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Chemistry Unit 1 > 1 Formulae, equations and amounts of substance > Flashcards

1 Formulae, equations and amounts of substance Flashcards

1
Q

What is the formula for sulphuric acid?

A

H2SO4

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2
Q

What is the formula for nitric acid?

A

HNO3

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3
Q

What is the formula for hydrochloric acid?

A

HCL

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4
Q

What is the formula for carbonic acid?

A

H2CO3

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5
Q

What is the formula for ethanoic acid?

A

CH3COOH

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6
Q

What is the formula for sodium hydroxide?

A

NaOH

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7
Q

What is the formula for magnesium oxide?

A

MgO

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8
Q

What is the formula for calcium oxide?

A

CaO

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9
Q

What is the formula for copper hydroxide?

A

Cu(OH)2

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10
Q

What is the formula for copper nitrate?

A

Cu(NO3)2

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11
Q

What is the formula for potassium nitrate?

A

KNO3

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12
Q

What is the formula for zinc nitrate?

A

Zn(NO3)2

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13
Q

What is the formula for lead nitrate?

A

Pb(NO3)2

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14
Q

What is the formula for silver nitrate?

A

AgNO3

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15
Q

What is produced when an acid and a metal react together?

A

SaltHydrogen

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16
Q

What is produced when an acid and a base react together?

A

SaltWater

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17
Q

What is produced when an acid and a metal carbonate react together?

A

SaltWaterCarbon dioxide

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18
Q

What is produced when 2 soluble salts react together?

A

Insoluble saltSoluble salt

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19
Q

What are the solubility rules?

A

•All sodium, potassium, ammonium salts dissolve•All nitrates are soluble•Sulphates are soluble except lead, barium, calcium•Chlorides, bromides and iodides are soluble except lead and silver•Oxides, carbonates, hydroxides are insoluble except sodium, potassium, ammonium

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20
Q

What is a redox reaction?

A

When both oxidation and reduction happen in one reaction

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21
Q

What is Avogadro’s number and what can it be used for?

A

6x10(23)particles per mol

The number of molecules in one mole

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22
Q

What is the equation for the number of moles?

A

Mass in g/ mass of 1 mole

23
Q

When reacting iron and copper sulphate, which iron is used? 1.1.7

A

Copper (II) sulphate

24
Q

What are the possible sources of errors when reacting iron and copper sulphate? 1.1.7

A

•Didn’t decant 3 times•Not getting all of the copper out of the beaker•Copper or iron sulphate could have been left on the filter paper

25
Q

What is the volume of 1 mole?

26
Q

Why is 24dm(3) a good approximation for the volume of a gas at room temperature?

A

The size of the molecules do not have a major effectNearly all of a gas at R.T.P is space

27
Q

What is the equation for working out number of moles in a gas?

A

Volume gas dm(3)/ volume of 1 mole 24dm(3)

28
Q

What is 1 dm(3) in cubic cm?

29
Q

What is ‘the Water of Crystallisation’?

A

When metal salts crystallise from aqueous solutions they trap water molecules within the crystal lattice

30
Q

What has to be taken into account when weighing crystals?

A

The Water of Crystallisation

31
Q

What is stoichiometry and how do you find it out?

A

The ratio of salt to to water moleculesLook it up as it’s not predictable

32
Q

What is the definition for empirical formula?

A 
The simplest formula of for a compound showing the whole number ratio of the number of atoms of each element present
Butane C(2)H(5)
33
Q

What does the molecular formula tell you?

A

How many atoms bonded together in one molecule

For butane C(4)H(10)

34
Q

What is structural formula?

A 
Representation of the molecular structure, showing how atoms are arranged and bonded
Butane CH(3)CH(2)CH(2)CH(3)
35
Q

What does the displayed formula show you?

A 
All the bonds in the molecule as individual lines
Methane
     H
      |
H- C-H
      |
     H
36
Q

What is the definition of an element?

A

A substance that cannot be broken down chemically into simpler substances

37
Q

What are spectator ions?

A

Ions that appear in exactly the same way on each side of the equation

38
Q

How do you work out how many atoms there are in a certain mass of a substance?

A

Divide mass of each element by its molecular mass

Times by Avogadro’s constant

39
Q

What does STP stand for?

A

Standard temperature and pressure

1atm 298K gases at 24dm(3)

40
Q

What does the overall ionic equation not include?

A

Spectators

41
Q

What is a solution?

A

A solute (solid, liquid or gas) dissolved in a solvent

42
Q

What is the units for concentration?

43
Q

How do you make a solution of accurate concentration?

A

Dissolve the way to sell you in a small quantity of solvent

Add more solvent until the solution is the right volume

44
Q

What does molarity mean?

A

Another word for concentration in moles per decimetre cubed

45
Q

What is a molar solution?

A

A solution of concentration 1moldm(-3)

46
Q

What are parts per million (ppm) of often used for?

A

Levels of pollutants in the air or water

47
Q

Why is the percentage yield of experiments rarely 100%?

A 
Reactants may not be pure
Equilibrium reaction
Product left behind an apparatus
Volatile products may evaporate
Human error
48
Q

What does good atom economy mean?

A

The reaction is very efficient at turning reactants into desired products with little waste

49
Q

What is the definition of a mole?

A

The amount of substance that contains as many particles are as there are in exactly 12 g of carbon 12

50
Q

What is molar volume?

A

One mole of any gas must occupy the same volume under the same conditions

51
Q

Why is relative atomic mass used for ions?

A

Atoms lose all gain electrons which have no mass

52
Q

What does relative molecular mass (Mr) mean?

A

The sum of the relative atomic masses in covalent compounds

53
Q

How can you experimentally work out the proportions in which compounds react together?

54
Q

What is Avagadro’s law?

A

Equal volumes of all gases contain equal numbers of molecules provided that they are at the same temperature and pressure

Chemistry Unit 1 (7 decks)

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