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AS Level Chemistry > General Chemical Skills > Flashcards

General Chemical Skills Flashcards

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0
Q

Define atom.

A

The smallest electrically neutral particle of an element that can take part in chemical change.

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1
Q

Define ion

A

An atom or group of atoms, which carries an electrical charge.

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2
Q

Define relative atomic mass

A

The ratio of the average mass of one atom of an element to one twelfth of the mass of an atom of carbon 12

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3
Q

Define compound

A

A substance formed when two or more chemical elements are chemically bonded together.

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4
Q

Define molecule.

A

The smallest electrically neutral particle of an element or compound that can exist on its own.

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5
Q

Define Avogadro’s number.

A

It is equal to 6.02 X 10^23 and it is the number of the carbon atoms to be found in 12 grams of carbon twelve

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6
Q

Define relative formula mass

A

The sum of the masses of the elements in the formula or compound

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7
Q

What does a I, II or III mean about the charge of an ion?

A

It is a +1 +2 or +3 charge.

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8
Q

What does an element ending with ide mean. E.g. Nitride, chloride

A

It is just the element.

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9
Q

What is the charge of phosphate?

A

-3

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10
Q

What does a V, VI or VII mean?

A

A -3, -2 or -1 charge

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11
Q

What is the equation of phosphate?

A

PO(4)

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12
Q

What does -ate mean at the end of an element? E.g. Chlorate, sulphate or carbonate?

A

Bonded with oxygen.

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13
Q

What is the charge of sulphate?

A

-2

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14
Q

What is the equation of sulphate ?

A

SO(4)

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15
Q

What is the equation of carbonate?

A

CO(3)

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16
Q

What is the charge of carbonate ?

A

-2

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17
Q

What is the charge of hydroxide?

A

-1

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18
Q

What is the equation of hydroxide ?

A

OH

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19
Q

What is the charge of nitrate?

A

-1

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20
Q

What is the equation of nitrate?

A

NO(3)

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21
Q

What is the charge of chlorate ?

A

-1

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22
Q

What is the equation of chlorate?

A

Cl O(3)

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23
Q

What is the charge of bromate?

A

-1

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24
Q

What is the equation of bromate ?

A

BrO(3)

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25
Q

What is the charge of iodate?

A

-1

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26
Q

What is the equation of iodate?

A

IO(3)

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27
Q

What is the charge of hydrogen carbonate?

A

-1

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28
Q

What is the equation of hydrogen carbonate?

A

HCO(3)

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29
Q

What is the equation for ammonium ?

A

NH(4)

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30
Q

What does mono or di hydrate mean?

A

It means a number of water molecules.

If you ever have it in an equation, put a . and the number of water molecules. E.g. .4H(2)O

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31
Q

What is the equation of hydrochloric acid?

A

HcL

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32
Q

What is the equation of nitric acid?

A

HNO(3)

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33
Q

What is the equation of phosphoric acid?

A

H(3)PO(4)

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34
Q

What is the equation of carbonic acid?

A

H(2)CO(3)

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35
Q

What is the equation of ethanoic acid?

A

CH(3)COOH

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36
Q

Are compounds containing group 1 elements soluble or insoluble?

A

Soluble

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37
Q

Are ammonium salts soluble or insoluble?

A

Soluble

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38
Q

Are nitrate salts soluble or insoluble?

A

Soluble

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39
Q

Are chlorate salts soluble or insoluble?

A

Soluble

40
Q

Are chloride, bromide and iodine salts soluble or insoluble?

A

Soluble apart from the ones containing Ag+, Pb2+ and Hg(2)2+ ions

41
Q

Yes apart from the ones containing Ag+, Pb2+ and Hg(2)2+ ions

A

Are chloride, bromide and iodine salts soluble or insoluble?

42
Q

Are sulphate compounds soluble?

A

Yes apart from Ba2+ , Sr2+ , Ca2+, Pb2+ and Hg2+ ions

43
Q

Yes apart from Ba2+ , Sr2+ , Ca2+, Pb2+ and Hg2+ ions

A

Are sulphate compounds soluble?

44
Q

Are hydroxide compounds soluble ?

A

No, apart from the ones containing group one metals and Ba2+ Ca2+ and Sr2+ ions

45
Q

No, apart from the ones containing group one metals and Ba2+ Ca2+ and Sr2+ ions

A

Are hydroxide compounds soluble ?

46
Q

Are sulfide compounds insoluble or soluble ?

A

Insoluble apart from ones containing group one and group two metals.

47
Q

What is one ppm?

A

1 mg (0.001g) per kilogram
1g per metric tonne.
It is also 0.0001% and 10000ppm is 1%

48
Q

What is the test for ammonium gas?

A

Get damp red litmus paper and it will then blue.

49
Q

What is the test for Cl”2” , SO”2” and NO”2”?

A

It turns damp blue litmus paper, red then is bleaches it.

50
Q

Define redox reaction.

A

Reduction and oxidation occur simultaneously. By exchanging electrons

51
Q

Define displacement reaction.

A

Where entities are exchanged.

52
Q

Define neutralisation reaction.

A

Interaction of protons and hydroxide ions to form water.

53
Q

What is the chemical test for water?

A

CoCl”2” paper will turn white to blue.

54
Q

What is an isotope?

A

Atoms with the same number of protons but a different number of neutrons.

55
Q

What is relative isotopic mass?

A

It is the mass of an atom of an isotope of an element relative to mass of the mass of an isotope of carbon 12

56
Q

How is the number of moles found with the number of particles?

A

No. Of moles= number of particles you have

Number of particles in a mole

57
Q

What is the molar mass?

A

The mass of one mole of something. It is measured in grams.

58
Q

What is 1 dm cubed?

A

1 litre or 1000 cm cubed.

59
Q

What is the equation linking moles, mass and molar mass?

A

Number of moles = mass / Molar mass

60
Q

How is the molecular formula found from the empirical formula and the mass?

A

Divide the true mass by the empirical mass and then multiply the result by the empirical formula.

61
Q

A chemical has a formula of C”4”H”3”O”2” and a molecular mass of 166g. Find the molecular formula.

A

The empirical mass is 83.
166/83 is 2.
Multiply the empirical mass by 2 giving, C”8”H”6”O”4”

62
Q

When a hydrocarbon is burnt with an excess of oxygen, 4.4 g of carbon dioxide and 1.8 g of water are made. What is the empirical mass of the hydrocarbon?

A

When calculated, there are 0.1 moles of hydrogen and CO2 produced.
This means there are 0.1 moles of carbon and 0.2 moles of hydrogen.
This means the C:H ratio is 0.1:0.2 so the molecular formula is CH”2”

63
Q

what is room temperature and pressure?

A

298 K and 101300 Pa

64
Q

What is the volume occupied by 1 mole of gas at r.t.p?

A

24dm cubed.

65
Q

How may moles are there in 6 dm cubed of oxygen gas?

A

6/24 = 0.25 moles.

66
Q

How can the number of moles be calculated from the volume of the gas?

A

Number of moles = volume cm³

24000

67
Q

What is a double salt?

A

It contains 2 cations or anions.

68
Q

What is atom economy?

A

Molecular mass of desired product ÷ sum of molecular masses of all products X 100

69
Q

What reactions have an atom economy of 100%?

A

Addition reactions as only one product is formed and this is the useful one.

70
Q

Are carbonate salts soluble ?

A

No apart from the group one ions.

71
Q

What is a spectator ion?

A

Species that don’t change state and aren’t included in ionic equations.

72
Q

What is the gas constant ?

A

8.31 JK^-1 K^-1

73
Q

What is the equation for gases and pressure ?

A 
PV=nRT
Pressure NM² 
Volume DM³ 
No of moles
Gas constant.
Temperature, (K)
74
Q

What are the general trends on heating nitrates?

A

Generally the metal oxide, brown fumes of NO₂ and O₂ gas are produced.
For group one metals that aren’t lithium, no NO₂ is produced.
The further down the table, the more energy is needed.

75
Q

What is the general trend on heating carbonates ?

A

CO₂ and the metal oxide will be produced.
This won’t work with group 1 metals other than lithium as bunson burners won’t reach those temperatures.
The lower down, the greater the energy needed.

76
Q

What are the 3 definitions of oxidation?

A

The loss of electrons.
The loss of hydrogen
The gain of oxygen.

77
Q

What metals will acids react with?

A

Ones less reactive than hydrogen.

78
Q

What happens when acid is mixed with water ?

A

They will fall apart to form positive hydrogen ions and the rest of the acid will form a negative ion.

79
Q

What happens when CoCl₂∙6H₂O is heated?

A

It is a purple powder. When heated water vapour is produced and blue CoCl₂ is produced. It can dissolve in its own water

80
Q

Explain the thermal decomposition of Cu(NO₃)₂∙2H₂O

A

The blue powder will emit water vapour. Oxygen gas will also be emitted. Nitrogen oxide will also be produced. The end result is black copper oxide.

81
Q

Explain the thermal decomposition of NaNO₃

A

It is a white powder to start. It will melt and then oxygen gas will bubble through it.

82
Q

Explain the thermal decomposition of ZnCO₃.

A

It begin with it is a white powder. This will decompose to zinc oxide. This is yellow while hot but white when cool.
CO₂ gas is also produced.

83
Q

What does isoelectric mean?

A

A pair of ions will be isoelectric if they have the same no.of electrons.

84
Q

What is a hydride?

A

A single type of atom bonded to hydrogen. NH₃ is a hydride.

85
Q

When you have copper sulfate-5-water in solution and you are boiling it to form crystals, how do you know when to stop?

A

As you heat, put a glass rod into the solution. If when you take it out, I t has crystals on it, stop boiling.

86
Q

What are cations and anions?

A

Anions are negative while cations are positive.

87
Q

What is the charge of ammonium?

A

+1

88
Q

What is the charge of a silver ion?

A

1 plus

89
Q

If you were to spill acid, what do you do?

A

Rinse with lots of water. Add some hydrogen carbonate and mop up

90
Q

What is a functional group?

A

Part of the molecule which determines how it will react/ group of atoms responsible for chemical properties.

91
Q

What is the difference between hazard and risk?

A

A hazard is something that could cause harm e.g. fire a murderer.
A risk is the likely hood that someone could be harmed.

92
Q

Define mole

A

the amount of any substance containing the same number of identical entities as there are in exactly 12 g of the carbon-12 isotope.

93
Q

How does an acid become a salt?

A

The H⁺ ion is replaced by a metal or ammonium acid.

94
Q

What is an alkali?

A

A soluble base that releases OH⁻ ions in aqueous solution.

95
Q

Acid + base =

A

Salt and water.

96
Q

Acid and carbonate=

A

Salt, water and carbon dioxide.

97
Q

Acid and metal=

A

Salt and hydrogen.

AS Level Chemistry (16 decks)

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