle of 180

95
Q

angle strain

A

increase in energy associated with bond angle that has deviated from preferred angle of 109.5

96
Q

most stable conformation of the cyclohexane ring is?

A

chair conformation

97
Q

In chair conformation, all H’s are?

A

staggered

98
Q

axial

A

parallel to vertical axis passing through center of ring

99
Q

equatorial

A

positioned at angles parallel to the sets of parallel lines

CHEM 140 (3 decks)

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