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Chem Miss D > Kinetics & Organic Chemistry > Flashcards

Kinetics & Organic Chemistry Flashcards

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1
Q

What happens to a reaction if the concentration is higher?

A

Higher - more particles collide - faster reaction

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2
Q

What happens to a reaction if the pressure is higher?

A

Higher - more particles closer together - more collisions - faster reaction

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3
Q

What happens to a reaction if the surface area is bigger?

A

Bigger - more particles exposed at once - faster reaction as more can react at once

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4
Q

What happens to a reaction if the temperature increases?

A

Higher - more activation energy - particles move faster - more collisions - faster reaction

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5
Q

What does a catalyst do and how does it work?

A

It speeds up a reaction without being used up as it lowers the activation energy by providing an alternative pathway.

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6
Q

What is activation energy?

A

Minimum energy required to break bonds or for the particles react.

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7
Q

Functional group

A

The atom or group of atoms that are responsible for most of the chemical reactions of a molecule

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8
Q

Homologous series

A

A family of compounds with the same general formula and similar chemical properties

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9
Q

Hydrocarbon definition

A

Molecule containing hydrogen and carbon atoms only

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10
Q

Hydrogenation definition

A

Addition of hydrogen

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11
Q

Saturated

A

Molecule containing no double bonds

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12
Q

Stereoisomers definition

A

Molecules with the same molecular and structural formulae but different spatial arrangement of atoms

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13
Q

Geometric isomers definition

A

A type of stereoisomerism - molecules which have different arrangement of groups around C=C

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14
Q

Structural isomers

A

Molecules with the same molecular formula but different structures

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15
Q

Chain isomers definition

A

Type of structural isomerism - structural isomer that differ by having a different carbon chain

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16
Q

Position isomers definition

A

Type of structural isomerism - structural isomers that differ by having the functional group in a different position

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17
Q

Functional group isomers definition

A

Type of structural isomerism - Structural isomers that differ by having a different functional group (has same molecular formula but different name)

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18
Q

Unsaturated definition

A

Molecule containing double bond(s)

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19
Q

Substitution reaction definition

A

Reaction where an atom/group replaces another atom/group

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20
Q

1 carbon atom

A

Meth

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21
Q

2 carbon atoms

A

Eth

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22
Q

3 carbon atoms

A

Prop

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23
Q

4 carbon atoms

A

But

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24
Q

5 carbon atoms

A

Pent

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25
Q

6 carbon atoms

A

Hex

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26
Q

Alkane

-suffix

A
  • ane

- normal carbon and hydrogen atoms

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27
Q

Alkene

- suffix

A
  • ene

- a double carbon bond

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28
Q

Halogenoalkane

- prefix

A
  • fluro - chloro - bromo - iodo

- normal carbon and hydrogen with one other element

29
Q

Alcohol

- prefix and suffix

A
  • hydroxy and ol

- normal hydrogen abs carbon and a OH

30
Q

Aldehyde

- suffix

A
  • al

- double O bond on end

31
Q

Ketone

-prefix abs suffix

A
  • oxo and one

- double o bond in middle

32
Q

Carboxylic acid

- suffix

A
  • oic acid

- double O bond and OH

33
Q

Nitrile

- suffix

A
  • nitrile

- triple nitrogen bond

34
Q

Amine

- prefix and suffix

A
  • amino and amine

- nitrogen with 2 hydrogens

35
Q

Acyl chloride

- suffix

A
  • oyl chloride

- double O bond with chlorine

36
Q

Acid anhydride

- suffix

A
  • oic anhydride

- one O in middle and two double O either side

37
Q

Ester

- suffix

A
  • oate

- one O and one double O

38
Q

Amide

- suffix

A
  • amide

- one double O and one nitrogen

39
Q

Molecular formula definition

A

How many of each element (C2H6)

40
Q

Empirical formula definition

A

Molecular formula simplifies (C2H6 - CH3)

41
Q

General formula for alkanes

A

CnH2n+2

42
Q

Structural formula definition

A

CH3CH2CH3

43
Q

Displayed formula definition

A

Drawing out each element

44
Q

Skeletal formula definition

A

Lines

45
Q

How to draw geometric isomers

A
  • draw displayed formula on angles so is clear which geometric isomers it is (opposite or together)
46
Q

Two types of geometric isomers

A
  • Opposite “Entgagen” (put E in front of name to distinguish which displayed formula it is)
  • Together “Zuzammen” (put Z in front of name)
47
Q

Things on Maxwell Boltzmann curve

A
  • most probable energy
  • average energy
  • area under graph will always be the same as particle number
48
Q

Which particles react on Maxwell Boltzmann curve ?

A

Only the particles that posses at least the activation energy are able to react

49
Q

Cooler temp on MB curve

A

Particles have less energy so so curve is taller sooner and lower faster

50
Q

Hotter temp on MB curve

A

Means particles have more energy so curve is wider and shorter throughout

51
Q

Why does MB curve flatten and move to right when temp is increased?

A

Particles have higher energy so less particles needed

52
Q

Catalyst abs MB curve

A
  • fraction of particles with energy increases then decreases and energy increases
53
Q

Why is there an additional number of particles that can react when the MB curve has a catalyst?

A

The value of the activation energy is lowered by the catalyst so more particles can react but the distribution curve doesn’t change.

54
Q

What are the two forms of catalyst?

A
  • Homogeneous catalysts (same phase)

- Heterogeneous catalysts (different phase)

55
Q

Optical Isomers definition

A

Different arrangements of 4 different groups about a central C atom in a molecule - non identical mirror images

56
Q

Possible differences of optical isomers

A
  • rotate plane polarised light in opposite directions

- one may be biologically active; the other not

57
Q

What is a 50:50 mixture of optical isomers called?

A

Racemate or racemic mixture (has no effect on plane polarised light)

58
Q

What is a type of optical isomers?

A

Enantisomers

59
Q

Enantisomer definition

A
  • have same chemical physical properties as each other

- interact differently with plane polarised light

60
Q

Molecular formula definition

A

Formula that gives the actual number of atoms of each element in one molecule

61
Q

Empirical formula definition

A

Formula that gives simplest ratio of atoms of each element in a compound

62
Q

How to work out empirical formula

A
  • write out mass or percentage of each element
  • divide by the Ar of element not the Mr
  • find simplest whole number ratio or these numbers by dividing by the smallest number
  • if the value comes out as near 1/2’s then times them by 2, if they are near 1/3’s then times by 3
63
Q

Percentage yield calculation

A

Actual yield/ theoretical yield x 100%

64
Q

What are the two stages of a percentage yield problem?

A
  • work out what you would get is the yield was 100%

- use this figure to calculate the actual percentage

65
Q

Factors of Atom economy

A
  • No atoms are gained or lost in the reaction
  • some stones in reactants may not end up in the desired product
  • they form other products so are regarded as by products
66
Q

Atom economy definition

A

The measure of the amount of starting materials that end up as useful products

67
Q

Why is it important to use reactions with high atom economy?

A

Sustainable development

Economic reasons

68
Q

Atom economy calculation

A

total Mr of the product / total Mr of all reactants x 100%

Chem Miss D (8 decks)

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