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Eddie - IGCSE Chemistry > The Periodic table > Flashcards

The Periodic table Flashcards

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1
Q

What is a “group” in the periodic table?

A

A column of the periodic table

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2
Q

What is a “period” of the periodic table?

A

A row of the periodic table

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3
Q

Where are metals found in the periodic table?

A

To the left of the zig zag line

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4
Q

Where are non-metals found in the periodic table?

A

To the right of the zig zag line

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5
Q

What pattern happens in groups of elements?

A

They have similar properties which gradually change down the group

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6
Q

How do you know how many valency electrons an atom has?

A

The group number indicates the amount of valency electrons

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7
Q

Where are alkali metals found in the periodic table?

A

In group 1 of the periodic table?

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8
Q

What are alkali metals’ physical properties and trend in reactivity?

A

Properties - relatively soft metals, low melting points compared to most metals, low density

Trend in reactivity - increases down the group

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9
Q

How do alkali metals react with water?

A

Vigorously

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10
Q

Where are halogens found in the periodic table?

A

Group 7

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11
Q

What is a halogens molecular structure?

A

Diatomic non-metals

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12
Q

What are halogens melting points?

A

Low melting points that increase down the group

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13
Q

What are halogens trend in reactivity?

A

Decreases down the group

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14
Q

What are halogens colour and physical state?

A

Halogens get darker in colour as you go down the group: Fluorine - yellow gas, Chlorine - green gas, Bromine - Red liquid, Iodine - dark grey solid

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15
Q

What are halides?

A

Halides are compounds which contain halide ions (F-, Cl-, Br-, I-)

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16
Q

What is a halide displacement reaction?

A

Where a more reactive halogen will displace a less reactive halogen from a solution of its halide.

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17
Q

Where are transition metals found on the periodic table?

A

The block in the middle of the periodic table

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18
Q

What are transition metals properties?

A

High density, High melting points, Good conductors, Pure metals look metallic, Compounds are coloured, Variable oxidation numbers.

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19
Q

What are important uses for transition metals and their compounds?

A

Good cataylsts

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20
Q

Where are noble gases found in the periodic table?

A

Group 0

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21
Q

Describe a noble gases’ structure and reactivity

A

Noble gases have a monatomic non-metal gases structure.

They are very unreactive due to their full outer shell of electrons.

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22
Q

Uses for each noble gas

A

Helium - Filling balloons and air ships
Neon - Advertising signs
Argon - Providing an inert atmosphere, welding
Krypton - In lasers for eye surgery, in car headlamps
Xenon - In lights

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23
Q

Define what an acid is

A

A proton (H+) donor

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24
Q

Define what a base is

A

A proton (H+) acceptor

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25
Q

Define what an alkali is

A

A soluble base

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26
Q

Which ions are responsible for making a solution acidic or alkaline?

A

Acidic - H+ ions

Alkaline - OH- ions

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27
Q

What is the difference between strong and weak acids

A

Strong acids dissociate completely into ions when dissolved in water, weak acids partially dissociate

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28
Q

What is the difference between strong and weak bases

A

Strong bases dissociate completely into ions when dissolved in water, weak bases do not dissociate completely.

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29
Q

What are the hazards of working with acids and alkalis?

A

Strong acids and bases are corrosive

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30
Q

Acid + Base =

A

Salt + water

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31
Q

Acid + metal =

A

Salt + hydrogen

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32
Q

Acid + carbonate =

A

Salt + water + carbon dioxide

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33
Q

Base + ammonium salt =

A

Salt + water + ammonia

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34
Q

Equation for insoluble salt production

A

Soluble salt + soluble salt –> insoluble salt + soluble salt

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35
Q

What salts are soluble?

A

All sodium, potassium & ammonium salts
All nitrates
Chlorides except silver & lead chloride
Sulphates except calcium, barium & lead sulphates

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36
Q

What is the Ph scale

A

The scale which measures the acidity or alkalinity on a scale of 1 to 14

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37
Q

What are three indicators used for the Ph scale

A

Universal indicator - acid = red/orange/yellow alkali = blue-purple, neutral = green

Litmus = Acid = red, alkali = blue, neutral = purple

Methyl orange = acid - red, alkali - orange, neutral - yellow

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38
Q

What is neutralisation?

A

Neutralisation occurs when an acid and a base react together

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39
Q

What is an agricultural use for neutralisation?

A

Acidic soil being neutralised by a base

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40
Q

What is an acidic oxide?

A

Something that reacts with bases and dissolves in water to produce an acid.

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41
Q

What is a basic oxide?

A

Something that reacts with acids

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42
Q

What is an amphoteric oxide?

A

Reacts with both acids and bases

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43
Q

What is a neutral oxide?

A

Do not react with acids or bases

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44
Q

What does the reactivity series show

A

It shows the tendency of a metal to form its positive ion when reacting with aqueous ions or oxides of the other metals

45
Q

What is a displacement reaction?

A

When a more reactive metal will displace a less reactive metal from its oxide.

46
Q

What is a thermal decomposition of carbonates reaction?

A

When a metal carbonate is broken down in a metal oxide and water

47
Q

What is a thermal decomposition of hydroxides?

A

Where a metal oxide is broken down into metal oxide and water

48
Q

What is a thermal decomposition of nitrates?

A

Where metal nitrate goes to form metal oxide + nitrogen dioxide + oxygen

49
Q

Why is aluminium not as reactive as expected?

A

Aluminium is not as reactive as expected because it is coated in a thin film of unreactive aluminium oxide.

50
Q

What is an “oxidation” reaction

A

Where oxygen is gained
loss of electrons
increase in oxidation number

51
Q

What is a “reduction” reaction

A

Loss of oxygen
gain of electrons
decrease in oxidation number

52
Q

What is a redox reaction

A

A reaction in which both oxidation and reduction occur

53
Q

What is an oxidising agent

A

A substance which oxidises another substance in a redox reaction

It is reduced

It gains electrons

54
Q

What is a reducing agent

A

A substance which reduces another substance in a redox reaction

It is oxidised
It loses electrons

55
Q

What does “oilrig” stand for

A

Oxidation is loss, reduction is gain (of electrons)

56
Q

How does the position of a metal in the reactivity series determine the method used to extract it from its ore?

A

Unreactive metals - found native or uncombined so extraction is easy

Metals less reactive than carbon - reduction in blast furnace

Metals more reactive than carbon - electrolysis

Refining using electrolysis - some metals which are extracted by reduction may be purified using electrolysis

57
Q

Name the apparatus and raw materials of iron ore extraction. What are the four steps

A

Apparatus - blast furnace
Raw materials - Iron ore (haematite), carbon (coke), Limestone.

  1. ) Coke is burned, giving off heat and carbon dioxide
  2. ) Carbon dioxide reacts with more coke to make carbon monoxide
  3. ) Iron oxide is reduced by carbon monoxide to iron
  4. ) Limestone decomposes thermally to form calcium oxide
58
Q

What is steel

A

It is an alloy of iron with other elements

59
Q

Describe the uses of iron

A

Mild steel - constructing buildings, making vehicles

Stainless steel - making cutlery, making equipment for use in chemical factories

60
Q

Definition of electrolysis

A

The breakdown of a molten or aqueous ionic compound by electricity

61
Q

Definition of cathode

A

The electrode connected to the negative terminal of the battery

62
Q

Definition of Anode

A

The electrode connected to the positive terminal of the battery

63
Q

Definition of electrolyte

A

A liquid that contains ions and therefore conducts electricity

64
Q

Which electrodes to cations and anions move to

A

Cations move to the cathode, gain electrons

Anions move to the anode, lose electrons

65
Q

What is produced at the anode and cathode

A

Anode - non metal
2Cl- –> Cl2 + 2E-

Cathode - metals
Fe2+ + 2E- –> Fe

66
Q

What form is zinc found in naturally?

A

Zinc sulphide a.k.a Zinc blende

67
Q

List the steps to extract zinc from its compound

A

step 1.) Zinc sulphide is roasted in air to produce zinc oxide and sulphur dioxide

2ZnS + 3O2 –> 2ZnO + 2SO2

step 2.) Zinc oxide is reduced with carbon monoxide
Zn2+ + 2E- –> Zn

68
Q

What are the uses of zinc

A

Galvanising iron

Making alloys

69
Q

How is copper refined

A

Copper is refined by electrolysis

Cathode - made of pure copper
Anode - made of impure copper

electrolyte - dilute solution of copper sulphate
result - copper (99.9% pure) will be deposited at the cathode

70
Q

Uses of copper

A

Electrical wiring
Cooking utensils
Water pipes

71
Q

What form is aluminium found in naturally?

A

Bauxite (aluminium oxide)

72
Q

What are uses of aluminium

A

Manufacturing air craft
Overhead electricity cables
Making food containers

73
Q

What is Brine?

A

A concentrated solution of sodium chloride

74
Q

State the products of brine electrolysis?

A

Hydrogen gas is formed at cathode
Chlorine gas is formed at the anode
Sodium hydroxide is also left in the solution

75
Q

What are uses for the products?

A

Hydrogen - Margarine, ammonia, refrigerants
Chlorine - hydrochloric acid, Bleach, PVC, solvents, paints, medicines, weed killers, pesticides
Sodium hydroxide - Soaps, detergents, oven cleaner, biodiesel, paper, textiles, dyes

76
Q

What is “electroplating”

A

Using electricity to coat one metal with another

77
Q

How is electroplating done?

A

1.) To coat metal A with metal B pass electricity through the following cell

Cathode - Metal A
Anode - metal B
Electrolyte - a solution of a soluble compound of metal B

78
Q

Uses of electroplating

A

To make cheaper metal look better

To prevent corrosion

79
Q

What are three natural sources of sulphur

A

The pure element - underground and near volcanoes
As a compound in metal ores - e.g. galena
In fossil fuels - coal, crude oil, natural gas

80
Q

What is produced in the “contact process”

A

Sulphuric acid

Raw materials used are sulphur or sulfur dioxide, air and water

step 1.) Sulfur is burned in air to make sulfur dioxide

step 2.) SO2 is mixed with more air and passed over a vanadium oxide catalyst at 450C, 1-5 atmospheres pressure to make sulfur trioxide

step 3.) So3 is dissolved in concentrated sulfuric acid to oleum

step 4.) Oleum is mixed with water to produce concentrated sulfuric acid

81
Q

What are the properties of conc. and dilute sulfuric acid?

A

Dilute sulphuric acid shows the usual reactions of acids

Conc. sulfuric acid is a dehydrating/ drying agent - it removes water

82
Q

What are the uses of sulfuric acid?

A 
Fertilisers
Paints
Fibres
Soaps
Car batteries
83
Q

What are the uses of sulfur dioxide?

A

As a bleach in the manufacturing of wood pulp for paper

As a food preservative (kills bacteria)

84
Q

What is the composition of clean air?

A

21% oxygrn
78% nitrogen
0.04% CO2
Rest is mainly argon

85
Q

Name and explain the process used to separate air into its components

A

Fractional distillation of liquid air -

Cleaning: Air is cleaned to remove water vapour, carbon dioxide and pollutants

Liquefying: The air is cooled to -200*c

Fractional distillation: The liquid air is warmed to in a fractionating column

86
Q

What are some examples of greenhouse gases

A

Carbon dioxide and Methane

87
Q

How carbon dioxide and methane produced

A

Carbon dioxide is produced by complete combustion of carbon containing fuels

methane is produced by decomposition of vegetation and is a waste gas from digestion in animals

88
Q

What problems do green house gases cause

A

An increase in greenhouse gas levels could cause global warming which might lead to climate change

89
Q

Name four air pollutants

A

Carbon monoxide, Sulfur dioxide, Nitrogen oxides, Lead compounds

90
Q

Explain where these air pollutants come from and the problems they cause

A

Carbon monoxide - Incomplete combustion of carbon fuels, it is a toxic gas that can bind to haemoglobin which means no oxygen

Sulfur dioxide - Combustion of fossil fuels, cause raspatory issues, dissolves in rain to form acid rain

Nitrogen oxides - causes raspatory (breathing issues) and it can cause acid rain

Lead compounds - car engines using leaded petrol, damages children’s brains, damages the nervous systems of adults

91
Q

What problems does acid rain cause?

A

Dissolves limestone/ marble buildings
Lowers Ph in lakes& rivers, kills fish
Kills trees and insects

92
Q

How do catalytic converters remove pollutants remove pollutants from car exhaust fumes?

A

Converts carbon monoxide into carbon dioxide
Converts nitrogen oxides into nitrogen
Unburnt hydrocarbons into carbon dioxide and water

93
Q

What three ways is carbon transferred in the carbon cycle

A

Combustion
Respiration
Photosythesis

94
Q

How is water treated in order to make it safe to drink? list the process

A
  1. ) Screening - Water is passed through a screen, which traps large particles, e.g. twigs
  2. ) Coagulation - A coagulant is added to the water to make very fine particles stick together. These are skimmed off.
  3. ) Filtration - Water is passed through a filter of fine sand to remove any remaining small particles.
  4. ) Chlorination - Chlorine is added to kill bacteria and other microbes
95
Q

Uses for water in the home

A

Drinking, cooking, washing, flushing toilets

96
Q

Uses for water in farms

A

As a drink for animals, for watering crops

97
Q

Uses for water in industry

A

As a solvent, to wash things, for cooling, manufacture of ethanol

98
Q

Uses for water in power stations

A

heated to make steam, which turns the turbines that generate electricity

99
Q

Three ways to prevent rusting

A

Coating - coat the metal in paint or grease to prevent oxygen and water from reaching the metal surface

Sacrificial protection - A more reactive metal is attached to iron/steel so that the more reactive metal corrodes instead of the iron/steel

Galvanising - Iron/steel is coated in zinc to prevent air and water from reaching the iron/steel

100
Q

What is the chemical name and formula of limestone

A

Calcium carbonate, CaCO3

101
Q

What is the equation for the thermal decomposition of limestone and the slaking of line?

A

Calcium carbonate —> Calcium oxide + Carbon dioxide

Slaking of lime - CaO + H2O —-> Ca(OH)2

102
Q

Uses for limestone

A

Making iron

Making cement

103
Q

Uses for lime/slaked lime

A

Neutralising acidic soil

Neutralising acidic industrial waste products

104
Q

What is the Haber process

A

An industrial process for the production of ammonia from nitrogen and hydrogen

N2 + 3H2 —> 2NH3

105
Q

Where are the raw materials obtained from in the Haber process

A

Nitrogen - extracted from the air

Hydrogen - from reacting methane with steam or from cracking alkanes

106
Q

What tempurature, catalyst, pressure is required for the Haber process

A

Tempurature - 450*C
Catalyst - Iron
Pressure - 200 atmospheres

107
Q

How can the equilibrium be forced to make more ammonia?

A

The ammonia is cooled, so that it condenses into a liquid and can be removed

108
Q

Uses of ammonia

A

Fertilisers
Explosives
Cleaning products

109
Q

Why are fertilisers necessary? give four examples of fertiliser, including formulae

A

Fertilisers make crops grow bigger and faster

examples of fertiliser are Ammonium nitrate NH ₄NO ₃
Ammonium sulphate (NH₄)₂SO₄
Ammonium phosphate (NH4)3PO4
Potassium sulphate K₂SO₄

Eddie - IGCSE Chemistry (5 decks)

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