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Chemistry > 9-16. Kinetics I and II > Flashcards

9-16. Kinetics I and II Flashcards

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1
Q

What is an isomer

A

Same molecular formula but atoms are arranged differently

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2
Q

What is a structural isomers

A

Different structural arrangements

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3
Q

What is a chain isomer and it’s properties

A

The carbon skeleton is arranged differently (straight and branched)
Similar chemical properties
Different physical properties

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4
Q

What is a positional isomer and it’s properties

A

The skeleton and functional group are the same but the functional group is attached to a different carbon atom
Different chemical and physical properties

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5
Q

What is a functional group isomer and it’s properties

A

The same atoms can be arranged into different functional groups
Very different chemical and physical properties

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6
Q

What bonds can atoms rotate around

A

Single carbon bonds

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7
Q

What bonds don’t rotate

A

Carbon double bonds

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8
Q

What does planar mean

A

All atoms lie in the same plane

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9
Q

What is stereoisomerism

A

Same structural formulae but a different arrangement

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10
Q

What is an E-Isomer

A

Has the same group positioned across the double bond

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11
Q

What is a Z-Isomer

A

Has the same groups either both above or below the double bond

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12
Q

What is collision theory

A

Particles must collide to react in the right direction and collide with at least a certain minimum amount of kinetic energy

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13
Q

What is activation energy

A

Minimum amount of energy the reactants must have for a reaction to happen

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14
Q

What happens when you increase the concentration of reactants

A

There is more particles so they collide more frequently which increases the rate of reaction

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15
Q

What happens if you increase the pressure

A

There are more particles in a given volume which increases the frequency of collisions

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16
Q

What does a catalyst do

A

Lowers the activation energy by providing a different way for bonds to be broken which allows more particles to have enough energy to react

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17
Q

What happens when you increase the temperature of a reaction

A

More particles have the minimum activation energy and will move faster.

18
Q

What is the definition of rate of reaction

A

The change in amount of reactants or product per unit of time

19
Q

What is initial rate

A

The rate at the start of a reaction

20
Q

What is a catalyst

A

Increases the rate of a reaction by providing an alternative reaction pathway with a lower activation energy so a greater proportion of collisions result in a reaction.

21
Q

Economic benefits of catalysts

A

Lower production costs, give more products in a shorter time
Using catalysts can change properties

22
Q

What’s a heterogenous catalyst

A

Catalyst in a different physical state from reactants
The reaction happens on the surface of a heterogeneous catalyst so increasing the surface area increases the rate of reaction

23
Q

What’s a homogenous catalyst

A

A catalyst in the same physical state as the reactants
During this the catalyst combine with the reactants to make an intermediate species which react to form products and reform the catalyst

24
Q

Ways to follow rates of reaction

A

Gas volum
Loss of gas
Change in pH
Colour change
Titration
Electrical conductivity

25
Q

What is 0 order reaction

A

If concentration of X changes and the rate stays the same the order of reaction with respect to X is 0

26
Q

What is 1st order reaction

A

If the rate is proportional to the concentration of X then the order with respect to X is 1

27
Q

What is 2nd order reaction

A

If the rate is proportional to the concentration of X^2 then the order of reaction with respect to X is 2

28
Q

What is Half life

A

The time it takes for half of the reactant to be used up

29
Q

How to work out the half life of a reaction

A

Work out the half life by drawing a concentration time graph. Draw lines scores from the Y- axis at points where the concentration has halved and read off the time taken

30
Q

Rate equation

A

Rate = k (A)^m(B)^n

31
Q

What is K

A

Rate constant
Bigger it is the faster the reaction

32
Q

What is the rate determining step

A

The slowest step in a multi step reaction mechanism.
The overall rate is decided by the rate determining step

33
Q

What is nucleophilic substitution

A

When a nucleophile attacks another molecule and is swapped for one of the attached groups.

34
Q

What type of mechanism for nucleophilic substitution for primary and secondary halogenoalkanes

A

Sn2

35
Q

What time of nucleophilic substitution mechanism is secondary and tertiary halogenoalkanes

A

Sn1

36
Q

What is the Arrhenius equation and what do the symbols mean

A

k = Ae ^Ea/RT

k= rate constant
A = frequency of collisions constant
e = constant e
-Ea = - activation energy
R = gas constant 8.31
T = temperature in Kelvin

37
Q

Arrhenius constant in logarithmic form

A

ln k = ln A - Ea/RT

38
Q

What is the graph of an Arrhenius plot

A

ln k against 1/T

39
Q

What is an optical isomer

A

Molecules that are mirror images of each other

40
Q

What is a chiral centre

A

A carbon atom that has four different groups attached to it

41
Q

Properties of optical isomers

A

2 enantiomers
Can’t be superimposed
Rotate plane polarised light

42
Q

What is a racemic mixture

A

Contains equal quantities of each negations of a chiral compound. Don’t rotate plane polarised light as they cancel.

Chemistry (14 decks)

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