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Chemistry > Section 2 chemistry of the elements > Flashcards

Section 2 chemistry of the elements Flashcards

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1
Q

in the periodic table what are the rows and columns called?

A

rows - periods

columns - groups

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2
Q

group 0 are inert what does this mean?

A

they dont react much

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3
Q

group 1 elements become more reactive as you go…………………..

A

down the group

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4
Q

What does a reaction with water and alkali metal produce?

A

The Metal hydroxide and hydrogen.

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5
Q

What alkali metal (in group 1) reacts the most?

A

Potassium - lilac flame sometimes explosion

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6
Q

Why is potassium more reactive than sodium or lithium?

A

It’s outer shell electrons are lost easier because they are further away from the nucleus so feel less nuclear attraction, so if can lose electrons easier, it is more reactive!

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7
Q

What is the name of the group 7 elements?

A

The halogens

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8
Q

As the atomic number of halogens increase the elements have a ………….

A

Darker colour
Higher
Melting point

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9
Q

The higher up group 7 the more ………….

A

Reactive it is

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10
Q

What can halogens combine with to form hydrogen halides?

A

Hydrogen

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11
Q

When hydrogen chloride dissociates what is formed?

A

Hydrochloric acid

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12
Q

What happens in a displacement reaction?

A

More reactive halogens displace less reactive ones

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13
Q

What does a halogen displacement reaction involve?

A

Transfer of electrons

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14
Q

How do you test for hydrogen?

A

Put lit split in test with a reaction

If hydrogen present, will make a squeaky pop

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15
Q

What salts will hydrochloric acid produce?

A

Chloride

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16
Q

What salts do sulfuric acid produce?

A

Sulfate salts

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17
Q

What is produced when metal and water reacts?

A

Metal hydroxide and hydrogen

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18
Q

What is the order of reactivity?

A

Potassium, Sodium, Lithium, Calcium, Magnesium, Aluminium, Zinc, Iron, Copper, Silver, Gold.

Remember this by using: Please Say Little Charlie’s Monkeys And Zebras In Cages Securely Guarded.

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19
Q

What corrodes to make rust?

A

Iron and steel

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20
Q

What are the two types of protecting rust?

A

Barrier - plastics, oil

Sacrificial - using a more reactive metal

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21
Q

What percentage of each gas is in the atmosphere?

A

78% - nitrogen
21% - oxygen
Nearly 1% - argon
0.04% - CO2

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22
Q

How can you investigate the proportion of oxygen in the atmosphere?

A

Using copper

Using iron or phosphorus

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23
Q

How can you make oxygen in a lab?

A

Using hydrogen peroxide - decomposition
Manganese oxide catalyst
Collection - over water or a gas a syringe
2H2O ….. 2H2O + O2

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24
Q

What happens when magnesium, carbon and sulfur react with oxygen?

A

Magnesium - bright white flame, white powder, magnesium oxide, alkaline in water
Carbon - orange flame, produces carbon dioxide, acidic in water
Sulfur - pale blue flame, produces sulfur dioxide, acidic in water

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25
Q

What is upward and downward delivery used for?

A

Upward - collect lighter than air gases

Downward - collect heavier than air gases

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26
Q

What does the thermal decomposition of metal carbonates produce?

A

Carbon dioxide

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27
Q

What is carbon dioxide used in?why?

A

Fizzy drinks - slightly soluble in water, produces carbonic acid, makes drinks fizz
Fire extinguisher - more dense than air, sinks into flame and stops oxygen

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28
Q

Explain how carbon dioxide can be produced?

A
  • Metal carbonate + acid ➡️ salt + water + carbon dioxide
  • Thermal decomposition:
    Metal carbonate ➡️ heat ➡️ carbon dioxide + metal oxide
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29
Q

What do greenhouse gases do?

A

Act as an insulating layer

Absorb heat and re radiate

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30
Q

How do you do a flame test?

A

Clean a platinum wire loop by dipping in HCL hold in the flame
Then dip in the sample and put back in the flame

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31
Q 
What colour does the flame burn for 
Lithium
Sodium
Potassium
Calcium
A

Lithium - crimson red
Sodium - orange
Potassium - lilac
Calcium - brick red

32
Q

How can you identify a metal hydroxide?

A

Add a few drops of sodium hydroxide

If colour you can identify

33
Q

What colour precipitate does copper and iron produce?

A

Copper - blue precipitate
Iron 2- green precipitate
Iron 3 - orange / brown precipitate

34
Q

How can you test for ammonia gas?

A

Ammonia turns damp red litmus paper blue

35
Q

How can you test for carbonates?

A

Add dilute hydrochloric acid to your sample

Carbon dioxide will be produced if carbonates are present.

36
Q

How can you test for sulphates?

A

Add dilute hydrochloric acid and barium chloride solution to metal sulphate.

White precipitate of barium sulphate produced if sulfate ions present.

37
Q

How can you test for halides?

A

Add nitric acid followed by silver nitrate

38
Q

What happens to chloride, bromide and iodide when testing for halogens?

A

Chloride ion - white precipitate of silver chloride
Bromide ion - cream precipitate of solver bromide
Iodide ion - yellow precipitate of silver iodide

39
Q

Why is acid used before the test for sulfates and halides?

A

To get rid of carbonates and sulfite ions

40
Q

How do you test for chlorine?

A

Turns blue litmus paper red then bleaches it white

41
Q

How do you test for oxygen?

A

Glowing splint will relight if oxygen is present.

42
Q

How do you test for carbon dioxide?

A

Bubble your gas into limewater

Will turn cloudy if carbon dioxide is present.

43
Q

How can you test for hydrogen?

A

Squeaky pop

44
Q

Wet copper sulfate is ……….

Dry copper sulfate is …….

A

Blue

White

45
Q

How do you test for water?

A

Add anhydrous copper sulfate and see if white powder turns blue. (will turn blue if water present)

46
Q

How do you test for pure water?

A

Pure water will always:
Boil at 100 degrees C
Freeze at 0 degrees C

47
Q

Dioxides are

Oxides are

A

Dioxides acidic

Oxides alkaline

48
Q

What does redox mean?

A

Redox reactions are when reduction and oxidation reactions happen at the same time.

49
Q

What is an oxidising agent?

A

An oxidising agent accepts electrons and gets reduced.

50
Q

What is a reducing agent?

A

A reducing agent donates electrons and gets oxidised.

51
Q

Describe the conditions under which iron rusts.

A

When the iron is in contact with both oxygen (from the air) and water.

52
Q

How can the rusting of iron be prevented?

A 
Paining it
Coating with plastic
Coating with grease
Coating with oil
Galvanising
53
Q

Explain the sacrificial protection of iron.

A

It involves placing a more reactive metal with the iron. The water and oxygen then react with this sacrificial metal instead of with the iron to prevent rusting.

54
Q

Explain the uses of iron in terms of properties.

A

It’s malleable, so is used to make gates and railings.

Can be mixed with elements to make alloys e.g. stainless steel for cutlery.

55
Q

Explain the uses of aluminium in terms of properties.

A

Reacts quickly with oxygen in air to form aluminium oxide.

Doesn’t corrode so useful for products in contact with water e.g. Drink cans.

Less dense than iron, making it lighter so useful for bicycle frames and planes.

56
Q

Name the metals in order of reactivity series from most reactive to least reactive.

Hint: Please Say Little Charlie’s Monkeys And Zebras In Lead Horrible Cages Securely Guarded Please

A 
Potassium
Sodium
Lithium
Calcium
Magnesium
Aluminium
Zinc
Iron
Lead
Hydrogen
Copper
Silver
Gold
Platinum
57
Q

Describe how reactions with water and dilute acids can be used to deduce the order of reactivity of metals.

A

Very reactive metals will react vigorously with water e.g. potassium, sodium, lithium, calcium.

Less reactive metals won’t react with cold water but will react with steam e.g. copper, silver, gold.

58
Q

What happens when lithium reacts with water?

A

Produces: lithium hydroxide and hydrogen

Observations: fizzing, gas, movement, floating, dissolves, exothermic.

59
Q

What happens when sodium reacts with water?

A

Produces: sodium hydroxide and hydrogen.

Observations: fizzing, turns into a ball, melts, movement, dissolves, exothermic.

60
Q

What happens when potassium reacts with water?

A

Produces: potassium hydroxide and hydrogen.

Observations: pink flame, fizzing, movement, dissolves.

61
Q

What happens when magnesium reacts with hydrochloric acid / sulphuric acid?

A

With hydrochloric acid it produces: magnesium chloride and hydrogen.

With sulfuric acid it produces: magnesium sulphate and hydrogen.

Observations: effervesses, exothermic, hydrogen gas.

62
Q

What happens when zinc reacts with hydrochloric acid / sulphuric acid?

A

With hydrochloric acid it produces: zinc chloride and hydrogen.

With sulphuric acid it produces: zinc sulphate and hydrogen.

Observations: slow and little reaction, few bubbles.

63
Q

What happens when iron reacts with hydrochloric acid / sulphuric acid?

A

With hydrochloric acid it produces: Iron chloride and hydrogen.

With sulphuric acid it produces: iron sulphate and hydrogen.

Observations: slow and little reaction, 1 or 2 bubbles.

64
Q

What happens when a metal reacts with an acid?

A

The metal salt and hydrogen are produced.

65
Q

How could you test metals to place them in order of reactivity?

A

Using reactions with water and dilute acids. The most vigorous reactions are the most reactive metals.

66
Q

What are the colours and physical States of the following elements at room temperature?

a) fluorine
b) chlorine
c) bromine
d) iodine

A

a) fluorine is a pale yellow gas at room temperature, produces yellow vapour.
b) chlorine is a pale green gas at room temperature, produces green vapour.
c) bromine is a red / orange liquid at room temperature, produces red / brown vapour.
d) iodine is a black / grey solid at room temperature, produces purple vapour.

67
Q

When do displacement reactions occur?

A

A more reactive metal displaces a less reactive metal from a compound.

So can be used to determine order of reactivity.

Might be happening when there is a temperature increase or colour change in the reaction.

68
Q

As you go down group 7 the reactivity of metals……….

A

Decreases

69
Q

Describe an experiment to show that a more reactive halogen will displace a less reactive halogen from a solution of one of its salts.

A

Add a a few drops of a halogen solution e.g. chlorine / bromine / iodine water to a salt solution e.g. Potassium chloride.
Look for a colour change, meaning a displacement reaction has occurred.

70
Q

Are displacement reactions reduction, oxidation or redox reactions? Why?

A

Redox because in displacement reactions reduction and oxidation happen simultaneously, which are called redox reactions.

71
Q

What are halides (F-, Cl-, Br-, I-, At- etc) also known as?

A

Anions.

72
Q

How could you test for different halides or anions?

A

Placing 2cm3 of halide into test tube
Add dilute nitric acids to acidify solution
Add a few drops of silver nitrate solution
Repeat test with another halide solution.

73
Q

How would you show that a substance contains a halide ion?

A 
Add dilute nitric acid
Add silver nitrate
If chloride present: White precipitate
If bromide present: cream precipitate
If iodide present: yellow precipitate.
74
Q

How can you test for the cations copper, iron II and iron III?

A

Add sodium hydroxide to your solution containing an unknown metal ion, a precipitate will form, if:

Blue = copper
Green = iron II
Orange / brown = iron III

75
Q

How can you test for the cations copper, iron II and iron III?

A

Add sodium hydroxide to your solution containing an unknown metal ion, a precipitate will form, if:

Blue = copper
Green = iron II
Orange / brown = iron III

76
Q

What is a oxidising agent?

A

Accepts electrons and gets reduced

77
Q

What is a reducing agent?

A

Donates electrons and gets oxidised

Chemistry (7 decks)

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