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IB chemistry > topic 10/20 > Flashcards

topic 10/20 Flashcards

1
Q

define a homologous series

A

a series of compounds of the same family, with the same general formula, which differ from each other by a common structural unit (CH2, methylene group)

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2
Q

explain the trend in boiling points and density of members of homologous series

A

boiling point/density increases as length of carbon chain increases:
- molecular mass increases/no of C atoms increases
- London forces increase as the molecules get bigger

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3
Q

describe and explain the trend in solubility of members of a homologous series

A

less soluble as homologous series is ascended:
hydrocarbon chain is non-polar (hydrophobic) and as no of carbons increase, this increases the percentage of the molecule that is unattractive to water.

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4
Q

what does the solubility of a compound in water depend on?

A

solubility in water depends on the ability of the water molecules to attract dipoles in the organic compound.

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5
Q

describe physical and chemical properties of homologous series

A
  • physical properties change gradually as the length of the carbon chain increases
  • similar chemical properties
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6
Q

general formula of alkanes

A

CnH2n+2

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7
Q

general formula for alkenes

A

CnH2n

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8
Q

general formula for alkynes

A

CnH2n-2

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9
Q

general formula for ketones

A

CnH2nO

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10
Q

general formula for alcohols

A

CnH2n+1OH

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11
Q

general formula for aldehydes

A

CnH2n+2

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12
Q

general formula for carboxylic acids

A

CnH2n+1COOH

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13
Q

define an empirical formula

A

the simplest ratio of the atoms within a molecule of the compound

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14
Q

define the molecular formula

A

shows the actual number of atoms of each type in the molecule

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15
Q

define the structural formula

A

shows the actual arrangement of the atoms in a molecule by drawing the bonds as lines between letters representing the atoms

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16
Q

define a skeletal formula

A

each carbon is represented by an angle, or termination in a line and the hydrogen atoms are just assumed

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17
Q

state the two ways that structural formulae can be represented.

A
  • full format
  • condensed format
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18
Q

describe alkanes as a class of organic compounds

A

saturated hydrocarbons

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19
Q

describe alkenes as a class of organic compounds

A

unsaturated hydrocarbons- carbon and hydrogen atoms with one or more carbon-carbon double bond in their chemical structure

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20
Q

describe alkynes as a class of organic compounds

A

organic molecules made of the functional group carbon-carbon triple bonds

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21
Q

describe halogenoalkanes as a class of organic compounds

A

organic compounds that contain one or more halogen atom (chlorine, bromine, fluorine, or iodine) attached to a carbon atom in an alkane molecule
- RX, where R=alkyl group, H= halogen

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22
Q

describe alcohols as a class of organic compounds

A

one or more hydroxyl (―OH) groups attached to a carbon atom of an alkyl group (hydrocarbon chain).

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23
Q

describe ethers as a class of organic compounds

A

characterized by an oxygen atom bonded to two alkyl or aryl groups
R−O−R′

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24
Q

describe aldehydes as a class of organic compounds

A

a carbon atom shares a double bond with an oxygen atom, a single bond with a hydrogen atom, and a single bond with another atom or group of atoms
R−CH=O

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25
Q

describe ketones as a class of organic compounds

A

R−C(=O)−R’

26
Q

describe esters as a class of organic compounds

A

any of a class of organic compounds that react with water to produce alcohols and organic or inorganic acids
R-C(=O)-O

27
Q

describe carboxylic acids as a class of organic compounds

A

any of a class of organic compounds in which a carbon atom is double bonded to an oxygen atom and to a hydroxyl group (―OH) by a single bond
R−COOH

28
Q

describe amines as a class of organic compounds

A

organic compounds that contain nitrogen atoms with a lone pair
R-CO- NH2

29
Q

describe amides as a class of organic compounds

A

R(CO)NR2

30
Q

describe nitriles as a class of organic compounds

A

any of a class of organic compounds having molecular structures in which a cyano group (―C ≡ N) is attached to a carbon atom (C)
R-C[triple]N

31
Q

describe arenas as a class of organic compounds

A

aromatic hydrocarbons- implies a particular sort of delocalized bonding
CnH2n−6

32
Q

define functional groups

A

a group of atoms that determines a molecule’s reactivity

33
Q

describe phenyl as a functional group

A

a benzene ring, minus a hydrogen

34
Q

describe hydroxyl as a functional group

A
  • OH
35
Q

describe carbonyl as a functional group

A

[C=O]

36
Q

describe carboxyl as a functional group

A

−COOH

37
Q

Describe a carboxamide as a functional group

A

-CO-NH2

38
Q

Describe aldehydes as a functional group

A

−CH=O

39
Q

Esters as a functional group

A

-COO-

40
Q

Ethers as a functional group

A

R−O−R

41
Q

Amines as a functional group

A

-NH2

42
Q

Nitrile as a functional group

A

−C≡N

43
Q

Alkyl functional group

A

−C≡N

44
Q

Alkyl as a functional group

A

formed by removing a hydrogen atom from the molecule of alkane.

45
Q

Alkenyl group

A

Hydrocarbon group formed when a hydrogen atom is removed from an alkene group

46
Q

Alkynyl group

A

Obtained by the removal of one hydrogen atom that is linked to a triply bonded carbon atom

47
Q

Define structural isomers

A

Compounds with the same molecular formula but different arrangement of atoms

48
Q

Define stereoisomers

A

Have the same structural formula but differ in their spatial arrangement

49
Q

Describe the different types of stereoisomerism

A
  • Stereoisomerism:
    Configurations isomerism (cis/trans E/Z, optical isomerism), conformational isomerism
  • Structural isomerism:
    Positional isomers, functional group isomers, chain isomerism
50
Q

Describe the difference between conformational isomers and configurational isomers

A

Conformational: can interconvert by rotation about a sigma bond
Configurational: can only interconvert by breaking and reforming a bond

51
Q

why do alkanes only undergo free radical substitution?

A

they have a low reactivity due to the:
- strength of the C-C and C-H bonds
- lack of polarity

52
Q

incomplete combustion of alkanes

A

C, CO, H2O

53
Q

complete combustion of alkanes

A

CO2, H2O

54
Q

combustion of alkanes is …

A

highly exothermic

55
Q

describe heterolytic fission

A

results in the formation of a positive and negative ion

56
Q

describe homolytic fission

A

results in the formation of two radicals

57
Q

what condition is necessary for free radical substitution?

A

UV light

58
Q

define free radical substitution

A

a type of substitution reaction where a radical replaces a different atom or group of atoms

59
Q

what bonds can UV light break/not break?

A

it can break bonds between halogens but not between C-H bonds (too strong)

60
Q

why would excess methane be needed in free radical substitution?

A

to reduce further substitution

61
Q

describe the free radical substitution mechanism

A

check notes

62
Q

give 3 limitations of free radical substitutions

A
  • any of the hydrogens can be substituted so a number of products can be formed
  • multi-substitutions may occur
  • it is not effective to create a specific halogenoalkane

IB chemistry (29 decks)

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