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CHEM 1570: Intro to Organic and Biological Chemistry > Prelim 1 > Flashcards

Prelim 1 Flashcards

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1
Q

How many bonds does C need for an octet?

A

4 bonds

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2
Q

What is a stable octet?

A

8 valence electrons

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3
Q

What do Lewis structures consist of?

A

Lewis structures consist of:
- dots showing individual electrons

  • “lone pairs”, which are 2 electrons next to each other
  • 1-3 lines between 2 atoms (can be the same type of atom) indicating a bond
  • the shorthand for the atom name (ex: C, N, H, O, etc.) written at the ends of each line indicating the atoms bonded to each other
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4
Q

What do condensed structures look like?

A

Condensed structures are a shorthand for drawing Lewis structures that consist of the atoms of the Lewis structures written in an ordered, single line.

Ex: CH3CH2CH2CH2CH2CH3 or CH3(CH2)4CH3

*Pretend the 3 is a subscript

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5
Q

What are the rules for creating condensed structures?

A
  • Atoms of the longest chain* must be written
    horizontally
  • Ligands (atoms that are bound to another atom) are
    written to the atom’s right
    Ex: NH3 (H3, the ligand, is written to the right of N)
  • Lone pairs of e- are not shown
  • Collapsing atoms
    - Subscripts are used to depict the # of atoms
  • Parentheses used to depict polyatomic ligands bonded
    to another atom
    Ex: HOCH2CH2CH(NH2)CH3
  • Bonds to C are omitted
    - If necessary, use explicit bonds to clarify
    attachment

*What counts as the “longest chain” depends on the molecule

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6
Q

What do Lewis structures look like?

A

Lewis structures:

                H         H         H        H         H
                |          |          |        |          | 
       H  --- C  ----  C   ---   C  ---- C  ----   C  --- H
                 |          |          |       |          |
                 H        H          H       H         H
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7
Q

What do line-bond/skeletal structures look like?

A

/\/\/

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8
Q

What are the rules for creating line-bond/skeletal structures?

A
  • Every “corner” is a C (unless labeled otherwise)
  • Every line end is a C (unless labeled otherwise)
  • Hs on Cs are invisible
    - Exception: If C is explicitly written, then its bonded
    Hs must be written
  • Hs on heteroatoms drawn, not necessarily w/ a bond
    - It CAN be drawn w/ a bond if you want to draw it
  • Lone pairs (non-bonding e-) on heteroatoms are
    optional
    - Exception: If the lone pair(s) are being used in a
    mechanism/indicated you must draw them
  • Complete octets on nearly everything
    - Exception: H (2 ve-), sometimes B*, etc.
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9
Q

What’s special about Halogens?

A
  • Halogens have 8 ve-
  • Halogens do not make bonds because they are stable
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10
Q

How to find the number of ve- in an atom?

A

Consult the periodic table:
- At the top of each column in some periodic tables it will have a number 1-8, which informs you how many valence electrons the elements in that column has

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11
Q

How many lone pairs are assumed in O?

A

2 lone pairs (4 electrons)

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12
Q

How many lone pairs are assumed in N?

A

1 lone pair (2 electrons)

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13
Q

How many lone pairs are assumed in Br?

A

3 lone pairs ( 6 electrons)

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14
Q

What is the rule for nonbonding e- on C?

A

Non-bonding e- on C must be explicitly drawn.

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15
Q

What is the rule for nonzero formal charges?

A

Nonzero formal changes MUST be shown.

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16
Q

What is the formal charge of a C w/ one bond?

A

The formal charge does not exist.

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17
Q

What is the formal charge of a C w/ 3 bonds?

A
  • Positive
  • Negative
  • No formal charge
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18
Q

What is the formal charge of an N w/ 1 bond?

A
  • The formal charge does not exist.
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19
Q

What is the formal charge of an N w/ 2 bonds?

A
  • Positive
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20
Q

What is the formal charge of an N w/ 3 bonds?

A
  • No formal charge
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21
Q

What is the formal charge of an N w/ 4 bonds?

A
  • Positive
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22
Q

What is the formal charge of an O w/ 1 bond?

A
  • Negative
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23
Q

What is the formal charge of an O w/ 2 bonds?

A
  • No formal charge
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24
Q

What is the formal charge of an O w/ 3 bonds?

A
  • Positive
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25
Q

What is the formal charge of an O w/ 4 bonds?

A
  • The formal charge does not exist
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26
Q

What is the formal charge of a halogen w/ 1 bond?

A
  • No formal charge
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27
Q

What is the formal charge of a halogen w/ 2 bonds?

A
  • Positive
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28
Q

What is the formal charge of a halogen w/ 3 bonds?

A
  • The formal charge does not exist
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29
Q

What is the formal charge of a halogen w/ 4 bonds?

A
  • The formal charge does not exist
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30
Q

How many ve- does C have?

A

4 ve-

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31
Q

How many ve- does H have?

A

1 ve-

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32
Q

How many ve- does O have?

A

6 ve-

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33
Q

How many ve- does N have?

A

5 ve-

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34
Q

How many ve- does P have?

A

5 ve-

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35
Q

How many ve- does S have?

A

6 ve-

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36
Q

How many bonds does H need for an octet?

A

1 bond

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37
Q

How many bonds does O need for an octet?

A

2 bonds

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38
Q

How many bonds does N need for an octet?

A

3 bonds

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39
Q

How many bonds does P need for an octet?

A

3 bonds

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40
Q

How many bonds does S need for an octet?

A

2 bonds

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41
Q

How to determine the number of ve- (in an entire molecule)

A
  • Find the sum of all the different ve- contributions from every atom present in the molecule

Ex: Find the number of ve- in H2S
*Pretend 2 is a subscript

H: 1 ve- S: 6 ve- # ve- = 1 ve- + 1ve- + 6ve- = 8ve-
(2 Hs= 2 ve-)

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42
Q

Hydrocarbon w/ CC single bonds.

A
  • Alkane
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43
Q

Hydrocarbon w/ CC double bonds

A
  • Alkene
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44
Q

Hydrocarbon w/ CC triple bonds

A
  • Alkyne
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45
Q

A functional group where in the hydrocarbon setup, a halogen(s) will take the place of hydrogen. (single bond)

A

-Halide

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46
Q

-ane

A
  • Alkane
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47
Q

-ene

A
  • Alkene
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48
Q

-yne

A
  • Alkyne
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49
Q

C single bonded to one OH group

A
  • Alcohol
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50
Q

-ol

A
  • Alcohol
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51
Q

C single bonded to one SH group

A
  • Thiol
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52
Q

-thiol

A
  • Thiol
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53
Q

O single bonded to C on either side

A
  • Ether
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54
Q

-sulfide

A
  • Sulfide
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55
Q

S single bonded to C on either side

A
  • Sulfide
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56
Q

-disulfide

A
  • Disulfide
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57
Q

2 Ss single-bonded to each other and single-bonded to one C on either side

A
  • Disulfide
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58
Q

-amine

A
  • Amine
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59
Q

C single bonded to N

A
  • Amine
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60
Q

C double bonded to N

A
  • Imine
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61
Q

-nitrile

A
  • Nitrile
62
Q

C triple bonded to N

A
  • Nitrile
63
Q

C double bonded to O

A
  • Carbonyls
64
Q

-al

A
  • Aldehyde
65
Q

C double bonded to O and single bonded to 1 H

A
  • Aldehyde
66
Q

-one

A
  • Ketone
67
Q

C double bonded to O and single bonded to 2 Cs

A
  • Ketone
68
Q

-oic acid

A
  • Carboxylic acid
69
Q

C double bonded to O and single bonded to an OH group

A
  • Carboxylic acid
70
Q

(-CN)

A
  • Nitrile
71
Q

(-COH)

A
  • Aldehyde
72
Q

(-COOH)

A
  • Carboxylic Acid
73
Q

-oate

A
  • Ester
74
Q

O single bonded to a carbonyl and single bonded to C

*There is typically a CH3 bonded to the C in the carbonyl

A
  • Ester
75
Q

-thiooate

A
  • Thioester
76
Q

N single bonded to a carbonyl

A
  • Amide
77
Q

-amide

A
  • Amide
78
Q

-oic anhydride

A
  • Carboxylic acid anhyrdide
79
Q

O single bonded to 2 carbonyls

A
  • Carboxylic acid anhydride
80
Q

Carbonyl w/ an -SR’ group

A
  • Thioester
81
Q

-phosphate

A
  • Phosphate
82
Q

P double bonded to O and single bonded to 3 Os

*All Os have a negative formal charge (1 bond)

A
  • Phosphate
83
Q

1 phosphate group bonded to another atom

*Depending on O that is bonded to another atom, it will have either a negative (2 bonds) or positive (3 bonds) formal charge.

A
  • Monophosphate
84
Q

2 phosphate groups bonded to each other, w/ one phosphate group bonded to another atom

A
  • Diphosphate
85
Q

-disphosphate

A
  • Diphosphate
86
Q

-triphosphate

A
  • Triphosphate
87
Q

3 phosphate groups bonded to each other, w/ one phosphate group bonded to another atom

A
  • Triphosphate
88
Q

-OPi

A
  • Monophosphate
89
Q

-OPiPi

A
  • Diphosphate
90
Q

-OPP

A
  • Diphosphate
91
Q

-OPPP

A
  • Triphosphate
92
Q

-OPiPiPi

A
  • Triphosphate
93
Q

What is an orbital?

A

The most probable location to find an electron

94
Q

What is the shape of an s-orbital?

A
  • Sphere
95
Q

What is the shape of a p-orbital?

A
  • Dumbbell
96
Q

What is the shape of a d-orbital?

A

4-Cloveleaf

97
Q

Which electrons emit lower energy levels?

A

Electrons closer to the nucleus

98
Q

Which electrons emit higher energy levels?

A

Electrons farthest the nucleus

99
Q

The prefix for 1

A

meth-

100
Q

The prefix for 2

A

eth-

101
Q

The prefix for 3

A

prop-

102
Q

The prefix for 4

A

but-

103
Q

The prefix for 5

A

pent-

104
Q

The prefix for 6

A

hex-

105
Q

The prefix for 7

A

hept-

106
Q

The prefix for 8

A

oct-

107
Q

The prefix for 9

A

non-

108
Q

The prefix for 10

A

dec-

109
Q

The ending for alkanes that has a branch

A

-yl

110
Q

di-

A

2

111
Q

tri-

A

3

112
Q

tetra-

A

4

113
Q

penta-

A

5

114
Q

What is a cycloalkane

A

A hydrocarbon ring with C single bonds

115
Q

What is a constitutional isomer?

A

Molecules that have the same chemical formulas, but different bonds connecting the atoms.

116
Q

“-yl”

A

Branching

117
Q

What is the first step in naming molecules?

A

Counting the longest Carbon chain

118
Q

Do molecules with -OH groups have high or low boiling points?

A

Molecules w/ -OH groups have high boiling points

119
Q

What is bond polarity?

A

The unequal sharing of e(-) within a covalent bond

120
Q

What does bond polarity lead to?

A

Charge seperation

Think: H2O (Water)

121
Q

What are non-polar bonds?

A

Bonds w/ very VERY little charge seperation

122
Q

What are polar bonds?

A

Polar bonds have some charge seperation

  • More electronegative atoms will have a more negative
    charge surrounding it. Less electronegative atoms will
    have a more positive charge surrounding it.
123
Q

FON

A

Hydrogen bonds

124
Q

Are hydrogen bonds strong or weak bonds?

A

Hydrogen bonds are strong dipole-dipole interactions

125
Q

What are the atoms involved in hydrogen bonding?

A

FON
F - H
O - H
N - H

126
Q

List the intermolecular forces from the strongest to weakest bonds

A

Strongest: Ionic bonds
Hydrogen bonds
Weakest: Dispersion / London Bridge bonds /
Vanderwaals Interactions

127
Q

What happens to the boiling point as intermolecular forces get stronger?

A

Boiling point increases

128
Q

Why does the boiling point of a molecule increase as the strength of intermolecular forces increases?

A

Stronger intermolecular forces require more energy to break. Heat is a form of energy, thus more heat is required to break the strong bonds.

129
Q

What is the relationship between surface area and dispersion forces?

A

The bigger the surface area, the higher the dispersion forces

130
Q

What happens to the boiling point of a molecule as the number of C increases?

A

The boiling point increases

131
Q

There are two molecules with the same carbon chain. However, one molecule has branched and the other does not. Out of the two molecules which one will have the higher boiling point?

A

The molecule without the branching b/c it has a higher surface area than the molecule with branching.

Larger surface area = higher boiling point.

132
Q

What is the relationship between branched molecules and boiling points?

A

More branching = lower surface area = lower boiling point

133
Q

What is solubility?

A

The ability of molecules to dissolve in water

134
Q

Hydrophobic

A

“Water fearing”

Refers to molecules that do not dissolve in water

135
Q

Hydrophilic

A

“Water loving”

Refers to molecule that dissolve in water

136
Q

What is the polarity of a molecule with no polar bonds?

A

Nonpolar

137
Q

What is the polarity of C-H bonds?

A

(For the sake of the class) Nonpolar

138
Q

What is the polarity of a molecule with at least 1 polar bond?

A

Polar

139
Q

What is the polarity of C-O bonds?

A

Polar

140
Q

What is the polarity of a molecule that has multiple polar bonds and the bond’s bipole movements oppose/cancel out each other?

Hint: Think CF(4)

A

Nonpolar

141
Q

Terahedron

A

A molecule w/ 4 bonds

  • 1 of the 4 bonds is in the plane of the page (dashes)
  • 1 of the 4 bonds is out of the plane of the page (wedge)
142
Q

Draw a tetrahedron molecule

A
  • 2 lines in the plane of the page
  • 1 dash
  • 1 wedge
143
Q

What is the hybridization of a tetrahedron?

A

sp^3

144
Q

What is the hybridization of a molecule with double bonds?

A

sp^2

145
Q

What is the hybridization of a molecule with triple bonds?

A

sp

146
Q

What is the hybridization of an atom with 4 regions of e- density?

A

sp^3
- Tetrahedron

147
Q

What is the hybridization of an atom with 3 regions of e- density?

A

sp^2

148
Q

What is the hybridization of an atom with 2 regions of e- density?

A

sp

149
Q

What counts as a region of e- density?

A

Bonds + lone pairs of e-

150
Q

What is conjugation?

A

When double bonds skip in a continuous array

CHEM 1570: Intro to Organic and Biological Chemistry (4 decks)

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