Brainscape's Knowledge GenomeTM


Top Flashcards (Certified)
All Flashcards

Additional Science > Additional Chemistry > Flashcards

Additional Chemistry Flashcards

1
Q

What are the masses and charges of these parts of an atom?

  • Proton
  • Neutron
  • Electron
A

Protons = +ve
(mass 1)

Neutrons = neutral
(mass 1)

Electrons = -ve
(mass approx 0)

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

Why do atoms usually have no overall electrical charge?

A

Atoms usually have no overall charge because they have equal numbers of protons (+ve) and electrons (-ve), which cancel one another out

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

All atoms of a particular element (e.g. carbon) all have the same number of what?

A

Protons

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

The number of Protons in the nucleus of an atom is called the

A

Atomic number

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

The number of Protons + Neutrons in the nucleus of an atom is called the

A

Atomic mass

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

What is an alloy and why are they used?

Give some examples

A

Alloys are mixtures of metals with other elements, e.g. iron + carbon → steel

They have a combination of properties, e.g. bronze, brass, steel etc…

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

What is a smart alloy and why are they used (shape-memory)?

Give some examples

A

Smart alloys can return to their original shape after being deformed – e.g. glasses and braces

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

What do these terms means: -

  • Element
  • Compound
  • Mixture
A

Element – pure substance with only 1 type of atom (e.g. gold)

Compound – 2 or more elements chemically bound (e.g. carbon dioxide)

Mixture – more than 1 element or compound not chemically bound (e.g

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

What are the symbols for the following atoms: -

Oxygen		Nitrogen
Chlorine		Hydrogen
Sodium		Copper
Potassium	Helium
Calcium		Zinc
Iron			Carbon
A 
Oxygen (O)		Nitrogen (N)
Chlorine (Cl)		Hydrogen (H)
Sodium (Na)		Copper (Cu)
Potassium (K)		Helium (He)
Calcium (Ca)		Zinc (Zn)
Iron (Fe)			Carbon (C)
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

What happens to atoms when they chemically react to form a compound?

A

They share, give away, or take electrons

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

What are the names of these compounds, and which atoms are found in them?

H2O
CaCO3
H2SO4
HCl
CO2
A

Water (H2O)

Calcium carbonate (CaCO3)

Sulfuric acid (H2SO4)

Hydrochloric acid (HCl)

Carbon dioxide (CO2)

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

What is an isotope?

A

An isotope is an atom with a different amount of neutrons

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

How can you tell which group an atom is in, just by looking at it’s outer shell structure?

A

The number of electrons in the outer shell is the same as their group number

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

How many electrons can occupy the 1st and 2nd shell (energy level) of an atom?

A

2 in the 1st shell and 8 in the 2nd shell

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

The electron structure of sodium can be represented as 2,8,1 – what does this mean?

Represent these atoms: -
•	Fluorine
•	Oxygen
•	Potassium
•	Magnesium
A

2,8,1 means 2 electrons in the 1st shell, 8 electrons in the 2nd shell and 1 electron in the 3rd shell

Fluorine = 2,7

Oxygen = 2,6

Potassium = 2,8,8,1

Magnesium = 2,8,2

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

Define these terms: -

  • Element
  • Compound
  • Mixture
A

Element – a pure substance made from 1 type of atom only

Compound – 2 or more elements chemically bound

Mixture – 2 or more elements or compounds mixed together which are not chemically bound

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

What happens to the electrons of 2 atoms when they chemically react?

A

During a chemical reaction electrons are either given away, taken, or shared

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

What is an ion?

How are +ve ions formed?

How are -ve ions formed?

A

An ion is an atom with a charge

+ve ions have lost electrons

-ve ions have gained electrons

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

Explain how the following atoms become ions (will they be +ve or –ve)?

  • Potassium
  • Magnesium
  • Chlorine
  • Oxygen
A

Potassium – loses 1 electron (K+)

Magnesium – loses 2 electrons (Mg2+)

Chlorine – gains 1 electron (Cl-)

Oxygen – gains 2 electrons (O2-)

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

What are the melting and boiling points of ionic compounds like?

Why is this?

A

Ionic compounds have high melting points and boiling points – to melt them you have to supply enough energy to break the 6 bonds attached to each ion

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

What happens to the electrons when atoms form ionic bonds and covalent bonds?

Which is the strongest?

A

Ionic bonds – 1 atom loses electrons and another gains electrons

Covalent bonds – electrons are shared

An individual covalent bond is stronger than an ionic bond

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

What are the melting and boiling points of covalent compounds like?

Explain why this is

A

Covalent compounds have low melting and boiling points (are often gases) are there is no attraction between the molecules

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

How are the elements of the periodic table arranged?

What are the rows called?

What are the columns called?

A

Elements are arranged in order of atomic number

Rows are called periods

Columns are called groups

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

Which 2 elements would be out of order in the periodic table if they were arranged by atomic mass instead of atomic number?

A

Potassium and Argon

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Why do elements in the same group have similar properties?
Elements in the same group have similar properties as they all have the same number of electrons in their outer shell
26
What do these symbols mean? * (s) * (l) * (g) * (aq)
(s) = solid (l) = liquid (g) = gas (aq) = aqueous
27
What are the symbols for these compounds? * Calcium carbonate * Sodium chloride * Hydrochloric acid
Calcium carbonate – CaCO3 Sodium chloride – NaCl Hydrochloric acid - HCl
28
Why do covalent compounds not conduct electricity when dissolved?
Covalent compounds do not conduct because they do no break down into ions
29
Give the names of 3 covalent compounds which have giant ionic structures? What is the structure of each like?
Diamond – 4 carbon-carbon covalent bonds Graphite – 3 carbon-carbon covalent bonds Silicon dioxide – 2 double silicon-oxygen covalent bonds
30
Why does graphite conduct electricity?
Graphite conducts electricity because it is only bonded 3x (meaning there is a delocalised electron to pass the charge)
31
Explain why ionic compounds have a giant structure
Ionic compounds have giant structures because the ions keep their charge and attract up to 6 other ions – forming a giant lattice
32
What does monatomic mean and why are noble gases monatomic?
Monatomic means an atom which only exists on its own (does not react) Noble gases are monatomic as they have a full shell and are un-reactive
33
What does diatomic mean and why are elements such as the halogens, hydrogen and oxygen diatomic
Diatomic – atoms in pairs, e.g. H2 and O2 Halogens will form diatomic molecules because they covalently bond with each other, forming pairs
34
What is the bonding in metals like?
The bonding in metals creates delocalised electrons (free to move and pass on electrical current)
35
Why do metals conduct electricity?
The bonding in metals creates delocalised electrons (free to move and pass on electrical current)
36
Why do ionic compounds conduct electricity when they are dissolved / molten?
Ionic compounds conduct electricity when dissolved or molten because they remain as ions (which will pass a current)
37
What are the symbols for these compounds? * Sulfuric acid * Sodium hydroxide * Nitric acid
Sulfuric acid = H2SO4 Sodium hydroxide = NaOH Nitric acid = HNO3
38
What are the symbols for these compounds? * Magnesium oxide * Ammonia * Methane
Magnesium oxide = MgO Ammonia = NH3 Methane = CH4
39
Which group of the periodic table do not form ions? Explain why this is
Noble gases do not form ions as they already have a full outer shell
40
What are the names of the following groups in the periodic table? * Group 1 * Group 2 * Middle metals * Group 7 * Group 0
Group 1 = alkali metals Group 2 = alkaline Earth metals Middle metals = transition metals Group 7 = halogens Group 0 = Nobel gases
41
What are nano-materials and what are they used for?
Nano-materials (1-100nm) are very small (one nano-metre = one-thousand-millionth of a metre) They are used for self-cleaning coats on glass etc
42
What are smart materials and what are they used for?
Smart materials return to their original shape, e.g. metals which can be stretched and then return to their original shape (metals used in braces / spectacles)
43
What is a macromolecule? Give some examples
Macromolecules – are formed by giant covalent bonds, e.g. diamond, graphite, silicon dioxide etc…
44
What is the bonding like in diamonds?
Each carbon atom forms 4 covalent carbon-carbon bonds with the carbons around them creating a giant structure and makes them very hard
45
What is the bonding like in graphite?
Each carbon forms 3 covalent carbon-carbon bonds with the carbons around them creating a sea of delocalised electrons which will pass an electrical current
46
What is meant by thermosetting plastic?
Thermosetting – sets when heated and will not melt again, e.g. a kettle
47
What is meant by thermosoftening plastic?
Thermosoftening – will melt when heated, and can be re-shaped
48
How is LD polythene and HD polythene made?
LD polythene – heating ethene to 200oC under high pressure HD polythene – heating ethene to a lower temperature and pressure with a catalysts
49
What is polymerisation?
Polymerisation is when small molecules are joined to make longer, more useful molecules (e.g. ethane makes poly(ethane))
50
Give 6 uses of polymers
New packaging, waterproof coatings, dental-polymers, hydrogels, smart materials (shape memory polymers)
51
What are the two types of polymer and how does this affect their properties?
Low density (LD) polymers (often flexible) High density (HD) polymers (often more rigid) E.g. LD polythene for plastic bags and HD polythene for water tanks
52
Why are metals easily shaped?
Metals are easily shaped because the atoms are closely arranged and can slide past one another
53
How can you calculate atomic mass?
Add the relative atomic masses of the elements within the compound
54
How can you calculate empirical formula?
Empirical formula (the simplest possible compound) – divide each element by its mass Divide each result by the smallest result Round the numbers up to find out the number of each element
55
How can you calculate percentage yield?
Percentage yield – work out the masses for each compound Divide the mass of one compound by the mass you have been given Divide the other compounds by this result
56
What is relative atomic mass based on?
Relative atomic mass used on a comparison of the mass with 12C isotope
57
What is a mole and how can the mass of a mole of an element be worked out?
The relative formula mass of a substance (grams) is known as one mole of that substance
58
How can you calculate the percentage of an element in a compound?
mass of element ÷ mass of compound) x 100
59
Give 3 reasons why a reaction may not give the theoretical yield
The reaction may not go to completion because it is reversible Some of the produce may be lost when it is separated from the reaction mixture Some of the reactants may react in ways different to the expected reaction
60
What is theoretical yield?
The maximum yield that could be obtained if all atoms reacted
61
What is atom economy?
In reactions with high atom economy all the atoms react and are not ‘wasted’
62
What is a reversible reaction? Give 3 examples
A reversible reaction is not a permanent reaction and will break back down into the reactants
63
What is equilibrium?
Equilibrium is reached when the reactions occur at exactly the same rate in both directions
64
What is the Haber process used to manufacture and what is the equation?
Ammonia N2 + 3H2 → 2NH3
65
What are the raw materials used for in the Haber process, and where can these be obtained?
Nitrogen – from the air Hydrogen – from natural gas / water
66
What are the conditions needed for the Haber process? * Temperature * Pressure * Catalyst
Temperature = 450°C Pressure = 200atm Catalyst = iron
67
What happens to the unused nitrogen and hydrogen?
Unused nitrogen and hydrogen are recycled
68
During the Haber process how is the ammonia removed?
It is liquefied
69
How can the relative amounts of substances in a reversible reaction be altered?
Changing the temperature / pressure
70
How does increasing the temperature affect a reversible reaction?
Increasing the temperature increases the amount of the endothermic side of the reaction
71
How does decreasing the temperature affect a reversible reaction?
Decreasing the temperature increases the amount of the exothermic side of the reaction (however it also slows it down)
72
How does increasing the pressure affect a reversible reaction?
Increasing the pressure increases the side of the reaction with the lowest volume
73
How does decreasing the pressure affect a reversible reaction?
Decreasing the pressure increases the side of the reaction with the highest volume
74
Why may it be important to companies to understand the conditions of a reversible reaction
So they can get the most amount of product (and therefore the most amount of profit)
75
What type of salts are made from the following? * Hydrochloric acid * Sulfuric acid * Nitric acid
Hydrochloric acid – chlorides Sulfuric acid – sulfates Nitric acid – nitrates
76
What is electrolysis used for?
Separating ions in solution
77
What types of ions do the following form? * Metals * Non-metals
Metals = +ve Non-metals = -ve
78
During electrolysis where are these ions attracted to? * Positive * Negative
+ve electrode attracts negative ions -ve electrode attracts positive ions
79
What are the scientific names for the following? * +ve electrode * -ve electrode
+ve electrode = anode -ve electrode = cathode
80
What is the gain of electrons called? What is the loss of electrons called?
Oxidation = loss Reduction = gain OIL RIG
81
During electrolysis where does oxidation occur?
Oxidation occurs at the –ve electrode (electrons are lost)
82
During electrolysis where does reduction occur?
Reduction occurs at the +ve electrode (electrons are gained)
83
Write out the half equations which happen during the electrolysis of brine
2Cl- → Cl2 + 2e- 2H+ + 2e- → H2
84
What are the products of the electrolysis of sodium chloride (brine)?
Hydrogen (-ve electrode) Chlorine (+ve electrode) Sodium hydroxide (solution)
85
What are the products of the electrolysis of sodium chloride, and what are they used for?
Hydrogen – margarine / Haber process Chlorine – swimming pools / cleaning products Sodium hydroxide – soap / paper
86
How can electrolysis be used to obtain pure copper from impure copper?
Impure copper used as the +ve electrode Pure copper as the –ve electrode Solution containing copper ions (e.g. copper sulfate)
87
What is an insoluble salt and how can it be formed?
Insoluble salts will not dissolve in water They are formed by mixing appropriate solutions and filtering the precipitate
88
How can precipitation of unwanted salts be used to treat drinking water?
Filter the precipitate (removing unwanted salts)
89
Give 3 ways in which a soluble salt can be prepared
Metal + acid Insoluble base + acid Acid + alkali
90
How can a solid salt be obtained from a salt solution?
Evaporating to leave the salt crystals
91
What is a base? Give some examples
Metal oxides and hydroxides are bases
92
What is the difference between a base and an alkali? Give some examples
Metal oxides and hydroxides are bases Soluble hydroxides are alkalis (e.g. sodium hydroxide)
93
How are ammonium salts made? What are they used for?
Ammonia is dissolved in water to produce an alkaline solution This can then be used to neutralise an acid to produce an ammonium salt These are important in the production of plant fertilisers
94
What type of ions are found in the following? * Acids * Alkalis
Acids = H+ (hydrogen) Alkalis = OH- (hydroxide)
95
What happens to the H+ ions and the OH- ions during a neutralisation reaction? Include an equation
H+ reacts with the OH- to produce water (H2O) H+(aq) + OH-(aq) → H2O(l)
96
What does a catalyst do to a reaction?
A catalyst lowers the activation energy needed to start the reaction Iron – Haber process Magnesium dioxide – decomposition of hydrogen peroxide
97
What happens to a catalyst at the end of a reaction?
Nothing – the catalyst is not used up and can be used again
98
How can the rate of a reaction be measured?
Amount of reactant used ÷ time Or Product formed ÷ time
99
Give 4 things which can increase the rate of a reaction?
Temperature Concentration / pressure Surface area Catalyst addition
100
Why does temperature affect the rate of reaction?
Increasing the temperature gives the particles energy – the particles move faster, colliding more often and with more force
101
Why does concentration / pressure affect the rate of reaction?
The higher the concentration of a liquid or the higher the pressure of a gas then the higher the chance of a collision = an increased rate of reaction
102
Why does surface area affect the rate of a reaction?
The larger the surface area the more exposed particles there are to react
103
How can you increase the surface area of reactants?
The surface area can be increased by cutting the object into smaller pieces – powder has a very large surface area
104
What must happen for a reaction to take place?
Particles must collide with enough force
105
What is activation energy?
The energy needed to start a reaction (minimum energy required by the particles to react)
106
What is an exothermic reaction? Give an example
A reaction which gives out energy (usually heat), e.g. combustion / respiration
107
What is an endothermic reaction? Give an example
A reaction which takes energy in from the surroundings, e.g. photosynthesis uses light energy
108
How can artificial colours be separated?
Chromatography (colours split based on ability to dissolve / molecular size)
109
What advantage do machines have at analysing unknown substances?
Very sensitive Very fast Very accurate
110
What is gas chromatography
Gas chromatography separates out mixtures of compounds allowing the substances present to be identified
111
What is an indicator and what is pH?
An indicator is a dye which changes colour pH (1-14) is a measure of how acid or alkaline a solution is
112
What is electroplating?
Electroplating uses electrolysis to coat the surface of one metal with another (e.g. silver onto brass to make it look nice)
113
In electrolysis why is cryolite used?
Aluminium oxide is dissolved in molten cryolite (ore of aluminium) lowering the temperature (and therefore the cost)

Additional Science (1 decks)

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