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Chemistry > S5 - Unit 2 > Flashcards

S5 - Unit 2 Flashcards

1
Q

How can alcohols be classified?

A

Depending on how many carbons are attached to a hydroxyl group

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2
Q

What name is given to an alcohol with 1 carbon attached to the hydroxyl group?

A

Primary

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3
Q

What name is given to an alcohol with 2 carbons attached to the hydroxyl group?

A

Secondary

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4
Q

What name is given to an alcohol with 3 carbons attached to the hydroxyl group?

A

Tertiary

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5
Q

What name is given to alcohols with more than one hydroxyl group?

A

Polyhydric alcohol

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6
Q

How can alcohols be oxidised?

A

By adding oxygen or removing hydrogen

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7
Q

How many steps can primary alcohols undergo in oxidation?
What happens in each step?
What is the product of each step?

A
  • 2
  • Removal of hydrogen and addition of
    oxygen between carbon and hydrogen
  • Alcohol ~> aldehyde
    Aldehyde ~> acid
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8
Q

How many steps can secondary alcohols undergo in oxidation?
What happens in each step?
What is the product of each step?

A
  • 1
  • Removal of hydrogen
  • Alcohol ~> ketone
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9
Q

How many steps can tertiary alcohols undergo in oxidation?
What happens in each step?
What is the product of each step?

A
  • 0
  • N/A
  • N/A
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10
Q

How to aldehydes and ketones differ?

A

Aldehydes have the function group (carbonyl) always attached to the first carbon whereas in ketones the functional group (carbonyl) is attached to two other carbons

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11
Q

What is the general formula for alkanals?

A

CnH2nO

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12
Q

What is the general formula for alkanones?

A

CnH2nO

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13
Q

What are the oxidising agents learned about?

A
  • Acidified potassium dichromate solution
  • Fehling’s solution
  • Tollen’s reagent
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14
Q

What are the observations made with each of the oxidising agents?

A

A.P.D.S = orange ~> green
F.S = Blue ~> orange
T.R = Colourless ~> silver

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15
Q

What is the corresponding salt name for each carboxylic acid?

A

Methanoate
Ethanoate
Propanoate
Butanoate
Pentanoate

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16
Q

What is the formula for a salt produced by a carboxylic acid and a metal?

A

CnH2n+1COO-__+

(__ = metal)

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17
Q

How are esters produced?

A

By carboxylic acids undergoing condensation reactions with alcohols

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18
Q

What is a condensation reaction?

A

When two molecules join together, usually in the presence of a catalyst, with the elimination of water or another simple molecule

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19
Q

How do you name esters?

A

Alcohols name + carboxylic acid salt name

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20
Q

What is the catalyst in a condensation and hydrolysis reaction?

A

Concentrated sulphuric acid

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21
Q

What is the role of a wet paper towel when making esters?

A

Acts as a condenser

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22
Q

Why is something used to cover the top of the test tube when making esters?

A

To contain any chemicals that may spurt out

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23
Q

What is used to neutralise any remaining acid in the ester once it has been formed?

A

Sodium hydrocarbonate

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24
Q

What properties do esters have?

A
  • Usually have sweet smells
  • More volatile than carboxylic acids
  • Insoluble in water
  • Much less polar than carboxylic acids
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25
Q

What are come uses of esters?

A

-Used as flavourings
- Used in perfumes
- Used as solvents

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26
Q

What is the functional group for aldehydes?

A

Carbonyl

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27
Q

What is the functional group for ketones?

A

Carbonyl

28
Q

What does the carbonyl functional group structure look like?

A

.
|
—-C=O
|

29
Q

What is hydrolysis?

A

The opposite of condensation - when water is added to break up the molecule

30
Q

What is the homologous series for the alkanones?

A

Ketones

31
Q

What is the homologous series for the alkanals?

A

Aldehydes

32
Q

What is the equation for carboxylic acids reacting with a metal?

A

Acid + metal ~> salt + hydrogen

33
Q

What else is produced when an ester formed?

A

Water

34
Q

What are diatomic elements?

A

Two atoms joined together by a shared pair of electrons

35
Q

What are discrete molecules?

A

Small groups of atoms held together by strong covalent bonds inside the molecule and weak intermolecular forces between the molecule

36
Q

What elements are most commonly discrete?

A

The diatomic elements

37
Q

What are the only elements that can form covalent networks?

A

Carbon (in the form of diamond or graphite), boron and silicon

38
Q

What are monatomic elements and what are examples?

A

Single, unattached atoms.
Elements in group 8 (they have a full outer shell of electrons

39
Q

What happens when monatomic elements are cooled?

A

The atoms move closer and are held by week LDF’s

40
Q

What are London Dispersion Forces?

A

Weak, short lived bonds between atoms and molecules

41
Q

How do LDF’s occur?

A

Due to the positioning of the electrons in the outer shell

42
Q

What happens if the electrons are unevenly distributed in the shells?

A

It can cause a temporary dipole allowing the atoms to be attracted to each other

43
Q

What happens to the m.p and the b.p as you go down group 1 and why?

A

They decrease as the atoms become less tightly held together.

44
Q

What can cause metallic bonds to get weaker?

A

If the delocalised electrons move further away from the nuclei of the positive ions

45
Q

What happens to the m.p and b.p as you go down group 7 and why?

A

They increase as the forces of attraction between the molecules increases with atomic number

46
Q

What does an increased number in electrons mean?

A

An increase in the number of shells and therefore greater LDF’s

47
Q

What are polar covalent bonds?

A

When atoms with different electronegativities form covalent bonds

48
Q

What are non-polar covalent bonds?

A

When atoms of the same electronegativities form covalent bonds

49
Q

Which element (the one with less electronegativity or the one with greater) will have a slightly negative charge?

A

The element with a greater electronegativity

50
Q

Which element (the one with less electronegativity or the one with greater) will have a slightly positive charge?

A

The element with a smaller electronegativity

51
Q

Ionic bonds have … electronegativites.
- Very high
- High
- Low
- No

A

High

52
Q

Covalent bonds have … electronegativites.
- Very high
- High
- Low
- No

A

No

53
Q

Polar covalent bonds have … electronegativites.
- Very high
- High
- Low
- No

A

Low

54
Q

What are intramolecular forces?

A

Forces that hold the atoms within a molecule together

55
Q

What are intermolecular forces?

A

Forces that exist between molecules

56
Q

What are the three van der Waal’s forces?

A
  • LDF’s
  • Permanent dipole - permanent dipole (pd. pd.)
  • Hydrogen
57
Q

What do pd. pd forces occur between?

A

Atoms in compounds with different electronegativities

58
Q

When does hydrogen bonding occur in compounds?

A

When N/O/F is linked to hydrogen

59
Q

Why do some compounds containing hydrogen have higher boiling points than expected?

A

Because hydrogen bonding holds the molecules together more tightly than other van der Waal forces

60
Q

What is viscosity directly proportional to?

A

The gfm of a molecule

61
Q

What else, other than a high gfm, might cause a substance to be viscous?

A

Hydroxyl groups

62
Q

What happens to the viscosity of a substance as the number of hydroxyl groups are increased?

A

It increases

63
Q

What will dissolve polar and ionic substances?

A

Polar covalent molecules

64
Q

What will dissolve non-polar substances?

A

A non-polar solvent

65
Q

What does miscible mean?

A

Soluble

66
Q

What does immiscible mean?

A

Insoluble

67
Q

What does hydrogen bonding do the the miscibility of a substance?

A

Increases it

Chemistry (9 decks)

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