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IB Chemistry > Reactivity 2.1 > Flashcards

Reactivity 2.1 Flashcards

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1
Q

What do chemical reactions show about products and reactants in a reaction?

A

The ratio

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2
Q

How does the balancing of a chemical equation relate to the Law of Conservation of Mass?

A

No matter can be created or destroyed, so the chemical equations must be balanced i.e. atoms in reactants = atoms in products

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3
Q

Reactants

A

Elements/compounds consumed in a chemical reaction

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4
Q

Products

A

Elements/compounds produced by a chemical equation

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5
Q

When is a chemical equation balanced?

A

When atoms in reactants = atoms in products

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6
Q

Steps for balancing a chemical reaction

A

Word equation, unbalanced chemical equation, balancing, symbols of state

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7
Q

What is a precipitate?

A

An insoluble ionic compound

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8
Q

Ionic compounds consisting of these ions are generally soluble (no exceptions)

A

Na+
K+
NH4+
NO3-
CH3COO-

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9
Q

Exceptions to ionic compounds containing ions of Cl-, Br-, I- being generally soluble

A

Ag+
Pb2+

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10
Q

Exceptions to ionic compounds consisting of ions of SO42-, Cr2O72- being generally soluble

A

Pb2+
Ba2+
Ag+
Ca2+

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11
Q

Exceptions to ionic compounds containing CO32-, PO43- and S2- being generally insoluble

A

Na+
K+
NH4+

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12
Q

Exceptions to ionic compounds containing OH- being generally insoluble

A

Na+
K+
NH4+
Ba2+
Ca2+

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13
Q

Ionic equation

A

Balanced equation which only contains species that underwent change during the chemical reactions i.e. only includes species that underwent bond breaking and/or bond making

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14
Q

Spectator ions

A

Ions (liquid or aqueous) that remain unchanged during the reaction

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15
Q

What happens to spectator ions in an ionic equation?

A

Omitted

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16
Q

In a precipitation reaction, which ions are included in the ionic equation?

A

Ions that eventually end up in precipitate

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17
Q

Steps for writing ionic equations

A

Write a full chemical equation for the reaction

Show the individual ions for any species that will be present as separate ions (liquid/ aqueous ionic compounds and aqueous acids)

Eliminate any spectator ions

Write the ionic equation

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18
Q

Which ions are written as separate ions in an ionic equation?

A

Liquid and aqueous ionic compounds

Aqueous acids

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19
Q

Element + oxygen ->

A

Elemental oxide

20
Q

Hydrocarbon + oxygen ->

A

Carbon dioxide and water

21
Q

Complete combustion

A

Hydrocarbon + oxygen -> carbon dioxide + water

22
Q

Reactive metal + water ->

A

Metal hydroxide + hydrogen

23
Q

Acid + metal ->

A

Salt + hydrogen

24
Q

Acid + base ->

A

Salt and water

25
Q

Neutralisation reaction

A

Acid + base -> salt + water

26
Q

Acid + metal carbonate ->

A

Salt + carbon dioxide + water

27
Q

Acid + metal hydrogen carbonate ->

A

Salt + carbon dioxide + water

28
Q

Which non-metals come in pairs?

A

N
O
F
Cl
Be
I

29
Q

Precipitation reaction reactants

A

Two aqueous solutions (ions swap)

30
Q

What can ionic equations be written for?

A

Ionisation of acids in aqueous solutions

Precipitation reactions

31
Q

For a substance to dissociate into ions, it must

A

Be ionic or dissociate in water

32
Q

Mass-mass stoichiometry

A

Write a balanced chemical equation for the reaction

Convert known mass to moles

Write the required mole ratio

Use the mole ratio to calculate the moles of the unknown reactant/product
Convert back to mass of unknown

33
Q

Mole ratio for mass-mass stoichiometry

A

n(unknown) / n(known) = coefficient (unknown) / coefficient (known)

34
Q
A
35
Q

What equations can be used for mole-mole stoichiometry?

A

n = m / M
n = PV / RT
n = c x V
n = V / Vm (at STP)

36
Q

Avogardo’s law

A

Equal volumes of all gases measured under the same conditions of temperature and pressure contain equal numbers of molecules

37
Q

What does Avogardo’s law mean in relation to stoichiometry?

A

Volume-volume stoichiometry can occur, with a volume ratio found in the same way as the mole ratio

38
Q

What are the assumptions when doing Volume-Volume stoichiometry?

A

Pressure and temperature are the same

39
Q

What is the limiting reagent?

A

Reactant that it is totally consumed when the reaction is completed

40
Q

What does the limiting reactant determine?

A

The theoretical amount of product produced

41
Q

How to identify the limiting reactant

A

Balanced chemical equation for the reaction

Identify what you know about each reactant

Convert known quantities to moles

Divide the moles of each reactant by the corresponding coefficient

Smallest value is the limiting reactant. Largest value = in excess

41
Q

How to predict quantity of product from limiting reactant

A

Use mole ratio of

n(unknown)/n(known) = coefficient (unknown) / coefficient (known)

42
Q

Theoretical yield

A

Amount of product theoretically produced

43
Q

Predicting quantity of the reactant in excess that will remain unreacted

A

n(excess)react / n(limiting) = coefficient excess / coefficient minting

Then,
n(excess)unreacted = n(excess)initial - n(excess)react

44
Q

Percentage yield

A

Experimental yield / theoretical yield. X 100%

45
Q

Atom economy

A

Molar mass of desired product / molar mass of all reactants. X 100%

45
Q

Green chemistry

A

An approach to chemical research and engineering that seeks to minimise the production and release into the environment of hazardous substances

IB Chemistry (10 decks)

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