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(GCSE) Chemistry > C10. Organic Reactions (Y11 - Spring 1) > Flashcards

C10. Organic Reactions (Y11 - Spring 1) Flashcards

1
Q

🟢 What are the 4 Homologous Series

A
  • Alkanes
  • Alkenes
  • Alochols
  • Carboxylic Acids
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2
Q

🟢 Alkanes:

  • General Formula
  • 1 x C
  • 2 x C
  • 3 x C
  • 4 x C
  • 5 x C
A

General Formula:
CnH2n+2

1 x C:
Methane, CH4

2 x C:
Ethane, C2H6

3 x C:
Propane, C3H8

4 x C:
Butane, C4H10

5 x C:
Pentane, C5H12

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3
Q

🟠 Alkenes:

  • General Formula
  • 1 x C
  • 2 x C
  • 3 x C
  • 4 x C
  • 5 x C
A

General Formula:
CnH2n

1 x C:
Need at least 2 carbon atoms per double carbon bond (c=c)

2 x C:
Ethene, C2H4

3 x C:
Propene, C3H6

4 x C:
Butene, C4H8

5 x C:
Pentene, C5H10

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4
Q

🟠 Alcohols:

  • General Formula
  • 1 x C
  • 2 x C
  • 3 x C
  • 4 x C
  • 5 x C
A

General Formula:
CnH2n+1OH

1 x C:
Methanol, CH3OH

2 x C:
Ethanol, CH3CH2OH

3 x C:
Propanol, CH3C2H4OH

4 x C:
Butanol, CH3C3H6OH

  • 5 x C:*
  • Pentanol, CH3C4H8OH*
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5
Q

🟠 Carbolxylic Acids (n=0)

  • General Formula
  • 1 x C
  • 2 x C
  • 3 x C
  • 4 x C
  • 5 x C
A

General Formula:
CnH2n+1COOH

1 x C:
Methanoic Acid, COOH

2 x C:
Ethanoic Acid, CH3COOH

3 x C:
Propanoic Acid, C2H5COOH

4 x C:
Butanoic Acid, C3H7COOH

  • 5 x C:*
  • Pentanoic Acid, C4H9COOH*
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6
Q

🟢 Formula and Displayed Formula of Methane

A

CH4

             H     
              |       
   H  -   C   -   H   
              |      
             H
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7
Q

🟢 Formula and Displayed Formula of Ethane

A

C2H6

            H        H
             |        |
   H  -   C   -   C   -   H   
             |         |
            H        H
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8
Q

🟢 Formula and Displayed Formula of Propane

A

C3H8

        H        H       H        
         |           |          |            H  -   C   -   C   -   C   -   H   
         |            |         |        
        H        H       H
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9
Q

🟢 Formula and Displayed Formula of Butane

A

C4H10

        H        H       H        H
         |           |          |        |    H  -   C   -   C   -   C   -   C   -   H
         |            |         |        |
        H        H       H       H
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10
Q

🟢 Formula and Displayed Formula of Pentane

A

C5H12

        H        H       H        H        H
         |           |          |        |           |    H  -   C   -   C   -   C   -   C   -   C   -    H
         |            |         |        |           |
        H        H       H       H          H
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11
Q

🟠 Formula and Displayed Formula of Methene

A

Doesn’t exist

Needs at least 2 carbon atoms per double carbon bond (c=c)

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12
Q

🟠 Formula and Displayed Formula of Ethene

A

C2H4

            H        H
             |        |
            C   =   C      
             |         |
            H        H
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13
Q

🟠 Formula and Displayed Formula of Propene

A

C3H6

        H                        H
         |                           |
        C   =   C     -    C      -    H
         |           |             |
        H         H            H
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14
Q

🟠 Formula and Displayed Formula of Butene

A

C4H8

        H                      H         H
         |                        |           |
         C   =   C   -   C   -   C   -   H
         |            |          |            |
        H        H          H          H
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15
Q

🟠 Formula and Displayed Formula of Pentene

A

C5H10

        H                   H          H          H
         |                         |         |           |
         C   =   C   -   C   -   C   -   C
         |            |           |           |           |
        H        H         H          H          H
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16
Q

🟠 Formula and Displayed Formula of Methanol

A

CH3OH

            H        
             |        
   H  -   C   -   O   -   H   
             |         
            H
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17
Q

🟠 Formula and Displayed Formula of Ethanol

A

CH3CH2OH

            H        H               
             |           |          
   H  -   C   -   C   -   O   -   H   
             |            |         
            H        H
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18
Q

🟠 Formula and Displayed Formula of Propanol

A

CH3C2H4OH

        H        H       H        
         |           |          |            H  -   C   -   C   -   C   -   O   -   H
         |            |         |        
        H        H       H
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19
Q

🟠 Formula and Displayed Formula of Butanol

A

CH3C3H6OH

        H        H       H        H        
         |           |          |        |               H  -   C   -   C   -   C   -   C   -   O   -    H
         |            |         |        |           
        H        H       H       H
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20
Q

🟠 Formula and Displayed Formula of Methanoic Acid

A

COOH

      C    =    O
       |
      O   -      H
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21
Q

🟠 Formula and Displayed Formula of Ethanoic Acid

A

CH3COOH

               H
                |
H     -     C      -     C    =    O
                |               |
               H             O   -   H
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22
Q

🟠 Formula and Displayed Formula of Propanoic Acid

A

C2H5COOH

       H              H
         |              | H    -    C     -     C      -     C    =    O
         |               |               |
       H              H             O   -   H
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23
Q

🟠 Formula and Displayed Formula of Butanoic Acid

A

C3H7COOH

        H          H            H
          |            |             | H   -    C    -    C     -     C      -     C    =    O
          |            |               |               |
        H          H             H             O   -   H
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24
Q

🟠 How does the reaction of Alkenes with Halogens work (Halogenation)

A

When you test ethene with bromine water, it reacts. Ethene takes the orange colour out of the reaction mixture and leaves it colourless. The orange colour in bromine water comes from Br2 (aq) molecules, which are converted into colourless product, called dibromoethane, when they react with ethene.

Ethene + Bromine —> Dibromoethane
C2H4 + Br2 —> C2H4Br2

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25
Q

🟠 How does the reaction of Alkenes with Hydrogen work (Hydrogenation)

A

The alkenes are unsaturated compounds, because of the C=C bond, their molecules do not contain the maximum number of hydrogen atoms possible in a hydrocarbon molecule. But the addition of a hydrogen molecule, H2, across the double bond will form a saturated hydrocarbon - an alkane. The reaction takes place at 60°C in the presence of a nickel catalyst. For example:

Penatene + Hydrogen —> (catalyst) pentane
C5H10 + H2 —> C5H12

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26
Q

🟠 Alkene reaction with Hydrogen

What temperature and catalyst is used

A

The reaction takes place at 60°C in the presence of a nickel catalyst.

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27
Q

🟠 What can an Alkene reaction with hydrogen be used for (Hydration)

A

This reaction is used to add hydrogen across the C=C bonds in unsaturated oils to traighten their molecules and increase their melting points. For example, the right amount of hydrogen is added to make a marharine that can be spread easily straight from the fridge.

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28
Q

🟠 How does the reaction of Alkenes with Water (steam) work

A

Ethanol (an alcohol) for industrial use as a fuel or solvent can be made from ethene gas. Ethene is the main by-product produced in cracking. Ethene gas can react with steam to make ethanol.

Ethene + Steam ⇌ (catalyst) Ethanol
C2H4 + H2O ⇌ C2H5OH

The reaction requires energy to heat the gases and to generate a high pressure. The reaction is reversible, so ethanol can break back down into ethene and steam. So unreacted ethene and steam are recycled over the catalyst.

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29
Q

🟠 What is Ethanol used for?

A

Ethanol (an alcohol) for industrial use as a fuel or solvent can be made from ethene gas. Ethene is the main by-product produced in cracking.

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30
Q

🟠 What are the required conditions for an Akene to react with water (steam) (+how can this be recycled?)

A

The reaction requires energy to heat the gases and to generate a high pressure. The reaction is reversible, so ethanol can break back down into ethene and steam. So unreacted ethene and steam are recycled over the catalyst.

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31
Q

🟠 What are alkenes?

A

Alkenes are a homologous series of unsaturated hydrocarbons with the general formula CnH2n .

32
Q

🟠 Displayed Formula of:

Butene + Chlorine —>
C4H8 + Cl2 —>

A

. H H Cl Cl
| | | |
H - C - C - C - C - H
| | | |
H H H H

33
Q

🟠 Displayed Formula of:

Propane + Bromine —>
C3H6 + Br2 —>

A

. H Br Br
| | |
H - C - C - C - H
| | |
H H H

34
Q

🟠 Displayed Formula of:

Propene + Hydrogen (60° with nickel catalyst) —>
C3H6 + H2 —>

A

.
H H H H
| | | |
H - C - C - C - C - H
| | | |
H H H H

35
Q

🟠 Displayed Formula of:

Butene + Steam (60° with nickel catalyst) ⇌
C4H6 + H2O ⇌

A

.
H H H H
| | | |
H - C - C - C - C - O - H
| | | |
H H H H

36
Q

🟠 E.g, Ethanol

  • Molecular Formula
  • Structural Formula
  • Displayed Formula
A

Molecular Formula:

C2H6O

Structural Formula:

CH3CH2OH

Displayed Formula:

            H        H               
             |           |          
   H  -   C   -   C   -   O   -   H   
             |            |         
            H        H
37
Q

🟠 Reactions of Alcohols:

Test: pH

Instructions & Observations

A

Added equal volumes of distilled water and then used a few universal indicator solution (UI solution)

38
Q

🟠 Reactions of Alcohols:

Test: pH

Inferences/Notes/Equations

A

Methanol - Green –> Yellow (pH 5)
Ethanol - Green–> Amber (pH 4)
Propanol - Green –> Orange (pH 3)

39
Q

🟠 Reactions of Alcohols:

Test: + Na (+ Sodium)

Instructions & Observations

A

The solution starts fizzing once the sodium is added and hydrogen gas is produced
To test for hydrogen gas, you can put a lighted splint in the tube, it will produce a speaky pop sound.

40
Q

🟠 Reactions of Alcohols:

Test: + Na (+ Sodium)

Inferences/Notes/Equations

A

HCl + Na –> X (too violent)

Redox
2H2O(l) + 2Na(s) –> 2NaOH(aq) + H2(g)

41
Q

🟠 Reactions of Alcohols:

Test: Combustion

Instructions & Observations

A

The alcohols are set alight. They all burn readily and cleanly (there is no soot in the flame) and are very flammable.

42
Q

🟠 Reactions of Alcohols:

Test: Combustion

Inferences/Notes/Equation

A

CH3OH + 1.5O2 –> CO2+ 2H2O
C2H5OH + 3O2 –> 2CO2 + 3H2O
C3H7OH + 4.5O2 –> 3CO2 + 4H2O

43
Q

🟠 Reactions of Alcohols:

Test: Oxidisation

Instructions & Observations

A

Add acidified potassium dichromate (oxidising agent)

Potassium dichromate (an orange) solution, turns green when adding it to ethanol

(Don’t need to remember, but do need to recognise)

44
Q

🟠 Reactions of Alcohols:

Test: Combustion

Inferences/Notes/Equations

A

Potassium Dichromate used
Colour goes fro Orange –> Green
It has been reduced

E.g, Ethanol + Oxidising Agent —> Ethanoic Acid + H2O

            H        H               
             |           |          
   H  -   C   -   C   -   O   -   H   + 2 [O] ---> 
             |            |         
            H        H
               H
                |
H     -     C      -     C    =    O   + H2O
                |               |
               H             O   -   H
45
Q

🟠 How are Alcohols used in Solvents

A

It is soluble in water and organic compounds, making it a good solvent as a result.

46
Q

🟠 How are Alcohols used in Fuels

A

Alcohol (ethanol and sometimes methanol) is flammable and burns with a clean flame. It can be used as a biofuel in cars, and it burns with a ‘clean’ blue flame. (It is renewavle through making ethanol through fermentation, making it a biofuel.)

47
Q

🟠 How are Alcohols used in Alcoholic Beverages

A

Ethanol (the main ingredient in acloholic drinks) is made by fermenting sugars from plant material with yeast

48
Q

🟠 What are Esters

A

Esters are closely related groups to carboxylic acids. If you replace the H atom in the -COOH group by a hydrocarbon (alkyl) group, such as -CH3 or - C2H3, you get an ester.

49
Q

🟠 Displayed Formula of an Ester

e.g Ethyl Ethanoate

A

CH3COOCH2CH3 (or shortened to CH3COOC2H5)
|
H - C - C = O
| |
H | H H
| | |
O - C - C - H
| |
H H

50
Q

🟠 What does an Ester’s structural formula contain (what is it) (e.g Ethyl Ethanoate)

A

An ester’s structural formula always contains the -COO- functional group. The structural for ula of ethyl ethanoate is CH3COOCH2CH3 (or shortened to CH3COOC2H5).

51
Q

🟠 How are Alcohols similar to water and how are they good Solvents

A

Alcohols dissolve many of the same substances as water. In fact, the alcohols with snaller molecules mix very well with water, giving neutralnsolutions. The alcohols can also dissolve many ither organic compounds. This property makes them useful as solvents.

For example, you can remove ink stains from permanent marker pens using methylated spirits

52
Q

🟠 What two ways is Ethanol made and what is Ethanol’s main uses

A

Alcohols, especially ethanol are commony used in everyday products. Ethanol is the main alcohol in alcoholic drinks. It is made by fermenting siga4s from plant material with yeast and is becoming an important alternative fuel to peterol and diesel. Ethanol made by fermentation is term a biofuel.

However, ethanol is also made from reacting ethene (obtained by cracking heavy fractions from crude oil) and steam in the prescence of a catalyst. This method uses up some of the diminishing supplies of crude oil, a non-renewable resource.

53
Q

🟠 What are Methylated Spirits made up of

A

Methylated spirits (‘meths’) is mainly ethanol, but as more toxic methanol mixed with it. It also has a purple dye and other substances added to make it unpleaseny to drink. Alcohols are also used as solvents in products such as perfumes, aftershaves, and mouthwashes.

54
Q

🟠 What does the Combustion of Alcohols show, and what is it used for

A

The use of ethanol (and also methanol) as fuels shows that the alcohols are flammable. Ethanol is used in spirit burners, and can be used as a biofuel in cars. It burns with a ‘clean’ blue flame.

55
Q

🟠 Combustion of Alcohols Equation (Word and Symbol)

A

It burns a ‘clean’ blue flame, according to the reaction in the following equation:

Ethanol + Oxygen –> Carbon Dioxide + Water
C2H5OH + 3O2 –> 2CO2 + 3H2O

56
Q

🟠 Description of the reaction of Alcohols with Sodium and what is produced

A

The alcohols react in a similar way to water when sodium metal is added. For example, woth ethanol, the sodium effervesces (gives iff bubbles of gas), producing hydrogen gas, and gets smaller and smaller as it forms a solution of sodium ethoxide in the ethanol. Their reactions are not as vigorous as the reaction you observe between sodium and water.

57
Q

🟠 Example of Alcohols reacting with sodium (Word and Symbol equation

(You don’t need to know the balanced symbol equation by heart)) for Ethanol

A

For example, with ethanol, the word equation is:

Sodium + Ethanol –> Sodium Ethoxide + Hydrogen

2Na + 2C2H5OH –> 2C2H5ONa + H2

(The balanced symbol equation doesn’t need to be memorised.) If sodium ethoxide, or any other sodium alkoxide, is dissolved in water, you get a strongly alkaline solution.

58
Q

🟠 How does the Oxidisation of Alcohols work (+ what happens)

A

Conbustion js one way to oxidise an alcohol. However, when you use chemical oxidising agents, such potassium dichromate (VI), you get different products. An alcohol is oxidised to a carboxylic acid when boiled with acidified potassium dichromate (VI) solution. So ethanol can be oxidised to ethanoic acid.

The same reaction takes place of ethanol is left exposed to air. Microbes in the air produce ethanoic acid from the ethanol. This is why bottles of beer or wine taste and smell like vinegar when they are left out for too long.

59
Q

🟠 Example of Alcohols being Oxidised (Word and Symbol equation

(You don’t need to know the balanced symbol equation by heart)) for Ethanol

A

Ethanol + Oxygen atoms from oxidising agent –> Ethanoic Acid + Water

C2H5OH + 2[O] –> CH3COOH + H2O

(You do not need to onow a balanced symbol equation for this reaction by heart.)

60
Q

🟠 What are Carboxylic acids, what solutions do they form when dissolved in water, and what reactions od they have

A

Carboxylic acids, as their name suggests, form acidic solutions when they dissolve in wayer.

Carboxylic acids have the typical reactions of all acids. For example, reaction with a metal carbonate forms a salt, water, and carbon diozide.

61
Q

🟠 Word Equation for (Carboxylic Acids)

Ethanoic Acid + Sodium Carbonate –>

A

Ethanoic Acid + Sodium Carbonate –> Sodium Ethanoate + Water + Carbon Dioxide

(2CH3COOH (aq) + Na2CO3 (s) –> 2CH3COONa (aq) + H2O (l) + CO2 (g))

(You don’t need to know the balanced symbol equation by heart)

62
Q

🟠 What gas is produced when magnesium reacts with ethanoic acid?

A

Hydrogen Gas

63
Q

🟠 Complete the word equation for the reaction:

Ethanoic Acid + Magnesium –>

A

Ethanoic Acid + Magnesium –> Magnesium Ethanoate + Hydrogen

64
Q

🟠 What gas is produced when potassium carbonate reacts with ethanoic acid?

A

Carbon Dioxide

65
Q

🟠 Complete the word equation for the reaction:

Ethanoic Acid + Potassium Carbonate –>

A

Ethanoic Acid + Potassium Carbonate –> Potassium Ethanoate + Water + Carbon Dioxide

66
Q

🟢 What does the conductivity experiment tell you? (Ethanoic Acid + Potassium Carbonate)

A

The ethanoic acid should conduct, as there are charge ions which are free to move.

67
Q

🟢 Ethanoic acid is described as a weak acid. Explain what this means in terms of ionisation.

A

This means that only some hydrogen ions fully ionise when dissoliving in water.

68
Q

🟠 What is the Chemical Reversible Reaction for Ethanoic Acid (involving ethanoate ions and hydrogen ions)

A

CH3COOH(aq) ⇌ CH3COO^- (aq) + H+ (aq)

Ethanoic acid ⇌ Ethanoate ions + Hydrogen ions

69
Q

🟢 Explain why the pH of 0.1 mol/dm3 hydrochloric acid is lower than the pH of 0.1 mol/dm3 ethanoic acid.

A

Because hydrochloric acid is a stronger acid, it fully ionises when added to water so more hydrogen ions are present. This higher concentration of hydrogen ions results in the pH if the hydrochloric acid being lower.

70
Q

🟢 Explain why 0.1 mol/dm3 hydrochloric acid reacts faster with magnesium than 0.1 mol/dm3 ethanoic acid.

A

Because hydrochloric acid is a stronger acid, it fully ionises when added to water so more hydrogen ions are present. This higher concentration of hydrogen ions results in a faster rate of reaction.

71
Q

🟠 What two things react to make esters and what is also formed in what type of reaction, and what type of catalyst is used

A

Carboxylic acids also react with alcohols to make esters. Water is also formed in this reversible reaction. An acid, usually sulphuric acid, is used as a catalyst.

72
Q

🟠 Characteristics of Esters and what are they used for

A

The esters for ed have distinctive smells. They are volatile (evaporate easily). Many smell sweet and fruity. This makes them ideal to use in perfumes and food flavourings.

73
Q

🟠 General Word Equation to make an Ester

A

In general:

Carboxylic Acid + Alcohol (acid catalyst) ⇌ (acid catalyst) Ester + Water

74
Q

🟠 Complete the equation (word and chemical)

Ethanoic Acid + Ethanol ⇌

A

Ethanoic Acid + Ethanol ⇌ Ethyl Ethanoate + Water

CH3COOH + C2H5OH ⇌ CH3COOC2H5 + H2O

75
Q

🟠 Displayed Formula for the Reaction of:

Ethanoic Acid + Ethanol (sulphuric acid catalyst) ⇌ (sulphuric acid catalyst) Ethyl Ethanoate + Water

A 
.
               H
                |
H     -     C      -     C    =    O   
                |               |
               H             O   -   H
                      \+
            H        H               
             |           |          
   H  -   C   -   C   -   O   -   H   
             |            |         
            H         H

(sulphuric acid catalyst) ⇌ (sulphuric acid catalyst)

        H        O                   H        H
         |           ||                   |             |    H  -   C   -   C   -   O   -   C   -   C   -   H
         |                                 |             |
        H                              H        H

              \+

       H2O
76
Q

🟠 Esters occur naturally in a number of different fruits. Find out the name of the ester present in the following fruits:

  • Strawberries
  • Pears
  • Bannanas
A

Strawberries:
Methyl Butanoate

Pears:
Ethyl Decadienoate

Banannas:
3-Methylbutyl Ethanoate

(GCSE) Chemistry (24 decks)

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