Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Chemistry > Chapter 9-13 > Flashcards

Chapter 9-13 Flashcards

You may prefer our related Brainscape-certified flashcards:
Periodic Table flashcards Chemistry 101 flashcards AP® Chemistry flashcards Organic Chemistry 101 flashcards
1
Q

acid

A

vinegar, citric acid (in juices), ascorbic acid (Vit. C)
smells sour, tastes sour
turns blue litmus paper red
can be neutralized by base

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

NaOH

A 
NaOH (in liquid plumber), NH3 (in windex)
	tastes bitter or chalky,
	feels slippery,
	turns red litmus paper blue
	can be neutralized by acid
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

salt

A

table salt, baking soda-any ionic compound that is not a hydroxide or an oxide.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Arrhenius acids :

A

H-containing covalent compounds that produce H+ ions in water.
HCl(ag)  H+(aq) + Cl- (aq

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Arrhenius bases:

A

Hydroxide-containing ionic compounds that produce OH- ions in water.
NaOH (aq)  Na+(aq) + OH-(aq)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

acids

A

are H-containing covalent compounds that dissociate and release H+ in aqueous solutions.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Binary acids.

A

HF hydrofluoric acid
HCl hydrochloric acid
HBr hydrobromic acid
HI hydroiodic acid

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Oxy acids

A

HNO3 nitric acid HNO2 nitrous acid
H2SO4 sulfuric acid H2SO3 sulfurous acid
HClO3 chloric acid HClO2 chlorous acid
H2CO3 carbonic acid
H3PO4 phosphoric acid H3PO3 phosphorous acid

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

water soluble hydroxides

A

NaOH sodium hydroxide
KOH potassium hydroxide
Ba(OH)2 barium hydroxide
Ca(OH)2 calcium hydroxide

	    Ca(OH)2 (aq) →  Ca 2+ + 2OH-
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

water solubl metal oxides

A

Base anhydride
Na2O Sodium oxide
CaO calcium oxide

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

salt

A

A salt is an ionic compound that is not classified as bases.

Water-soluble salts (solubility rules) are always considered as 100% dissociated in water to produce ions. Therefore, soluble salts are strong electrolytes.

NaCl, NaHCO3, CaCO3, MgSO4, CuCl2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

The Hydrogen Cation & The Proton

A

Recall hydrogen atom has 1 proton and 1 electron.
When a H atoms loses its electron,
H● → H+ + e-
H+ = the nucleus of hydrogen
= a proton

Therefore, another name for H+, is a proton.

Remember, H+  =  proton
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

Bronsted-Lowry acid is

A

a proton (H+) donor;

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Bronsted-Lowry base is

A

a proton (H+) acceptor.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

Bronsted-Lowry Acid-Base Theory

thinking acid-base in terms of proton (H+) transfer

A

Any acid-base reaction involving a Bronsted-Lowry acid must also involve a Bonsted-Lowry base.
Proton donation cannot occur unless an acceptor is present.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

H3O+ =

A

hydronium ion
= H+-H2O (the way H+ actually exist in aqueous solution)

	= a hydrated hydrogen cation
	= a hydrated proton
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

Arrhenius vs. BrØnsted Acids & Bases

A

The Bronsted-Lowry theory is consistent with the Arrhenius definition.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

Conjugate Acid-Base Pairs

A

In any acid-base reaction, there are two conjugate
acid-base pairs
Each pair related by the loss and gain of H+ .
One occurs in the forward direction.
One occurs in the reverse direction.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

A Conjugate Acid-Base Pairs are related to each other by

A

gain or loss of H+.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

To write the conjugate base of an acid (remove H+)

A

1) remove one H from the formula of acid
2) add a “-” charge to the remaining formula.
the conjugate base of HSO4- is SO42-

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

To write the conjugate acid of a base (add H+)

A

1) add one H to the formula of base
2) add a “+” charge to the formula.
the conjugate acid of HPO42- is H2PO4-

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

Acid-Base Neutralization Reactions

A

When acids and bases are mixed, they react with one another to produce water and a salt. This is called neutralization reactions
HX + MOH  MX + HOH
acid + base → salt + water
(MX is the salt of acid HX)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

Acid Base Neutralization reactions are

A

double replacement reactions.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

Writing balanced equations for neutralization Reactions

A

HCl + NaOH → NaCl + HOH
(Na salt of HCl)
Acid + Base → Salt + HOH
** salt is an ionic compound; the total charges of cations and anions must be the same.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

auto-ionization

A

A very small population of water molecules become ionized when 2 H2O molecules collide and H+ is transferred from one H2O molecule to another
- a reversible reaction that overwhelmingly favors the neutral H2O side

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q

Out of every 1 billion water molecules, how many exists as H3O+ and OH-

A

only 2 actually exist as H3O+ and OH-

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q

The Chemical Equation of

Water Auto-ionization

A

H2O + H2O H3O+ + OH−
Hydronium ion is a hydrated hydrogen cation.

For simplicity reason, we often write H3O+ as H+

             H2O                 H+  +   OH-
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
28
Q

The Quantities of H3O+ and OH- in Pure Water

A

Notice equal number of H3O+ and OH- are formed during the ionization
- Pure Water is Neutral

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
29
Q

Auto-ionization of water is a reversible reaction in which the molar concentrations of H3O+ and OH- are determined by a constant called

A

ion product constant, Kw
- Kw = [H3O+][OH-] = [1x 10-7][1x10-7] = 1 x 10-14

If [H3O+] goes ↑, [OH-] must goes ↓

If [H3O+] goes ↓, [OH-] must goes ↑

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
30
Q

Adding Acid to H2O, makes

A

[H3O+] ↑, [OH-] ↓

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
31
Q

Adding base to H2O makes

A

[OH-]↑, [H3O+.] ↓

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
32
Q

pH

A

(power of Hydronium ion)

Notice the symbol is lower case p and capital H

The pH of a solution is the negative logarithm of the molar concentration of its hydronium ions.

		pH = - log [H3O+]
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
33
Q

Buffers are

A

solutions that can maintain its pH or resist major changes in pH when small amounts of acid or base are added to it.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
34
Q

Buffers are important in

A

the proper functioning of cells and blood.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
35
Q

Buffers in the body absorb

A

H3O+ or OH¯ from foods and cellular processes to maintain pH.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
36
Q

Buffer maintains the pH of our blood to

A

close to 7.4. A change in the pH of the blood affects the uptake of oxygen and cellular processes.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
37
Q

A buffer solution contains

A

equal moles of a weak (acid and its conjugate base (salt) or equal moles of weak base and its conjugate acid.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
38
Q

Any acid that is NOT in the strong acid table is a

A

weak acid

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
39
Q

examples of buffer

A

1) a weak acid and its conjugate base (or salt of the acid):

	H3PO4 + NaH2PO4(H2PO4-), 
	H2CO3 + NaHCO3(HCO3-)

2) a weak base and its conjugate acid: 

	 NH3  +  NH4Cl (NH4+)
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
40
Q

acidosis

A

(CO2 pH ): emphysema, pneumonia, stroke, renal disease

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
41
Q

alkalosis

A

(CO2 pH ): hyperventilation, vomiting, exercise, hypoxia

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
42
Q

What is an Organic Compound?

A

Chemicals were classified as organic if they originated from living organisms rather than rocks.

The German scientist Wöhler synthesized the compound urea (a component of urine) without the use of any living organism, proving that it was possible to generate organic compounds independent of a living creature.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
43
Q

Organic chemistry is defined today as

A

the chemistry of the element carbon and its compounds.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
44
Q

Organic compounds contain

A 
carbon and only a few other type of atoms (heteroatoms)
H, O, N,
the halogens (especially Cl, Br, and I)
S and (to a lesser extent), P
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
45
Q

Inorganic compounds are those

A

which are not based mainly on carbon.
- by convention, not all carbon-containing compounds are considered to be organic (for example: diamond, graphite, CO2, Na2CO3)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
46
Q

The simplest type of organic compounds are

A

hydrocarbons: compounds that are made of only H and C.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
47
Q

Saturated hydrocarbon

A

a hydrocarbon in which all carbon-carbon bonds are single bonds.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
48
Q

Unsaturated hydrocarbon is

A

a hydrocarbon that contains one or more carbon-carbon multiple bonds.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
49
Q

The simplest open-chain (acyclic) saturated hydrocarbons are called

A

alkanes

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
50
Q

IUPAC Names And Condensed Structures For the First Ten Linear-Chain Alkanes

A 
CH4 meth methane
C2H6 eth ethane
C3H8 prop propane
C4H10 but butane
C5H12 pent pentane
C6H14 hex Hexane
C7H16 hept heptane
C8H18 oct octane
C9H20 non nonae
C10H22 dec decane
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
51
Q

The general chemical formula of alkane:

A

CnH2n+2 C3H2(3) +2 = C3H8

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
52
Q

Extended structural formula

A

shows all atoms and all bonds in a molecule.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
53
Q

Condensed structural formula

A

shows all bonds except C-H single bonds by writing the Hs to the right of C atom that is bonded to.
CH3-CH2-CH3

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
54
Q

Skeletal Structure:

A

C-C-C

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
55
Q

Alkanes with more than three carbon atoms can be arranged or joined in a multiple number of ways, forming different

A

isomers.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
56
Q

Structual isomers have the same

A

chemical formulas

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
57
Q

Since atoms are hooked up differently structural isomers are

A

distinct molecules with distinct properties

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
58
Q

Sturcture isomers are also called

A

constitutional isomers.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
59
Q

The Number of Structural Isomers With Increasing Number Of C

-increasing exponentially with # of C

A 
C1: 	1 isomer — methane 
C2: 	1 isomer — ethane 
C3: 	1 isomers — propane 
C4: 	2 isomers — n-butane, isobutane 
C5: 	3 isomers — n-pentane, isopentane, neopentane
C6:     5 isomers
C12: 	355 isomers 
C32: 	27,711,253,769 isomers 
C60: 	22,158,734,535,770,411,074,184 (> 2.2 X 1022) 	isomers
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
60
Q

Naming Branched Alkanes

A

Find the longest linear chain as the “parent chain”.

Treat the branch as a substitution of a hydrogen on the carbon at the branch point.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
61
Q

Alkyl Groups (R group)

A

An alkane that is missing one H from the terminal C.
Then binds to a carbon chain as a “substituent”
Named with a –yl ending.

  • methyl CH3-
  • ethyl
  • propyl
  • butyl
  • pentyl
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
62
Q

The Cycloalkanes

A

C atoms connecting to one another in a cyclic arrangement

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
63
Q

The general chemical formula of cycloalkane:

A

CnH2n C5H2(5) = C5H10 cyclopentane

64
Q

Physical Properties Of Alkanes and Cycloalkanes

A

Alkanes and cycloalkanes are nonpolar molecules and therefore insoluble in water
Less dense than water (d

65
Q

Chemical Properties of Alkanes

A

Are typically not very reactive due to strong C-C single bonds
Fossil fuels are the major source of alkanes, existing on the earth for hundreds of millions of years.

66
Q

combustion

A

by reacting with oxygen to produce carbon dioxide, water, and energy.
- alkane + O2 CO2 + H2O + energy

67
Q

substitution

A

reaction by reacting with halgens which replace one of more H of the hydrocarbon
- CH3-CH3 + Cl2  CH3-CH2 –Cl + HCl

68
Q

Combustion of Saturated Hydrocarbon

A

exothermic reaction:

650 kJ/mole per CH2 group

69
Q

Substitution Reaction (Halogenation)

A

When we add a halogen (usually Br2 or Cl2) to an alkane, a halogen atom may substitute for a hydrogen atom.

Heat or light is essential for this reaction to work.

We will only consider monohalogenation in this class, where exactly one hydrogen atom is substituted. Halogenation occurs most readily on the most branched C atom in the alkane molecule.

In reality, more than one hydrogen atom may be substituted, giving many different products

70
Q

The combustion reactions of alkane are

A

highly exothermic. Therefore, alkane are often used as fuels, such as methane (nature gas), propane, and butane (cigarette lighter), gasoline and diesel (for automobiles).

71
Q

The most abundant source of alkanes is

A

fossil fuels, such as coal and petroleum/oil.

72
Q

fractional distillation

A

boiling points of an alkane increases with its size. Therefore, hydrocarbons of different sizes can be separated by their boiling point

73
Q

Oil Refinery: Fractional Distillation

A

Separating crude oil by the bp/size of alknaes.
The largest alkanes (highest bp) collect at the bottom.
The smallest alkanes (lowest bp) collect at the top.

74
Q

Unsaturated hydrocarbons contain

A

at least one double and/or triple bond in their structure.

75
Q

These groups are called unsaturated because

A

they can react with hydrogen under specific conditions to add more hydrogen to the molecule and to generate saturated hydrocarbons.

76
Q

does saturated hydrocarbons react with hydrogen

A

no

77
Q

3 major classes of unsaturated hydrocarbons

A

Alkenes contain a -C=C- double bond in their structure
Alkynes contain a –C=C- triple bond in their structure
Aromatic compounds contain a benzene ring in their structure

78
Q

Naming for Alkenes & Alkynes

A

The parent hydrocarbon is the longest chain which contains the double or triple bond
For an alkene, change the suffix of the parent hydrocarbon from “-ane” to “-ene”
For an alkyne, change the suffix of the parent hydrocarbon from “-ane” to “-yne”
Number in the direction which gives the double or triple bond the lowest possible number. Use the lower of the 2 C that has unsaturation to indicate the position of the double/triple bond.

79
Q

Cis-Trans Isomerism in Alkenes

A

The double bond in alkenes is rigid and cannot rotate.
The groups attaching to the carbons of the double bond are fixed relative to each other.
Cis-trans isomers occur when both C on the double bond are connect to different groups.

80
Q

in the cis isomer the H

A

on the same side

81
Q

in the trans-isomer the H

A

are on opposite side

82
Q

Physical Properties of of Alkenes & Alkynes

A

insoluble in water, soluble in non-polar solvent,
lower density than water.
Alkenes with less than 4 carbon atoms are gases at room temperature,
Alkenes with 5 to 17 carbon atoms are liquids.

83
Q

Chemical Properties of of Alkenes & Alkynes

A

More active than alkanes.

84
Q

Reactions of Alkenes and Alkynes

A

Combustion reaction
Addition reaction
Polymerization reaction

85
Q

Addition Reactions for Alkenes & Alkynes

A

a reaction in which atoms are added to double bond

86
Q

hydrogenation

A

adding hydrogen atoms to the carbon atoms of double/triple bonds. (A metal catalyst, e.g., Ni, or Pt is required)

87
Q

Hydrogenation of Oils

A

Vegetable oils are unsaturated fatty acids.
Adding H2 to double bonds in vegetable oils produces
Compounds with higher melting points.
Solids at room temperature such as margarine,
soft margarine, and shortening.

88
Q

halogenation

A

adding halogen atoms add to the carbon atoms of a double bond or triple bond.

89
Q

Bromine reacts with alkanes by

A

substitution, a reaction that requires light or heat.

90
Q

Bromine reacts with

A

alkenea by addition, a reaction that occurs rapidly and does NOT require light or heat

91
Q

Hydrohalogenation

A

adding the atoms of a hydrogen halide to the carbon atoms of a double bond or triple bond. (usually chloride or bromide)

92
Q

Hydration

A

adding the atoms of a hydrogen halide to the carbon atoms of a double bond or triple bond. (usually chloride or bromide)

93
Q

Aromatic Unsaturated Hydrocarbons

A

Benzene (C6H6):
A cyclic hexene with 3 conjugated double bonds that are hybridized among the 6 C atoms, turning all bonds inside the ring into 6 identical hybridized bonds. (Recall resonance structure from Chapter 4)
The identity of the 6 hybridized bonds is represented as a hexagon with a circle drawn inside.

94
Q

Chemical Stability of The Benzene Ring

A

Benzene is chemically like saturated alkane, only substitution reactions occur in which the C-H bond is substituted by a C-X bond.

95
Q

Aromatic compounds are named

A

With benzene as the parent chain.

Name R group or other atoms on the benzene ring as substitution.

96
Q

Common Benzene Derivatives

Compounds “derived” from benzene

A

Toluene Aniline Phenol
(methylbenzene) (benzenamine) (Hydroxybenzene)
or aminobenzene

(check drawing)

97
Q

Aromatic Compounds with 2 Groups

A

1, 3 1,4 1,2
Meta para ortho
m- p- o-

98
Q

What Is a Functional Group?

A

a group of atoms that are bonded together in a unique binding pattern

99
Q

The presence of a functional group in a compound gives the compound certain

A

characteristic chemical/physical properties

100
Q

a functional group is

A

the part of a molecule where most of its chemical reactions occur.

101
Q

example of a functional group

A

alkane — all single bonds, very stable
double bond: alkane → alkene
triple bond: alkane → alkyne

102
Q

Functional Groups Containing

C-Heteroatom Single Bonds C-X

A

R = The hydrocarbon chain with attached X

Name of the Class Functional group(X)
Halogenated Hydrocarbons R-X, F, Cl, Br, I
Alcohols R-OH -OH
Ethers R-O-R -O-
Thiols R-SH -SH
Amines R-NH2 -NH2

103
Q

Functional Groups Containing the C=O bond (The Carbonyl Group)

A

There are 5 major classes of carbonyl-containing organic compounds. They differ from one another by the atoms/groups attaching to the C atom.
- (check power point for structure ch12 pg4)

104
Q

Most functional groups contain

A

highly electronegative atoms and, therefore, polar bonds.

105
Q

Comp’ds with functional group have

A

higher polarity and stronger IMF.

106
Q

R-X has higher

A

bp., mp. And water solubility than R-H of the same size.

107
Q

R - X

A

R = Non-polar
Water insoluble X = Polar
Water soluble

Two opposing tendencies

108
Q

When R is small (C

A

X dominant, polarity dominant

R-X is water soluble

109
Q

When R is large (C > 4),

A

R dominant, non-polarity dominant

R-X is water insoluble

110
Q

functional group IUPAC Prefix

Halgens
alcohols
amines
thiols
ether
A
  • halo-
  • hydroxyl -
  • amino-
  • thio-
  • alkyoxy-
111
Q

functional group suffix

alcohols
amines
thiols

A
  • ol
  • amine
  • thiol
112
Q

as halogenated hydrocarbon-use prefix

Halogen atoms are called

A

fluoro-, chloro-, bromo- or iodo-.

113
Q

When double bond exist, the parent chain must include

A

the double bond and the chain is number from the end closest to the double bond, regardless of where X are located.

114
Q

Naming Alcohols, R-OH

A

In IUPAC system replace –e of alkane name with -ol.

That are common names use the name of the alkyl group followed by alcohol.

115
Q

Phenols

A

A phenol contains a hydroxyl group (—OH) attached to a benzene ring.

116
Q

To name a phenol with two substituents

A

Assign C-1 to the carbon attached to the –OH.
Number the ring to give the lowest numbers.
Use prefixes o, m, and p for common names

117
Q

Alcohols are classified by the number of

A

alkyl (R) groups attached to the OH (hydroxy) –bearing carbon into primary (1°), secondary (2°), or tertiary(3) alcohol.

118
Q

Water Solubility of Alcohols

A
  • “Like dissolves Like” and the IMF in water is hydrogen bonds.
  • Compounds which are able to form hydrogen bonds are generally much more soluble in water than those which cannot
  • Compounds able to form hydrogen bonds with water include alcohols, phenols, amines, and others
119
Q

In general, compounds with (i) many carbon atoms and (ii) comparatively few oxygen and nitrogen atoms are

A
  • not very soluble in water

alcohol with 1-4 carbon (up to butanol) is very soluble in water, but alcohols with 5 or more carbon are not.

120
Q

Water Solubility of Phenol

A

Is soluble in water.
Has a hydroxyl group that ionizes slightly
Is weak acid, corrosive and irritating to the skin

121
Q

Chemical Reactions of Alcohols

A
  1. Combustion is the reaction of an alcohol
    with O2 to produce CO2 and H2O.2CH3OH + 3O2 → 2 CO2 + 4H2O + Heat
  2. Dehydration
  3. Oxidation
122
Q

Dehydration of alcohol

A
  • check power oint ch 12 pg 22
123
Q

Oxidation of Primary (1) Alcohols

A

When a primary alcohol is oxidized [O],
One H is removed from the –OH.
Another H is removed from the carbon bonded to the OH.
An aldehyde is produced.

124
Q

Oxidation of Secondary (2) Alcohols

A

When a secondary alcohol is oxidized [O],
One H is removed from the –OH.
Another H is removed from the carbon bonded to the OH.
A ketone is produced.

125
Q

Oxidation of Tertiary (3)Alcohols

A

Tertiary alcohols do not readily oxidize!

			   [O] Tertiary alcohol			no reaction
126
Q

Amines

A

R-NH2
Are derivatives of ammonia NH3.
Contain N attached to one or more alkyl or aromatic groups.

127
Q

Naming Simple Amines

A

Amines are derivatives of NH3, with one or more alkly group attaching to N
Simple amines are named as alkylamines

128
Q

The simplest aromatic amine, a benzene ring has an amino group is called

A

aniline

129
Q

Amines are classified as

A

primary, secondary, or tertiary, based on the number of alkyl group attaching to the nitrogen atom (N).

130
Q

Classification of Amines

A 
In a primary (1°) amine, one carbon group is bonded to the nitrogen atom.
A secondary (2°) amine has two carbon groups.
A tertiary (3°) amine has three carbon groups
131
Q

Amines in Our Body

A

Many hormones and neurotransmitters are amines.

These biologically active amines regulates important body activities, from immunity, blood pressure to sleep, emotions.

132
Q

Properties of Amines

A

N in amine can form H-bonding with water. Amines with fewer than six carbon atoms are soluble in water.

Amines have strong, characteristic odors, and are toxic. The smells of ammonia, old fish, urine, rotting flesh, and semen are all mainly composed of amines

133
Q

The most important chemical property of amines

A

Amines, like ammonia, are weak base!

134
Q

Water Solubility of Amine Salts, RNH3+Cl-

A

Amine salts are ionic compounds.
They are solid at room temperature and but they are water soluble.
Many commonly used drugs are sold in the form of amine salts. A form that is not only stable/convenient but also easily absorbed by the body.

135
Q

Alkaloids

A

Alkaloids are naturally-occurring amines, often with a complex molecular structure
Common examples include
morphine, codeine, heroin (painkiller)
caffeine, nicotine (stimulant), ephedrine

136
Q

A heterocyclic organic compound

A

a cyclic compound in which one or more of the C atoms is the ring have been replaced with heteroatoms.
Cocaine is a heterocyclic amines

137
Q

Extraction of Cocaine and Alkaloids

A

Cocaine and alkaloids are often isolated from natural sources (usually plants) by treating them with hydrochloric acid
The resulting amine salts formed are usually water-soluble, and readily dissolve in the acid solution.

138
Q

Ethers, R-O-R

A

Ethers contain an ─O─ between two carbon groups.

Simple ether molecules are named by listing the alkyl names in alphabetical order followed by ether

139
Q

Ethers as Anesthetics

A

Ethers Inhibit pain signals to the brain.
Ethyl ether CH3─CH2─O─CH2─CH3 were used for over a century, but caused nausea and were flammable.
Developed by 1960s were nonflammable

140
Q

MTBE

A 
Methyl tert-butyl ether 
			    CH3
                          │
		CH3─O─C─CH3
                          │
		               CH3
Is one of the most produced organic chemicals.  
Is a fuel additive 
Is used to improve gasoline combustion.
Use is questioned since the discovery that MTBE has contaminated water supplies.
141
Q

Thiols, R-SH

A

The –SH group is called sufhydryl group
Thiols often have strong odors.
Are used to detect gas leaks.
Are found in onions, oysters, and garlic.

142
Q

Chemical Reaction Of Thiols

A

An important reaction for the 3D shape of proteins.

R-SH + HS-R2 –[O}–> R1-S-S-R2 + H2O Disulfide

143
Q

The Carbonyl Group C=O

A

There are 5 major classes of carbonyl-containing organic compounds. They differ from one another by the atoms/groups attaching to the C atom of the carbonyl group.

  • aldehyde RCHO
  • Carboxylic acid RCOOH
  • Amide RCONH2
  • Ketone RCOR
  • Ester RCOOR
144
Q

The Carbonyl Group C=O

A

There are 5 major classes of carbonyl-containing organic compounds. They differ from one another by the atoms/groups attaching to the C atom of the carbonyl group.

  • aldehyde RCHO
  • Carboxylic acid RCOOH
  • Amide RCONH2
  • Ketone RCOR
  • Ester RCOOR
145
Q

Physical Properties OF C=O-containing Comp’ds: General

A

The CARBONYL group is polar, which causes dipole-dipole interactions between molecules.
A carboxylic acid has a hydroxyl group (OH) attaching to C of the C=O group giving additional H-bonds between carboxylic acid molecules.
Recall polarity↑, IMF↑, water solubility↑, b.p.↑
When R are small, RCHO, RCOR, RCOOH are water soluble,
water solubility ↓, when R ↑.
Orders of b.p./m.p.:
RCOOH > ROH > Aldehye/Ketone > Alkanes

146
Q

Chemical Reactions of Ketones

A

Ketones can NOT be oxidized!

Ketones can undergo the following reactions:

1) Reduction
2) Addition Reaction: addition of alcohol to form hemiketal, followed by reaction of hemiketal with a 2nd alcohol to form ketal

147
Q

Chemical Reactions of Ketones

A

Ketones can NOT be oxidized!

Ketones can undergo the following reactions:

1) Reduction
2) Addition Reaction: addition of alcohol to form hemiketal, followed by reaction of hemiketal with a 2nd alcohol to form ketal

148
Q

Benedict’s Test For Aldehydes

A

Among the 5 classes of Carbonyl functional groups, only aldehydes can be oxidized by mild oxidizing agents, such as the Benedict’s Reagent.
Aldehyde, not ketone, turn the blue Benedict Reagent cloudy with brick red solid.

149
Q

Oxidation of Ethanol in the Body

A

In the body,
Ethanol is oxidized by enzymes in the liver.
Aldehyde product impairs coordination

150
Q

Addition Reactions of Aldehydes

A

Addition of an alcohol to a C=O double bond produces a hemiacetal, where the H atom of the alcohol adds to the O atom and R of the alcohol adds to the C atom.

Hemiacetals will react with an additional alcohol to form an acetal, where the new OR’ replaces the OH group of the hemiacetal.

151
Q

Addition Reactions of Ketones

A

Ketones react with alcohols similarly as aldehydes, the products are hemiketals and ketals.

152
Q

Carboxylic Acids, RCOOH

A

The –COOH functional group is called the carboxyl group.
IUPAC Name: Select the longest C chain as parent chain that includes the C of the carboxyl group. Name the parent chain by changing the –e ending of alkanes to –oic acid. The carboxyl C should be #1.

153
Q

Reactions of Carboxylic Acids-2

A

RCOOH reacts with alcohol R’OH to produce an ester RCOOR’ and water, when a strong acid is added as a catalyst. This reaction is called esterification.

RCOOH reacts with amine RNH2 to produce an amide RCONHR and water. (This reaction underlies the formation of protein from amino acids)

154
Q

Reactions of Carboxylic Acids-2

A

RCOOH reacts with alcohol R’OH to produce an ester RCOOR’ and water, when a strong acid is added as a catalyst. This reaction is called esterification.

RCOOH reacts with amine RNH2 to produce an amide RCONHR and water. (This reaction underlies the formation of protein from amino acids)

155
Q

The name of an ester contains the names of

A

The alkyl group from the alcohol.

The carbon chain from the acid with –ate ending

Chemistry (17 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions