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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
A simplified version of the displayed formula is called the
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.
26
list of homologous series
Alkanes Alkenes Alkynes Alcohols Haloalkanes (Alkylhalides) Aldehydes Ketones Carboxylic acids Esters
27
alkane General formula
CnH2n+2
28
alkane functional group
C-C Alkyl
29
Alkane Example
Ethane propane
30
name ending suffix of alkane
-ane
31
Alkenes general formula
CnH2n
32
Alkenes functional group
C=C Alkenyl
33
Alkenes Example
propene ethene
34
name ending suffix of Alkenes
-ene
35
Alkynes general formula
CnH2n-2
36
alkynes functional group
alkynyl C≡C
37
Alkynes suffix name ending
-yne eg-propyne
38
Alcohols general formula
CnH2n+1OH
39
Alcohols functional group
-OH (hydroxyl group)
40
Alcohols name ending suffix
-ol
41
Haloalkanes (Alkylhalides) general formula
Cn H2n+1X X = F, CI, Br or I
42
Haloalkanes (Alkylhalides) suffix ending
-ane
43
Haloalkanes (Alkylhalides) functional group
c-c
44
Aldehydes general formula
CnH2nO
45
Aldehydes functional group
CHO
46
Aldehydes name ending suffix
-al
47
Ketones general formula
CnH2nO
48
Ketones functional group
carbonyl group (CO)
49
Ketones name ending suffix
-one eg-propanone
50
Carboxylic acids general formula
CnH2nO2
51
Carboxylic acids functional group
carboxyl group (COOH)
52
Carboxylic acids name ending suffix
-anoic (acid) eg-propanoic acid
53
Esters functional group
COO
54
Esters name ending suffix
-noate eg- methyl ethanoate
55
Different classes of compounds have different functional groups. The functional group determines what?
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
By substituting a number for n in the general formula you get
the molecular formula of a particular compound containing that functional group.
57
the prefix indicates
the number of carbon atoms present in the main chain
58
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?
the longest continuous carbon chain count from the end that gives the lower number
59
The double bond in alkenes makes them
more reactive
60
Arenes are a family of
hydrocarbons that contain a benzene ring made up of six carbons
61
In a benzene ring the carbon atoms are numbered
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
In chain isomerism, the isomers arise due to
branching of the carbon chain.
63
Position isomerism is where
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
in functional group isomerism
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
Geometric isomerism occurs where
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
Carbon is unique in that it
forms a large variety of compounds
67
carbon has the ability to form many compounds largely due to
- the types of bonds it can form | - the number of different elements that can bond with it
68
once formed, the carbon to carbon (C—C) single covalent bonds are
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
properties of carbon which makes it one of the most versatile elements on the periodic table (3)
- carbon is tetravalent - carbon has the property catenation - carbon has the ability hybridization
70
how carbon being a tetravalent makes it one of the most versatile element on the periodic table
carbon is tetravalent which means it has 4 electrons on it outermost shell that are available for covalent bonding
71
example of carbon being a tetravalent
in methane the tetravalent carbon atom can form a covalent bond with each of 4 hydrogen atoms
72
how carbon having the property catenation makes it one of the most versatile elements on the periodic table
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
Catenation is
the covalent bonding of an element to itself to form chains or rings
74
carbon-carbon strong bonds is important because
it allows carbon to form a large number of compounds
75
what happens to organic and inorganic compounds and chemicals when heated
Most organic compounds burn or char (go black) when heated. Most inorganic chemicals just melt
76
Hybridization is
the mixing of several atomic orbitals to form the same total number of equivalent hybrid orbitals
77
sp3 hybridization is
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
As a result of hybridization, carbon can form
single, double and triple bonds with itself.
79
the four sp3 hybrid orbitals allows
carbon to form four single bonds
80
in sp2 hybridization
one of the sp2 hybrid orbitals and the one pure p orbitals give rise to a double bond
81
all three types of bonding pattern (sp3, sp2 and sp) are
very strong and contribute to the formation of stable organic compounds
82
organic compounds can be placed into various well-defined groups called
homologous series
83
all members of a homologous series have
- 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
how members of the homologous series have the same general formula
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
how members of the homologous series differs from its nearest neighbor by a molecular mass of 14 or a CH^2 group
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
how members of the homologous series have the same functional group
eg- all alkenes have a double bond (C=C) whereas all the alcohols have a hydroxyl (OH) group
87
how members of the homologous series have similar chemical properties
because reactivity is determined by the functional group and since they have the same functional group they will react similarly
88
how to calculate the empirical formula from the percentage mass of a compound
- 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
when butene was analyzed it was found to contain 85.72% carbon an 14.28%. calculate its empirical formula
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
Resonance is where
the structure of a compound is a single form which is 'in-between' two or more extreme structures
91
A homologous series is a
group of organic compounds with the same functional group in which each successive member increases by the unit —CH2
92
The IUPAC rules We use a set of rules to name compounds. Naming compounds in a particular way is called a
systematic nomenclature. Systematic names can be used to tell us about the structure of organic carbon compounds.
93
Simple carbon compounds may have several parts to their name which are:
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
Naming branched-chain alkanes
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
Isomers are
molecules that have the same molecular formula but the atoms are arranged differently.
96
The two main types of isomerism are
structural isomerism and stereoisomerism
97
There are three types of structural isomerism
chain isomerism functional group isomerism positional isomerism.
98
There is free rotation about
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
Stereoisomerism is where
two (or more) compounds have the same atoms bonded to each other but the atoms have a different arrangement in space.
100
There are two types of stereoisomerism:
geometrical isomerism (also called cis trans isomerism) optical isomerism
101
Geometrical (cis-trans) isomerism is
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
Optical isomerism happens when
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
The amino acids and carbohydrates in our bodies are particular forms of
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
The word chiral comes from
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
Aryl compounds contain at least one
benzene ring
106
If a single alkyl group is attached to the ring, we do not
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
The larger the number of carbon atoms in a hydrocarbon, the greater is
the number of possible isomers.
108
Cellulose, a very large molecule built up from carbon, hydrogen and oxygen, provides
structural tissue in plants.
109
Living organisms also produce many other organic compounds, some of which are very useful to us. examples include
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
Many complex molecules which occur in living organisms (known as natural products) can be made in
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
Biosynthesis means
synthesis carried out by living organisms
112
synthesis means
combination reactions/putting together
113
A carbon atom has six electrons, four of which are involved with
making four covalent bonds.
114
The simplest unsaturated hydrocarbon is called
ethene because it is derived from ethane.

CHEMISTRY UNIT 2 (3 decks)

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