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Chemistry IGCSE > Unit 3 - Stoichiometry > Flashcards

Unit 3 - Stoichiometry Flashcards

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1
Q

Molecular formula

A

The number and type of different atoms in a molecule e.g. CO2

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2
Q

Empirical formula

A

Simplest whole number ratio for different atoms e.g. H2O2 = OH

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3
Q

Valency

A

Number of electrons gained or lost

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4
Q

Valency of all groups

A
  • Group I = 1
  • Group II = 2
  • Group III = 3
  • Group IV = 4
  • Group V = 3
  • Group VI = 2
  • Group VII = 1
  • group VIII = 0
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5
Q

Ionic compound features

A
  • Ions are charged to get full outer shells
  • Compounds final charge must be neutral e.g. k+ + F- = KF
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6
Q

Word equation

A

Chemical names of all reactants and products

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7
Q

Symbol equation

A

Names of substances are replaced by element symbols

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8
Q

Polyatomic ions

A

Ions that have more than one element, e.g. SO4, covalently bonded but unequal protons and electrons

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9
Q

Charges of polyatomic ions

A
  • Hydroxide/OH = 1-
  • Carbonate/CO3 = 2-
  • Chlorate/ClO4 = 1-
  • Nitrate/NO3 = 1-
  • Sulfate/SO4 = 2-
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10
Q

Law of conservation of mass

A

In a reaction the mass of the reactants will equal the mass of the products - mass is conserved

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11
Q

State symbols

A
  • Solid = (s)
  • Liquid = (l)
  • Gas = (g)
  • Aqueous = (aq)
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12
Q

Notation for multiple molecular ions

A

Brackets around ion with amount e.g. Al(NO3)3

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13
Q

Ammonium

A

NH4 = 1+

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14
Q

Ammonia

A

NH3

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15
Q

Relative atomic mass

A

Every atom’s mass is relative to 1/12th of carbon - 12

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16
Q

Symbol for relative atomic mass

A

Ar

17
Q

Relative molecular mass

A

The mass of all atoms in a compound or molecule - can be used for ionic compounds

18
Q

Symbol for relative molecular mass

A

Mr

19
Q

Avogadro’s constant

A

1 mole of a substance has 6.02 x 10^23 atoms in it

20
Q

Relationship with moles and Ar or Mr

A

1 mole of a substance is weighs its Ar or Mr in grams e.g. 1 mole of H20 = 18g

21
Q

Mole, mass and Mr equation

A
  • Mass = Moles x Mr
  • Moles = Mass ÷ Mr
  • Mr = Mass ÷ Moles
22
Q

Molar gas volume law

A

Under same temperature and pressure conditions, equal volumes of different gasses contain an equal number of molecules

23
Q

Molar gas volume constant

A

1 mole of a gas = 24dm^3 = 24000cm^3 = 0.024m^3

24
Q

Room temperature and pressure conditions

A

25˚C and 1 atmospheric pressure

25
Q

moles and gas volume equation

A
  • Moles = Gas volume ÷ 24
  • Gas volume = moles x 24
26
Q

Concentration equation (mass and volume)

A
  • Concentration = Mass ÷ Volume
  • Mass = Concentration x Volume
  • Volume = Mass ÷ Concentration
27
Q

Molar concentration

A

The amount of moles of a substance dissolved in 1dm^3

28
Q

Concentration equation (moles and volume)

A
  • Concentration = Moles ÷ Volume
  • Moles = Concentration x Volume
  • Volume = Moles ÷ Concentration
29
Q

Titrations

A

Used for neutralizing an acid or alkali, can be used to find an unknown volume

30
Q

Limiting reagent

A

The reactant that is completely used in the reaction and controls the amount of product formed

31
Q

Excess reagent

A

The reactant that is left over at the end of the reaction

32
Q

Theoretical yield

A

Moles of product in a balanced equation

33
Q

Actual yield

A

Moles or total mass obtained experimentally

34
Q

Percentage yield

A

Percentage of theoretical yield obtained experimentally

35
Q

Percentage yield equation

A

Percentage yield = (Actual yield ÷ Theoretical yield) x 100

36
Q

Percentage purity of a substance equation

A

Percentage purity = (Mass of pure product ÷ Mass of impure product) x 100

37
Q

Steps to ionic equations

A

1.Identify solids, liquids or gases ( can’t be changed)
2.Identify the ions of the aqueous substances
3.Cross out any ions that appear on both sides of the equation
4.Rewrite the equation without including the species you crossed out

38
Q

Spectator ion

A

An ion that remains unchanged throughout a chemical reaction

39
Q

Steps to finding ratios in a compound

A

1.Find the atomic mass of each element
2.Divide the percentages of the elements in the compound by their masses
3.Divide these numbers by the smallest value to find the ratio

Chemistry IGCSE (12 decks)

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