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Chemistry > Chemistry Of The Elements > Flashcards

Chemistry Of The Elements Flashcards

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1
Q

What happens to the element as you go down group 1 in the periodic table?

A

They become more reactive as you go down

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2
Q

Metal + Water = ?

A

Metal Hydroxide + Hydrogen

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3
Q

What happens to the Halogens in group 7 as you go down the periodic table in terms of boiling point and colour

A

Boiling point increases

The colour gets darker

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4
Q

The colour of Iodine as a solid?

A

Dark grey

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5
Q

Physical state of Iodine at Room Temperature.

A

Solid

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6
Q

Physical state of Bromine at room temperature.

A

Liquid

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7
Q

Physical state of chlorine at room temperature

A

Gas

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8
Q

Colour of Bromine as a liquid?

A

Red-Brown

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9
Q

Colour of chlorine as a gas

A

Green

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10
Q

Hydrogen + Halogens = ?

A

Hydrogen Halides

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11
Q

State of Hydrogen Chloride at room temperature?

A

Gas

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12
Q

What happens when hydrogen chloride is dissolved in water and what solution is formed?

A

It Dissociates - The HCL molecules split into H+ ions and Cl- ions. The solution formed is Hydrochloric acid.

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13
Q

What does Hydrogen Chloride not dissolve in

A

Methylbenzene

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14
Q

What is a Displacement reaction?

A

The more reactive halogens will displace the less reactive one in a compound

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15
Q

The colour of Potassium iodide solution

A

Colourless

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16
Q

Colour of Potassium a chloride Solution?

A

Colourless

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17
Q

Colour of bromide solution?

A

Colourless

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18
Q

The colour of Bromine water?

A

Orange

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19
Q

Acid + Metal = ?

A

Salt + Hydrogen

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20
Q

How is the rate of reaction calculated when acid react with metals.

A

The rate at which the bubbles of hydrogen are given off.

Hydrogen is confirmed by burning splint test

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21
Q

How fast do zinc and iron react with dilute acids

A

Slowly but more strongly if you heat them up.

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22
Q

Which metals react vigorously with water?

A

Potassium, Sodium, Lithium and Calcium

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23
Q

Copper won’t react with either water or steam

True or false?

A

True

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24
Q

Name the Reactivity Series starting from the top;

A 
Potassium 
Sodium 
Lithium 
Calcium
Magnesium 
Aluminium
Zinc 
Iron 
Cooper 
Silver Gold
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25
Q

Iorn oxide + Aluminium = ?

What happens to the Iron

A

Aluminium oxide + Iron

Iron would be displaced from Iron Oxide by the mor reactive Aluminium

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26
Q

The word equation for the Rusting of Iron

A

Iron + Oxygen +’Water –> Hydrated Iron (|||) oxide (rust?

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27
Q

2 barriers that can prevent rusting

A

Painting, a coating with plastic

Oiling and Greasing

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28
Q

Sacrificial method for prevent rusting.

A

For more reactive metals
Coating of Zinc - galvanising
Zinc is more reactive that iron

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29
Q

Percentage of Nitrogen. carbon Dioxide, Oxygen and Argon in the atmosphere ,

A

Oxygen 21%
Nitrogen 78 %
Argon nearly 1%
Carbon Dioxide 0.04 %

30
Q

3 ways of investigating the proportion of Oxygen in the Atmosphere

A

Using copper
Iron
Phosphorous

31
Q

Describe how you can use Coper to investigate the proportion of Oxygen in the Atomsphere

A
  1. Copper reacts with oxygen in the air to make Copper (||) oxide - so the reaction uses up oxygen
  2. If you heat an excess of copper inc a tube and lass air over it using two syringes, you can use the markers on the syringes to tell how much oxygen has been used up.
  3. If you start with 100cm3 of air, you’ll end up with about 80 cm3 when the reactions finished and the air has cooled. If 20 cm3 of air has gone then around 20% of the air must be oxygen
32
Q

Describe the investigation to find the proportion of oxygen in the Atomsphere

A
  1. Iron reacts with oxygen in the a or to form rust so the iron will remove oxygen from the air.
  2. Soak iron wool in acetic acid ( the acid will catalysed the reaction)
  3. Push the wool into a test tube, put your thumb over the end and invert the tube into a beaker of water.
  4. Over time the level of water in the test tube will rise. This is because the iron reacts with the oxygen in the air to make iron oxide. The water rises to fill the space the oxyGen took up.
  5. To work out percentage of the air that is oxygen, you need to mark the starting and finishing position of the water and pour the contents into s measuring cylinder to find out the volume of air at the start and the end. Use the difference between the starting and finishing volume
33
Q

When do Ionic Compounds conduct electricity

A

When they are molten or in solution - ions are free to move so they conduct electricity

34
Q

What happens when an ionic compound melts?

A

The ions are free to move and will carry electric current

35
Q

Describe the stricture of Metals.

A

Giant structure of positive ions surrounded by a sea of delocalised free electrons
Hold together by metallic bonding

36
Q

Describe the elements in group 0.

A

All inert - don’t react with much at all - They have a full outer shell of electrons
Colourless gas

37
Q

What is electrolysis?

A

If you pass an electric current through an ionic substance that’d molten or in solution it breaks down into elements .

38
Q

In the electrolysis of Molten Lead bromide what is produced at the Cathode? Write the half equation.

A

Pb2+ + 2e- —> Pb

39
Q

In the Electrolysis of Molten Lead bromide what is produced at the Anode? Write the half equation

A

2Br- —> Br2 + 2e-

40
Q

How can you prepare oxygen in the lab?

A

Decompose Hydrogen Peroxide with manganese oxide as a catalyst.
Catalyst speeds up rate of reaction and you can collect oxygen in a syringe.

41
Q

What happens when you burn Magnesium in Oxygen?

A

Magnesium burns with bright white flame in air and a white powder that is formed is magnesium oxide

42
Q

What happens when Carbon burns with Oxygen?

A

Carbon will burn in air of its very strongly heated.

It has an orangey/yellow flame and produces carbon dioxide gas.

43
Q

What happens when sulfur burns in oxygen?

A

Produces pale blue flame and produces Sulfur dioxide

44
Q

When do you use upward delivery to collect gas?

A

Gases that are heavier than air

45
Q

When do you use unaware.d delivery when collecting gas?

A

Gases that are lighter than air

46
Q

Colour of Copper (||)carbonate

A

Green powder

47
Q

Describe how Thermal Decomposition can be used to prepare Carbon dioxide

A

Thermal decomposition of Metal Carbonates

Heat the Metal Carbonate and collect the Carbon dioxide Gas

48
Q

Describe how dilute Acids can react with Calcium Carbonate to Produce Carbon Dioxide.’

A

Calcium Carbonate (Marble chips) is put in the bottom of a flask and dilute Hydrochloric acid is added
The dilute HCL Reacts with the Calcium carbonate to produce calcium chloride, water and carbon dioxide gas.
C02 collected in gas syringe

49
Q

Describe the Test for Flame Tests.

A

Clean a platinum wire loop by dipping it in some dilute HCL and then holding it in a flame. Once you hold the loop in the flame and it burns without any colour you can dip it into the sample you want to test then put it back into the flame

50
Q

Flame test colours for lithium Sodium Potassium and Calcium

A 
Lithium = Crimson red flame 
Sodium = Yellow - Orange flame
Potassium = Lilac
Calcium = brick-red flame
51
Q

A solution has had sodium hydroxide added to it and a blue precipitate forms. What is the metal ion present?

A

Copper (||) Cu2+

52
Q

A solution has sodium hydroxide added to it. It forms a sludgy green precipitate. What is the metal ion present?

A

Iron (||) Fe2+

53
Q

A solution has sodium hydroxide added to it. A reddish brown precipitation. What is the metal ions present?’

A

Iron (|||) Fe3+

54
Q

Test for ammonia

A

Turns damp red litmus paper blue

55
Q

How to test if ammonium had is in a substance?

A

Add some sodium hydroxide solution and if ammonia is given off ammonium ions are present.

56
Q

Test for chlorine

A

Bleaches damp litmus paper - turning it white.

57
Q

Test for Oxygen

A

Re lights a glowing splint

58
Q

Test for C02

A

Turns limewater cloudy - just bubble a had through a test tube of limewater

59
Q

Test for Hydrogen

A

Makes a squeaky pop with s lighted splint. Noise come from the Hydrogen brining with the oxygen In The air to form H20

60
Q

Test for Water

A

Add anhydrous copper (||) Sulfate and see if the White powder turns blue.
Isn’t pure

61
Q

Testing for Pure Wate

A

Boil at 100 degrees

Freeze at 0 degrees

62
Q

Test for Carbonates

A

Add dilute HCl to your sample then if Carbonates are Present Carbon Dioxide will be given released. CO2 Can be tested using limewater

63
Q

Test for Sulfate

A

Add dilute HCl then Barium Chloride solution
HCL added to get rid of any traces of carbonate or Sulfite ions
Gives a white precipitate

64
Q

Test for halides

A

Add Dilute Nitric Acid
Then Silver nitrate solution
Acid added to get rid of carbonate of Sulfite ions

65
Q

Precipice of Chloride, Bromide, Iodide ions?

A

White precipitate = silver chloride
Cream precipitate = bromide
Yellow precipitate = silver iodide

66
Q

What is a hydrated salt

A

Their lattices contain water molecules as well as positive and negative ions

67
Q

What are the electrodes made from in electrolysis?

A

Inert (unreactive) material so they don’t take part in the reaction

68
Q

Properties of the same elements, have similar what?

Why is this?

A

Similar chemical properties

Have the same number of electrons on the outer shell

68
Q

As the atomic number of halogens increase.. What happens?

A

The elements have a darker colour and a higher boiling point (which is why they go from gases at the op to solids at the bottom?

68
Q

Why is it that the higher up an element is in group 7, the more reactive it is?

A

The shell with the missing electron is nearer to the nucleus so the pull from the positive nucleus is greater

68
Q

Why are the elements in group 1 more active as you go down?

A

The outermost electron is in a shell that’s further from the nucleus
The attraction between the outermost electron snc the nucleus becomes less
As you go down group 1, the atoms get bigger, the outer electrons is more easily lost and the metals are more reactive

Chemistry (5 decks)

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