Chemistry paper 1 c1-7 Flashcards
1
Q
Name the 3 subatomic particles
A
Protons, neutrons, electrons
2
Q
Name the 2 subatomic particles in the nucleus
A
Protons and neutrons
3
Q
Give the location of electrons in the atom
A
Orbiting the nucleus in shells
4
Q
Give the maximum number of electrons in the first shell
A
Maximum of 2
5
Q
Give the maximum number of electrons in the second and third shells
A
Maximum of 8
6
Q
Give the charge of a proton
A
Positive (+1)
7
Q
Give the charge of a neutron
A
Neutral (0)
8
Q
Give the charge of an electron
A
Negative (-1)
9
Q
Explain why the overall charge of an atom is zero
A
Same number of protons and electrons
10
Q
Define an atom
A
Smallest particle that makes up all matter
11
Q
Define an element
A
Substances made from only one type of atom
12
Q
Define a compound
A
Substances made from two or more types of atoms bonded together
13
Q
Define a mixture
A
Groups of atoms, elements and compounds that are mixed but not bonded
14
Q
Define an ion
A
Charged particle formed when an atom has lost or gained electrons
15
Q
Define an isotopes
A
Atoms of the same element (same number of protons) with a different number of neutrons
16
Q
Name the process to separate two liquids
A
Distillation
17
Q
Name the process to separate an insoluble solid from a liquid
A
Filtration
18
Q
Name the process to separate a soluble solid from a liquid
A
Crystallisation
19
Q
Name the four scientists involved in the development of the periodic table
A
John Dalton, John Newlands, Dimitri Mendeleev, Henry Moseley
20
Q
Describe the contribution of Dalton to develop the periodic table
A
Ordered elements based on their atomic mass
21
Q
Describe the contribution of Newlands to develop the periodic table
A
Kept atomic mass. Discovered a repeating pattern every 8th element
22
Q
Describe the contribution of Mendeleev to develop the periodic table
A
Switched positions of elements that did not fit patterns. Left gaps for undiscovered elements
23
Q
Describe the contribution of Moseley to develop the periodic table
A
Ordered elements based on the number of protons they had
24
Q
Give the properties of alkali metals
A
Very reactive, low melting/boiling points, react vigorously with water and halogens
25
Give the properties of the halogens
Low melting/boiling points, poor conductors of heat/electricity, toxic, react with alkali metals
26
Give the properties of noble gases
Very unreactive, stable, full outer shell, exist as single atoms
27
Identify the pattern of reactivity in group 1 (Alkali metals)
The Alkali metals become more reactive as you go down the periodic table
28
Identify the pattern of reactivity in group 7 (Halogens)
The Halogens become less reactive as you go down the periodic table
29
Give the word equation for the reaction between an alkali metal and water
Alkali metal + water → Alkali metal hydroxide + hydrogen
30
Define a displacement reaction
When a more reactive element takes the place of a less reactive element in a compound
31
List the three types of bonding
Ionic, covalent, metallic
32
State the type of bonding that occurs between metals
Metallic
33
State the type of bonding that occurs between non-metals
Covalent
34
State the type of bonding that occurs between metals and non-metals
Ionic
35
Describe what happens in ionic bonding
Electrons are lost or gained
36
Describe what happens during covalent bonding
Electrons are shared
37
List the properties of solids
Fixed shape, fixed volume, cannot be compressed, particles arranged in rows, particles vibrate in fixed positions
38
List the properties of liquids
Can change shape, fixed volume, cannot be compressed, particles not arranged in rows, particles can slide past each other
39
List the properties of gases
Can change shape, can change volume, can be compressed, particles arranged randomly, particles move freely in all directions
40
Describe the properties of ionic compounds
High melting and boiling points, conducts electricity when molten/dissolved, brittle
41
Give the structure that ionic compounds form
Giant lattices
42
Explain why ionic compounds have high melting/boiling points
Strong electrostatic forces between oppositely charged ions, lots of energy needed to overcome them
43
Explain why simple covalent molecules have low melting/boiling points
Weak intermolecular forces between molecules, these are easily overcome
44
State the material that diamond, graphene and graphite are made from
Carbon atoms
45
List the properties of diamond
Hard, strong, cannot conduct electricity
46
Explain why diamond is hard and strong
Forms 4 covalent bonds per atom. This is the max number of bonds. Lots of energy required to break them
47
Describe the structure of Graphene
2D sheet of carbon atoms arranged in hexagons
48
Describe the structure of graphite
3D structure made from multiple graphene layers
49
List the properties of graphite
Soft, brittle, can conduct electricity, 3D
50
Explain why graphite is soft
Graphite has layers. There are weak forces between layers. These layers can slide over each other
51
Explain why graphite can conduct electricity
Only forms 3 bonds per atom. This means there is 1 spare electron that can conduct electricity
52
List the properties of metals
High melting/boiling points, conduct electricity, malleable
53
Describe the structure of metals
Positive metal ions. A sea of delocalised electrons. Strong electrostatic forces between them
54
Define atomic number
The number of protons in the nucleus of an atom
55
Define mass number
The number of protons PLUS the number of neutrons
56
Define isotope
Isotopes have the same number of protons but a different number of neutrons
57
Define relative formula mass
The mass of a molecule
58
Describe how to calculate relative formula mass
Add up all the relative atomic masses of each atom in the molecule
59
State how to calculate % by mass
(Ar of the element / Mr of the compound) x 100
60
State the equation for calculating concentration
Concentration = mass / volume
61
State the units for concentration
g/dm3
62
Describe how to convert from cm3 to dm3
Divide by 1000
63
Describe how to convert from dm3 to cm3
Times by 1000
64
Define the reactivity series
List of metals in order of reactivity
65
Name the metals that can be extracted using carbon
Zinc, iron, tin, lead, copper, silver, gold, platinum
66
Name the metals that can only be extracted using electrolysis
Potassium, sodium, calcium, magnesium, aluminium
67
Define displacement reaction
When a more reactive metal takes the place of a less reactive metal
68
Give the general word equation for the reaction between a metal and oxygen
Metal + Oxygen → Metal oxide
69
Give the general word equation for the reaction between a metal and acid
Metal + acid → salt + hydrogen
70
Give the general word equation for the reaction between a metal oxide and carbon
Metal oxide + carbon → Metal + carbon dioxide
71
Give the general word equation for the reaction between an acid and a base
Acid + base → Salt + water
72
Give the general word equation for the reaction between a metal carbonate and acid
Metal carbonate + acid → Salt + water + carbon dioxide
73
Give the general word equation for the reaction between a metal and water
Metal + water → Metal hydroxide + hydrogen
74
Name the salt produced by hydrochloric acid
Metal chloride
75
Name the salt produced by sulphuric acid
Metal sulphate
76
Name the salt produced by nitric acid
Metal nitrate
77
Define an ore
A rock that contains enough metal atoms to make extracting them commercially viable
78
Define oxidation
Gain of oxygen, loss of electrons
79
Define reduction
Loss of oxygen, gain of electrons
80
Define salt
An ionic compound with no overall charge
81
Which ion makes a substance acidic?
H+
82
Which ion makes a substance alkaline?
OH-
83
Define a base
Chemicals capable of neutralising acids
84
Give three examples of bases
Metal oxides, Metal hydroxides, Metal carbonates
85
Define an alkali
Soluble base
86
Define electrolysis
Splitting a compound using electricity
87
State the states of matter required for electrolysis to take place
Molten (melted) or aqueous (dissolved in water)
88
Explain why electrolysis works with molten/aqueous compounds
Ions are free to move towards the electrodes
89
Explain why electrolysis won’t work if the compound is solid
Ions are arranged in rows and cannot move towards the electrodes
90
State the type of compounds that can be split by electrolysis
Ionic compounds
91
State the types of elements found in ionic compounds
Made from a metal and a nonmetal
92
Define ion
Charged particle formed when atoms lose or gain electrons
93
State the type of element that forms cations
Metals
94
State the type of element that forms anions
Non-metals
95
State the name of the positive electrode
Anode
96
State the name of the negative electrode
Cathode
97
Explain which ions are attracted to the anode
Anions, since they are negatively charged and attracted to the positively charged anode
98
Explain which ions are attracted to the cathode
Cations, since they are positively charged and attracted to the negatively charged cathode
99
Explain what happens to ions at the anode
Anions lose electrons to become atoms. They are oxidised
100
Explain what happens to ions at the cathode
Cations gain electrons to become atoms. They are reduced
101
Explain why cryolite is used in the electrolysis of aluminium oxide to make aluminium
Cryolite reduces the melting point of aluminium oxide so less energy is needed to melt it
102
Explain why the anodes need constant replacing in the extraction of aluminium
The anodes are made of graphite. This reacts with the oxygen produced at the anode, forming carbon dioxide gas
103
State which ions are contributed by water in solutions of ionic compounds
Hydrogen ion H+, Hydroxide ion OH-
104
Explain how the product produced at the cathode during electrolysis of solutions is determined
If the metal ion from the ionic compound is more reactive than hydrogen, then hydrogen is formed. If it is less reactive, then the metal is formed
105
Explain how the product produced at the anode during electrolysis of solutions is determined
If the anion is a halide ion (chloride, bromide, iodide), then the halogen (chlorine, bromine, iodine) is produced. If the anion is anything else (e.g. sulfate, nitrate) then oxygen is produced
106
Explain how a third product of electrolysis of solutions can be made
The ions that are left behind in the solution following electrolysis form a third product
107
Define an exothermic reaction
An exothermic reaction is one that transfers energy from the reacting chemicals to the surrounding area
108
Define an endothermic reaction
An endothermic reaction is one that transfers energy from the surrounding area to the reacting chemicals
109
Define activation energy
The minimum energy needed for a reaction to take place
110
Define bond energy
The energy required to break a specific chemical bond
111
Define a reaction profile
The relative difference in the energy of reactants and products
112
Give the charge for an endothermic reaction in bond energy
positive
113
Give the charge for an exothermic reaction in bond energy
Positive
114
Give the reaction type when the energy of the products is lower than the energy of the reactants
Exothermic
115
Give the reaction type when the energy of the products is higher than the energy of the reactants
Endothermic
116
Give an example of an exothermic reaction
Fireworks, combustion, self heating cans, hand warmers
117
Give an example of an endothermic reaction
Thermal decomposition, ice packs
118
Identify if making bonds is exothermic or endothermic
Exothermic
119
Identify if breaking bonds is exothermic or endothermic
Endothermic
