Chapter 2: Functional Groups and Nomenclature Flashcards
1
Q
what are functional groups
A
- a collection of specific atoms connected in a specific way
- molecules featuring the same functional group will undergo the same reactions
- knowing the reactivity of the functional groups allows us to predict what transformations will occur, even for new molecules
2
Q
aldehyde
A
c double bonded with oygen
3
Q
alkanes
A
- are made up of single bonds
(C-C and C-H)
4
Q
alkenes
A
- are functional groups with double bonds between two carbons
5
Q
alkynes
A
- functional groups with triple bonds between two carbons
6
Q
aromatic rings
A
- are functional groups with a ring with altering single and double bonds between bonds
7
Q
primary, secondary and tertiary alcohols
A
- alcohols are functional groups where a carbon is connected to an oxygen, which is then connected to a hydrogen
- subdivided based on the number of carbons bonded to the main carbon of the alcohol
8
Q
ethers
A
- are functional groups where a carbon is connected to an oxygen, which is then connected to another carbon
9
Q
aldehydes
A
- are functional groups where a carbon is double bonded to an oxygen and is connected to a hydrogen
10
Q
ketones
A
- are functional groups where a carbon is double bonded to an oxygen and is connected to two other carbons
11
Q
carboxylic acid
A
- are functional groups where a carbon is double bonded to an oxygen and is connected to another oxygen which is connected to a hydrogen
12
Q
esters
A
- are functional groups where a carbon is double bonded to an oxygen and is connected to another oxygen which is connected to another carbon
13
Q
acid halides
A
are functional groups where a carbon is double bonded to an oxygen and is connected to a halogen
14
Q
hydrates
A
- functional groups where a carbon is connected to two oxygens and both oxygens are connected to hydrogens
15
Q
hemiacetals
A
- functional groups where a carbon is connected to two oxygens and one oxygen is connected to another carbon, one to a hydrogen
16
Q
acetals
A
- functional groups where a carbon is connected to two oxygens and both oxygens are connected to other carbons
17
Q
amides
A
- functional groups where a carbon is double bonded to an oxygen and connected to a nitrogen
18
Q
amines
A
- are functional groups where a nitrogen is connected to carbons and/or hydrogens
- subdivisions based on the number of carbons attracted to the nitrogen
19
Q
nitros
A
- functional groups where a nitrogen is double bonded to an oxygen and is connected to another oxygen
- the atoms have formal charges, but overall the functional group is natural
20
Q
nitriles
A
functional groups where a nitrogen is triple bonded to a carbon
21
Q
imines
A
- functional groups where a nitrogen is double bonded to a carbon
22
Q
halides
A
functional groups where a halogen is connected to carbon
- subdivided based on the halogen
23
Q
thio equivalents
A
if there is a sulfur instead of an oxygen in a group
24
Q
carbonyl group
A
- carbon double bonded to oxygen with (two other things) very common
- carbonlys are nor functional groups on their own
25
intermolecular forces
- two or more molecules can attract each other through intermolecular forces
- all these intermolecular forces are the result of the attraction of opposite charges
- functional groups play a big role in intermolecular forces
26
electrostatic interactions
- electrostatic interactions arise from permanent (formal) charges
- a positive charge (cation) is attracted to a negative charge (anion)
27
dipole - dipole
- interactions arise from permanent (partial charges) (polar bonds)
- a partial positive is attracted to a partial negative
- these are usually the second strongest intermolecular forces
28
hydrogen bonding
- is a type of dipole dipole interaction that is so common it gets its own name
- the partial positive is on a hydrogen attached to a heteroatom ( O or N)
- the partial negative is on another heteroatom (O or N)
29
hydrogen bonding
- molecules that have a lone pair on an electronegative heteroatom are hydrogen bond acceptors
- molecules that have a hydroogen attached to an electronegative heteroatom are hydrogen bond donars
30
disperson
- dispersion arises from temporary (partial charges)
- the electron density cloud around methane is fairly even
- they are not all around each area they all just move loads
- at any point the electrons are randomly distributed in the cloud
- random means sometimes there are areas with more that usual and areas with less than usual
- they temporarily have partial negative and partial positive charges
31
boiling and melting effects
- attractive forces from a molecule to another equivalent of itself can affect melting and boiling points
- when things melt/boil, the molecules get further apart. more intermolecular forces (attraction) means more energy and heat needed to more them apart
- dispersion is a weak force, but enough dispersion can have an effect
- the heavier the molesule the less dispersion there is and the easier it is to handle
- the lighter the molecule (gas) the more difficult it is to handle
32
dispersion of forces
- having substitutes decreases how close two molecules can get, so it reduces the amount of dispersion interactions
- similar carbon numbers and weight the only difference is the dispersion of forces
33
what is the order of forces to weakest to strongest
- dispersion, dipole-dipole, hydrogen bonding and electrostaitic
34
soluability effects
- attractive forces from a molecule to molecules of solvent can affect solubility
- easiesy way to remeber the trend is "like dissolves like" (molecules prefer solvents with similar intermolecular forces
- not all forces affect solubility equally, so it is easier to classify solvents and molecules
35
how to classify solvents
solvents are generally classed using two parameters
polar vs non polar ( whether is does or does not have a permanent net dipole)
protic or aprotic (whether or not is can donate a hydrogen bond)
36
hydrophilicity and hydrophobicity
- water is so common that there are special terms to refer to whether compounds (or parts of compounds) like to dissolve in it (hydrophilic = water loving) or not (hydrophobic = water fearing)
- anything that increases electrostatic and dipole dipole (hydrogen bonding) interactions increase hydrophilicity
- anything that decreases dispersion increases hydrophilicity
37
basics in nomenclature
1. a prefix = coming off the main chain
2. root name = how many C are in each
3. suffix = which functional group/ groups are represented
38
1 carbon
meth
39
2 carbons
eth
40
3 carbons
prop
41
4 carbons
but
42
5 carbons
pent
43
6 carbons
hex
44
7 carbons
hept
45
8 carbons
oct
46
9 carbons
non
47
10 carbons
dec
48
branched alkanes
- alkane substituents are named using the appropriate root name and adding yl at the end
- numbering is done so that the substituent gets the smallest number
- if there is more than one substituent = numbering starts at end of chain closest to the branching point (substituents are listed in alphabetical order
49
greek numerical prefixes
- is more than one identical substituent use the prefixes di, tri or tetra
50
cyclic alkanes
- prefix cyclo is used for compounds a hydrocarbon ring
- if there is only one substituent no number is needed
51
alkenes
the suffix is ene
- position of the alkene on chain indicated by number
- more than one alkene = diene or triene
- double bond
52
alkynes
- triple bond
- the suffix is yne
- if both alkene and alkyne are present it is an enyne
53
priority and functional groups are indicated with prefix or suffix, depending on priority,
the suffix comes from the group with the highest priority
54
highest to lowest priority
- carboxylic - oic acid
- aldehyde - al
- ketone - one
- alcohol - ol
- amine - amine (NH2)
- halide - fluoro, chloro, bromo, iodo
55
numbering cycloalkanes
- numbering starts at the highest
- proceeds clockwise or counter clockwise to give the other groups the smallest possible numbers
- the label 1 doesnt have to be written
56
cycloalkenes
- with multiple substituents, numbering starts at the highest priority first group and proceeds clockwise or counterclockwise
- giving the alkene the smallest possible number
57
