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Organic Chemistry > Exam 1 > Flashcards

Exam 1 Flashcards

(57 cards)

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1
Q

Name this functional group.

A

Alkane

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2
Q

Draw out the Alkane functional group.

A
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3
Q

Name this functional group.

A

Alkene

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4
Q

Draw out the Alkene functional group.

A
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5
Q

Name this functional group.

A

Alkyne

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6
Q

Draw out the Alkyne functional group.

A
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7
Q

Name this functional group.

A

Alcohol

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8
Q

Draw out the Alcohol functional group.

A
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9
Q

Name this functional group.

A

Ether

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10
Q

Draw the Ether functional group.

A
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11
Q

Name this functional group.

A

Epoxide

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12
Q

Draw the Epoxide functional group.

A
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13
Q

Name the functional group.

A

Haloalkane

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14
Q

Draw a haloalkane functional group.

A
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15
Q

Name the functional group.

A

Aldehyde

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16
Q

Draw a Aldehyde functional group.

A
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17
Q

Name the functional group.

A

Ketone

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18
Q

Draw a Ketone functional group.

A
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19
Q

Name the functional group.

A

Carboxylic Acid

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20
Q

Draw a Carboxylic Acid functional group.

A
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21
Q

Name the functional group.

A

Ester

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22
Q

Draw a Ester functional group.

A
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23
Q

Name the functional group.

24
Q

Draw an Amide functional group.

25
Name the functional group.
Amine
26
Draw an Amine functional group.
27
Name the functional group.
Thiol
28
Draw a Thiol functional group.
29
What structure is this?
Isopropyl
30
What structure is this?
Sec-butyl
31
What structure is this?
Tert-butyl
32
What structure is this?
Isobutyl
33
What is the formula for calculating formal charge?
of valence electrons - (# of non-bonded electrons + # of bonds)
34
Why do hybrid resonance structures have lower energy/ are more stable?
There is delocalization or "spreading out" of electrons.
35
What are the 3 rules for bond length?
1. Bond length decreases across a period. 2. Bond length decreases with increasing bond order 3. Bond length increases as you go down a group.
36
What is the bond angle for a linear electron geometry?
180*
37
What is the bond angle for a trigonal planar electron geometry?
120*
38
What is the bond angle for a tetrahedral electron geometry?
109.5
39
What is the equation to find the # of hybrid orbitals?
of lone pairs + # of sigma bonds
40
What is the equation for bond order?
(bonding orbital electrons - antibonding orbital electrons)/2
41
If the bond order is <1, it is ______.
Not stable
42
Why are staggered rotations more stable in Newman projections?
It decreases Van der Waal repulsions
43
What is a primary carbon?
Bonded to 1 other carbon
44
What is a secondary carbon?
Bonded to 2 other carbons
45
What is a tertiary carbon?
Bonded to 3 other carbons
46
What is a quaternary carbon?
Bonded to 4 other carbons
47
What is a primary hydrogen?
Bonded to a primary carbon
48
As the # of carbons increases the boiling point ________ because _______.
increases; As the molecule gets larger, the London dispersion forces increase.
49
As the # of carbons increases the melting point ________ because _______.
increases; As the molecule gets larger, the London dispersion forces increase.
50
A Lewis acid is an electron ______.
Acceptor
51
A Lewis base is an electron ______.
Donor
52
A Bronsted Acid is a species that ______ a proton.
Donates
53
A Bronsted base is a species that ______ a proton.
Accepts
54
If the product side is favored, then Keq is ____ than 1.
Greater than
55
If the reactant side is favored, then Keq is _____ than 1.
Less than
56
An electrophile is a _________.
Lewis Acid
57
A neutrophile is a ________.
Lewis base

Organic Chemistry (5 decks)

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