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chemistry > paper 2 > Flashcards

paper 2 Flashcards

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1
Q

define volatility

A

how easy a liquid can turn into a gas

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2
Q

why are smaller alkanes more useful in fuels?

A

as they are more volatile and flammable

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3
Q

define viscosity

A

a measure of the liquids ability to flow

if it is viscous, it is syrupy

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4
Q

how can you separate crude oil?

(into smaller alkanes)

A

fractional distillation

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5
Q

define cracking

and what is the product?

A

breaking down larger hydrocarbons into smaller ones.

alkanes and alkenes

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6
Q

What are the 2 types of cracking?

A

steam
catalytic

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7
Q

what is required for thermal cracking?

A

very high temp and pressure

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8
Q

what is required for catalytic cracking?

A

high temp
Zeolite catalyst

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9
Q

what is the formula for alkenes?

A

CnH2n

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10
Q

what is the formula for alkanes?

A

CnH2n+2

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11
Q

what is the test to distinguish alkanes and alkenes?

A

Add them to bromine water. If an alkene is present the water will go colourless. If an alkane is present, it will stay orange.

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12
Q

what is the functional group of alcohols?

A

-OH

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13
Q

What is an isomer?

A

compounds with the same molecular formula but different structure.

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14
Q

what is the functional group of carboxylic acid?

A

-COOH

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15
Q

what is the formula for carboxylic acid?

A

CnH2n+1

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16
Q

what is the formula for alcohols?

A

CnH2n+1

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17
Q

How can carboxylic acids be formed?

A

via oxidising alcohols

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18
Q

what are polymers?

what are monomers?

A

very long molecules that are made up of repeating units

the repeating units

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19
Q

what is a condensation polymer?

A

A polymer where a small molecule is also made

(monomers react to make the polymer and a small moleculer)

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20
Q

what is the functional group for an amide?

A

-CoNH

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21
Q

what is the functional group for an ester?

A

-COO

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22
Q

what solution is added to copper sulfate to show the copper (ii) ions

A

sodium hydroxide

blue precipitate

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23
Q

define distillation

A

the cooling down of gases, and then the heating of their liquid to separate them based off of boiling point.

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24
Q

why are most gases gases at room temp?

e.g oxygen

A

due to weak intermolecular forces

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25
Q

what is earths source of oxygen?

A

photosynthesis

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26
Q

what is earths source of cabron dioxide?

A

volcanoes

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27
Q

name the 3 greenhouse gases

A

carbon dioxide, methane, water vapour

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28
Q

what is an alloy?

A

a mixture of 2 + elements where at least 1 is a metal

29
Q

define a pure substance

A

a substance which contains only one compound or element

30
Q

What is a formulation?

give an example

A

mixtures that have been prepared using a specific formula

cleaning agents

31
Q

this refers to chromatography

what is the mobile and stationary phase?

A

mobile phase-a substance the molecules can move in e.g solvent
stationary- a substance the molecules cannot move in e.g the paper

32
Q

describe the method to test for chlorine

A
  1. add damp litmus paper to the test tube with the gas in it.
  2. if it turns white, chlorine is present
33
Q

describe the method to test for oxygen

A
  1. add a glowing splint to the test tube with the gas in it
  2. if oxygen is present it will re-light
34
Q

describe the method to test for hydrogen

A
  1. slowly place burning splint into test tube with gas in it
  2. if hydrogen is present, a squeaky pop noise will be made
35
Q

describe the method to test for carbon dioxide

A
  1. add carbon dioxide to lime water
  2. limewater will turn cloudly if CO2 present
36
Q

what is the word equation for the production of ethanol?

A

glucose -> ethanol + carbon dioxide

37
Q

what conditions are needed for fermentation?

A

addition of yeast
absence of oxygen
temp of 5-45 degrees

38
Q

why are alkenes able to form polymers, unlike alkanes?

A

they are unsaturated
they are able to bond to other molecules

39
Q

what 3 gases make up our atmosphere?
from most to least

A

nitrogen
oxygen
argon

40
Q

State two differences between the atmosphere today and the atmosphere of billions of years ago.

A

amount of CO2 is much lower
amount of O2 is much higher

41
Q

what are the 3 ways of measuring the rate of a reaction?

A

colour change
change in mass
volume of gas gained or lost

42
Q

what is a homologous series?

A

compounds with the same functional group

43
Q

why are hydrocarbons used as fuel?

A

they release a large amount of energy when combusted

44
Q

give 4 factors which affect a chemical rate of reaction

A

temperature
concentration
surface area
catalyst

45
Q

what does the collision theory state?

A

for particles to react, they have to collide with sufficient energy

46
Q

what is equilibrium?

A

where a forwards and backwards reaction occur at the same rate

47
Q

what system is required to reach equilibrium?

A

a closed system

48
Q

how does the equilibrium shift left or right?

A

it shifts to the side where there is more of the substance. e.g if there are more products than reactants, it will shift to the right.

49
Q

what is le chateliers principle?

A

if the conditions of a reversible reaction are changed, the position of the equilibrium will shift to try counteract the change

50
Q

if temperature is decreased in an exothermic reaction, which way will the equilibrium shift?

A

right

51
Q

give 3 factors which affect the position of equilibrium

A

temperature
pressure
concentration

52
Q

what is the difference between saturated (alkanes) and unsaturated (alkenes) hydrocarbons?

A

saturated- contains no double bonds
unsaturated- contains double bonds

53
Q

what is the word equation for complete combustion?

A

hydrocarbon + oxygen = carbon dioxide + water

producing loads of energy

54
Q

name the steps of fractional distillation

A

The first step is to heat the crude oil to a very high temperature so that all of the compounds are evaporated from liquid to gas.
The hot gaseous hydrocarbons then rise up the fractionating column (because hot gas rises).
As they rise, they cool down, because the top of the column is cooler than the bottom.
The hydrocarbons will condense when they become cooler than their boiling point, and the liquid hydrocarbons then collect in trays and drain out.
The longer chain hydrocarbons condense at the bottom of the fractionating column because they have high boiling points.
Meanwhile the shorter chain hydrocarbons condense at the top of the column because they have much lower boiling points.

55
Q

what is the word equation for cracking?

A

long chain alkane= short chain alkane + alkene

balanced

56
Q

what type of reaction is cracking?

A

thermal decomposition

57
Q

what type of reactions do alkenes create due to their double bond?

A

addition reactions (double bond breaks)

58
Q

give 2 uses of ethanol

A
  1. alcoholic drinks
  2. used as a biofuel
59
Q

why are carboxylic acids weak?

A

as they dont fully ionise in water

60
Q

what reacts to form an ester?

A

carboxylic acid and alcohol

61
Q

give 2 properties of esters

A
  1. sweet smelling
  2. volatile
62
Q

how are condensation polymers formed?

A

by reacting dicarboxylic acid and diol monomers

63
Q

why are condensation polymers biodegradeable?

A

ester links can be broken down by micro-organisms

64
Q

Which monomers combine to form a polypeptide?

A

amino acids

condensation reaction

65
Q

in paper chromotography, what is the equation for the rf value?

A

distance travelled by substance/ distance travelled by solvent

66
Q

give 2 solvents usually used in chromotography

A
  1. water
  2. ethanol
67
Q

describe the test for carbonates

A
  1. add dilute hcl acid to the sample
  2. bubble any gas formed through limewater
  3. if carbonate is present, limewater will turn cloudy
68
Q

describe the test for sulfates

A
  1. add dilute hcl acid to sample to remove unwanted ions
  2. add barium chloride solution to the sample
  3. if sulfates are present there will be a white precipitate
69
Q

describe the test for halide ions

A
  1. add dilute nitric acid to remove unwanted ions
  2. add silvernitrate to sample
  3. if chloride ions present: white precipitate
  4. if bromide ions present: cream precipitate
  5. if iodide ions present: yellow precipitate

chemistry (6 decks)

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