Organic Chemistry

Front 1

Define crude oil.

Back 1

a fossil fuel which is a mixture of hundreds ofdifferent compounds.

Front 2

How is crude oil formed?

Back 2

Crude oil is found trapped in sedimentary rocks.

1. Millions of years ago, microscopic animals and plants fell to the bottom of the sea. Their remains then covered by mud.

2. More sediment buried the mud sediment, it started to change into rock, as temperature and pressure increased. The remains were ‘cooked’ by this process, and changed into crude oil.

3. Oil will rise as a result of pressure from below, escaping altogether if the rocks are permeable.

Front 3

Environmental considerations of burning fossil fuels

Back 3

· One of the products of burning fossil fuels is carbon dioxide which contributes significantly to global warming.

· Air pollution leading to respiratory diseases

· Water and land pollution (acid rain, oil spills)

Front 4

What makes a good fuel?

Back 4

A fuel which releases a lot of heat energy per gram, is non-polluting and is easy to transport.

Front 5

Define fossil fuel.

Back 5

fuel formed from the remains of tiny dead sea creatures and plants over millions of years.

Crude oil, coal, natural gas.

Front 6

What is natural gas mainly made of?

Back 6

methane.

Front 7

Define fractional distillation.

Back 7

the separation of a liquid mixture into fractions differing in boiling point (and hence chemical composition) by means of distillation, typically using a fractionating column.

Front 8

What fractions does fractional distillation produce?

Back 8

refinery gas, gasoline, naphtha, kerosone, diesel, fuel oil

residues: lubricating oils and bitumen

Front 9

Define petroleum.

Back 9

a liquid mixture of hydrocarbons which is present in suitable rock strata and can be extracted and refined to produce fuels including petrol, paraffin, and diesel oil; oil.

Front 10

What is nylon used for?

Back 10

fabric, cookware and machine parts

Front 11

What is kerosene used for?

Back 11

fuel for jet aircrafts

Front 12

What is naphtha used for?

Back 12

making chemicals, especially plastics

Front 13

What is diesel oil used for?

Back 13

fuel for lorries and tractors

Front 14

What is gasoline used for?

Back 14

fuel for cars

Front 15

What is fuel oil (heavy gas oil) used for?

Back 15

fuel for power stations, ships and home heating

Front 16

Define cracking.

Back 16

the process of breaking down certain hydrocarbons into simpler ones of lower boiling points by means of excess heat, distillation under pressure, etc., in order to give a greater yield of low- boiling products than could be obtained by simple distillation.

Front 17

Complete combustion

Back 17

methane+oxygen=carbon dioxide+water

CH4 + O2 = CO2 + H2O

Front 18

Incomplete combustion

Back 18

methane+oxygen=carbon dioxide+water+carbon

CH4 + O2 = CO2 + H2O + C

Front 19

Define hydrocarbon.

Back 19

acompound of hydrogen and carbon, such as any of those which are the chiefcomponents of petroleum and natural gas.

Front 20

Define homologous series.

Back 20

a series of compounds with the same general formula.

Front 21

What are alkanes?

Back 21

any of the series of saturated hydrocarbons includingmethane, ethane, propane, and higher members.

Front 22

Describe bonding in alkanes

Back 22

Covalent bonds.

Front 23

Chemical properties of alkanes.

Back 23

- they do not react with acids or alkalines

-they burn under special conditions with a clear blue flame when plenty of oxygen is present. Complete combustion.

Front 24

What are alkenes?

Back 24

any of the series of unsaturated hydrocarbonscontaining a double bond, including ethylene and propene.

Front 25

What is the molecular formula for methane, ethene and propene.

Back 25

CH4

C2H4

C3H8

Front 26

How to test for saturated fats?

Back 26

when shaken with bromine water, the water becomes colourless if it is with an unsaturated oil,but it stays orange-brown when shaken with a saturated fat.

Front 27

Why are alkenes so usefulin comparison to alkanes?

Back 27

Alkenes,with a catalyst, can make several kinds of polymers (plastics) through additionreaction. Also the double bond makes it more reactive as carbon likes to makefour bonds. The more reactive it is the more you can do with it.

Front 28

Name the prefixes up until nine

Back 28

meth-

eth-

pro-

but-

pen-

hex-

hept-

oct-

non-

Front 29

What are isomers?

Back 29

each of two ormore compounds with the same formula but a different arrangement of atoms inthe molecule and different properties.

Front 30

What are structural isomers?

Back 30

compounds which have the same molecular formula but have different structural formulae.

Front 31

Define hydrogenation

Back 31

the addition of hydrogen to an unsaturated compound

Front 32

Equation for hydrogenation

Back 32

Hydrogen+alkene= alkane

catalyst is often used.

Front 33

Define an alcohol.

Back 33

a substancecontaining an -OH group attached to a hydrocarbon group.

Front 34

Examples of an alcohol.

Back 34

Methanol, ethanol, butanol, propanol, heptanol, hexanol etc.

Front 35

Define an endothermic reaction.

Back 35

accompanied byor requiring the absorption of heat.

-Δ = energyin

Front 36

Define an exothermic reaction.

Back 36

accompanied by the release of heat.

+Δ = energy out

Front 37

How to make an alcohol.

Back 37

Alkene+steam= alcohol

Fermentation

Front 38

What conditions are needed for ethene to react with steam to produce ethanol?

Back 38

High temperature and high pressure.

Front 39

Define fermentation.

Back 39

the chemical breakdown of asubstance by bacteria, yeasts, or other micro-organisms, typically involvingeffervescence and the giving off of heat.

Front 40

Ethanol to ethanoic acid

Back 40

- oxidation in the air
enzymes from bacteria which is naturally present in the air speed up the conversion of ethanol to ethanoic acid. Requires oxygen.

- acified potassium managanate

Front 41

Name a naturally occurring alcohol.

Back 41

Vinegar.

Front 42

Define a carboxylic acid.

Back 42

a weak organic acids with –COOH as the functionalgroup. Their names all end in –oic acid.

Front 43

Properties of carboxylic acids.

Back 43

-they are only partially ionised in water.

-the hydrogen of the -COOH group is the only one that is responsible for the acidity of carboxylic acids.

Front 44

What type of linkage is formed when a carboxylic acids reacts with an alcohol?

Back 44

an ester linkage

Front 45

Define functional group.

Back 45

a group of atoms responsible for the characteristic reactions of a particular compound.

Front 46

Write the formula of the functional groups of carboxylic acids, alcohols and amines

Back 46

carboxylic acids, -COOH

alcohols, -OH

amines, NH2

Front 47

What is the general structure of a di-carboxylic acid?

Back 47

H H

I I

HO - C - C - OH

I I

H H

Front 48

Define monomer.

Back 48

a molecule that can be bonded to other identicalmolecules to form a polymer.

Front 49

Define polymerization.

Back 49

a process of reactingmonomer molecules together in a chemical reaction to form polymer chains or three-dimensional networks.

Front 50

Define addition polymerization.

Back 50

the formation of polymers from monomers where no other substance than the polymer is formed.

Front 51

Define a plastic. Examples.

Back 51

a synthetic material made from a wide range of organic polymers such as polyethylene, PVC, nylon, etc., that can be moulded into shape while soft, and then set into a rigid or slightly elastic form.

Front 52

What type of molecules are plastics and proteins?

Back 52

Macromolecules.

Front 53

Define macromolecule.

Back 53

a molecule containing a very large number of atoms, such as a protein, nucleic acid, or synthetic polymer.

Front 54

Advantages and disadvantages of polymerizationto produce plastics

Back 54

Advantages:

· They can be easily moulded and have excellent finishing.

· Durability

· Chemical resistance.Plasticis strong, good and cheap to produce.

Disadvantages:
· Produces toxic fumes when it is burnt· It isa recycle process, but it is very costly.· Non-renewableresourceDoes not biodegrade rkA6>?

Front 55

Explain the chemical reaction for building a polymer from a set ofmonomers.

Back 55

in thisprocess, two monomers are covalently bonded by the removal of awater molecule. Each organic monomer has a hydroxyl group (-OH) onone side and a hydrogen (H) on the other. When two monomers lineup side by side, they will have these two functional groups facing oneanother (H & OH). The H and the OH will break off of their respectivemonomers and bond forming a water molecule.

Front 56

Describe the polymerization of ethene to produce poly(ethen).

Back 56

Front 57

What type of reaction occurs when ethene molecules are polymerised?

Back 57

addition polymerization

Front 58

What feature of ethene is responsible for its ability to polymerise?

Back 58

its double bond which opens up to create new bonds with other monomers.

Front 59

Uses of polypropene.

Back 59

packaging, labelling, textiles and so on.

Front 60

What is PET used for?

Back 60

Plastic bottles, containers and pots

Front 61

Define condensation polymerization.

Back 61

polymerization in which a single molecule iseliminated —distinguished from additionpolymerization

Front 62

Examples of condensation polymers.

Back 62

Polyesters, polyamides, proteins and polysaccharides such ascellulose, are all examples of condensation polymers.

Front 63

Define ester.

Back 63

a compound produced by the reaction between an acid and an alcoholwith the elimination of a molecule of water

Front 64

How to make an ester.

Back 64

Carboxylic acid+ alcohol= ester +water

Front 65

Define an ester linkage.

Back 65

The -COO group found in esters, fats and oils

Front 66

Define polyester.

Back 66

A polymer with -COO- linkages

Front 67

Example of a polyester.

Back 67

Terylene.

Front 68

What kind of monomers are needed to form polyesters?

Back 68

carboxylic acids and alcohols

Front 69

Define hydrolysis.

Back 69

the breakdown of a compound by reaction with water. Acids or alkalis speed up hydrolysis.

Front 70

How to make a soap (equation).

Back 70

Fat+ sodium hydroxide= soap+ glycerol

Front 71

Define amine.

Back 71

a compound with an -NH2 functional group

Front 72

Reaction of an amine with a carboxylic acid.

Back 72

amine+ carboxylic acid= amide + water

Front 73

What kind of monomers are needed to form a polyamine?

Back 73

Di-amines and di-carboxylic acids

Front 74

What is the general structure of the di-amine monomers that made a polyamide?

Back 74

H H H

I I I

N - C - N

I I I

H H H

Front 75

Explain why carboxylic acids and di-amines are able to join together to form a long chain polyamide polymer.

Back 75

when condensation polymerization occurs when di-amines and di-carboxylic acisa are present, more OH and H atoms can be eliminated to produce water molecules

Front 76

Define polyamide.

Back 76

polymers where the repeating units are held together by amide links, -CONH- links.

Front 77

Example of a polyamide.

Back 77

nylon.

Front 78

Define carbohydrate.

Back 78

the general name for complex sugars.

Front 79

How can complex carbohydrates be made into simple sugars? What is this an example of?

Back 79

complex carbohydrates can be hydrolysed to simple sugars by concentrated hydrochloric acid.

In our bodies starch is hydrolysed to glucose using enzymes.

Front 80

Hydrolysis breaking down complex carbohydrates using simplified formula.

Back 80

starch+ water=(using hydrochloric acid and heat) glucose

Front 81

What functional groups react to join glucose monomers together to form starch?

Back 81

-OH

Front 82

What is the natural polymer starch made from?

Back 82

it is made from the monomer glucose

Front 83

How does a breathalysers work?

Back 83

Oxidation with acified potassium dichromate

Glass tube containingpotassium dichromate- sulphuric acid coated on silica gel beads. As the personblows the plastic bag fills with air.

Orange- theoriginal colour of potassium dichromate.

Green- theethanol in the persons breath changes to green