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Fall 2013 > Organic Chemistry > Flashcards

Organic Chemistry Flashcards

(93 cards)

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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
# Define: Induction
The withdrawl of electrons toward oxygen. Induction will cause partial positive and negative charges.
22
Carboxylic Acid
22
Ester
24
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) An 0.5 difference in electronegativity will create a coavelnt bond
24
What geometry does sp2 create? a) Trigonal Planar b) Bent c) Tetrahedral d) Linear e) Trigonal Pyramidal
a) Trigonal Planar
25
Amine
27
Alkene
28
Amine
28
# Define: Bronsted-Lowry Acids & Bases
Acid: Proton (H+) donor Nase: Proton acceptor Acids react with bases. An Acid - Base is a Proton- Transfer reacton.
29
An sp3-hybridized orbital forms a) A single bond b) A double bond c) A tripple bond
a) A single bond
29
Equation: Keq = \_\_\_\_\_\_\_\_
Keq = [H3o+][A-] ---------------------- [HA] [H2O]
30
Halogens
Group 7A (Florine, Chlorine, Bromine and Iodine)
30
Alcohol
31
What geometry does sp3 create? a) Trigonal Planar b) Bent c) Tetrahedral d) Linear e) Trigonal Pyramidal
c) Tetrahedral
32
Tetrahedral geometry with no lone pairs has a __________ arangement of atomsm
Tetrahedral
33
Linear geometry has a __________ arangement of atoms
Linear
35
Trigonal planar geometry with one lone pairs has a __________ arangement of atoms
Bent
36
Equation: How to determine how many double/triple/ring bonds exist in a structure.
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
Carboxylic Acid
40
Alkyl Halide
40
Alcohol
42
Tetrahedral geometry with two lone pairs has a __________ arangement of atoms
Bent
43
Define: Valence
Describes the number of bonds that are usually formed by each element
44
How to count _Sigma_ and _Pi_ bonds
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
Determine the Formal Charge of
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
Define: Electronegativity
A measure of the ability of an atom to attract electrons
47
Define: Monovalent
The atom will, generally, form 1 bond (Example: Halogens & Hydrogen)
49
Alkyl Halide
50
Define: Lone pair
A pair of unshared or nonbonding electrons
51
# Define: Solubility
Like disolves like
52
# Define: Steric Number
Total number of sigma bonds plus lone pairs
54
Steric number = 3 a) sp3 b) sp2 c) sp
b) sp2
55
Equation: Keq= \_\_\_\_\_\_\_\_\_
Kep = 10(pKa(larger) - pKa(smaller))
57
Define: Formal Charge
Associated with an atom that does not exhibit the appropriate number of valence electrons
58
Tetrahedral geometry with one lone pair has a __________ arangement of atoms
Trigonal pyramidal
60
Steric number = 2 a) sp3 b) sp2 c) sp
c) sp
61
Ether
62
The larger the pKa value, the ________ the acid.
WEAKER
63
Electronegativity Trend in the Periodic Table
Electronegative values increase from left to right and from bottom to the top
64
An *sp-hybridized* orbital forms a) A single bond b) A double bond c) A tripple bond
c) A tripple bond
65
# Define: Lewis Theory
Acid: Electron - Pair acceptor Base: Electron - Pair donor
66
Ketone
67
Define: Valence Electrons
The electrons in the outermost shell of an atom
68
Equation: pKa = \_\_\_\_\_\_\_\_\_
pKa = - log(Ka)
69
Ketone
70
# Define: Hund's Rule
When dealing with degenerate orbitals, such as *p* orbitals, on electron is placed in each degenerate orbital first, before electrons are paired up.
71
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
c) A difference in electronegativity greater then 1.7 will result in non-shared electrons
72
Ester
73
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
74
# Define: Conjugate Pairs
Conjugate pairs differ by an H+
75
An sp2-hybridized orbital forms a) A single bond b) A double bond c) A tripple bond
b) A double bond
76
# Define: Exothermic
In an exothermic process, the system gives energy to the surroundings. Therefore ΔH is negative.
77
# Define: Endothermic
In an endothermic process, the system receives energy from the surroundings. Therefore ΔH is positive.
78
Equation: Gibb's free Energy
ΔG = ΔH -TΔS
79
Equation: Rate
Rate = k [A]x[B]y
80
# Define: Nucleophile
A nucleophile (Lewis base) is an electron-rich atom capable of donating a pair of electrons.
81
# Define: Electrophile
An electrophile (center of the atom) is an electrion deficient atom that is capable of accepting a pair of electrons.
82
# Define: Primary Carbon
A carbon attached to one other carbon. (R - C - Cl)
83
# Define: Secondary Carbon
A carbon that is attached to two other carbons.
84
Define: Tertiary Carbon
A carbon that is attached to three other carbons.
85
Equation: Substitution Reaction - Nucleophilic Attack
Nuc:- + Substrate -- LG -------\> Substrate -- Nuc + LG-
86
Equation: Substitution Reaction - Loss of a Leaving Group
Substrate -- LG ----LG---\> Substrate ---:Nuc---\> Substrate -- Nuc
87
Define: Concerted Process
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
Define: Stepwise Process
In a stepwise process, loss of the leaving group occurs first followed by the nucleophilic attack.
89
SN2 A) Unimolecular B) Bimolecular
B)
90
SN1 A) Unimolecular B) Bimolecular
A)
91
# Define: Inversion of Configuration
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
# Define: Rate-Determining Step
The slowest step of the reaction. For SN1, this will be the step that it loses the leaving group.
93
# Define: Racemic
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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