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Organic Chemistry > Exam 1 > Flashcards

Exam 1 Flashcards

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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.

A

Amide

24
Q

Draw an Amide functional group.

A
25
Q

Name the functional group.

A

Amine

26
Q

Draw an Amine functional group.

A
27
Q

Name the functional group.

A

Thiol

28
Q

Draw a Thiol functional group.

A
29
Q

What structure is this?

A

Isopropyl

30
Q

What structure is this?

A

Sec-butyl

31
Q

What structure is this?

A

Tert-butyl

32
Q

What structure is this?

A

Isobutyl

33
Q

What is the formula for calculating formal charge?

A

of valence electrons - (# of non-bonded electrons + # of bonds)

34
Q

Why do hybrid resonance structures have lower energy/ are more stable?

A

There is delocalization or “spreading out” of electrons.

35
Q

What are the 3 rules for bond length?

A
  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
Q

What is the bond angle for a linear electron geometry?

A

180*

37
Q

What is the bond angle for a trigonal planar electron geometry?

A

120*

38
Q

What is the bond angle for a tetrahedral electron geometry?

A

109.5

39
Q

What is the equation to find the # of hybrid orbitals?

A

of lone pairs + # of sigma bonds

40
Q

What is the equation for bond order?

A

(bonding orbital electrons - antibonding orbital electrons)/2

41
Q

If the bond order is <1, it is ______.

A

Not stable

42
Q

Why are staggered rotations more stable in Newman projections?

A

It decreases Van der Waal repulsions

43
Q

What is a primary carbon?

A

Bonded to 1 other carbon

44
Q

What is a secondary carbon?

A

Bonded to 2 other carbons

45
Q

What is a tertiary carbon?

A

Bonded to 3 other carbons

46
Q

What is a quaternary carbon?

A

Bonded to 4 other carbons

47
Q

What is a primary hydrogen?

A

Bonded to a primary carbon

48
Q

As the # of carbons increases the boiling point ________ because _______.

A

increases; As the molecule gets larger, the London dispersion forces increase.

49
Q

As the # of carbons increases the melting point ________ because _______.

A

increases; As the molecule gets larger, the London dispersion forces increase.

50
Q

A Lewis acid is an electron ______.

A

Acceptor

51
Q

A Lewis base is an electron ______.

A

Donor

52
Q

A Bronsted Acid is a species that ______ a proton.

A

Donates

53
Q

A Bronsted base is a species that ______ a proton.

A

Accepts

54
Q

If the product side is favored, then Keq is ____ than 1.

A

Greater than

55
Q

If the reactant side is favored, then Keq is _____ than 1.

A

Less than

56
Q

An electrophile is a _________.

A

Lewis Acid

57
Q

A neutrophile is a ________.

A

Lewis base

Organic Chemistry (5 decks)

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