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Chemistry > C3 - Chemical reactions > Flashcards

C3 - Chemical reactions Flashcards

1
Q

1 what are the chemical formulas for

copper
mercury
lead
sodium
helium

A

Cu
Hg
Pb
Na
He

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2
Q

1 what is in CH3COCH3

A

3 carbon
6 hydrogen
1 oxygen

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3
Q

1 whats in Zn(NO3)2

A

1 zinc
2 nitrogen
6 oxygen

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4
Q

1 what are group 7 elements

A

diatomic molecules- so they exist as X2
Phosphorus is P4

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5
Q

1 what is the conservation of atoms and mass

A

during a chemical reaction atoms cant be created or destroyed only rearranged
same type and number of atoms are present in reactants and products
atoms are conserved just like mass

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6
Q

1 2H2 + O2 =

A

2H2O

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7
Q

2 whats an ionic formula

A

aim is to balance the charge on the ions
written as empirical formula, showing the simplest whole number ratio of ions in the lattice structure

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8
Q

2 ions of
group 1
2
3
4
5
6
7
8

A

1 = 1+
2 = 2+
3 = 3+
4 = /
5 = 3-
6 = 2-
7 = 1-
8 = 0

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9
Q

2 ionic compound of

lithium nitrate
magnesium oxide
aluminium floruide

A

Li+ + N3- = Li3N

Mg2+ + O2- = MgO

Al3+ + F- = AlF3

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10
Q

2 NEED TO KNOW IONS

Sulfate
nitrate
carbonate
hydroxide
ammonium
phosphate

A

SO4 2-
NO3 -
CO3 2-
OH -
NH4 +
PO4 3-

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11
Q

2 what is
potassium carbonate

silver phosphate

Sodium carbonate

A

K+ + CO3 2- = K2CO3

Ag+ + PO4 3- = AG3PO4

Na+ + CO3 2- = Na2(Co3)1

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12
Q

2 what are roman numerals?

A

give charge on metals

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13
Q

3 what is a half equation

A

represents the loss or gain of electrons during the formation of one particular ion

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14
Q

3 what are the four state symbols

A

aq - aqueous
s - solid
l - liquid
g - gas

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15
Q

3 Half equations for
2Na +Cl2 = 2NaCl

A

Na = Na+ + e-
formation of a sodium ion (lose an electron) to get a full outer shell results on a sodium ion and an electron

Cl2 + 2e- = 2Cl-
formation of a chloride ion is gaining an electron

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16
Q

3 what does OILRIG stand for

A

O xidation
I s
L oss
R eduction
I s
G ain

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17
Q

4 what is insoluble

soluble

precipitation

precipitate

A

a substance that won’t dissolve in water

a substance that will dissolve in water

the reaction in which a solid forms

an insoluble product in the solid state formed during a reaction between two solutions

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18
Q

4 what is a displacement reaction

A

reactions in which the more reactive metal or nonmetal takes the place of the less reactive metal or nonmetal in a compound

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19
Q

4 what does a complete ionic equation show

what are spectator ions

what is a net ionic equation

A

shows all the ions and molecules present in a reaction

are present in a reaction mixture but do not take part. they are the same on both sides of the equation, so can be cancelled out.

shows the ions and molecules present in the reaction mixture minus the spectator ions

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20
Q

4 what is the net ionic equation
H+ + Cl- + Na+ + OH- = Na+ + Cl- + H2O

A

H+ + OH- = H2O

Neutralisation

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21
Q

5 what is a redox reaction

A

a reaction in which reduction and oxidation happen at the same time
in terms of oxygen transfer:
REDUCTION is loss of oxygen
OXIDATION is gain of oxygen

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22
Q

5 What is being reduced and what is being oxidised?
Iron (III) Oxide + Aluminium = Aluminium Oxide + Iron

A

reduced = Iron (III) Oxide
Oxidised = Aluminium

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23
Q

5 What is being reduced and what is being oxidised?
Magnesium + Copper (II) Oxide = Magnesium oxide + Copper

A

Reduced = Copper (II) oxide
oxidised = Magnesium

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24
Q

5 why is an element oxidised
why is it reduced

A

oxidised substances lose electrons
reduced substances gain electrons

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25
Q

6 what is The Mole

how big is it

aka

A

an amount of substance that contains the same number of particles as there are atoms in exactly 12 grams of Carbon-12

6.02x10(23)

Avogadro’s constant

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26
Q

6 what is the molar mass

A

the mass of one mole of a substance

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27
Q

6
1m = C atoms = 6.02x10(23) = 12g
2m = C atoms = 1.204x10(24) = 24g
0.5m = C atoms = 3.01x10(23) = 6g
1m = H2O molecules = 6.02x10(23) = 18g
2m = H2O molecules = 1.204x10(24) = 36g
1m = Na2O units = 6.02x10(23) = 62g

A
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28
Q

7 what is the relationship between the amount of substance, the mass, and the molar mass?

A

n = m/Mr
n= amount of substance in moles
m= mass in grams
Mr= molar mass - grams per mole

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29
Q

7 how many moles in 120g of calcium

what is the mass of 5 moles of helium

A

n = m/Mr
n= 120/40.1
n=2.99 mol

5 x 4 = 20g

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30
Q

7 how many moles in 79g of Fe2O3

A

Fe2= 111.6
O3= 49
79/160.6 = 0.492 mol

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31
Q

8 what is stoichiometry

A

a balanced reaction gives the molar ratios of reactants and products- this ratio is called the stoichiometry of the reaction

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32
Q

8 what does the stoichiometry of a reaction mean

A

if the amount of moles in one of the reactants or products is known, the number of moles of other reactants or products can be calculated

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33
Q

8 what is your plan for any stoichiometry equation

A

X given -> X mol -> Y mol -> Y find
mass -> mol -> mol -> mass
etc

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34
Q

8 what’s the layout for a stoichiometry question

A

given = X
find = Y
1 mol X 2 mol of Y Mr of Y
X x ———– x ————– x ———– = Y
Mr of X 2 Mol of X 1 mol of Y

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35
Q

8 what does ‘in excess’ mean

A

one reactant is usually in excess
means more of it is present than is needed
some will be left over at the end

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36
Q

8 what does ‘limiting’ mean

A

other reactant is in limiting amount
it will run out first
determines how much product is formed

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37
Q

9 what is a concentrated solution

A

a solution with large amounts of solute particles in a given volume of a solvent

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38
Q

9 what is a dilute solution

A

a small amount of solute particles in a given volume of a solvent

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39
Q

9 what are the unit for concentration in grams
equation for concentration

A

g/dm^3

volume (dm^3)

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40
Q

9 what are the unit for concentration in moles
equation for concentration

A

mol/dm^3

volume of solution (dm^3)

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41
Q

9 how many cm in 1 dm

cm^3 to dm^3?

A

10 cm = 1 dm

cm^3 /1000 = dm^3
dm^3 x1000 = cm^3

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42
Q

11 what is activation energy

A

the minimum energy needed to break reactant bonds and start a reaction
aka EA

43
Q

11 how do you break bonds

A

you need input energy to overcome the attractive force
its an endothermic process

breaking or making the same chemical bond will require the same energy input or output

44
Q

11 how do you make bonds

A

energy is released when chemical bonds are formed
an exothermic process

breaking or making the same chemical bond will require the same energy input or output

45
Q

11 what is the energy change equation?

A

bonds broken - bonds made

negative number means exothermic
positive number means endothermic

46
Q

13 what is the pH scale for

A

measure how strong acids or alkalis are

47
Q

13 what is pH< 7 ?

A

acids

48
Q

13 what is pH > 7?

A

alkalis

49
Q

13 what is pH 7 ?

A

neutral

50
Q

13 what is universal indicator

how can you be more accurate

A

when added to a solution, it changes the compound to the colour to match its strength or weakness

use a pH probe

51
Q

13 what is a weak acid

A

5/6

52
Q

13 what is a weak alkali

A

13/14

53
Q

14 what are properties of acids

examples?

A

taste sour
pH of less than 7
neutralise bases and alkalis
corrosive
turn blue litmus paper red
react with metal and metal compounds to form salts (ionic)

vinegar
lemon juice
citric acid

54
Q

14 what are properties of alkalis

examples?

A

taste bitter
feel slippery
pH of more than 7
neutralise acids
corrosive
turn red litmus paper blue
react with acids to form salts and water

washing up liquid
over cleaner
sodium bicarbonate

55
Q

14 what is the difference between an alkali and a base

A

they have the same properties
if a base dissolves in water it is known as an alkaline

56
Q

14 what is neutralisation

A

where an acid reacts with an alkali to produce a neutral solution of salt and water

57
Q

14 what is the neutralisation equation

A

H+ + OH- = H2O

58
Q

15 how do you measure pH

A

universal indicator and a colour chart
-measurement is approximate and only precise to whole numbers

pH probe
-calibrated using buffer solutions
-measurements are accurate to 2 decimal places

59
Q

15 how do you name a salt

A

first name = metal that has reacted
second name = acid used

60
Q

15 what salt names are these acids

Hydrochloric acid
sulfuric acid
nitric acid
phosphoric acid

A

metal chloride
metal sulfate
metal nitrate
metal phosphate

61
Q

15 what does….. make

hydrochloric acid + zinc hydroxide
sulfuric acid + lead oxide
nitric acid + iron hydroxide
phosphoric acid + calcium oxide

A

zinc chloride + water
lead sulfate + water
iron nitrate + water
calcium phosphate+ water

62
Q

15 what does …. make

acid + metal
acid + metal oxide
acid + metal hydroxide
acid + metal carbonate

A

salt + hydrogen gas
salt + water
salt + water
salt + water + carbon dioxide

63
Q

15 what do …. make

zinc + hydrochloric acid
magnesium oxide + nitric acid
lithium hydroxide + hydrochloric acid
copper (II) carbonate + hydrochloric acid

A

zinc chloride +hydrogen
magnesium nitrate + water
lithium chloride + water
copper (II) nitrate + water + carbon dioxide

64
Q

15 how ionised are strong acids

common strong acids

A

fully ionised
all molecules release h+(aq) ion

HCl
HNO3
H2SO4
H3PO4

65
Q

15 how ionised are weak acids

common examples

reversible?

A

partially ionised
only a small fraction of molecules
release H+(aq) ions

citric acid
lactic acid
ethanoic acid
reversible

66
Q

15 nitric acid reaction?
propanoic acid reaction?

A

HNO3 (aq) –> H+(aq) + NO3-(aq)

CH3CH2COOH(aq) <—> H+(aq) + CH3CH2COO-(aq)

67
Q

15 what does pH measure

A

how many hydrogen ions are present in a solution

greater H+ ions conc- lower pH more acidic
lower H+ ions conc- high pH more alkaline

68
Q

16 what is the pH of 6 in H+ ions

what is the pH of 3 in H+ ions

A

10(-6) mol/dm^3

x1000

10(-3) mol/dm^3

69
Q

16 how is pH linked to H+ ion concentration

A

as H+ ion conc increases by a factor of 10, pH solution decreases by a factor of 1
concentrated acid will have a lower pH than a dilute acid
at the same concentration a string acid will have a lower pH than a weak acid because its conc of H+ ions is greater due to the fact it fully ionises

70
Q

16 what is a pH titration curve

A

shows the effect of pH of changing the hydrogen ion concentration during a neutralisation reaction

71
Q

16 what is the pH & conc as a decimal

10(-1)
10(-2)
10(-3)
10(-4)
10(-5)
10(-6)

A

pH mol/dm^3
1 0.1
2 0.01
3 0.001
4 0.0001
5 0.00001
6 0.000001

72
Q

16 what is a concentrated acid

what is pH

what is a weak acid

A

a solution that contains a high ratio of acid to the volume of the solution

a scale used to show how acidic or alkaline a solution

a substance in which only a small fraction of the acid molecules ionise releasing hydrogen ions

73
Q

16 what is corrosive

what is a strong acid

what is a dilute acid

A

a substance that attacks and destroys living tissue

a substance in which all of the acid molecules ionise releasing hydrogen ions

a solution that contains a low ratio of acid to the volume of the solution

74
Q

17 what is electrolysis

A

the process in which an electric current is passed through an electrolyte, causing an ionic compound to split apart into its elements

75
Q

17 what happens during electrolysis

A

when an ionic compound is molten, the ionic bonds are broken
positive cations and negative anions are free to move
when electricity is passed through the ions are attracted to the charged electrodes
the negative cathode attracts cations
the positive anode attracts anions
at the electrodes oxidation and reduction reactions occur turning the ions into atoms

76
Q

17
An
Ox
Red
Cat

A

AN ode
OX idation
RED uction
CAT hode

77
Q

17 what is at the anode and cathode of these compounds

potassium bromide
aluminium oxide
barium iodide
sodium chloride
calcium flouride

A

anode cathode
bromine potassium
oxygen aluminium
iodine barium
chlorine sodium
fluorine calcium

78
Q

17 why do ionic compounds have to be molten

A

allows the ions to move more freely around in electrolysis

79
Q

17 what happens when electrolysing lead (II) bromide
anode

A

anode
- negative bromide ions Br-
- lose electrons and are oxidised
- bromide ions combine to make bromine gas molecules
- 2Br- –> Br2 + 2e-

80
Q

17 what happens when electrolysing lead (II) bromide
cathode

A

cathode
- positive lead ions Pb2+
- gain electrons and are reduced
- lead ions become atoms
- Pb2+ + 2e- —> Pb

81
Q

18 how is water ionic

A

can be split into H+ ions and OH- ions
ions are present in aqueous solutions as well as the ions from the ionic compound to be split

82
Q

18 what happens with electrolysis in water

A

hydroxide ions are discharged at the anode forming water and oxygen
4OH- (aq) -> 2H2O (l) + O2 (g) + 4e- (REDUCTION)

hydrogen ions are discharged at the cathode as gas
4H+ (aq) + 4e- -> 2H2 (g) (OXIDATION)

83
Q

18 when you remove the spectator ions what do you get

A

2H2O -> 2H2 + O2

84
Q

18 what is an aqueous solution

A

contains the ions of the dissolved ionic compounds but will also contain hydrogen H+ ions and hydroxide OH- ions from the water

85
Q

18 what are these elements when in an aqueous solution?
sodium
hydrogen
chlorine
hydroxide
water

A

sodium = Na+
hydrogen = H+
chlorine = Cl-
hydroxide = OH-
water = H2O

86
Q

18 what is a discharged ion

A

when an ion forms atoms or molecules at the electrodes
th ions lose their charges

87
Q

18 what cations are hard to discharge

A

K+
Na+
Ca+2
Mg+2
Zn+2
Fe+2
Pb+2
H+
Cu+2
Ag+

88
Q

18 what anions are hard to discharge

A

SO4-2
NO3-
Cl-
Br-
I-
OH-

89
Q

18 what will form at the cathode

A

hydrogen USUALLY
if an ion from a LESS reactive metal is present, the metal will be produced instead

90
Q

18 what will form at the anode

A

oxygen USUALLY
if ions from a GROUP 7 element is present, the GROUP 7 will be produced instead

91
Q

18 what is at the anode and cathode
KBr (aq)
cations = K+ H+
anions = BR- OH-

A

cathode = H2
anode = Br2

92
Q

18 what is formed at the negative electrode
what is formed at the positive electrode

A

negative = cation
positive = anion

93
Q

18 what is the rule for the cathode

what is the rule for the anode

A

cathode = hydrogen or less reactive

anode = oxygen or group 7

94
Q

19 what is electroplating

A

when one metal is covered by another metal using electrolysis with non-inert electrodes

95
Q

19 non-inert?

inert?

A

reactive

non-reactive

96
Q

19 what are the uses of electroplating

A

protection
aesthetics

97
Q

19 what is copper purification

A

both electrodes are made of copper
anode has impure copper
cathode has pure copper
electrolyte is copper sulfate

cathode gains copper atoms and increases in mass
anode loses copper and decreases in mass
impurities collect at the bottom

98
Q

19 whats at the anode for copper purification

A

Cu atoms->Cu ions
Cu -> Cu+2 + 2e-
OXIDATION

99
Q

19 whats at the cathode for copper purification

A

Cu ions -> Cu atoms
Cu+2 + 2e- -> Cu
REDUCTION

100
Q

19 in electro plating what is the cathode

A

the object you wish to plate
ions are reduced at the cathode
gain electrons

101
Q

19 in electroplating what is the anode

A

the metal you want to object plated in
atoms are oxidised
lose electrons

102
Q

19 in electroplating what is the electrolyte

A

contains ions of the metal you are plating with

103
Q

19 when plating a silver spoon what happens at the anode

A

OXIDATION
Ag -> Ag+ + e-
silver atoms lose electrons

104
Q

19 when plating a silver spoon what happens at the cathode

A

REDUCTION
Ag+ + e- -> Ag
silver ions gain electrons

Chemistry (7 decks)

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