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Chemistry > A- Atmosphere > Flashcards

A- Atmosphere Flashcards

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0
Q

List 5 factors that affect rates of reaction

A 
Any from:
Concentration
Pressure
Surface area
Temperature
Catalyst
Radiation intensity
Particle size
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1
Q

What is special about homogeneous catalysts?

A

They form an intermediate compound with the reactants

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2
Q

How do you convert an alkane into a halogenoalkane?

A

Br2 (l) + sunlight (provides UV)

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3
Q

How do you convert an alkene into an alkane?

A

H2 (g) / Ni
150 degrees Celsius
5 atm

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4
Q

How do you convert an alkene into a halogenoalkane?

A

HBr/ HX (depending on halogen)

Room temperature

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5
Q

How do you convert a halogenoalkane into an alcohol?

A

NaOH (aq)

Heat under reflux

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6
Q

How do you convert an alcohol into a halogenoalkane?

A

NaBr(s)/ c.H2SO4

Heat under reflux

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7
Q

How do you convert a halogenoalkane into an amine?

A

c.NH3 (aq)

Heat in a sealed tube

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8
Q

How do you convert a halogenoalkane into a nitrite/ cyano?

A

NaCN in aqueous ethanol solution

Heat under reflux

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9
Q

What two things affect the changes that can occur for a chemical absorbing energy?

A

The chemical involved

The amount of energy involved

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10
Q

What does ‘energy is quantified’ mean?

A

with fixed levels

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11
Q

How much argon is in the atmosphere?

A
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12
Q

How much carbon dioxide is in the atmosphere?

A

0.035%

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13
Q

What is Planck’s constant?

A

6.63 X 10-34 Joules

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14
Q

What is the difference between dissociation and excitation?

A 
Dissociation = Homolysis (in the context of halogens like Cl2)
Excitation = Electrons jump to higher energy level but eventually drop back to original state releasing this energy
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15
Q

In heterolytic fission, what happens to the SHARED electrons within the covalent bond?

A

Both go to just one atom, turning it into an anion so that the other atom becomes a cation.

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16
Q

In homolytic fission, what happens to the SHARED electrons within the covalent bond?

A

One of the two electrons goes to each atom so that each has an unpaired electron -> radicals

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17
Q

What is initiation?

A

The production of free radicals

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18
Q

What is propagation?

A

The use and generation of radicals (on both sides of the reaction)

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19
Q

What is termination?

A

The production of new molecules through removal of radicals

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20
Q

What are CFCs good for?

A

Aerosols
Propellants
Coolant (in fridges)
Fire extinguishers

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21
Q

How to radicals operate/ try to fill their outer shells?

A

Taking an electron from another molecule (often in the form of a hydrogen)

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22
Q

What are the conditions of radical chain reactions?

A

Gas phase/ non-polar solvent

Initiation by heating/ light (UV radiation)

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23
Q

What is the speed of radical chain reactions?

A

Very fast

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24
Q

Where do radical chain reactions mainly take place?

A

Troposphere + Stratosphere

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25
Q

What are examples of radical chain reactions?

A

Combusion/ Explosions

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26
Q

Outline the collision theory

A

Reactions occur when particles of reactants collide WITH a minimum amount of kinetic energy
Any factor that increases the number of collisions PER UNIT OF TIME will increase reaction rate

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27
Q

What is the activation enthalpy?

A

The minimum energy required for a successful reaction between particles after collision

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28
Q

True or false? Molecules in a gas have the same amount of energy

A

False

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29
Q

What two things affect the changes that can occur for a chemical absorbing energy?

A

The chemical involved

The amount of energy involved

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30
Q

What does ‘energy is quantified’ mean?

A

with fixed levels

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31
Q

How much argon is in the atmosphere?

A
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32
Q

How much carbon dioxide is in the atmosphere?

A

0.035%

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33
Q

What is Planck’s constant?

A

6.63 X 10-34 Joules

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34
Q

What is the difference between dissociation and excitation?

A 
Dissociation = Homolysis (in the context of halogens like Cl2)
Excitation = Electrons jump to higher energy level but eventually drop back to original state releasing this energy
How well did you know this?
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35
Q

In heterolytic fission, what happens to the SHARED electrons within the covalent bond?

A

Both go to just one atom, turning it into an anion so that the other atom becomes a cation.

36
Q

In homolytic fission, what happens to the SHARED electrons within the covalent bond?

A

One of the two electrons goes to each atom so that each has an unpaired electron -> radicals

37
Q

What is initiation?

A

The production of free radicals

38
Q

What is propagation?

A

The use and generation of radicals (on both sides of the reaction)

39
Q

What is termination?

A

The production of new molecules through removal of radicals

40
Q

What are CFCs good for?

A

Aerosols
Propellants
Coolant (in fridges)
Fire extinguishers

41
Q

How to radicals operate/ try to fill their outer shells?

A

Taking an electron from another molecule (often in the form of a hydrogen)

42
Q

What are the conditions of radical chain reactions?

A

Gas phase/ non-polar solvent

Initiation by heating/ light (UV radiation)

43
Q

What is the speed of radical chain reactions?

A

Very fast

44
Q

Where do radical chain reactions mainly take place?

A

Troposphere + Stratosphere

45
Q

What are examples of radical chain reactions?

A

Combusion/ Explosions

46
Q

Outline the collision theory

A

Reactions occur when particles of reactants collide WITH a minimum amount of kinetic energy
Any factor that increases the number of collisions PER UNIT OF TIME will increase reaction rate

47
Q

What is the activation enthalpy?

A

The minimum energy required for a successful reaction between particles after collision

48
Q

True or false? Molecules in a gas have the same amount of energy

A

False

49
Q

Why does a substance feel hotter?

A

Particles are moving more energetically

50
Q

What often happens with a 10 degrees C increase in temperature?

A

The rate of reaction doubles

51
Q

What are the stages of homogeneous catalysis?

A

Reactant + reactant + catalyst = intermediate

Intermediate breaks down -> Product + reformed catalyst

52
Q

What is a catalyst?

A

A substance that speeds up chemical reactions without being permanently changed in the process

53
Q

How does a catalyst work?

A

Provides an alternative reaction pathway with a lower activation enthalpy than the original pathway

54
Q

What is a heterogeneous catalyst?

A

A catalyst [substance that speeds up chemical reactions…] that is in the same phase as the REACTANTS

55
Q

What are the advantages of homogeneous catalysis?

A

More specific
More controllable
Fewer unwanted products formed
Infinite contact between catalyst + reactants - more efficient reaction

56
Q

What are the disadvantages of homogeneous catalysis?

A

Harder to separate from products- energy [money] required for separation

57
Q

What are the advantages of heterogeneous catalysis?

A

Easy to separate from products

58
Q

What are the disadvantages of heterogeneous catalysis?

A

Limited contact between catalyst + reactants - less efficient reaction

59
Q

What is the catalytic cycle?

A

A continuous process of converting reactants into products with a catalyst

60
Q

What is dynamic equilibrium?

A

The rate of the forward and reverse reactions are the same in a closed system

61
Q

What would reactions look like on a macroscopic scale?

A

Nothing would appear to change

62
Q

What would reactions look like on a microscopic scale?

A

Molecules would be constantly moving

63
Q

What is ‘position’ of equilibrium describing?

A

A particular set of equilibrium concentrations for a reaction

64
Q

What happens to the rate of the reaction during equilibrium?

A

It remains the same

65
Q

What happens to the concentration of the reaction during equilibrium?

A

It is constantly changing

66
Q

What happens to the rate of the reaction during equilibrium with the addition of a catalyst?

A

The rate of BOTH the forward and reverse reactions increase

67
Q

Outline le Chateiler’s principle

A

If a system is at equilibrium and a change is made in any of the conditions, the system responds to counteract this change as much as possible

68
Q

What is the difference between a steady state system and equilibrium

A

Equilibrium is always in a CLOSED system, steady state is in an OPEN system

69
Q

What are the similarities between CO2 and SO2?

A

Oxides of G4
Same molecular formula
Neither can conduct electricity

70
Q

What are the differences between CO2 and SO2?

A

CO2 has weaker intermolecular bonds; gas at rtp
SO2 is part of a giant covalent network; solid at rtp
SO2 has high M+B Points whereas for CO2 they’re low
CO2 is slightly soluble in water, SO2 is insoluble
CO2 has double bonds whereas SO2 has single bonds

71
Q

What does ‘allotrope’ mean?

A

A different form/ arrangement

72
Q

List 3 of the properties of covalent MOLECULAR structures:

A 
-Consist of discrete molecules
Phosphorus -> P4
Sulfur -> S8
-Strong INTRAmolecular covalent bonds
-The strength of the INTERmolecular bonds determines the physical state.
73
Q

List 3 examples of covalent NETWORK structures:

A

Boron, Silicon (Tetrahedral) , Carbon (2 of its varied forms are network structures)

74
Q

List the properties of DIAMOND

A

Giant lattice made from carbon
Tetrahedral- joining each carbon to four others
Highly symmetrical structure

75
Q

List 5 of the reasons why GRAPHITE is found in pencils

A

GRAPHITE
Giant flat carbon layers
Each layer is a 2D network
Each carbon is joined (strong covalent) to three other carbons; hexagonal rings formed
Fourth electron contributes to extended delocalised electron clouds forming between layers
Weakly held layers- can slide over each other
Delocalised electrons are free to move across the layer
Soft, brittle solid

76
Q

What is the chemical term for ‘Bucky- Balls’?

A

Fullerenes (C60)

77
Q

How are fullerenes formed?

A

Pass an electric arc between graphite rods

78
Q

What colour is formed when fullerenes dissolve in benzene?

A

RED

79
Q

Why can fullerenes dissolve in benzene?

A

They favour being a molecule than a network

80
Q

What are ‘Buckytubes/Nanotubes’?

A

Elongated fullerenes

81
Q

What could synthesis of longer fullerene molecules mean?

A

The creation of super strong, lightweight fibres

82
Q

Why can C60 act as an optical limiter?

A

Shining light on its solution turns it darker

Absorbs more light; intensity of transmitted light is limited to a maximum value

83
Q

What can Fullerenes/ C60 currently be used for?

A

Making protective goggles for people working with lasers

84
Q

What are the main greenhouse gases?

A

Water vapour, carbon dioxide, methane

85
Q

What does anthrogenic mean?

A

Caused by human activity

86
Q

Why is ozone in the troposphere dangerous?

A

It’s harmful

Contributes to photochemical smog

87
Q

Why did scientists initially reject the readings taken by the satellite mapping ozone levels?

A

The readings were very low so considered to be anomalous.

88
Q

How is ozone destroyed?

A

By a homogeneous catalyst (e.g. Nitrogen oxide)

Chemistry (12 decks)

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