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Fall 2013 > Organic Chemistry > Flashcards

Organic Chemistry Flashcards

1
Q

Locate Partial Charges and Polar Bonds in the given structure

A

Step 1:

Identify all polar covalent bonds.

Step 2:

Determine the direction of each dipole.

Step 3:

Indicate the location of partial charges.

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1
Q

Define: Node

A

The place in the electron cloud where there is no electron density

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1
Q

Define: Degenerate Orbitals

A

Orbitals that have the same energy level.

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1
Q

What geometry does sp create?

a) Trigonal Planar
b) Bent
c) Tetrahedral
d) Linear
e) Trigonal Pyramidal

A

d) Linear

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1
Q

Trigonal planar geometry with no lone pairs has a __________ arangement of atoms

A

Trigonal planar

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1
Q

Define: Hydrocarbons

A

Comounds that contain only carbon and hydrogen atoms

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1
Q

Hydrogen bonding causes a(n) ______ in boiling/melting point.

Branching causes a(n) _______ in boiling point.

A

increase; decrease

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1
Q

Ether

A
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2
Q
A

Amide

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3
Q

Define: Divalent

A

The atom will, generally, form 2 bonds (Example: Oxygen)

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3
Q

Define: Functional Group

A

A characteristic group of atoms/bonds that possess a predictable chemical behavior.

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4
Q

Define: The Aufbau Principle

A

The lowest-energy orbital is filled first

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6
Q

Amide

A
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7
Q

Steric number = 4

a) sp3
b) sp2
c) sp

A

a) sp3

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8
Q

Define: Pauli Exclusion Principle

A

Each orbital can accomodate a maximum of two electrons that have opposite spin

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9
Q
A

Alkyne

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10
Q

Define: Tetravalent

A

The atom will, generally, form 4 bonds (Example: Carbon)

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12
Q

Define: Trivalent

A

The atom will, generally, form 3 bonds (Example: Nitrogen)

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13
Q

If Ka < 1

A) Strong Base

B) Strong Acid

A

A)

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15
Q

If Ka > 1

A) Strong Base

B) Strong Acid

A

B)

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16
Q

Define: Covalent Bond

A

The result of two atoms sharing a pair of electrons

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17
Q

Alkene

A
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18
Q

Alkyne

A
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19
Q

A polar covalent bond corresponds to

a) 0.5 difference in electronegativity
b) between 0.5 and 1.7 difference in electronegativity
c) 1.7 difference in electronegativity

A

b)

Between 0.5 and 1.7 difference will result in a polar covalent bond

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20
Q

Define: Induction

A

The withdrawl of electrons toward oxygen.

Induction will cause partial positive and negative charges.

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22
Q

Carboxylic Acid

A
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22
Q

Ester

A
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24
Q

A covalent bond corresponds to

a) 0.5 difference in electronegativity
b) between 0.5 and 1.7 difference in electronegativity
c) 1.7 difference in electronegativity

A

a)

An 0.5 difference in electronegativity will create a coavelnt bond

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24
Q

What geometry does sp2 create?

a) Trigonal Planar
b) Bent
c) Tetrahedral
d) Linear
e) Trigonal Pyramidal

A

a) Trigonal Planar

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25
Q
A

Amine

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27
Q
A

Alkene

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28
Q

Amine

A
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28
Q

Define: Bronsted-Lowry Acids & Bases

A

Acid: Proton (H+) donor

Nase: Proton acceptor

Acids react with bases. An Acid - Base is a Proton- Transfer reacton.

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29
Q

An sp3-hybridized orbital forms

a) A single bond
b) A double bond
c) A tripple bond

A

a) A single bond

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29
Q

Equation: Keq = ________

A

Keq = [H3o+][A-]
———————-
[HA] [H2O]

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30
Q

Halogens

A

Group 7A (Florine, Chlorine, Bromine and Iodine)

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30
Q

Alcohol

A
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31
Q

What geometry does sp3 create?

a) Trigonal Planar
b) Bent
c) Tetrahedral
d) Linear
e) Trigonal Pyramidal

A

c) Tetrahedral

32
Q

Tetrahedral geometry with no lone pairs has a __________ arangement of atomsm

A

Tetrahedral

33
Q

Linear geometry has a __________ arangement of atoms

A

Linear

35
Q

Trigonal planar geometry with one lone pairs has a __________ arangement of atoms

A

Bent

36
Q

Equation: How to determine how many double/triple/ring bonds exist in a structure.

A

CNumber of - 1/2 (HNumber of) - 1/2(HalogensNumber of) + 1/2 (NNumber of) + 1

An HDI of 1 means there is 1 double bond or 1 ring. NO triple bonds.

An HDI of 2 means there is 1 double bond and 1 ring, 2 double bonds, 2 rings, or 1 triple bond.

38
Q
A

Carboxylic Acid

40
Q
A

Alkyl Halide

40
Q
A

Alcohol

42
Q

Tetrahedral geometry with two lone pairs has a __________ arangement of atoms

A

Bent

43
Q

Define: Valence

A

Describes the number of bonds that are usually formed by each element

44
Q

How to count Sigma and Pi bonds

A

A single bond contains 1 sigma bond.

A double bond contains 1 sigma bond and 1 pi bond.

A tripple bond contains 1 sigma bond and 2 pi bonds.

45
Q

Determine the Formal Charge of

A

Step 1: Determine the appropriate number of valence electrons.

Step 2: Determine the actual number of valence electrons.

Step 3: Assign a formal charge.

Because the Nitrogen exhibits 4 valence electrons the charge will be possitive.

46
Q

Define: Electronegativity

A

A measure of the ability of an atom to attract electrons

47
Q

Define: Monovalent

A

The atom will, generally, form 1 bond (Example: Halogens & Hydrogen)

49
Q

Alkyl Halide

A
50
Q

Define: Lone pair

A

A pair of unshared or nonbonding electrons

51
Q

Define: Solubility

A

Like disolves like

52
Q

Define: Steric Number

A

Total number of sigma bonds plus lone pairs

54
Q

Steric number = 3

a) sp3
b) sp2
c) sp

A

b) sp2

55
Q

Equation: Keq= _________

A

Kep = 10(pKa(larger) - pKa(smaller))

57
Q

Define: Formal Charge

A

Associated with an atom that does not exhibit the appropriate number of valence electrons

58
Q

Tetrahedral geometry with one lone pair has a __________ arangement of atoms

A

Trigonal pyramidal

60
Q

Steric number = 2

a) sp3
b) sp2
c) sp

A

c) sp

61
Q
A

Ether

62
Q

The larger the pKa value, the ________ the acid.

A

WEAKER

63
Q

Electronegativity Trend in the Periodic Table

A

Electronegative values increase from left to right and from bottom to the top

64
Q

An sp-hybridized orbital forms

a) A single bond
b) A double bond
c) A tripple bond

A

c) A tripple bond

65
Q

Define: Lewis Theory

A

Acid: Electron - Pair acceptor

Base: Electron - Pair donor

66
Q

Ketone

A
67
Q

Define: Valence Electrons

A

The electrons in the outermost shell of an atom

68
Q

Equation: pKa = _________

A

pKa = - log(Ka)

69
Q
A

Ketone

70
Q

Define: Hund’s Rule

A

When dealing with degenerate orbitals, such as p orbitals, on electron is placed in each degenerate orbital first, before electrons are paired up.

71
Q

An electronegativity difference of ____ means that the electrons are not shared at all

a) 0.5 difference in electronegativity
b) between 0.5 and 1.7 difference in electronegativity
c) 1.7 difference in electronegativity

A

c)

A difference in electronegativity greater then 1.7 will result in non-shared electrons

72
Q
A

Ester

73
Q

Predict the geometry for the central atom in each of the compounds below

(a) NH3 (b)H3O+ (c) BH4- (d) BCl3
(e) BCl4- (f) CCl4 (g) CHCl3 (h) CH2Cl2

A
74
Q

Define: Conjugate Pairs

A

Conjugate pairs differ by an H+

75
Q

An sp2-hybridized orbital forms

a) A single bond
b) A double bond
c) A tripple bond

A

b) A double bond

76
Q

Define: Exothermic

A

In an exothermic process, the system gives energy to the surroundings.

Therefore ΔH is negative.

77
Q

Define: Endothermic

A

In an endothermic process, the system receives energy from the surroundings.

Therefore ΔH is positive.

78
Q

Equation: Gibb’s free Energy

A

ΔG = ΔH -TΔS

79
Q

Equation: Rate

A

Rate = k [A]x[B]y

80
Q

Define: Nucleophile

A

A nucleophile (Lewis base) is an electron-rich atom capable of donating a pair of electrons.

81
Q

Define: Electrophile

A

An electrophile (center of the atom) is an electrion deficient atom that is capable of accepting a pair of electrons.

82
Q

Define: Primary Carbon

A

A carbon attached to one other carbon.

(R - C - Cl)

83
Q

Define: Secondary Carbon

A

A carbon that is attached to two other carbons.

84
Q

Define: Tertiary Carbon

A

A carbon that is attached to three other carbons.

85
Q

Equation: Substitution Reaction - Nucleophilic Attack

A

Nuc:- + Substrate – LG ——-> Substrate – Nuc + LG-

86
Q

Equation: Substitution Reaction - Loss of a Leaving Group

A

Substrate – LG —-LG—> Substrate —:Nuc—> Substrate – Nuc

87
Q

Define: Concerted Process

A

In a concerted process, nucleophilic attack and loss of the leaving group occur at the same time. Thus it is a one step process.

88
Q

Define: Stepwise Process

A

In a stepwise process, loss of the leaving group occurs first followed by the nucleophilic attack.

89
Q

SN2

A) Unimolecular

B) Bimolecular

A

B)

90
Q

SN1

A) Unimolecular

B) Bimolecular

A

A)

91
Q

Define: Inversion of Configuration

A

When a nucleophile attacks the back side of the molecule (the side opposite the leaving group), the absolute configuration of the product will be opposite the absolute configuration of the reactant.

92
Q

Define: Rate-Determining Step

A

The slowest step of the reaction. For SN1, this will be the step that it loses the leaving group.

93
Q

Define: Racemic

A

A molecule with a chiral carbon, when racted, will create a 50/50ish split between its enantiomers with a slight favor to the non-inverted enantiomer.

Fall 2013 (4 decks)

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