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CHEMISTRY UNIT 2 > 1. Introduction to organic chemistry > Flashcards

1. Introduction to organic chemistry Flashcards

1
Q

Living things are made of

A

atoms covalently bonded to form molecules of organic compounds.

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2
Q

The great variety of organic compounds is possible because

A

every carbon atom can bond with other carbon atoms to form chains and rings

These chains and rings are often found bonded to
atoms of other elements, such as hydrogen, oxygen
and nitrogen

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3
Q

not all carbon compounds are classified as organic compounds.
examples of inorganic compounds are

A

the oxides of carbon and compounds containing carbonate and hydrogencarbonate ions

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4
Q

The substances that form the basis of all living things are

A

organic compounds.

Carbon atoms tend to form the ‘backbone’ of organic molecules – from the proteins in muscles and enzymes to the DNA that determines our characteristics

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5
Q

Hydrocarbons are

A

compounds of carbon and hydrogen only

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6
Q

Organic compounds comprise the

A

largest group of compounds on earth

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7
Q

Many things around you have carbon as the most abundant atom in them, including

A

food, clothes, paper, coal, fuel, diamonds … the list is endless

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8
Q

A long time ago, clothes were made from cotton only, which is made up of carbon atoms.

The second industrial revolution brought about

A

the process of synthesis, when people realized that they can make new products from existing materials and turn the material into something completely new through a range of reactions that usually mimic something that already exists naturally.

Polymers are such an example.

To a large extent, they have replaced cotton through reactions that produce synthetic materials such as polyester, polyamides, etc.

These play an important role in the clothing industry, and in many other industrial and home products

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9
Q

A macromolecule is a

A

molecule that consists of a large number of atoms.

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10
Q

The most common macromolecules in biochemistry are

A

biopolymers (nucleic acids, proteins, carbohydrates and lipids)

large non-polymeric molecules (such as lipids and macrocycles) and

carbohydrates (polymers of simple sugars.)

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11
Q

A polymer is a

A

large molecule composed of smaller monomer units that are covalently bonded to each other in a repeating pattern

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12
Q

A monomer is a

A

small organic molecule that can be covalently bonded to each other in a repeating pattern.

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13
Q

Polymerisation is a

A

chemical reaction in which monomer molecules join to form a polymer

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14
Q

Condensation polymerisation is when

A

molecules of two monomers with different functional

groups undergo condensation reactions with the loss of small molecules, usually water

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15
Q

A carboxylic acid monomer and an alcohol monomer can join in

A

an ester linkage.

They are all joined by ester linkages, the polymer chain is a polyester

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16
Q

We can represent organic molecules by

A

a variety of different types of formula

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17
Q

which type of formula gives us the least detail

A

The empirical formula

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18
Q

empirical formula tells us what?

A

the simplest ratio of the different types of atoms present in the molecule.

For example, an organic compound called propene has the empirical formula CH2.
This tells us that it has twice as many hydrogen atoms as carbon atoms in its molecules.

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19
Q

We can calculate empirical formulae from

A

experimental data on the mass of each element, and hence the number of moles of each element, in a sample of a compound

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20
Q

Calculate the empirical formula of a compound of carbon, hydrogen and iodine that contains 8.45% carbon, 2.11% hydrogen and 89.44% iodine by mass.

(Ar values: C = 12.0, H = 1.0, 1= 127.0).

A

CH3I (iodine)

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21
Q

molecular formula shows us

A

the actual numbers of each type of atom in a molecule.

(the numbers and types of atom present in a molecule)

The functional group is shown separately from the hydrocarbon chain — for example, C2H5OH rather than C2H6O.

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22
Q

To find the molecular formula we need to know

A

the relative molecular mass of the compound.

The relative molecular mass of propene is 42.
We know that its empirical formula is CH2; this CH2 group of atoms has a relative mass of 14, as the relative atomic mass of C = 12 and H = 1.
By dividing the relative molecular mass by the relative mass of the empirical formula (42/14 = 3), we see that there must be (3 × CH2 ) atoms in a propene molecule. So its molecular formula is C3 H6.

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23
Q

structural formula shows

A

the arrangement of the atoms in a molecule

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24
Q

A displayed formula shows

A

the correct positioning of the atoms and the bonds between them.

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25
Q

A simplified version of the displayed formula is called the

A

skeletal formula.

It has all the symbols for carbon and hydrogen atoms removed, as well as the carbon to hydrogen bonds.

The carbon to carbon bonds are left in place.

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26
Q

list of homologous series

A

Alkanes

Alkenes

Alkynes

Alcohols

Haloalkanes (Alkylhalides)

Aldehydes

Ketones

Carboxylic acids

Esters

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27
Q

alkane General formula

A

CnH2n+2

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28
Q

alkane functional group

A

C-C

Alkyl

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29
Q

Alkane Example

A

Ethane

propane

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30
Q

name ending suffix of alkane

A

-ane

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31
Q

Alkenes general formula

A

CnH2n

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32
Q

Alkenes functional group

A

C=C

Alkenyl

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33
Q

Alkenes Example

A

propene

ethene

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34
Q

name ending suffix of Alkenes

A

-ene

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35
Q

Alkynes general formula

A

CnH2n-2

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36
Q

alkynes functional group

A

alkynyl

C≡C

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37
Q

Alkynes suffix name ending

A

-yne

eg-propyne

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38
Q

Alcohols general formula

A

CnH2n+1OH

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39
Q

Alcohols functional group

A

-OH (hydroxyl group)

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40
Q

Alcohols name ending suffix

A

-ol

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41
Q

Haloalkanes (Alkylhalides) general formula

A

Cn H2n+1X X = F, CI, Br or I

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42
Q

Haloalkanes (Alkylhalides) suffix ending

A

-ane

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43
Q

Haloalkanes (Alkylhalides) functional group

A

c-c

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44
Q

Aldehydes general formula

A

CnH2nO

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45
Q

Aldehydes functional group

A

CHO

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46
Q

Aldehydes name ending suffix

A

-al

47
Q

Ketones general formula

A

CnH2nO

48
Q

Ketones functional group

A

carbonyl group (CO)

49
Q

Ketones name ending suffix

A

-one

eg-propanone

50
Q

Carboxylic acids general formula

A

CnH2nO2

51
Q

Carboxylic acids functional group

A

carboxyl group (COOH)

52
Q

Carboxylic acids name ending suffix

A

-anoic (acid)

eg-propanoic acid

53
Q

Esters functional group

A

COO

54
Q

Esters name ending suffix

A

-noate

eg- methyl ethanoate

55
Q

Different classes of compounds have different functional groups. The functional group determines what?

A

determines the characteristic chemical properties of the compounds that contain that specific functional group.

The functional group in an alkene is the C=C double bond.

The functional group in a carboxylic acid is the COOH group.

56
Q

By substituting a number for n in the general formula you get

A

the molecular formula of a particular compound containing that functional group.

57
Q

the prefix indicates

A

the number of carbon atoms present in the main chain

58
Q

Hydrocarbon molecules do not have only straight chains, they can be branched. when naming a branched molecule remember to use what as the basic hydrocarbon?

A

the longest continuous carbon chain

count from the end that gives the lower number

59
Q

The double bond in alkenes makes them

A

more reactive

60
Q

Arenes are a family of

A

hydrocarbons that contain a benzene ring made up of six carbons

61
Q

In a benzene ring the carbon atoms are numbered

A

clockwise from the uppermost atom.

You only need to use this numbering system if there is more than one group attached to the ring.

62
Q

In chain isomerism, the isomers arise due to

A

branching of the carbon chain.

63
Q

Position isomerism is where

A

the position of the functional group is different in each isomer.

the carbon chain is fixed, but the position of substituent groups can vary.

64
Q

in functional group isomerism

A

where the molecular formula of the isomers is the same but the functional groups are different

This is important because it changes the chemical reactions that the molecule undergoes.

65
Q

Geometric isomerism occurs where

A

there is restricted rotation around a bond, such as in alkenes.

It also needs two groups, one on each end of the double bond, such as in 1,2-dichloroethene

These two forms are different because the double bond prevents the rotation needed to make the two forms identical.

66
Q

Carbon is unique in that it

A

forms a large variety of compounds

67
Q

carbon has the ability to form many compounds largely due to

A
  • the types of bonds it can form

- the number of different elements that can bond with it

68
Q

once formed, the carbon to carbon (C—C) single covalent bonds are

A

very strong in comparison to other single covalent bonds.

Bond energies:

C—C = 350kJmol-1 ; N—N = 160kJmol-1 ;

O—O = 150kJmol-1

It takes a lot of energy to break these strong bonds, so the compounds formed are stable.

69
Q

properties of carbon which makes it one of the most versatile elements on the periodic table (3)

A
  • carbon is tetravalent
  • carbon has the property catenation
  • carbon has the ability hybridization
70
Q

how carbon being a tetravalent makes it one of the most versatile element on the periodic table

A

carbon is tetravalent which means it has 4 electrons on it outermost shell that are available for covalent bonding

71
Q

example of carbon being a tetravalent

A

in methane the tetravalent carbon atom can form a covalent bond with each of 4 hydrogen atoms

72
Q

how carbon having the property catenation makes it one of the most versatile elements on the periodic table

A

it means that carbon has the ability to bond with other carbon atoms to form straight chain, branched chains and ring compounds with interconnecting C-C bonds which are fairly strong and abnormally stable which is important as it allows carbon to form a large number of compounds

73
Q

Catenation is

A

the covalent bonding of an element to itself to form chains or rings

74
Q

carbon-carbon strong bonds is important because

A

it allows carbon to form a large number of compounds

75
Q

what happens to organic and inorganic compounds and chemicals when heated

A

Most organic compounds burn or char (go black) when heated.

Most inorganic chemicals just melt

76
Q

Hybridization is

A

the mixing of several atomic orbitals to form the same total number of equivalent hybrid orbitals

77
Q

sp3 hybridization is

A

A type of hybridization that results from the combination of the s orbital and all three p orbitals in the second energy level of carbon, resulting in four hybrid orbitals and occurs when a carbon atom is bonded to four other atoms.
The geometric arrangement of those four hybrid orbitals is called tetrahedral.

78
Q

As a result of hybridization, carbon can form

A

single, double and triple bonds with itself.

79
Q

the four sp3 hybrid orbitals allows

A

carbon to form four single bonds

80
Q

in sp2 hybridization

A

one of the sp2 hybrid orbitals and the one pure p orbitals give rise to a double bond

81
Q

all three types of bonding pattern (sp3, sp2 and sp) are

A

very strong and contribute to the formation of stable organic compounds

82
Q

organic compounds can be placed into various well-defined groups called

A

homologous series

83
Q

all members of a homologous series have

A
  • same general formula
  • each member differs from its nearest neighbor by a molecular mass of 14 or a CH^2 group
  • same functional group
  • similar chemical properties
  • physical properties vary directly to the number of C atoms in the homologous series
84
Q

how members of the homologous series have the same general formula

A

they all have the same general formula and it is a common relationship that exists between the numbers of different atoms in the compounds.

eg- ethene (C2H4) and propene (C3H6) have the same general formula CnH2n where n is the number of carbon atoms in the compound

85
Q

how members of the homologous series differs from its nearest neighbor by a molecular mass of 14 or a CH^2 group

A

each member differs from its nearest neighbor by a molecular mass of 14 or a CH^2 group

eg- the molecular mass of ethene (C2H4) is 28 whereas that of propene (C3H6) IS 42, a mass difference of 14 or a CH2 unit

86
Q

how members of the homologous series have the same functional group

A

eg- all alkenes have a double bond (C=C) whereas all the alcohols have a hydroxyl (OH) group

87
Q

how members of the homologous series have similar chemical properties

A

because reactivity is determined by the functional group and since they have the same functional group they will react similarly

88
Q

how to calculate the empirical formula from the percentage mass of a compound

A
  • divide the percentage of each element by its atomic mass to convert to moles
  • divide the values obtained by the smallest number to find the ratio of moles
  • if need be multiply by a common factor to bring all to whole numbers
89
Q

when butene was analyzed it was found to contain 85.72% carbon an 14.28%. calculate its empirical formula

A

carbon
percentage- 85.72%
divide by atomic mass- 85.72/12=7.14
divide by smaller ratio- 7.14/7.14= 1

hydrogen
percentage- 14.28%
divide by atomic mass- 14.28/1= 14.28
divide by smaller ratio- 14.28/7.14=2

empirical formula is CH2.

90
Q

Resonance is where

A

the structure of a compound is a single form which is ‘in-between’ two or more extreme structures

91
Q

A homologous series is a

A

group of organic compounds with the same functional group in which each successive member increases by the unit —CH2

92
Q

The IUPAC rules We use a set of rules to name compounds. Naming compounds in a particular way is called a

A

systematic nomenclature.

Systematic names can be used to tell us about the structure of organic carbon compounds.

93
Q

Simple carbon compounds may have several parts to their name which are:

A

the stem: this tells us how many carbon atoms there are along the main chain of a compound

A suffix: this is often added to the end of the stem.
This tells us about the functional groups present.
For example, the sufx -ol in the name propanol tells us that the compound is in the alcohol homologous series, and the stem, prop- tells us it has three carbon atoms.

A prefix: for some homologous series, the functional group appears as a prex before the stem.
For example, the bromo- in the name bromobutanol tells us that the compound is in the halogenoalkane homologous series and the but- tells us it has four carbon atoms.

94
Q

Naming branched-chain alkanes

A

The position of side chains or functional groups is shown by numbering the carbon atoms.

The longest possible chain of carbon atoms is chosen.

Numbering starts at the end that gives the smallest number possible for the side chain.

The side chain prexes (comes before) the stem name.

The side chain is named according to the number of carbon atoms it contains.

These groups are called alkyl groups. The alkyl group name is formed by changing the ‘ane’ of ‘alkane’ to ‘yl’.

If there is more than one of the same alkyl side chain or functional group we use the prexes di-, tri- and tetra-

numbers are separated from each other by commas numbers are separated from words by hyphens.

If there are different side chains, they are listed in alphabetical order

95
Q

Isomers are

A

molecules that have the same molecular formula but the atoms are arranged differently.

96
Q

The two main types of isomerism are

A

structural isomerism and stereoisomerism

97
Q

There are three types of structural isomerism

A

chain isomerism

functional group isomerism

positional isomerism.

98
Q

There is free rotation about

A

single bonds.

Because of this, you need to take care when drawing structural formulae of different isomers, making sure that you don’t repeat the same structure

99
Q

Stereoisomerism is where

A

two (or more) compounds have the same atoms bonded to each other but the atoms have a different arrangement in space.

100
Q

There are two types of stereoisomerism:

A

geometrical isomerism (also called cis trans isomerism) optical isomerism

101
Q

Geometrical (cis-trans) isomerism is

A

when the substituent groups either side of a double bond are arranged either on the same side (cis) or on the opposite sides (trans).

102
Q

Optical isomerism happens when

A

four different groups are attached to a central carbon atom.

The two isomers formed are mirror images of each other.

They are not identical because they cannot be superimposed (matched up exactly) on one another.

However you try to rotate them, they do not match up exactly.

103
Q

The amino acids and carbohydrates in our bodies are particular forms of

A

optical isomers.

Our bodies cannot deal with their mirror images.

It is fortunate for us that the amino acids and carbohydrates we get from our food are the correct optical isomers for our bodies.

104
Q

The word chiral comes from

A

the ancient Greek for ‘hand’.

Your left hand is a mirror image of your right hand but you cannot superimpose one exactly on the other.

105
Q

Aryl compounds contain at least one

A

benzene ring

106
Q

If a single alkyl group is attached to the ring, we do not

A

number this group.

If there is more than one alkyl group attached to the ring we show their positions by giving them the smallest numbers possible.

107
Q

The larger the number of carbon atoms in a hydrocarbon, the greater is

A

the number of possible isomers.

108
Q

Cellulose, a very large molecule built up from carbon, hydrogen and oxygen, provides

A

structural tissue in plants.

109
Q

Living organisms also produce many other organic compounds, some of which are very useful to us.

examples include

A

Quinine, C20H24N2O2, is found in the bark of trees of the genus Cinchona.
For many years quinine was the most important drug for treatment of malaria and many modern anti-malarial drugs are similar in structure.

■ Table sugar is sucrose, C12H22O11.
The production of sugar from sugar cane was one of the driving forces behind the transatlantic slave trade and the eventual formation of modern West Indian societies.

■ Cholesterol, C27H46O, is found in animals.
An accumulation of cholesterol in the walls of blood vessels may lead to many illnesses, including strokes and heart attacks.

Cholesterol, however, is the starting material for the formation of other important natural compounds such as sex hormones.

110
Q

Many complex molecules which occur in living organisms (known as natural products) can be made in

A

the laboratory (synthesized) from simple compounds.

Synthesis is one of the important areas of organic chemistry, and each year chemists succeed in synthesizing many natural compounds with very complicated structures.

In principle, we should be able to synthesize any natural organic compound - but some are extremely large and complex macromolecules that probably no one will synthesize.

The speed and efficiency with which living organisms synthesize complex molecules from simple starting materials (carbon dioxide and water in plants, glucose in animals) is truly amazing.

111
Q

Biosynthesis means

A

synthesis carried out by living organisms

112
Q

synthesis means

A

combination reactions/putting together

113
Q

A carbon atom has six electrons, four of which are involved with

A

making four covalent bonds.

114
Q

The simplest unsaturated hydrocarbon is called

A

ethene because it is derived from ethane.

CHEMISTRY UNIT 2 (3 decks)

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