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Chemistry > 10. Organic Chemistry > Flashcards

10. Organic Chemistry Flashcards

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1
Q

What is catenation?

A

The joining of many identical atoms to form chains and rings.

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2
Q

What are the 3 advantages of Lewis structures?

A
  • Location of bonding and non-bonding electrons is shown.
  • Shows how atoms are arranged relative to each other.
  • Allows the application of VSEPR theory to predict the molecular shape and bond angles.
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3
Q

What are the 3 disadvantages of Lewis structures?

A
  • Takes a long time to draw the full structure.
  • Does not show the proportional atomic radii or bond lengths.
  • Assumes that atoms are spherical, and that bonding electrons lie halfway between two nuclei.
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4
Q

What is the stereochemical formula?

A

A 3D representation of how atoms are arranged in space.

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5
Q

Define ‘homologous series’.

A

A family of compounds grouped based on similarities.

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6
Q

List the 4 features of a homologous series.

A
  • The same general formula.
  • Similar chemical properties.
  • A graduated trend in physical properties.
  • Members of the family vary by CH2 units.
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7
Q

Define ‘hydrocarbon’.

A

A compound that contains carbon and hydrogen atoms only.

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8
Q

What is the general formula of the alkanes?

A

CnH2n+2

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9
Q

Are alkanes saturated or unsaturated? Why?

A

Saturated as they only contain single carbon to carbon bonds.

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10
Q

Describe how to name a compound using IUPAC nomenclature.

A
  • Prefix= the locants of hydrocarbon branches.
  • Stem= the longest unbranched carbon chain.
  • Suffix= main functional group.
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11
Q

What type of intermolecular force forms between alkanes?

A

London dispersion forces.

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12
Q

What is the relationship between carbon chain length of alkanes and boiling point?

A
  • As the length increases, so does boiling point. This is because, in longer carbon chains, the strength of London dispersion forces increases as there are more electrons, which requires more energy to break.
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13
Q

What happens to the rate of boiling point increase as the chain gets longer? Why?

A
  • The rate decreases. This is because there is a reduced percentage mass for each successive CH2 added.
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14
Q

Why are alkanes relatively inert?

A
  • Their carbon-carbon bonds require a lot of energy to break.
  • They are non-polar.
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15
Q

Define ‘homolytic fission’.

A

One electron from the pair of electrons goes to each of the products.

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16
Q

What mechanism allows halogenation of an alkane?

A

Free radical substitution.

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17
Q

What is required to initiate free radical substitution?

A

UV light.

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18
Q

What are the three steps of free radical substitution called?

A
  1. Initiation
  2. Propagation
  3. Termination
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19
Q

What does a fish hook arrow represent?

A

The movement of a single electron.

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20
Q

What does a double-barbed arrow represent?

A

A pair of electrons moving.

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21
Q

What is the general formula of a halogenoalkane?

A

CnH2n+1X

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22
Q

What is a positional isomer?

A

Two molecules with the same general formula but the functional group in a different place.

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23
Q

What is a chain isomer?

A

When the carbon chain changes length.

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24
Q

What is a primary halogenoalkane?

A

The functional group is attached to a carbon atom that is bonded to 2 hydrogen atoms.

25
Q

What is a secondary halogenoalkane?

A

The functional group is attached to a carbon atom that is also bonded to 1 hydrogen atom.

26
Q

What is a tertiary halogenoalkane?

A

The functional group is attached to a carbon atom that is bonded to 0 hydrogen atoms.

27
Q

Why are halogenoalkanes polar?

A
  • The halogen has a greater electronegativity than carbon, polarising the Carbon-halogen bond.
  • The molecule is asymmetrical.
28
Q

Why do halogenoalkanes undergo substitution reactions?

A

They are saturated.

29
Q

Define ‘nucleophile’.

A
  • An electron-rich species that will donate a pair of electrons to an electron-deficient atom.
  • Contains a lone pair of electrons.
30
Q

Define ‘heterolytic fission’.

A

Both electrons from the pair go to only one of the products.

31
Q

Define nucleophilic substitution.

A

When the nucleophile takes the place of a halogen.

32
Q

What mechanism do halogenoalkanes undergo?

A

Nucleophilic substitution.

33
Q

Why do alcohols have higher boiling points than ethers?

A
  • Alcohols have London forces and hydrogen bonding.
  • Some ethers do not have dipole-dipole forces as they are symmetrical.
34
Q

What is formed: carboxyl + oxidising agent —> ?

A

Aldehyde

35
Q

Does distillation achieve partial or full oxidation? Why?

A
  • Partial oxidation.
  • The aldehyde is removed (vaporised) before being fully oxidised.
36
Q

Does reflux achieve partial or full oxidation? Why?

A
  • Full oxidation.
  • The condenser cools the aldehyde, condensing it and returning it to the oxidising mixture for full oxidation.
37
Q

Using distillation, primary alcohol + oxidising agent —> ?

A

Aldehyde

38
Q

Using reflux, primary alcohol + oxidising agent —> ?

A

Carboxyl

39
Q

Using reflux, secondary alcohol + oxidising agent —> ?

A

Ketone

40
Q

What is needed to reduce an alkyne to an alkene?

A

Hydrogen gas and a catalyst.

41
Q

What is required to reduce an alkene to an alkane?

A

Hydrogen gas and a transition metal catalyst.

42
Q

What is required to convert an alkyne directly to an alkane?

A

Excess hydrogen gas and a transition metal catalyst.

43
Q

What type of mechanism do Alkenes undergo?

A

Electrophilic addition.

44
Q

Define ‘electrophile’.

A

An electron deficient species that will accept a pair of electrons.

45
Q

What is the test for unsaturation?

A

The decolorisation of bromine water.

46
Q

Is the sigma or pi bond stronger?

A

Sigma

47
Q

Describe a sigma bond.

A

The head on overlap of orbitals.

48
Q

Describe a pi bond.

A

The sideways overlap of p-orbitals.

49
Q

Define ‘isomer’.

A

Molecules with the same molecular formulae but different structural formulae.

50
Q

Describe the 3 features of a stereoisomer.

A
  • Involves a different spatial arrangement of atoms in the molecule.
  • Sigma bonds rotate freely.
  • Pi bonds have restricted rotation, which is the source of isomers.
51
Q

What is required for CIS/ TRANS isomerism?

A
  • Each carbon of the C=C must have 2 different groups attached.
  • The locked pi bonds must be broken.
  • Both carbon atoms in the C=C must have the same group attached.
52
Q

What is a CIS isomer?

A

They have the same groups on the same side of the double bond.

53
Q

What is a TRANS isomer?

A

They have the same groups on opposite sides of the double bond.

54
Q

Describe the features of optical isomers.

A
  • Require a carbon (or silicon/ geranium) molecule with four different groups attached.
  • They are non-superimposable.
55
Q

What is the carbon centre of an optical isomer called?

A

Chiral centre

56
Q

Define ‘enantiomers’.

A
  • Opposite chirality at each chiral centre.
  • Two non-superimposable mirror images.
57
Q

Define ‘diastereomer’.

A
  • Opposite chirality at some chiral centres.
  • Molecules whose chiral centres are not all reflected.
  • Diastereomers are not mirror images.
58
Q

What is an enantiopure mixture?

A

A mixture that only contains one optical isomer.

59
Q

What is a racemic mixture?

A

A mixture of different optical isomers.

Chemistry (10 decks)

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