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Chemistry Paper 1 > Topic C3 - Quantitative Chemistry > Flashcards

Topic C3 - Quantitative Chemistry Flashcards

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1
Q

How do you work out isotopes?

A

Neutrons + Protons

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2
Q

How many electrons fill up each shell?

A 
1st = 2
2nd = 8
3rd = 8
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3
Q

What does one mole = ?

A

6.02 x 10^23

particles of a substance

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4
Q

The number of a moles in a sample =

A

Mass of that element or compound
——————————————————
Relative Formula Mass

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5
Q

What is a mole?

A

A unit we use to measure the amount of chemical we have.

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6
Q

What is Avogrados Constant?

A

6.02 x 10^23

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7
Q

Relative formula mass =

A

All atomic mass values added together for all the atoms in its formula

e.g CO2

Carbon = 12
Oxygen = 16.        Oxygen x2 = 32

12+32 = 44 = relative formula mass

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8
Q

Relative formula mass symbol?

A

M r

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9
Q

Relative Atomic Mass symbol

A

A r

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10
Q

Can atoms be created or destroyed in a chemical reaction?

A

No

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11
Q

In chemical reaction what happens to the total mass of the reactants and products?

A

They will both be the same.

MASS IS CONSERVED

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12
Q

How could there be a decrease in mass during a chemical reaction?

A

If a gas is made during the reaction and escapes the vessel

It’s mass is no longer accounted for.

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13
Q

How could there be an increase in mass during a chemical reaction?

A

If a gas from the air is a reactant. And so it’s mass is added to the mass in the vessel.

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14
Q

What do balanced equations tell us about moles?

A

How many moles of each substance take part in the reaction.

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15
Q

Concentration definition

A

Amount of substance dissolved in a certain volume of solution.

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16
Q

What happens to concentration when you increase the amount of solute?

A

Concentration increases when amount of solute increases.

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17
Q

What happens too concentration when the volume of solvent is increased?

A

Concentration decreases when the volume of solvent increases.

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18
Q

What is the formula for concentration?

A

Concentration

=

Mass of solute  —————————   Volume of solvent
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19
Q

What is MASH?

A

Metal + acid —> salt + hydrogen

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20
Q

What is MASH but with metal carbonate?

A

Metal carbonate + acid

—>

salt + water + carbon dioxide

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21
Q

What is PANIC?

A

Positive
Is
Anode

Negative
Is
Cathode

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22
Q

Limiting reactant definition

A

A reactant that gets completely used up in a reaction, so limits the amount of product formed.

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23
Q

How can the mass of the product be worked out with the limiting reactant.

A

1) write a balanced equation for reaction
2) divide limiting reactant mass by its relative formula mass to find the no. Of moles
3) use balanced equation to find the number of moles of the product
4) multiply that number of moles by the relative formula mass of the product to work out its mass

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24
Q

What 2 ways can pH be measured?

A

1) Universal Indicator - gives a pH colour

2) pH probe - gives accurate value of the pH

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25
Q

What colour are acids on the Ph scale?

A

Red/Yellow

26
Q

What colour are alkalis on the pH scale?

A

Blue/Purple

27
Q

What colour is neutral on the pH scale?

A

Green

28
Q

What number is neutral on the pH scale?

A

7

29
Q

What are neutralisation reactions?

A

When the products of reactions are neutral

30
Q

What does the first part of a salts name come from in a reaction?

A

Comes from the positive ion in the base, alkali, or carbonate.

e.g HCl produces: chloride salt

31
Q

How are soluble salts made?

A

By adding metals or insoluble metal compounds to acids.

Excess solid is filtered off and the remaining salt solution is crystallised.

32
Q

String acid definition

A

An acid that completely ionises in water to produce hydrogen ions

33
Q

What are examples of strong acids?

A

1) Hydrochloric acid
2) Sulfuric acid
3) Nitric acid

34
Q

Weak acid definition

A

An acid that partially ionises in water to produce hydrogen ions.

35
Q

Examples of weak acids

A

1) ethanoic acid
2) citric acid
3) carbonic acid

36
Q

What is pH definition

A

A measure of the concentration of H+ ions in a solution.

37
Q

What is acid strength a measure of?

A

The proportion of acid molecules that ionise in water

38
Q

What is acid concentration a measure of?

A

The number of acid molecules in a certain volume of water.

39
Q

What happens to metals and ability to form positive ions on the reactivity series?

A

More reactive

=

Easier to form positive ions

40
Q

What are the three Cs in the reactivity series in order?

A

Calcium

Carbon

Copper

41
Q

What is a way to remember the reactivity series?

A 
Please 
Send 
Lions
Cats 
Monkeys
Cute
Zebras
Into
Hot 
Countries
42
Q

What is the reactivity series?

A 
Potassium
Sodium
Lithium
Calcium
Magnesium 
Carbon
Zinc 
Iron
Hydrogen
Copper
43
Q

What

A
44
Q

What metals are extracted from molten compounds using electrolysis?

A 
Please
Send
Lions
Cats 
Monkeys
45
Q

What does a metal + oxygen produce?

A

Metal oxide

46
Q

What does a metal + acid produce?

A

Salt + hydrogen

47
Q

What does a metal + water produce?

A

Metal hydroxide + hydrogen

48
Q

Displacement reaction definition

A

When a more reactive element displaces a less reactive metal from its compound

49
Q

How does: K, Na, Li, and Ca react when put in acid or water?

A

When in cold dilute acid:
- explosive reaction

When in water:
- reaction

50
Q

How does: Mg, Xn, Fe react when in acid or water?

A

Cold dilute acid:
- moderate reaction

Water:
- no reaction

51
Q

How does copper react with acid or water?

A

No reaction at all.

52
Q

The more reactive the metal, the faster bubbles…

A

the faster bubbles of hydrogen will be produced

53
Q

Oxidation is the…

A

Gain of oxygen and loss of electrons.

54
Q

Reduction is the…

A

Gain of electrons and loss of oxygen

55
Q

Redox reaction definition

A

Where one substance in a reaction is reduced and another is oxidised.

Metal-acid reactions are redox reactions.

56
Q

Ionic equations only show the particles…

A

the particles that react and the products they form.

57
Q

Endothermic takes…

A

Takes in energy

Shown by a fall in temperature

58
Q

Exothermic transfers…

A

Energy to the surroundings

Shown by a rise in temperature

59
Q

Exothermic reactions examples?

A

Combustion
Neutralisation
Most oxidation reactions.

60
Q

Endothermic reactions example?

A

Thermal decompositions

61
Q

Uses of Exothermic reactions

A

Hand warmers

62
Q

Uses of endothermic reactions?

A

Sport injury packs

Chemistry Paper 1 (1 decks)

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