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Chemistry Edexcel GCSE > Separate Chemistry 2 > Flashcards

Separate Chemistry 2 Flashcards

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1
Q

What colour flame does Lithium have

A

Crimson

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2
Q

What colour flame does Sodium have

A

Yellow

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3
Q

What colour flame does Potassium have

A

Lilac

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4
Q

What colour flame does Calcium have

A

brick red/ orangey

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5
Q

What colour flame Copper have

A

blue-green

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6
Q

How to carry out a flame test

A

Clean a nichrome wire loop by dipping it in HCl

Then dip into metal compound and place loop into the clear blue part of a bunsen flame

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7
Q

What colour precipitate does aluminium form

A

White
But dissolves with excess NaOH

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7
Q

How to test for metal ions that form precipitates

A

Add NaOH

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8
Q

What colour precipitate does Calcium form

A

White

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9
Q

What colour precipitate does Copper (2) form

A

Blue

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10
Q

What colour precipitate does Iron (2) form

A

Green

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11
Q

What colour precipitate does Iron (3) form

A

Brown

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12
Q

How to test for ammonia

A

add NaOH solution

If present then damp red litmus will go blue

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13
Q

How to test for halide ions

A

Nitric acid and then Silver Nitrate solution

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14
Q

What colour precipitates do the halides form when tested

A

Chloride - white
Bromide - cream
Iodide - yellow

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15
Q

How to test for carbonates

A

Add dilute acid
Then use CO2 test

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16
Q

How to test for sulfate ions

A

HCl and Barium Chloride

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17
Q

What colour precipitate will a sulphate form

A

White

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18
Q

What does flame photometry allow us to do

A

Identify ions in a mixture or in a dilute solution

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19
Q

How is it carried out
(flame photometry)

A

A sample is placed in a flame

The electrons are excited and as they drop back down to their original energy level the emit energy in the form of light

This passes through a spectroscope a a line spectrum is produced

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20
Q

What is flame photometry useful for

A

Concentration of ions in solution
Intensity of light
Intensity of solution

21
Q

What are alkanes

A

Saturated hydrocarbons
Formula CnH2n+2

22
Q

What are alkenes

A

Unsaturated hydrocarbons
Formula CnH2n

23
Q

Test for alkene

A

Bromine water
Decolourise orange to colourless

24
Q

What are addition polymers

A

Polymers made from unsaturated monomers (alkenes)

25
Q

Uses of polymers

A

Poly(ethene) - Flexible, electrical insulator, cheap - used in plastic bags, bottles and wire insulation

Poly(propene) - flexible, strong, touch, mouldable - crates, furniture, ropes

Poly(chloroethene) (PVC) - tough, cheap - window frames, water pipes

Poly(tetrafluoroethene) - unreactive, tough, non-stick - non-stick pans, waterproof clothing

26
Q

What type of monomer does polymerisation reactions involve

A

2 different types of monomer

27
Q

What are polymers made from

A

Crude oil

28
Q

Pros and cons of burning polymers

A

Pros:
Energy released can be used for electricity
Reduces volume of waste

Cons:
CO2 is made
Toxic gases are also made

29
Q

Pros and cons of landfill

A

Pros:
Cheap
Easy
No need to sort waste

Cons:
Destroys environment
Waste is dangerous to animals
Eyesore

30
Q

Pros and cons of recycling

A

Pros:
Conserves a vital raw material (crude oil)
Less waste to landfill

Cons:
Sorting plastics is time consuming
Expensive

31
Q

What is the general formula of an alcohol

A

CnH2n+1OH

32
Q

What happens to alcohols to form carboxylic acids

A

Oxidised

32
Q

What happens if you meet a mixture of an alcohol and an acid catalyst

A

An alkene and water are formed
This is called a dehydration reaction

33
Q

How are carboxylic acids similar to normal acids

A

React with carbonates to form CO2, salt and water

Can partially ionise in solutions

34
Q

What is the general formula for Carboxylic acids

A

Cn-1H2n-1COOH

35
Q

What is a substitution reaction

A

Where a H gets substituted by another atom eg. Bromine
This must happen under UV

Eg
CH4 + Br2 –> CH3Br + HBr

36
Q

What is an addition reaction

A

When an alkene reacts with a halogen

The double bonds is broken and the halogen goes onto the 2 Cs with the double bond

eg.
C2H4 + Br2 –> C2H4Br

37
Q

Equation for breakdown of glucose

A

C6H12O6 –> 2C2H5OH + 2CO2

38
Q

What does the breakdown of glucose

A

Enzymes in the yeast

39
Q

Examples of things that can be used for the glucose in production of ethanol

A

Sugar cane
Sugar beef
Grapes

40
Q

Why is the concentration of ethanol around 10-20%

A

Because the yeast dies

41
Q

What is used to concentrate the ethanol

A

Fractional distillation
Then a Leibig condenser

42
Q

How to measure which alcohol is the most efficient fuel

A

Spirit burner with alcohol in it and use a mass balance to measure the mass

Measure 100cm^3 of distilled water into a copper calorimeter

Insulate the container

Cover with an insulating lid

Take initial temp

Light wick

Stir

When temp has increased by 20 degrees blow out the wick

Reweigh immediately

Repeat

43
Q

What are the size of nanoparticles

A

1-100 nanometers across

44
Q

What is a nanoparticle surface area to volume ratio like

A

High

45
Q

Uses of nanoparticles

A

Catalysts (high SA to V ratio)
Cosmetics - eg. sunscreen
Electric circuits (conduct electricity)
Sports equipment plastics (durable and stronger)

46
Q

What could potential problems of nanoparticles be

A

They don’t break down as easily so perhaps they could start to build up in cells and cause problems such as lung inflammation

47
Q

What are composites

A

They are made of one material (the reinforcement) embedded in another (matrix)

48
Q

What happens when ethanol + oxygen

A

Carboxylic acid formed

49
Q

How are esters formed

A

Carboxylic acid + water

Characteristic smells
Insoluble in water

Chemistry Edexcel GCSE (9 decks)

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