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Organic Chemistry Test 1 > General Review > Flashcards

General Review Flashcards

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1
Q

The nucleus contains ______ and ________

A

Protons and neutrons

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2
Q

Protons are ______ charged and neutrons are _______

A

Positively charged, neutral

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3
Q

How many electrons can each shell contain?

A

2n^2, where n=shell number

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4
Q

How many electrons can shell 1 contain?

A

2 electrons

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5
Q

How many electrons can shell 2 contain?

A

8 electrons

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6
Q

How many electrons can shell 3 contain?

A

18 electrons

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7
Q

Shell 3 is _______ in energy than shell 1

A

Higher

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8
Q

Why are higher shells higher in energy?

A

Electrons are further away from the nucleus

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9
Q

Why are lower shells lower in energy?

A

Electrons are closer to the nucleus

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10
Q

What subshells is each shell broken into?

A

s, p, d, and f

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11
Q

What does electron configuration describe?

A

The number and position of electrons in orbitals

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12
Q

What is the ground state configuration?

A

The lowest energy configuration

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13
Q

What rules is ground state determined by?

A

The Aufbau Principle, the Pauli Exclusion Principle, and Hund’s Rule

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14
Q

What does the Aufbau Principle state?

A

Orbitals must be filled from lowest energy to highest energy

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15
Q

What does the Pauli’s Exclusion Principle state?

A

Only 2 electrons per orbital, and spins must be opposite (spin up with spin down)

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16
Q

What does Hund’s Rule state?

A

Add one electron to each orbital equal in energy to minimize electron repulsion

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17
Q

Why do we mainly focus on valence electrons?

A

They affect the physical and chemical properties of their atoms and they are involved in bonding

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18
Q

What does the octet rule state?

A

Each element is constantly trying to achieve a noble gas configuration (8 electrons in their valence shell)

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19
Q

Why do chemical bonds form?

A

Chemical bonds are formed in an attempt to complete an octet and thus achieve noble gas configuration

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20
Q

What is a molecule with a net positive electric charge known as?

A

A cation

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21
Q

What is a molecule with a net negative electric charge known as?

A

An anion

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22
Q

Is sodium (Na) more likely to lose one electron or gain 7 electrons to complete its octet?

A

Lose one electron

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23
Q

What other element’s configuration will sodium achieve by losing one electron?

A

Neon

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24
Q

Is fluorine more likely to lose 7 electrons or gain 1 electron to complete its octet?

A

Gain one electron

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25
Q

What other element’s configuration will fluorine achieve by gaining one electron?

A

Neon

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26
Q

What is a covalent bond?

A

A bond formed by sharing electrons between 1 or more atoms

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27
Q

How many electrons do single bonds share?

A

2 electrons

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28
Q

How many electrons do double bonds share?

A

4 electrons

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29
Q

How many electrons do triple bonds share?

A

6 electrons

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30
Q

What are non-binding electrons known as?

A

Lone pairs

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31
Q

What kind of bond is formed when electrons are not shared equally between atoms?

A

Polar bonds

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32
Q

How can one predict the polarity of a particular bond?

A

Use the periodic table to observe the electronegativity trend (increases from left to right and down to up)

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33
Q

What is an ionic bond?

A

A bond in which electrons are fully transferred

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34
Q

What occurs as a result of an ionic bond?

A

A formal charge

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35
Q

1 lone pair = how many regions of electron density?

A

One region

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36
Q

A single bond = how many regions of electron density?

A

One region

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37
Q

A double bond = how many regions of electron density?

A

One region

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38
Q

A triple bond = how many regions of electron density?

A

One region

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39
Q

What is the geometry of a molecule with four regions of electron density spread out over a sphere?

A

Tetrahedral

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40
Q

What is the angle between regions of electron density in a tetrahedral molecule?

A

109.5 degrees

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41
Q

What is the geometry of a molecule with three regions of electron density spread out over a sphere?

A

Trigonal planar (within the same plane)

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42
Q

What is the angle between regions of electron density in a trigonal planar molecule?

A

120 degrees

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43
Q

What is the geometry of a molecule with two regions of electron density spread out over a sphere?

A

Linear

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44
Q

What is the angle between regions of electron density in a linear molecule?

A

180 degrees

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45
Q

What is a resonance structure?

A

An altered form of a molecule. Two or more valence bond structures of the same molecule.

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46
Q

How do electrons move around a molecule?

A

In clouds of electron density

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47
Q

A resonance hybrid depicts ____________.

A

The actual structure of a compound

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48
Q

How does one obtain a resonance hybrid?

A

Add resonance structures together

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49
Q

(T/F) All resonance structures do not have to have the same number of electrons.

A

False. Resonance structures should contain the same number of electrons regardless of the various structures

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50
Q

(T/F) All structures must be valid Lewis structures

A

True

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51
Q

(T/F) Atoms and electrons can move in resonance structures

A

False. Only electrons can move around a molecule.

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52
Q

(T/F) Single and double bonds can be broken in order to move electrons.

A

False. Only double bonds can be broken. A broken single bond would result in the loss of the original molecule

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53
Q

(T/F) The number of unpaired electrons must remain the same

A

True

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54
Q

What are some patterns to determine whether a molecule has resonance (5 patterns)?

A

1) A lone pair next to a pi bond
2) A lone pair next to a positive charge
3) A pi bond next to a positive charge
4) A pie bond between two atoms (especially when one of the atoms is more electronegative)
5) Pi bonds that go all the way around a ring

55
Q

How can one tell which resonance structure is most important (4 patterns)?

A

1) Filled valence shell structures contribute more
2) Maximum number of covalent bonds
3) Least separation of unlikely charges (neutral if possible)
4) Negative charge on the more electronegative atom

56
Q

An s orbital has how many defined spaces where electrons can move?

A

One. S orbitals are spherically shaped, and electrons in this sphere are more likely to be closer to the nucleus

57
Q

A p orbital has how many defined spaces where electrons can move?

A

Two. P orbitals are bow-tie shaped, and less likely to be found at the nucleus

58
Q

P orbitals exist in _____ dimensions

A
  1. Along the x axis, y axis, and z axis
59
Q

When waves are added, ________ interference occurs

A

Constructive

60
Q

When waves are subtracted, _______ interference occurs

A

Destructive

61
Q

When orbitals are in phase, ________ interference occurs

A

Constructive (addition)

62
Q

When orbitals are out of phase, _________ interference occurs

A

Destructive (subtration)

63
Q

Sigma star bonds are (higher, lower) in energy than sigma bonds

A

Higher

64
Q

What is hybridization?

A

The mixing of orbitals together to get hybrid orbitals with the geometries needed

65
Q

When hybridizing orbitals, the number of atomic orbitals in has to equal ________

A

The number of atomic orbitals out

66
Q

Tetrahedral molecules use ______ ________ orbitals (how many of what kind of hybridized orbital?)

A

4 sp3

67
Q

Trigonal planar molecules use ______ ________ orbitals (how many of what kind of hybridized orbital?)

A

3 sp2

68
Q

Linear molecules use ________ ________ orbitals (how many of what kind of hybridized orbital?)

A

2 sp

69
Q

What is s character?

A

The percent of the orbital composed of s orbitals

70
Q

What is the s character of an sp3 orbital?

A

25%

71
Q

What is the s character of an sp2 orbital?

A

33.3%

72
Q

What is the s character of an sp orbital?

A

50%

73
Q

When orbitals are degenerate, they are _______.

A

Equal in energy

74
Q

What is the hybridization of an atom with 1 region of electron density?

A

s

75
Q

What is the hybridization and bond angle of an atom with 2 regions of electron density?

A

sp, 180 degrees

76
Q

What is the hybridization and bond angle of an atom with 3 regions of electron density?

A

sp2, 120 degrees

77
Q

What is the hybridization and bond angle of an atom with 4 regions of electron density?

A

sp3, 109.5 degrees

78
Q

Double bonds are composed of __ and __ bonds

A

Sigma and pi bonds

79
Q

What are pi bonds ALWAYS made of?

A

Extra p orbitals

80
Q

If a lone pair can be involved in resonance, should it be in a p orbital or remain a lone pair?

A

In a p orbital

81
Q

Based on overlap, is a pi bond or sigma bond considered a stronger bond?

A

Sigma

82
Q

Double and triple bonds (lengthen, shorten) a bond length

A

Shorten

83
Q

The more s character, the (stronger, weaker) the bond

A

Stronger

84
Q

The shorter the bond, the (stronger, weaker) the bond

A

Stronger

85
Q

Which bonds can rotate? Which can’t?

A

Single bonds can rotate, double and triple bonds cannot

86
Q

What is a stereoisomer?

A

Same connectivity, but different orientations in space

87
Q

What is a constitutional isomer?

A

Same molecular formula, but different connectivity

88
Q

What is a molecular dipole?

A

The vector sum of bond dipoles

89
Q

What is an ion ion force?

A

The strong electrostatic force between positive and negative ions

90
Q

As a result of ion ion forces, molecules have (high, low) _____ melting points and (high, low) boiling points

A

High, high

91
Q

What are the 3 kinds of Van der Waals forces?

A

1) Dipole-dipole
2) Hydrogen bonds
3) Dispersion forces

92
Q

Dipole-dipole forces originate from the fact that _______________________________.

A

Some molecules have permanent dipoles (are polar). These molecules orient so that the positive of one molecule interacts with the negative of another

93
Q

Dipole-dipole forces cause molecules to have (higher, lower) boiling points vs. not having this interaction

A

Higher

94
Q

Define the hydrogen bond force.

A

Strong interaction between a heteroatom with hydrogen and a heteroatom with a lone pair

95
Q

Hydrogen bonds are (stronger, weaker) than covalent bonds

A

Weaker

96
Q

Hydrogen bonds are (stronger, weaker) than dipole-dipole forces

A

Stronger

97
Q

The more hydrogen bonds, the (higher, lower) the boiling point

A

Higher

98
Q

What are dispersion forces?

A

Forces that arise from the interactions based on temporary induced dipoles

99
Q

What is the weakest interaction between molecules?

A

Dispersion forces

100
Q

Dispersion forces produce attractive forces between ________ molecules

A

Nonpolar

101
Q

Smaller molecules experience (more, less) attraction than large molecules. Why?

A

Less. Larger molecules have more surface area, and thus can experience more attraction

102
Q

Branching (increases, reduces) boiling point

A

Reduces

103
Q

Why does branching reduce boiling point?

A

There is less surface area (think in terms of large vs. small molecules)

104
Q

(T/F) Polar dissolves non-polar

A

False. Polar dissolves polar, non-polar dissolves non-polar

105
Q

Why doesn’t water dissolve in oil?

A

It would cost a lot of energy to break the hydrogen bonding of water to mix with something that cannot provide that interaction

106
Q

Ions dissolve well in _______ and a few other _____ solvents

A

Water and a few other polar solvents.

107
Q

What does it mean if a molecule is capable of solvating?

A

It is capable of encapsulating an ion

108
Q

Polar and ionic solids usually dissolve in ______ solvents

A

Polar

109
Q

Polar liquids are _________

A

Miscible (fully mixable)

110
Q

Non-polar solids are soluble in ________ solvents

A

Non-polar

111
Q

Non-polar liquids are _______

A

Miscible (fully mixable)

112
Q

What is the label for a molecule that is incompatible for water?

A

Hydrophobic

113
Q

What is the label for a molecule that is compatible with water?

A

Hydrophilic

114
Q

Can molecules contain both hydrophilic and hydrophobic regions within itself?

A

Yes

115
Q

In a Bronsted Lowry acid base reaction, the Bronsted acid acts as the proton (donor, acceptor)

A

Donor

116
Q

In In a Bronsted Lowry acid base reaction, the Bronsted base acts as the proton (donor, acceptor)

A

Acceptor

117
Q

What is a mechanism?

A

A description of the events that take place as reactants become products

118
Q

How can we describe what’s going on with electrons and hydrogens?

A

Arrow pushing

119
Q

What if a base has 2 or more possible acceptors?

A

Use resonance structures to find out which acceptor will actually accept the proton

120
Q

How do we tell how strong an acid is?

A

pKa

121
Q

How does one calculate Keq?

A

[products]/[reactants]

122
Q

Ka=?

A

[A-][H3O+]/[HA]

123
Q

pKa=?

A

-log(Ka)

124
Q

When molecules contain the same functional groups, their pKa’s will be (approximately equal, different)

A

Approximately equal

125
Q

Equilibrium lies towards the (stronger, weaker) acid

A

Weaker

126
Q

A stable anion is (more, less) acidic

A

More

127
Q

What are the ways to stabilize an anion (5 ways)?

A

1) Electronegative atom
2) Larger atom
3) Resonance stabilized
4) Induce electron withdrawing group
5) Hybridization

128
Q

As electronegativity of an atom increases, acidity (increases, decreases)

A

Increases

129
Q

(T/F) Size is better for handling a negative charge

A

True. Larger surface area is able to distribute the charge more

130
Q

(T/F) Resonance makes molecules less acidic

A

False. Resonance allows two atoms to share the negative charge, and this is a stabilizing effect. Stable atoms=more acidic molecules

131
Q

(T/F) The help that induction provides increases with distance

A

False. The help that induction provides decreases rapidly with distances

132
Q

(T/F) Molecules with higher s character are more acidic

A

True. Think in terms of hybridized orbitals:

sp3: 25% s character, electrons not as close to nucleus
sp2: 33.3% s character
sp: 50% s character, electrons help tighter to nucleus, stabilizing effect

133
Q

What 5 strong acids should you have memorized?

A

H3PO4, H2SO4, HCl, HBr, HI

134
Q

How do Lewis acids and bases differ from Bronsted acids and bases?

A

Lewis acids act as the electron acceptor, and Lewis bases act as the electron donor. Both form covalent bonds

Organic Chemistry Test 1 (1 decks)

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