Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Chemistry Year 11 > Module 3 (Reactive Chemistry) > Flashcards

Module 3 (Reactive Chemistry) Flashcards

1
Q

What are the 5 common ways to observe a chemical change?

A

A solid is formed (precipitate)
A gas is evolved
Permanent change of colour
Disappearance of solid
Significant change in temperature

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

What is a physical change? What is an example?

A

Physical changes are changes affecting the form of a chemical substance, but not its chemical composition. In a physical change, there is no new substance formed and physical changes are easily reversible

An example of this is the boiling of water in which the form of the chemical changes from a liquid to a gaseous state, and no chemical bonds were broken in the process. It is also easy to reverse with little energy

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

What is a chemical change? What is an example?

A

a usually irreversible chemical reaction involving the rearrangement of the atoms of one or more substances and a change in their chemical properties or composition, resulting in the formation of at least one new substance.

Another definition could be the breaking down and rearrangement of chemical bonds.

An example of this is the electrolysis of water (Turning water into hydrogen and oxygen molecules), in which chemical bonds are being broken and rearranged. However, it is hard to reverse and requires a lot of energy

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

List three advantages of using models for chemistry

A

Any of the three:

Models can communicate observations and ideas to other people

Models help visualise ideas or abstract concepts

Models can be used to make and test predictions

Can be used to help illustrate and explain scientific theories or prove them wrong

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

List three disadvantages of using models for chemistry

A

Any of the three:

Don’t include all the details of the objects they represent

Models don’t behave like the things they represent

Accuracy is lost when trying to simplify things into a model

Approximations are used

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Why do chemical reactions exist?

A

They exist because the law of conservation of mass states that matter can be neither created nor destroyed but merely changed from one form to another. In a chemical reaction, mass is conserved through the balancing of both sides so that the number of atoms of each element is conserved

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

What is a chemical reaction?

A

a process in which one or more substances, the reactants, are converted to one or more different substances, the products.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

How is a chemical reaction formatted?

A

Reactants on the left side and products on the right side.

Reactants —–> Products

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

What are the three ways of representing chemical reactions?

A

Word equations - Chemical names only

Symbolic/ Chemical equations - Chemical Formulae only

Balanced Chemical equations - Number prefixes and states

Need to practice irl

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

What are the different state symbols?

A

Solids - ‘S’
Liquid - ‘l’
Gas - ‘g’
Aqueous (dissolved in water - ‘aq’

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

What is a synthesis/combination reaction? What would the general equation look like?

A

This reaction is where two reactants produce a single product. This reaction is typically accompanied with a release of energy in the form of heat and/or light

A + B —> AB

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

What are some (2) examples of synthesis reactions?

A

Hydrogen + Oxygen —> water
Magnesium + Oxygen —> Magnesium oxide

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

What are decomposition reactions? What would the general equation look like?

A

These are basically the opposite of synthesis reactions. Here, the reaction is where a compound is decomposed into two or more other substances. These decomposed substances can be elements or other compounds

AB —> A + B

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

What is an example of a decomposition reaction

A

Silver Bromide —> Silver + Bromine

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

What are the three types of decomposition reactions?

A

Thermal
Electrical
Light

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

Where can the energy required for decomposition reactions be derived from?

A

Heat, light or electricity

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

What is thermal decomposition?

A

Thermal decomposition is caused by heat. In this reaction, a chemical reaction occurs when a compound breaks down when heated. It is endomorphic

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

What is an example of thermal decomposition?

A

Copper Carbonate + Heat (In an equation, don’t have to mention) —> Carbon dioxide + Copper oxide

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

What is electrical decomposition?

A

Electrical decomposition is caused by electricity. In this reaction, an electrical current is passed through a liquid or solution to induce a chemical reaction

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

What is an example of electrical decomposition?

A

Electrolysis of water.

Water + electricity (In an equation, don’t have to mention) —> Hydrogen + Oxygen

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

What is light decomposition?

A

This type of decomposition is caused by light/photons. In this reaction, light or photons are used to break the reactants to form several products

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

What is an example of light decomposition?

A

Silver chloride +light photons (In an equation, don’t have to mention) —> Silver + Chlorine

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

What is a combustion reaction?

A

Combustion reactions are reactions in which substances react with oxygen and heat is released. It can often be referred to as an oxidation reaction. Typically a combustion reaction will involve a hydrocarbon. Combustion is a self sustaining chemical reaction that occurs at temperatures above those of the surroundings

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

What are (3) characteristics of combustion?

A

Emission of large quantities of heat and light (exothermic)

Formation of new substances

Inability to reverse the reaction

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

What does combustion of hydrocarbons produce?

A

Carbon dioxide and water (as long as there is enough oxygen)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q

What are hydrocarbons?

A

Compounds which contains mostly the elements carbon and hydrogen

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q

What are the three different types of hydrocarbons?

A

Alkanes, Alkenes, Alkynes

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
28
Q

What are alkanes and their properties? (4)

A

Alkanes are saturated (meaning that all carbon atoms hold the highest allowed amount of hydrogen atoms). All the bonds between hydrogen and carbon are single bonds. The general formula is C(n) H(2n+2). The suffix is -ane

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
29
Q

What are alkenes and their properties? (4)

A

Alkenes are unsaturated (meaning that all carbon atoms do not hold the highest allowed amount of hydrogen atoms). In alkenes, there is at least one carbon to carbon double bond. The general formula is C(n) H (2n). The suffix is - ene

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
30
Q

What are alkynes and their properties? (4)

A

Alkynes are unsaturated (meaning that all carbon atoms do not hold the highest allowed amount of hydrogen atoms). In alkynes, it consists of at least one carbon to carbon triple bond. The general formula is C(n) H(n). The suffix is -yne

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
31
Q

How are alkanes named?

A

They are named by combining a prefix which describes the number of carbon atoms in the molecule with the root ending ‘ane’

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
32
Q

How are alkenes named?

A

They are named by combining the prefix which describes the number of carbon atoms in the molecule with the root ending ‘ene’

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
33
Q

What are the ‘stem names’ for the numbers of carbon atoms in a hydrocarbon chain (1-10)

A

1 - meth-
2- eth-
3- prop-
4- but-
5- pent-
6- hex-
7- hept-
8- oct-
9- non-
10- dec-

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
34
Q

What are complete combustions?

A

In complete combustions, products are only carbon dioxide and water.

Fuel + oxygen —> carbon dioxide + water (and energy)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
35
Q

What are the 4 steps in writing balanced equations?

A
  1. Write the word equation
  2. Write the chemical formulae
  3. Balance coefficients in front of each chemical
  4. Add state symbols
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
36
Q

What are incomplete combustions?

A

Incomplete combustions occur when there is insufficient oxygen to completely react with fuel. Incomplete combustions is inefficient as it does not use the full energy content of the fuel. Here, the amount of fuel consumed is dependent on how much oxygen is available. It produces environmental pollutants such as carbon and carbon dioxide

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
37
Q

What are the products of an incomplete combustion (in a reaction)?

A

In an incomplete combustion the products may include carbon monoxide, carbon dioxide or carbon, and water.

In other words the product of an incomplete combustion can be any of these: carbon, carbon monoxide, carbon dioxide (we pick which one(s) we want to be the product), PLUS HAVE TO INCLUDE water. SO PICK ANY OF THE CARBONS PLUS WATER

I.e. combustion of methane could result in carbon and water; carbon, carbon dioxide and water; carbon, monoxide, carbon dioxide and water; carbon dioxide and water.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
38
Q

What is a precipitate?

A

A precipitate is an insoluble salt

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
39
Q

Why are some substances insoluble?

A

Some substances will be insoluble if the intermolecular forces between the substance and the water are weaker than those between the solute particles by themselves and the forces between the water molecules themselves

Because of this, ionic lattices stay together, the ions don’t dissociate and the substance remains a solid

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
40
Q

What are solutes?

A

The substancethat dissolves in a solvent to produce a homogeneous mixture.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
41
Q

What are solvents?

A

A substance that has the ability to dissolve a given solute to form a solution with it

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
42
Q

What is a precipitation reaction?

A

A precipitation reaction is a type of double displacement reaction, where there is the formation of an insoluble substance

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
43
Q

What causes a precipitation reaction?

A

When solutions of two ionic substances are mixed, precipitation occurs if one type of positive ion present is able to combine with another type of negative ion present to form an insoluble substance

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
44
Q

What are neutral species equations? Example using sodium chloride and silver nitrate

A

Neutral Species equations are the normal chemical reaction equations.

I.e. 2NaCl (aq) +Ag(NO3)2 (aq) —> 2NaNO3(aq) +AgCl2 (s)

Where silver chloride is the precipitate

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
45
Q

What are complete ionic equations? Example

A

Complete ionic equations are where each compound is broken up into their disassociated ion equivalents except for the precipitate on the products side (i.e. NaCl would turn into Na^2+ + 2Cl^-)

I.e. 2Na+ + 2Cl- + Ag2+ + 2(NO3)- –> AgCl2 + 2Na+ + 2(NO3)-

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
46
Q

What are Net ionic equations? Example using sodium chlroide and silver nitrate

A

Net Ionic equations are basically complete ionic equations, however, the spectator ions are removed (The ion is unchanged on both sides of a chemical equation)

I.e. (following from the sodium chloride and silver nitrate example)

2Cl- + Ag2+ + —> AgCl2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
47
Q

What is a saturated solution?

A

A saturated solution is one in which no more of a particular solute can be dissolved in a given quantity of solvent at a specified temperature

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
48
Q

What is an unsaturated solution?

A

Basically the opposite of a saturated solution and is one where there is not as much of a particular solute being dissolved in a given quantity of solvent at a specified temperature

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
49
Q

What is the concentration of a solution?

A

The concentration of a solution is the amount of solute present in a specified amount of solvent or solution

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
50
Q

What is an equilibrium?

A

When a solution becomes saturated, ions still continue to break away from crystals of solid and go into solution, however at the same time an EQUAL number of ion pairs from solution go on to the solid.

This situation is referred to as equilibrium

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
51
Q

What symbol indicates equilibrium?

A

The ‘state rail’ sign indicates equilibrium. The state rail is basically a sign that looks like half an arrow pointing one way, and another half of an arrow pointing the other way

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
52
Q

State the solubility rules regarding substances which are SOLUBLE

Eight

A

All Nitrates

All Acetates

All Sulfates (except calcium, barium, lead, mercury and silver)

All Chlorides, bromides, iodides (Group 7)(except lead, mercury and silver)

All ammonium compounds

Group 1 metals

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
53
Q

What are the exceptions to sulfates and chlorides, bromides, iodides being soluble?

A

Sulfates - Calcium, lead, mercury, silver, barium

Chloride, bromides, iodides - Lead, Mercury, Silver

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
54
Q

State the solubility rules regarding substances which are INSOLUBLE

5

A

All carbonates (except sodium, potassium, ammonium)

All oxides and hydroxides (except sodium, potassium, calcium, magnesium and barium)

All sulfides (except sodium, potassium, magnesium, calcium, barium and ammonium)

All phosphates (except sodium, potassium and ammonium)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
55
Q

What are the products of an acid and reactive metal reaction? Give the layout of the equation

I.e. Magnesium Hydrochloric acid

A

The products are metal salt typically in the aqueous state (double check) and hydrogen gas

Acid + Metal –> Salt + hydrogen gas

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
56
Q

What are the products of an acid and base reaction? Give the layout of the equation

I.e. Sodium hydroxide and Hydrochloric acid

A

(Known as a neutralisation reaction)
The products are Metal salts and water

Acid+ Metal hydroxide (base) –> Salt + water

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
57
Q

What are the products of an acid and a metal carbonate reaction? Give the layout of the equation

I.e. Sulfuric acid and calcium carbonate

A

The products are metal salts, carbon dioxide gas and water.

Acid+ metal carbonate –> Salt + carbon dioxide gas + water

Note: the products of acid carbonate and acid hydrogen carbonate reactions are the same

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
58
Q

How are the ‘salts’ calculated in a chemical reaction?

A

They are calculated by combining the anions and cations of the first and second reactants which won’t produce any of the products which are guaranteed to have to be the product

I.e. Na + HCl:

H2 would be the guaranteed product, and the rest would combine to give a salt

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
59
Q

What are displacement reactions?

A

Displacement reactions occur when a more reactive metal displaces a less reactive metal and takes its place in a compound (the two switch)

I.e. Cu + 2AgNO3 –> 2Ag + Cu (NO3)2

This occurs because the copper is more reactive than silver

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
60
Q

How does reactivity of metals determine if a displacement reaction occurs?

A

This is because the more reactive the metal, the more likely it is to lose its electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
61
Q

What is the order of the reactivity series? From most reactive to least reactive. (16)

A

Potassium
Sodium
Lithium
Calcium
Magnesium
Aluminium
Zinc
Iron
Tin
Lead
Hydrogen
Copper
Mercury
Silver
Gold
Platinum

62
Q

What is a mnemonic to remember the reactivity series? (16)

Hint: Has something to do with animals

A

Please - Potassium
Send - Sodium
Lions - Lithium
Cats - Carbon
Monkeys - Magnesium
And - Aluminium
Zebras - Zinc
Into - Iron
Lovely - Lead
Hot - Hydrogen
Countries - Copper
Signed - Silver
General - Gold
Penguin - Platinum

63
Q

What is a redox reaction?

A

They are ‘electron transfer reactions’

64
Q

What are the products of a metal and oxygen reaction?

Give a general equation

A

The product is a metal oxide

Equation: Active metal + oxygen –> metal oxide

65
Q

How does the reactivity of metals affect the metals reactions with oxygen

A

The more reactive it is, the less heat is required to make it react with oxygen

66
Q

What 4 elements react slowly at room temperature but burn vigorously if heated?

A

Magnesium, Aluminium, Zinc and Iron

67
Q

What three elements react slowly with oxygen and only if heated?

A

Tin, Lead, Copper

68
Q

What three elements have no reaction with oxygen?

A

Gold, Platinum, Silver

69
Q

What three elements have no reaction with oxygen?

A

Gold, Platinum, Silver

70
Q

What are three properties of metal oxides?

A

They are ionic compounds

They are basic oxides

Metal oxides generally dissolve in water to form hydroxides

71
Q

How does the reactivity of metals affect the reaction of metals and water?

A

The more reactive metals are able to react with just cold water, whereas the less reactive metals only react with hot water or steam

72
Q

What is a general equation for a metal and water reaction?

A

Reactive metal + water —> Hydrogen + Metal hydroxide

73
Q

What 5 elements react with water at room temperature?

A

Lithium, Sodium, Potassium, Calcium and Barium

74
Q

What 4 elements will react with steam?

A

Magnesium, Aluminium, Zinc, Iron

Note: product is metal oxide not metal hydroxide unlike the water reaction (still have the hydrogen)

75
Q

What 6 elements won’t react with any form of water?

A

Tin, Lead, Copper, Silver, Gold, Platinum

76
Q

What does OIL RIG mean in redox reactions?

A

Oxidation = Loss of electrons

Reduction = Gain of electrons

Just a mnemonic

77
Q

What occurs in an oxidation reaction?

A

Loss of electrons

78
Q

What occurs in a reduction reaction?

A

Gain of electrons

79
Q

What are half equations?

A

Half reaction equations are a method of balancing redox reactions

80
Q

What happens in an oxidation half equation? Give examples

A

(For elements which are cations) In an oxidation half reaction, there is the element on the left before an arrow. On the right hand side (products), there will be the ion form of the element on the left plus the amount of electrons that it takes to bring the ion back to the element form.

I.e. Na(s) –> Na+(aq) + e-

Note: The oxidation number is simply the amount of valence electrons that the element has

81
Q

What happens in a reduction half equation? Give examples

A

On the left hand side, there is the element as well as electrons (enough to turn the element into it’s ion counterpart). On the right there is the ion of the element

I.e. Cl2(g) + 2e- —> 2Cl- (aq)

Another question that may be asked is the reduction of an ion. Here, there is the ion (typically a cation) which is added with as many electrons as required to turn the ion back into an element. On the right hand side is the element

82
Q

What can redox reactions be used for?

A

Chemical reactions that produce electrical energy in batteries are redox reactions. In batteries, electrons are transferred from one reactant to another through the wires that make up the electric circuit

83
Q

What is an oxidising agent or an oxidiser?

A

An oxidiser or oxidising agent oxidises something else, therefore it, itself is reduced

84
Q

What is a reducing agent or reducer?

A

A reducing agent or reducer reduces something else, therefore it, itself is oxidised

85
Q

Why do oxidation numbers exist?

A

Because not all redox reactions are easy to identify, so scientists assigned oxidation states (numbers) to atoms which help track the number of electrons transferred in a redox reaction

86
Q

What is an oxidation number?

A

An oxidation number is the charge, real or imagined that an atom would have if it occurred as an ion in a compound. They are typically equal to the charges.

87
Q

What is the oxidation number of an atom in the elemental state?

A

Zero

88
Q

What is the oxidation number of a monatomic ion? (A monatomic ion is an ion consisting of exactly one atom)

A

It is equal to its charge

89
Q

what is the algebraic sum of the oxidation numbers in the formula of a compound equal to?

A

Zero

90
Q

What is the oxidation number of hydrogen in a compound? What is the exception?

A

1+, except when hydrogen forms compounds called hydrides with active metals, and then it is 1-

91
Q

What is the oxidation number of oxygen in a compound? What are the exceptions?

A

2-, except in peroxides when it is 1- (two O’s)

I.e. H2O, the oxygen is 2-, but in H2O2, it is 1-

92
Q

What is the sum of oxidation numbers in the formula for a polyatomic ion equal to?

A

It is equal to the charges on that ion.

I.e, in the sulfate ion, the sum of the oxidation numbers in the formula is 2-, and the oxygens and sulfur add up to 2-, where the oxygens are 2- each, and the sulfur is thus 6+

93
Q

What is a galvanic cell?

A

A galvanic cell is a device that makes a chemical reaction occur in a way that generates electricity.

94
Q

How are redox reactions used in galvanic cells?

A

They allow for the arranging of the oxidation and reduction half reactions to occur at different locations, and provides a wire for the electrons to flow through which creates an electrical current

95
Q

Are the more reactive metals oxidised or reduced in both chemical equations, redox reactions and galvanic cells?

A

More reactive metals will be oxidised, whilst less reactive metals will be reduced

96
Q

What is the structure of a galvanic cells?

A

Consists of two half-cells linked by an external metal conductor and an internal salt bridge

97
Q

What are half cells?

A

Half cells are physically separate compartments where oxidation and reduction occur

98
Q

How do you draw a galvanic cell? (7)

A
  1. Draw two beakers with the metal solutions (i.e., on the left hand side, could have zinc nitrate, and on thee right hand side, could have copper nitrate)
  2. Draw the anodes and cathodes which are simply the metals ‘dipped ‘ in their respective solutions
  3. Draw a connecting ‘salt bridge’ (typically is KNO3)
  4. Draw a ‘wire’ linking the tops of the anodes and cathodes, with a voltmeter in the middle
  5. Draw an arrow indicating the flow of electrons (The arrow will have it’s origin at the site of oxidation (anode)(More reactive metal), and it’s head at the site of reduction (cathode)(less reactive metal)
  6. Draw half equations of what’s happening in each beaker below
  7. Show where the anions and cations are moving to in the salt bridge
99
Q

What happens as time goes on in a galvanic cell? Why? (4)

A

The strip of anode metal will slowly dissolve (Because the anode metal is constantly being oxidised into the metal ion and electrons), and will eventually disappear

The metal form of the cathode will be deposited onto the metal cathode (Because it is the side of reduction, and the electrons which come from the electron flow will help reduce the metal ion into the metal form)

The cations in the cathode solution will decrease (Because the cations are constantly being reduced by the incoming electrons which decreases the cations in the less reactive solution)

The cations in the anode solution will increase (Because the metal is constantly being oxidised into cations and electrons, however the electrons are travelling through the wire to the cathode, and no electrons are left to react with the cations, thus build up of cations)

100
Q

What is the cathode and anode?

A

Cathode - the site of reduction (less reactive metal side). The electrode where reduction takes place

Anode - the site of oxidation (more reactive metal side). The electrode where oxidation takes place

101
Q

What is an example of what changes occur as time goes on in a galvanic cell. With relation to the example of Copper and Silver

A

When drawing the chemical reactions which are occurring in a galvanic cell of Copper (More reactive), and silver(less reactive), the following changes can be observed:

Metallic silver deposits onto the silver strip
Some of the copper strip dissolves
The [Ag+] in the beaker decreases
The [Cu2+] in the other beaker increases

102
Q

What is an electrode?

A

An electrode is a conductor of a cell which gets connected to external circuits

103
Q

What is a salt bridge?

A

An electrolyte or electrolyte gel which joins two half-cells to complete the circuit in a galvanic cell and allows for the movement of ions to maintain a balance of charges.

104
Q

What is the role of the salt bridge?

A

The salt bridge contains a solution of relatively unreactive electrolytes, and because of this, these ions are free to move so that they can balance the charges formed in the two half-cells. This process involves the cations in the salt bridge moving towards the cathode, while anions in the salt bridge move towards the anode

Without the salt bridge, there will be a build up of positive or negative charges, which will prevent further reactions to occur

105
Q

What is galvanic cell notation?

A

It’s a shorthand form of representing cells

106
Q

In galvanic cell notation, what does ‘/’ denote?

A

It denotes a change in phase ( metal in contact with ion)

107
Q

In galvanic cell notation, what does ‘//’ denote?

A

It denotes a salt bridge

108
Q

What is EMF (Electromotive force)?

A

This is the potential difference (voltage) across the electrodes of the cell. It is the maximum voltage that the cell can deliver.

109
Q

What is a reduction potential?

A

They are a measure of the relative tendency of a substance to gain one or more electrons compared to the normal hydrogen half cell

110
Q

What is E^0?

A

Standard reduction potential, also known as e-nought

111
Q

Does having a negative volt on the standard reduction potentials sheet indicate a strong reducing or oxidation agent?

A

Strong reducing agent (Reduces others, oxidises itself) (typically more reactive)

112
Q

Does having a positive volt on the standard reduction potentials indicate a strong reducing or oxidation agent?

A

Strong oxidation agent (Oxidises others, reduces itself) (Typically less reactive)

113
Q

How could you utilise the standard potentials sheet to determine the reactivity of metals?

A

Since the negative volts indicate a strong reducing agent, that means it will be the most reactive, (Because most reactive is most likely to be oxidised) and as the negative volts get smaller (towards zero) and then pass zero into positive numbers, then it indicates less reactive elements.

114
Q

How do you form a redox reaction given two half reactions?

A

Literally add them together, whilst balancing the electrons, remember, there should be both oxidation and reduction occurring

115
Q

How do you calculate EMF of a given equation?

A

Given an equation, break it down into its half reactions. The total EMF is the sum of E-nought value of the reduction and then the E-nought value of the oxidation.

116
Q

What are dependent variables?

A

Dependent variables are the factors which are observed or measured

117
Q

What is reliability? How do you improve it in an experiment?

A

When a scientist repeats an experiment with a different group of people or a different batch of the same chemicals and gets very similar results then those results are said to be reliable. To improve reliability, it has to be done several times and get similar results

118
Q

What is accuracy? How do you improve it in an experiment?

A

Accuracy describes how well a measuring instrument determines the variable it is measuring. Greater accuracy can be achieved by using accurate measuring instruments and picking instruments which is an appropriate measure of accuracy.

119
Q

What is validity? How do you improve it in an experiment?

A

Validity describes whether the results of an experiment really do measure the concept being tested, discuss whether or not the results are actually helpful. It could be improved through picking a correct experiment to test out a hypothesis about a certain subject.

120
Q

Does doubling the half reactions (to balance electrons) alter the E-nought value?

A

Doubling the half reaction does NOT change the E-nought value

121
Q

What are homogenous reactions?

A

Reactants are in the same phase (I.e state such as liquid or aqueous)

122
Q

What are heterogenous reactions?

A

Reactants are in different phases (I.e. reactants are in different states such as a solid and liquid reacting together)

123
Q

What does collision theory state?

A

In order for a chemical reaction to take place, the reactant particles must:

Collide with the right orientation

Collide with sufficient energy (Above the activation energy barrier)

Note: both of these must be achieved, not only one for a successful chemical reaction

124
Q

Why do reactant particles have to collide with the right orientation? Give an example using the formation of a chlorine gas molecule from a singular chlorine atom and chlorine nitrite

A

To ensure that bonds can be broken and reformed. I.e., the new molecule which is meant to be formed actually have to have the parts of the new molecule hitting each other, it can’t be a different atom hitting it as it will create a different molecule which isn’t wanted

If The Nitrogen atoms hit the chlorine atom, they can’t form Cl2, so that’s an example of wrong orientation, however, if the chlorine atom hits the chlorine atom, then it will be able to form Cl2.

125
Q

What is activation energy?

A

Activation energy refers to the minimum amount of energy which is required for a chemical reaction to take place.

It can be thought of a ‘barrier’ that stops reactants from being converted into products, thus energy must bee supplied to reactants to enable them to form the products

126
Q

What symbol represents activation energy, and how is it expressed (i.e. units)

A

E with a subscript ‘a’

Is expressed in KH mol ^ -1

127
Q

What are endothermic reactions?

A

Chemical reactions wheere the reactants absorb energy from the surroundings

128
Q

What are exothermic reactions?

A

Chemical reactions which releases energy into it’s surroundings, typically in the form of heat

129
Q

What is the relationship between endothermic reactions and activation energy?

A

Energy must be continuously supplied to reactants to form the activated complex as energy is absorbed by the bond-making process

130
Q

What is the activated complex?

A

The intermediate step between reactants and products

131
Q

What is the relationship between exothermic reactions and activation energy?

A

The overall release of energy into the environment can be used by reactants to reach the activated complex; thus the reaction becomes self-sustaining

132
Q

What factors can impact the rate of reaction in homogenous reactants? (3)

A

Increasing the concentration of reactants

Increasing the temperature

Using a catalyst

133
Q

What factors can impact the rate of reaction in heterogenous reactants? (5)

A

Increasing the concentration of reactants/increasing pressure of gasses

Increasing the temperature

Using a catalyst

Increasing surface area of reactants

Increasing rate of mixing/stirring (kind of)

134
Q

How does temperature affect the reaction rate?

A

An increase in temperature increases the average kinetic energy of the reactant molecules, and changes the distribution of molecular kinetic energies. The increased velocities of the molecules leads to greater collision and thus faster rate of reaction

135
Q

How does an increase in temperature affect the graph?

A

The graph flattens a bit, as the temperatures increase kinetic energy, and increases the percentage of molecules which can reach the activation energy

136
Q

How does concentration affect reaction rates?

A

Increasing concentration of reactants in solution increases the rate of reaction as there are a greater number of particles available to react. Thus increasing the frequency of collisions between particles

137
Q

What is concentration?

A

The amount of a substance in a space

138
Q

What does increasing pressure in gases do?

A

Increases the concentration, and thus increases the rates of reaction

139
Q

How does surface area affect reaction rates?

A

Increasing the surface area of solid reactants increases the number of particles that are exposed and are available to react and thus increases the frequency of particle collisions, increasing rate of reaction

140
Q

How do catalysts affect reaction rates?

A

A catalyst is a substance that provides an alternative pathway with a lower activation energy for reactants to form products, therefore increasing the rate of chemical reactions, whilst catalyst remains unchanged at the end of the reaction

141
Q

How does stirring affect reaction rates?

A

Stirring keeps reactant particles in continual motion, thus increasing the chances of collision , and increasing rate of reaction

142
Q

What is a catalyst?

A

A substance that provides an alternative pathway with a lower activation energy for reactants to form products, however it is not actually involved in the chemical reaction

143
Q

What happens to the graph when catalysts are introduced?

A

The Activation energy is moved to the left (or at least towards a less kinetic energy (on the x-axis))

144
Q

What trends do the trends of reactivity follow (i.e. electronegativity)? (3)

A

Electronegativity. ionisation energy, atomic radius

145
Q

What does the collision theory say about solids?

A

particles are close together and vibrating in fixed positions, has a definite shape, definite volume and cannot be compressed or diffused

146
Q

What does the collision theory say about liquids?

A

Particles are close together but they are moving more freely - rolling and sliding over each other, they shape will depend on the container, it has a definite volume, cannot be compressed and can diffuse(spread through another substance)

147
Q

What doeees the collision theory say about gases?

A

Particles are far apart and moving very freely and rapidly, the shape depends on the container fits all available space and can be both compressed or diffused

148
Q

Does the state of a substance affect rate of reaction?

A

Yes

149
Q

What happens if you attempt to make two solids react?

A

tend to react very slowly, if they even do react. Solid particles can only vibrate in a fixed position, so particles will not come into contact with enough force to allow them to react

150
Q

What happens if you attempt to make a solid and a liquid/gas react?

A

They will react, especially if solid is cut into small pieeces

151
Q

What happens if you attempt to make solutions of ionic chemicals react?

A

React very quickly as their ions are ready to react, and are also free to move within the solution. Particles of a liquid are continually moving and coming into contact with each other

152
Q

What happens if you attempt to make gas particles react?

A

They tend to react even faster because their particles are moving freely at high speeds, however, they also tend to be further apart

Chemistry Year 11 (9 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2025 Bold Learning Solutions. Terms and Conditions