Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Edexcel IGCSE Chemistry > Section 2: Chemistry of the Elements > Flashcards

Section 2: Chemistry of the Elements Flashcards

You may prefer our related Brainscape-certified flashcards:
Periodic Table flashcards Chemistry 101 flashcards AP® Chemistry flashcards Organic Chemistry 101 flashcards
1
Q

Define isomer

A

Two or more compounds with the same molecular formula but a different structural formula

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

Name 3 indicators

A

Phenolphthalein, metyl orange, universal indicator

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

What groups of the periodic table are the following in:
The halogens
The alkali metals
The noble gases

A

halogens - 7
alkali metals - 1
noble gases - 8/0

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

What is a group and period in the periodic table

A

A column is a group and a row is a period

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

What pH are the oxides of metals and non-metals?

A

Metal oxides are usually alkaline, non-metal oxides are usually acidic

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Why do elements in the same group have similar chemical properties?

A

They have the same number of electrons on the outer shell

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Why are the noble gases unreactive?

A

They have a full outer shell

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Why are the group 1 metals so reactive?

A

They only have 1 electron in the outer shell. It is easy to lose this one electron so they are reactive

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

What are the word and balanced symbol equations for the reactions of the three group 1 metals with water?

A

lithium + water –>lithium hydroxide and hydrogen
2 Li(s) + 2 H20(l) –>2 LiOH (aq) + H2(g)
sodium + water –> sodium hydroxide and hydrogen
2 Na(s) + 2 H20(l) –>2 NaOH (aq) + H2(g)
potassium + water –>potassium hydroxide and hydrogen
2 K(s) + 2 H20(l) –>2 KOH (aq) + H2(g)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Observations for lithium reacting with water

3 things

A

Lithium floats, effervesence,dissolves as it reacts

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

Observations for sodium reacting with water (4 things)

A

Sodium melts into ball, moves around surface of water, effervesence, burns orange flame until it disappears

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

Observations for potassium reacting with water (5 things)

A

potassium melts into ball, floats around surface of water, ignites instantly, lilac flame with sparks, sometimes small explosion before it disappears

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

What is thetrend in reactivity of Group 1? Why?

A

As you go down the group, the elements become more reactive. This is because there more shells of electrons and the outer electron is further from the nucleus, the attraction between electron and nucleus is then weaker and therefore easier to lose

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

What is the charge on a group 1 ion? Why?

A

Group 1 metals lose 1 electron so form an ion with a single positive charge

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

What are the Electronic configurations of lithium, sodium and potassiumas a regular element and ion

A

Li Normal: 2.1 Ion: 2
Na Normal: 2.8.1 Ion: 2.8
K Normal: 2.8.8.1 Ion: 2.8.8

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

Give equations to show how lithium, sodium and potassium become ions?

A

Li –> Li+ + e-
Na –> Na+ + e-
K –> k+ + e-

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

The harder it is to extract the more/less reactive the metal is

A

more

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

A metal that is oxidised in a reaction is called the ______ agent?

A

Reducing

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

What is another name for iron (III) oxide?

What conditions does iron rust in? (two things)

How can rusting be prevented?
(4 things)

A

Rust.

When it is in contact with oxygen and water

Galvanising, painting, coating, oiling

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

What type of reaction is when the more reactive metal takes a least reactive metals place in a compound?

A chemical reaction in which a compound is broken down into two or more smaller substances?

What is a redox reaction?

A

Displacement

Decompositon

A reaction where both reduction and oxidation take place

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

General Equation for reacting a metal with an acid is?

A

Acid+Metal—>Salt+Hydrogen

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

Which metal is more reactive? Lithium, Copper, or Zinc?

A

Lithium

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

What are reactants in the thermite reaction?

A

Aluminium and iron oxide

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

Why does aluminium not corrode as quickly as steel and iron?

A

It has a protective oxide layer

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

Which metal is often used for sacrifical protection of iron?

A

Magnesium

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q

What gases are present in air? (4 main ones) and give their percentages

A

Nitrogen, Oxygen, Argon and Carbon Dioxide.

78% N2, 21% O2, 0.9% Ar and 0.03% CO2.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q

How canexperiments involving the reactions of elements be used to investigate the percentage by volume of oxygen in air?

A

Copper, iron and phosphorus all react with the oxygen in air. If you know the volume of air that you have, then react it with on of these, then re measure the volume of air; what has been lost is all oxygen that reacted.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
28
Q

What environmental issue is associated with carbon dioxide?

A

Greenhouse effect and global warming.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
29
Q

Describe the solubility and density of carbon dioxide.

A

Denser than air, soluble in water at high pressure.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
30
Q

What is produced when calcium carbonate is heated strongly?

A

Calcium oxide and carbon dioxide.

31
Q

Which word best describes magnesium oxide?

acid, neutral, alkali, base

A

Base

32
Q

Describe the reaction of magnesium with oxygen.

A

Burns very brightly and at a very high temperature. Magnesium metal turns into a white powder

33
Q

What observations could be made from burning sulfur?

A

Strong blue flame, poisonous and colorless gas is produced.

34
Q

Name the products of each of these reactions Hydrochloric acid + Magnesium ->
Hydrochloric acid + Aluminium ->
Hydrochloric acid + Zinc ->
Hydrochloric acid + Iron ->

A

Magnesium Chloride +Hydrogen
Aluminium Chloride + Hydrogen
Zinc Chloride + Hydrogen
Iron Chloride + Hydrogen

35
Q 
Name the products of each of these reactions 
Sulfuric Acid +Magnesium ->
Sulfuric Acid +Aluminium ->
Sulfuric Acid +Zinc ->
Sulfuric Acid +Iron ->
A

Magnesium Sulfate + Hydrogen
Aluminium Sulfate + Hydrogen
Zinc Sulfate + Hydrogen
Sulfuric Acid + Hydrogen

36
Q

Are Acid + Metal reactions endothermic or exothermic?

A

Exothermic

37
Q

Hydrogen + Oxygen ->

A

Water

38
Q

Is combustion of hydrogen exothermic or endothermic?

A

Highly Exothermic

39
Q

What is the colour of Anhydrous copper sulphate and hydrated copper sulphate?

A

White and then blue

40
Q

Describe a physical test to show whether water is pure.

A

If water boiled/evaporated, container is left clean, and the water boils at 100oC

41
Q

Describe the exothermic / endothermic nature of the reversible reaction of copper sulphate and water

A

In the forward direction (water and anhydrous copper sulphate reacting) it is exothermic and in the backward direction (decomposition of the hydrated copper sulphate) it is endothermic

42
Q

What are the similar properties of the transition metals? (6 things)

A

They are strong with high melting points, yet are malleable, ductile and sometimes lustrous. They all conduct electricity.

43
Q

How many electron shells are present in caesium?

A

There are six.

44
Q

Describe the following elements at room temperature

chlorine
bromine
iodine

A

chlorine - A greenish-yellow gas.
bromine - A red-brown liquid.
iodine - Solid, shiny, purple crystals.

45
Q

List the Group 7 elements in order of reactivity.

A

Flourine, Chlorine, Bromine, Iodine, Astatine

46
Q

What happens when a more reactive halogen reacts with a compound containing a less reactive halogen?

A

The less reactive halogen is displaced.

47
Q 
Describe a flame test and identify the colours the following would make a flame:
lithium
sodium
potassium
calcium
A 
dip a clean flame test loop in the sample solution, hold the flame test loop at the edge of a bunsen burner flame, wash with acid in between test
lithium - red
sodium - yellow-orange
copper - blue-green
potassium - lilac
calcium - orange-red
48
Q 
How do you test for the following gases:
chlorine
ammonia
carbon dioxide
oxygen
hydrogen
A

chlorine - Turns litmus paper red before bleaching it
ammonia - damp red litmus paper should turn blue if ammonia is present
carbon dioxide - limewater test- should turn milky
oxygen - relights a glowing splint
hydrogen - squeaky pop test

49
Q

Sodium hydroxide will produce what colour precipitate with the following ions

Fe2+
Fe3+
Cu2+
NH4+ (ammonium)

A

Fe2+ green, turns orange/brown over time
Fe3+ orange/brown
Cu2+ pale blue
NH4+ (ammonium) put red litmus paper at the end of the test tube and it should turn blue (gently heat tube sometimes required)

50
Q

How do you test for Halide’s?

A

The test solution is acidified using a few drops of dilute nitric acid, and then a few drops of silver nitrate solution are added.
White = chlorine
cream = bromine
yellow = iodine

51
Q

How do you test for the following ions:

carbonate ion (CO32-)

sulphate ion (SO42-)

A

React with acid, there will be effervescence which is carbon dioxide.

The test solution is acidified using a few drops of dilute hydrochloric acid, and then a few drops of barium chloride solution are added. A white precipitate of barium sulfate forms if sulfate ions are present.

52
Q

Describe the trend in the reactivity of the Group 7 elements

A

The Group 7 elements become more reactive as you go up the group. This is because there are less shells of electrons, so an electron that will be gained is closer to the nucleus. The means that attraction between the nucleus and electron is greater and so the electron is more easily gained.

53
Q

What is the difference in mining unreactive and reactive elements?

A

Unreactive elements (gold, silver) can be mined as the element, whereas reactive elements will have formed compounds (iron oxide) which need to be mined and then the metal extracted from the compound.

54
Q

What are the pH’s of the following types of substances:
Acids
Neutral
Alkalis

A

Acids - pH 1-6. Neutral - pH 7. Alkali - pH 8-14

55
Q

Give the colours of the indicators litmus, phenolphthalein, universal indicator and methyl orange in acid and alkaline solutions

A

Litmus - Acid = red, alkali = blue.

Phenolphthalein - acid = colourless, alkali - pink.

Universal Indicator - strong acid = red, strong alkali = purple

Methyl orange - acid = red, alkali = yellow

56
Q

What are the ions that make a substance acidic or alkaline?

A 
H+ = acidic.    
OH- = alkaline
57
Q 
Complete the following general equations:  
Metal + Acid ->
Metal oxide (base) + acid->
Metal hydroxide (alkali) + acid ->
Metal carbonate + acid ->
A

Metal + Acid -> Salt + Hydrogen
Metal oxide (base) + acid-> Salt + Water
Metal hydroxide (alkali) + acid -> Salt + Water
Metal carbonate + acid -> Salt + Water + Carbon Dioxide

58
Q

What are the rules for solubility of salts? (sodium, potassium, ammonium, nitrates, chlorides, sulphates, carbonates

A

Sodium, potassium ammonium, nitrates - all soluble.

chlorides - all except silver
sulphates - soluble except barium and calcium
carbonates - insolube except sodium, potassium and ammonium.

59
Q

Describe an experiment to form a soluble salt from an acid and an alkali

A

Carry out a titration using indicator to determine the exact amount of alkali needed to neutralise the acid. Repeat the process without indicator using exactly the same volume of alkali. Evaporate the water from the mixture to leave the salt behind

60
Q

Describe an experiment to form a soluble salt from an acid and a base

A

React a solution of the acid with base. Once you add base and it does not dissolve as it reacts then all of the acid must have reacted. Filter the mixture to remove excess base and then evaporate the wate to leave just the salt

61
Q

Descirbe an experiment to form an insoluble salt using a precicpitation reaction

A

For example silver choldride is an insoluble salt- to form you need a soluble silver salt and a soluble chloride salt. Silver nitrate and sodium chloride are both soluble salts and when combinded form soluble sodium nitrate and insoluble silver chloride.The silver chloride forms as tiny particles in the mixture- forms a precipitate. The precicpitate can be washed, rinsed with water and left to dry on the filter paper.

62
Q

Describe how to carry out a titration

A

Use a pipette and add 25cm^3 of alkali to a clean conical flask. Add indicator to the akali solution and place on a white tile, which allows for colour to be easily seen. Fill the burette with acid and note the starting volume. Slowly add the acid to the alkali while swirling the mixture. Stop adding the acid when the end point is reached (final colour is achieved) and record the volume left on the burette. To calculate how much acid was used take the final volume from the starting volume. Continue to repeat the steps till your readings are consistent.

63
Q

How is the method of extracting a metal determined?

A

Metals below carbon in the reactivity series can be extracted by reduction with carbon (Zinc, iron, tin, lead).

Metals above carbon have to be extracted by electrolysis

64
Q

Describe the process of extracting via reduction

A

The metal oxide is heated in the presence of carbon or carbon monoxide to be reduced to the pure metal

65
Q

Give one particular property of aluminium and iron and suggest a use for it based on that property

A

Aluminium has a low density and is used for aircraft. Iron has a high tensile strength so is used for buildings

66
Q

Describe the corrosion resistance of iron and aluminium

A

Iron corrodes easily (and is called rust) when it comes into contact with water and oxygen, and this layer is brittle.

Aluminium forms a more solid oxide layer on its surface which prevents further corrosion

67
Q

What are the raw materials in the Haber Process, and how are they obtained?

A

nitrogen from air and hydrogen from reactions of natural gas with steam

68
Q

What are the conditions for the Haber Process (T, P and cat?)

A

Temperature - 450oC. Pressure - 200 atm. Catalyst - Fe

69
Q

How is ammonia separated from the products?

A

The reaction mixture is cooled and ammonia condenses. Nitrogen and hydrogen have lower boiling points so remain as gases.

70
Q

What are the uses of ammonia? (3)

A

fertilisers,nitric acid and cleaning products

71
Q

Explain the temperature of the Haber Process

A

The temperature of 450oC is high to inncrease the rate of the reaction but not so hugh that it reduces the yield too much. It is a compromise

72
Q

Explain the pressure of the Haber Process

A

The pressure of 200 atm is high to increase rate and yield but not so high as it is very expensive and can be dangerous

73
Q

What is the equation for the Haber Process?

A

N2 + 3 H2 ⇌ 2 NH3

74
Q

Describe the electrolysis of sodium chloride solution, including its products and the uses for each product.

A

Concentrated sodium chloride is electrolysed in a diaphragm cell to produce hydrogen (fuel, chemical synthesis), chlorine (bleach, disinfectant) and sodium hydroxide (soap)

Edexcel IGCSE Chemistry (4 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions