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Chemistry > 13 (everything in organic until alkanes) > Flashcards

13 (everything in organic until alkanes) Flashcards

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1
Q

Hydrocarbon

A

a compound made up of C and H atoms only

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2
Q

Functional group

A

an atom or group of atoms which determines the physical and chemical properties of the molecule

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3
Q

Homologous series

A
  • organic compounds with the same functional group, but with each successive member differ by CH2
  • same general formula
  • same chemical properties
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4
Q

Alkanes

A

simple hydrocarbons with no functional group

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5
Q

Trend of alkanes

A

B.p increases
- more C and H bonds
- more id-id forces
- more energy/higher temp is needed to break bonds

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6
Q

Aliphatic compound

A

straight or unbranched-chain and also includes cyclic organic compounds that do not contain a benzene ring

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7
Q

Molecular formula

A

shows the number and type of each atom in a molecule
- ethanoic acid would be C2H4O2

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8
Q

Empirical formula

A

shows the simplest whole number ratio of the elements present in one molecule of the compound
- ethanol would be CH2O

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9
Q

Saturated hydrocarbons

A

contain single bonds

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10
Q

Unsaturated hydrocarbons

A

carbon-carbon double or triple bonds

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11
Q

Homolytic fission

A

breaking a covalent bond in such a way that each atom takes an electron from the bond to form 2 radicals

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12
Q

Heterolytic fission

A

breaking a covalent bond in such a way that the more electronegative atom takes both the electrons from the bond to form a negative ion and leaves behind a positive ion

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13
Q

Free radical

A

a species with one or more unpaired electrons

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14
Q

Example of a free radical reaction (initiation, propagation and termination)

A

in notes

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15
Q

Nucleophile

A

electron-rich species that can donate a pair of electrons

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16
Q

Electrophile

A

electron-deficient species that can accept a pair of electrons

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17
Q

Addition

A
  • organic reaction in which 2 or more molecules combine
  • give a single product
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18
Q

Substitution

A
  • involves replacing an atom or group of atoms with another
19
Q

Elimination

A

small molecule (such as H2O) is removed from an organic molecule

20
Q

Hydrolysis

A

a compound is broken down by water (can also refer to the breakdown of a substance by dilute acids or alkalis)

21
Q

Condensation

A

2 organic molecules join together and in the process eliminate a small molecule (such as H2O or HCI)

22
Q

Oxidation

A
  • oxygen is added
  • oxidation number increases
  • electrons are removed
  • H is removed
  • [O] one atom of oxygen from an oxidizing agent
23
Q

Reduction

A
  • oxygen is removed
  • oxidation number decreases
  • electrons are added
  • H is added
  • [H] one atom or hydrogen from a reducing agent
24
Q

Mechanisms (free-radical substitution, electrophilic addition, nucleophilic substitution, and nucleophilic addition

A

in notes

25
Q

Examples of straight-chain, branched, and cyclic molecules

A

in notes

26
Q

Hybridisation: sp3
(single bonds)

A
  • carbon atoms that form 4 sigma bonds
  • each carbon atom forms 4 sigma bonds to adopt a tetrahedral configuration (109.5)
  • minimises repulsion between the bonding pair of electrons

Example: ethane

27
Q

Hybridisation: sp2
(1 double bond)

A
  • when carbon atoms use only 3 of their electron pairs to form a sigma bond
  • the overlap of the 2 p orbitals results in the formation of a pi bond
  • the 3 bonding pairs of electrons repel each other to force the molecule into a planar configuration (120)

Example: ethene

28
Q

Hybridisation: sp
(1 triple bond)

A
  • carbon atoms can also use only 1 of their electron pair to form a sigma bond
  • the overlap of the p orbitals results in the formation of 2 pi bonds
  • which adopts a linear arrangement (180)

Example: ethyne

29
Q

Double bond and triple bond

A

Double
- a combination of a sigma and pi bond

Triple
- a combination of 1 sigma and 2 pi bonds

30
Q

Strength of bonds

A

single < double < triple
- due to increased electron density around the C-C atom, making the bond stronger and more difficult to break

31
Q

Sigma bond

A
  • formed from the end-on overlap of atomic orbitals
  • electron density is symmetrical
32
Q

Pi bonds

A
  • formed from the sideways overlap of p orbitals
  • the 2 lobes that make up the pi bond lie above and below the plane of the atoms which maximises the overlap of the p orbitals
  • in triple bonds there is an additional overlap of p orbitals, the 2 lobes lie in front and behind the plane which maximises the overlap of the p orbitals
33
Q

Planar molecules

A

Linear- 180
Non-linear- 104.5
Trigonal planar- 120
Square planar- 90

34
Q

Structural isomers

A
  • compounds that have the same molecular formula but different structural formulae

3 different types:
- chain
- positional
- functional group

35
Q

Chain isomerism

A

when compounds have the same molecular formula, but their longest hydrocarbon chain is not the same
- caused by branching

Example- pentane and 2,2-dimethyl propane

36
Q

Positional isomerism

A
  • arise from differences in the position of a functional group in each isomer

Example- butan-1-ol and 2-butanol

37
Q

Functional group isomerism

A
  • when different functional groups result in the same molecular formula, functional group isomers arise
  • the isomers have very different chemical properties as they have different functional groups

Example- butan-1-ol and ethoxyethane

38
Q

Functional group isomer groupings

A
  • aldehydes and ketones
  • esters and carboxylic acids
  • alkenes and cycloalkanes
39
Q

Stereoisomers

A
  • compounds that have the same atoms connected to each other, however the atoms are differently arranged in space

2 types:
- geometrical (cis/trans) isomerism
- optical isomerism

40
Q

Geometrical isomerism

A
  • seen in unsaturated (double bond containing) or ring compounds that have the same molecular formula and order of atoms but different shapes

Cis- have functional groups on the same side of the double bond/carbon ring

Trans- have functional groups on opposite sides of the double bond/carbon ring

  • causes the compounds to have different chemical and physical properties (reaction rates or m.p and b.p points)
41
Q

Optical isomerism

A
  • arise when a carbon atom in a molecule is bonded to 4 different atoms or groups of atoms (chiral centre)
  • the carbon atom is asymmetric
  • chiral centre gives rise to 2 enantiomers which are mirror images of each other and are non-superimposable (dont match)
  • differ in their ability to rotate the plane of polarised light
42
Q

Unsaturated compounds and geometrical isomerism

A
  • in unsaturated compounds, the groups attached to the C=C carbons remain fixed in their position
  • this is because free rotation of the bonds about the C=C bond is not possible due to the presence of a pi bond
43
Q

Chiral centre

A
  • a carbon atom that has 4 different atoms or groups of atoms attached
  • gives rise to 2 optical isomers (enantiomers)
  • the enantiomers are mirror images of each other and cannot be superimposed
  • each chiral centre gives rise to 2 optical isomers, therefore the molecule has a total of 4 optical isomers
44
Q

The maximum number of stereoisomers that a molecule can have is

A

2 to the power of n

Chemistry (19 decks)

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