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N5 Chemistry > Unit 3: Chemistry in Society > Flashcards

Unit 3: Chemistry in Society Flashcards

1
Q

Metal + Oxygen

A

Metal Oxide

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2
Q

Metal + Water

A

Metal Hydroxide + Hydrogen

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3
Q

Metal + Acid

A

Salt + Hydrogen

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4
Q

Ways that metals can be extracted from ores

A

Heating, heating with carbon, electrolysis

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5
Q

What metals produce high voltages when paired in an electrochemical cell?

A

Metals that are far apart in the electrochemical series

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6
Q

Metallic bonding

A

The electrostatic attraction between positive ions and delocalised electrons

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7
Q

Structure of solid metals

A

Positive ions surrounded by a sea of delocalised electrons

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8
Q

Why are metals malleable?

A

Metal atoms can ‘slip’ past each other because the metallic bond is not fixed in all directions

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9
Q

Why are metals good conductors?

A

The presence of delocalised electrons–electrons can move freely

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10
Q

In terms of the reactivity series, what metals react with what compounds?

A

Metals that are high in the ECS react with water, acid, and oxygen, metals that are in the middle of the ECS react with acid and oxygen, metals that are lower in the ECS only react with oxygen, the lowest metals in the ECS (such as gold) do not react with any of the three

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11
Q

Insoluble metal ores can be reacted with acid to form…

A

A soluble salt solution
Passing electricity through this solution will split the compound, causing the metal to accumulate on the negative electrode

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12
Q

Why must a D.C supply be used for electrolysis?

A

So that the products can be identified

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13
Q

Displacement reactions

A

A more reactive metal (higher in the ECS) can displace less reactive metals from compounds

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14
Q

Oxidation

A

Loss of electrons

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15
Q

Reduction

A

Gain of electrons

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16
Q

OIL RIG

A

Oxidation is loss, reduction is gain

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17
Q

In the data booklet, the equations in the ECS are…

A

Reductions

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18
Q

How to find oxidation reactions in the data booklet

A

Reverse the reduction reactions

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19
Q

Redox reaction

A

A reaction involving a transfer of electrons between two species
(Oxidation and reduction happen simultaneously)

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20
Q

What must be balanced in a redox equation?

A

Electrons

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21
Q

How to write a redox equation

A

Combine the ion-electron equations for the reduction and the oxidation, and balance the electrons

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22
Q

How do you tell which metals are being oxidised/reduced in a redox reaction?

A

Electrons travel from the metal higher in the ECS to the metal lower in the ECS, so the metal that is higher undergoes oxidation while the metal that is lower undergoes reduction

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23
Q

Steps for writing a redox equation

A

Find both equations in the ECS
Reverse the one higher up
Balance the electrons
Cancel out electrons
Combine

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24
Q

What does a simple electrochemical cell consist of?

A

2 electrodes, an electrolyte, and an external circuit

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25
Electrolyte
Electrically conducting solution containing ions
26
Electrode
A solid conductor (metal or graphite)
27
All electrochemical cells convert...
Chemical energy into electrical energy (electricity)
28
Electricity passes along metal wires as...
A flow of electrons
29
Electricity passes through an electrolyte as...
A flow of ions
30
Electrochemical cell using two half cells
Metal electrodes are placed in solutions of their own ions, connected with an ion bridge
31
Ion bridge
Completes the circuit--it is soaked in an electrolyte and allows the solutions to touch
32
Ions flow along the..., electrons flow along the...
Ions flow along the ion bridge, electrons flow along the wires
33
Electrons flow in cells is always
Oxidation --> Reduction
34
Where on an electrochemical cell diagram should the direction flow of electrons be shown?
On or above the wire
35
What non metal can be used as an electrode?
Graphite
36
Why is graphite useful to use as an electrode?
It does not corrode overtime
37
Monomers
Small molecules that can be joined to produce polymers
38
Polymers
Long chain molecules formed by joining a large number of small molecules called monomers
39
To to get a polymer name from the monomer name
Add 'poly' to the monomer name
40
Why can brackets be added to polymer names?
To name the monomer easier to identify, however, this is optional
41
Addition polymerisation
A chemical reaction in which unsaturated monomers are joined, forming a polymer
42
What makes alkenes suitable for addition polymerisation?
The C=C functional group--he double bond can break, allowing the freed electrons to form covalent bonds with neighbouring alkene molecules
43
What must be drawn at the end of polymer structures?
End bonds, to signify that only a fragment is shown, not a complete molecule (which could be made of 1000+ monomers)
44
How to draw the structure of polymers made from branched alkenes:
Focus on the double bond, then arrange everything else around it
45
Repeating unit
The shortest section of a polymer chain which, if repeated, would yield the complete polymer chain
46
What are the 3 essential elements for plants?
Phosphorus, nitrogen, potassium (PNK)
47
What are the two types of fertiliser?
Natural (e.g. compost), Synthetic (e.g. nitrate salts)
48
What is the role of fertilisers?
They boost crop yield by supplying the soil with elements essential for plant growth
49
Synthetic fertilisers
Soluble salts produced as a result of neutralisation reactions
50
What salts are commonly used as fertilisers and why?
Ammonium and nitrate salts, because they are highly soluble
51
Ammonia
A toxic, colourless gas with a sharp, unpleasant smell It is highly soluble in water and forms an alkaline solution
52
Ammonia and neutralisation
Ammonia acts as a base in neutralisation reactions Only a salt is produced, no water
53
Uses of ammonia
Manufacture of nitric acid Manufacture of dyes and explosives Cleaning products Manufacture of nylon
54
Haber process
Used to make ammonia
55
Haber process equation
N2 (g) + 3H2 (g) --> 2NH3 (g) (reversible reaction)
56
Haber process catalyst
Iron
57
What is the Haber process also known as?
The Haber-Bosch process
58
Why are the conditions in the Haber process a compromise?
Because the reaction is reversible For example, the reaction is too slow at room temp, but increasing the temp also favours the breakdown of ammonia Exerting pressure increases the yield, but it also increases the cost
59
What helps to increase the yield of ammonia in the Haber process?
Recycling unreacted gases, using a catalyst
60
Ostwald process
Used to produce nitric acid from ammonia, oxygen, and water
61
Ostwald process catalyst
Platinum
62
Remember the catalysts used in the Haber and Ostwald processes
Hippo--haber iron, platinum ostwald
63
What do atoms contain?
Protons, electrons, neutrons
64
Isotopes
Atoms with the same atomic number but different mass numbers
65
What is nuclide notation used for?
To represent individual isotopes
66
Where is radiation emitted from?
From the nucleus of a radioactive isotope
67
What is radiation emitted in the form of?
Particles or waves
68
Radioactive isotope/radioisotope
An isotope with an unstable nucleus that undergoes nuclear decay
69
As the ratio of neutrons to protons increases...
The nucleus becomes more unstable
70
Why do nuclei emit radiation?
To become more stable
71
What are the three types of radiation emitted when nuclear decay occurs?
Alpha, beta, gamma
72
What stops alpha radiation?
A thin sheet of paper
73
What stops beta radiation?
A thin sheet of aluminium
74
What stops gamma radiation?
A thick slab of lead or concrete
75
What happens to alpha/beta/gamma particles when an electric field is applied?
Alpha and beta particles are attracted to oppositely charged plates This is because alpha particles have a positive charge and beta particles have a negative charge Gamma rays are unaffected because they have no charge (Note: Alpha particles are heavy so their trajectory is less affected than that of beta particles)
76
What are alpha particles?
Helium nuclei
77
What happens to atoms when an alpha particle is emitted?
Mass number decreases by 4, atomic number decreases by 2
78
What happens to atoms when a beta particle is emitted?
Atomic number increases by 1, mass number stays the same
79
When does beta decay occur?
When a neutron changes into a proton and an electron--the electron is then released as a beta particle
80
Gamma rays
High frequency electromagnetic radiation
81
When atoms decay by emitting alpha/beta particles, the new atom may still have too much energy to be completely stable. What is the excess energy emitted as?
Gamma rays
82
How can the activity of a radioactive source by measured?
Using a Geiger-Muller tube connected to a ratemeter
83
Half life
The tine is takes for half of the nuclei of an element to decay
84
Can you increase the rate of nuclear decay?
No, there is no way to change it
85
Chemical test for hydrogen
Burns with a squeaky pop
86
Chemical test for oxygen
Relights a glowing splint
87
Chemical test for carbon dioxide
Turns limewater from clear to cloudy
88
Chemical test for water
Cobalt chloride paper turns from blue to pink
89
Chemical test for glucose
Benedict's solution goes from blue to brick red
90
Chemical test for starch
Iodine turns blue/black in the presence of starch
91
Test for metal ions
Flame test
92
An acid and an insoluble base can react to form
A soluble salt
93
What techniques are used when preparing a soluble salt?
Filtration and evaporation (After the reaction, filter off excess carbonate and evaporate the solvent)
94
When reacting solid metal carbonate with acid, how do you know when the reaction has finished?
When effervescence stops
95
Standard solution
A solution of accurately known concentration
96
What piece of equipment is used to prepare standard solutions?
Volumetric flask (also known as a standard flask)
97
Features of a volumetric flask
Narrow next with an etched line to mark volume, wide bottom, a stopper so it can be inverted to mix the solution
98
Preparing a standard solution
Accurately weigh solute Measure the solute in a small volume of distilled water Add to the volumetric flask with rinsings Make up to the mark with distilled water Stopper and invert to mix the solution
99
Why must distilled water be used for standard solutions?
Because it has no impurities
100
Why must rinsings be done when preparing standard solutions?
To make sure that all the solute is transferred to ensure the concentration is accurate
101
Why does the flask have to be inverted when preparing a standard solution?
To mix the solution, making sure the solute is evenly dispersed, avoiding a concentration gradient
102
Acid-base titration
An experimental technique used to work out an unknown concentration of an acid/base by accurately measuring the volumes used in a neutralisation reaction
103
What glassware should be used during a titration?
A burette and a pipette
104
What is used to show the end point of titration?
An indicator (e.g. phenolphthalein)
105
When is the end point of neutralisation during a titration?
The first permanent colour change
106
Titration technique
Use a white tile to see the end point Read the bottom of the meniscus when measuring volume Read the burette at eye level Do a rough titre first Repeat titrations until you get concordant results

N5 Chemistry (3 decks)

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