C4 - The Periodic Table Flashcards
(112 cards)
1
Q
C4 - The Periodic Table
What is a neutron?
A
Has 0 charge and a relative atomic mass of 1
2
Q
C4 - The Periodic Table
What is an electron?
A
Has a charge of -1 and a relative atomic mass of 0.0005
3
Q
C4 - The Periodic Table
What is a proton?
A
Has a charge of +1 and a relative atomic mass of 1
4
Q
C4 - The Periodic Table
What is the atomic number?
A
(BOTTOM NUMBER) The number of protons (or number of electrons)
5
Q
C4 - The Periodic Table
What is the mass number?
A
(TOP NUMBER) Number of neutrons plus number of protons
6
Q
C4 - The Periodic Table
What is the order of reactivity for Group 1?
A
As they go down the group, the reactivity increases (get more reactive)
7
Q
C4 - The Periodic Table
What is the order of reactivity for Group 7?
A
As they go down the group, the halogens become less reactive
8
Q
C4 - The Periodic Table
What produces a white precipitate?
A
Chloride ions
9
Q
C4 - The Periodic Table
What produces a cream precipitate?
A
Bromide ions
10
Q
C4 - The Periodic Table
What produces a pale yellow precipitate?
A
Iodide ions
11
Q
C4 - The Periodic Table
What are the processes in water purification?
A
Filtration, Sedimentation, Chlorination
12
Q
C4 - The Periodic Table
What is filtration?
A
A layer of sand or gravel filters remaining small particles and sometimes removes microbes
13
Q
C4 - The Periodic Table
What is sedimentation?
A
Chemicals are added to make solid particles and bacteria settle
14
Q
C4 - The Periodic Table
What is chlorination?
A
Chlorine is added to kill remaining microbes
15
Q
C4 - The Periodic Table
What pollutants are found in water?
A
Nitrates - from fertilisers via eutrophication Lead compounds - from water pipes to houses Pesticides - from spraying crops
16
Q
C4 - The Periodic Table
What is a superconductor?
A
Materials which can conduct electricity with little or no resistance
17
Q
C4 - The Periodic Table
What are the two types of superconductor?
A
Type I - metals Type 2 - alloys
18
Q
C4 - The Periodic Table
What are the benefits of superconductors?
A
Loss free power transmission, superfast electronic circuits and powerful electromagnets
19
Q
C4 - The Periodic Table
What are the difficulties with superconductors?
A
They only work at very low temperatures, limiting their use and superconductors that work at room temperature need to be developed.
20
Q
C4 - The Periodic Table
What is the Period number?
A
(ROWS - ACROSS) Number of electron shells
21
Q
C4 - The Periodic Table
What is the Group number?
A
(COLUMN - DOWN) Number of electrons in outer shell
22
Q
C4 - The Periodic Table
What is an isotope?
A
An atom of the same element but with different mass numbers (different number of neutrons)
23
Q
C4 - The Periodic Table
Give one example of an isotope…
A
Carbon-12 and Carbon-14
24
Q
C4 - The Periodic Table
What did John Dalton do?
A
(1803) Said atoms where solid spheres and there was a different sphere for each element
25
# C4 - The Periodic Table
What did J.J Thomson discover?
(1897) That atoms weren't solid spheres and there were negatively charged particles - electrons. Theory was called the "Plum Pudding Model".
26
# C4 - The Periodic Table
How did Rutherford describe the atom?
(1911) Theory of the Nuclear Atom - Gold Foil experiment found that the positive nucleus was surrounded by negative electrons after positive particles passed through the gold, rather than be deflected.
27
# C4 - The Periodic Table
What did Niels Bohr describe?
(1913) Electrons had fixed orbits and fixed energy which prevented the electrons being attracted to the positive nucleus. They orbited in shells.
28
# C4 - The Periodic Table
What are the properties of ionic compounds?
Typically dissolve in water, conduct electricity when in a solution/molten, have very high melting points and their structures are described as giant ionic lattices.
29
# C4 - The Periodic Table
What is a covalent bond?
A shared pair of electrons
30
# C4 - The Periodic Table
lithium + water
lithium hydroxide + hydrogen (2Li + 2H₂O → 2LiOH + H₂)
31
# C4 - The Periodic Table
sodium + water
sodium hydroxide + hydrogen (2Na + 2H₂O → 2NaOH + H₂)
32
# C4 - The Periodic Table
potassium + water
potassium hydroxide + hydrogen (2K + 2H₂O → 2KOH + H₂)
33
# C4 - The Periodic Table
Why is potassium more reactive than lithium?
Because potassium is able to lose its outer electron easier than lithium because the larger radius means that the force of attraction from the nucleus is weaker.
34
# C4 - The Periodic Table
What colour flame does lithium produce?
Red or crimson
35
# C4 - The Periodic Table
What colour flame does sodium produce?
Orange
36
# C4 - The Periodic Table
What colour flame does potassium produce?
Purple or lilac
37
# C4 - The Periodic Table
What is the method for the flame test?
Wash the nichrome wire to clean and make compound stick. Dip into metal compound and hold in Bunsen Burner to produce coloured flame. Repeat with different metal compound.
38
# C4 - The Periodic Table
What are halogens?
Salt formers' - they (Group 7s) react with Group 1 to make salts
39
# C4 - The Periodic Table
Potassium + chlorine
potassium chloride (2K + Cl₂ → 2KCl)
40
# C4 - The Periodic Table
Sodium + chlorine
sodium chloride (2Na + Cl₂ → 2NaCl)
41
# C4 - The Periodic Table
Potassium + bromine
potassium bromide (2K + Br₂ → 2KBr )
42
# C4 - The Periodic Table
Complete and what is this an example of: Cl₂ + 2NaBr
2NaCl + Br₂ an example of a displacement reaction
43
# C4 - The Periodic Table
What elements are bonded by covalent bonds?
Non metals. E.g. Hydrogen (H₂) or Carbon Dioxide (CO₂)
44
# C4 - The Periodic Table
Which elements are bonded ionically?
A metal and a non metal. E.g. Magnesium and oxygen forms magnesium oxide.
45
# C4 - The Periodic Table
What are the properties of Group 1 Metals?
Low melting point and boiling point. Low density (lithium, sodium and potassium float on water). Very soft - can be cut with a knife.
46
# C4 - The Periodic Table
Describe chlorine at room temperature...
Fairly reactuve, poisonous green gas (low boiling point)
47
# C4 - The Periodic Table
Describe bromine at room temperature...
A dense, poisonous orange liquid
48
# C4 - The Periodic Table
Describe iodine at room temperature...
A dark grey crystalline solid (high boiling point)
49
# C4 - The Periodic Table
Why are metals strong and able to bend into different shapes?
High tensile strength makes them hard to break. Can be hammered to different shapes because they are malleable.
50
# C4 - The Periodic Table
How are metals bonded?
With strong metallic bonds. Strong bond between delocalised electrons and positive ions. Outer electrons of each atom can move freely - delocalised and makes them good conductors of heat and electricity.
51
# C4 - The Periodic Table
What can transition metals be used for?
Catalysts - e.g. Iorn is used in Haber Process and nickel is used in hydrogenation of alkenes (making margarine).
52
# C4 - The Periodic Table
What colour are iron and copper compounds?
USUALLY: Iron (II) = light green Iron (III) = orange/brown Copper = blue
53
# C4 - The Periodic Table
What do transition metal carbonates usually thermally decompose into?
A metal oxide and carbon dioxide - usually results in a colour change
54
# C4 - The Periodic Table
What is a precipitate?
Where two solutions react and as solid forms in the solution
55
# C4 - The Periodic Table
What solution is used to test for sulphate ions?
Barium chloride - if a white precipitate forms then sulphate ions are present
56
# C4 - The Periodic Table
What solution is used to test halide ions?
Silver nitrate solution - a coloured precipitate will form if chloride, bromide, or iodide ions are present.
57
# C4 - The Periodic Table
Has 0 charge and a relative atomic mass of 1
What is a neutron?
58
# C4 - The Periodic Table
Has a charge of -1 and a relative atomic mass of 0.0005
What is an electron?
59
# C4 - The Periodic Table
Has a charge of +1 and a relative atomic mass of 1
What is a proton?
60
# C4 - The Periodic Table
(BOTTOM NUMBER) The number of protons (or number of electrons)
What is the atomic number?
61
# C4 - The Periodic Table
(TOP NUMBER) Number of neutrons plus number of protons
What is the mass number?
62
# C4 - The Periodic Table
As they go down the group, the reactivity increases (get more reactive)
What is the order of reactivity for Group 1?
63
# C4 - The Periodic Table
As they go down the group, the halogens become less reactive
What is the order of reactivity for Group 7?
64
# C4 - The Periodic Table
Chloride ions
What produces a white precipitate?
65
# C4 - The Periodic Table
Bromide ions
What produces a cream precipitate?
66
# C4 - The Periodic Table
Iodide ions
What produces a pale yellow precipitate?
67
# C4 - The Periodic Table
Filtration, Sedimentation, Chlorination
What are the processes in water purification?
68
# C4 - The Periodic Table
A layer of sand or gravel filters remaining small particles and sometimes removes microbes
What is filtration?
69
# C4 - The Periodic Table
Chemicals are added to make solid particles and bacteria settle
What is sedimentation?
70
# C4 - The Periodic Table
Chlorine is added to kill remaining microbes
What is chlorination?
71
# C4 - The Periodic Table
Nitrates - from fertilisers via eutrophication Lead compounds - from water pipes to houses Pesticides - from spraying crops
What pollutants are found in water?
72
# C4 - The Periodic Table
Materials which can conduct electricity with little or no resistance
What is a superconductor?
73
# C4 - The Periodic Table
Type I - metals Type 2 - alloys
What are the two types of superconductor?
74
# C4 - The Periodic Table
Loss free power transmission, superfast electronic circuits and powerful electromagnets
What are the benefits of superconductors?
75
# C4 - The Periodic Table
They only work at very low temperatures, limiting their use and superconductors that work at room temperature need to be developed.
What are the difficulties with superconductors?
76
# C4 - The Periodic Table
(ROWS - ACROSS) Number of electron shells
What is the Period number?
77
# C4 - The Periodic Table
(COLUMN - DOWN) Number of electrons in outer shell
What is the Group number?
78
# C4 - The Periodic Table
An atom of the same element but with different mass numbers (different number of neutrons)
What is an isotope?
79
# C4 - The Periodic Table
Carbon-12 and Carbon-14
Give one example of an isotope...
80
# C4 - The Periodic Table
(1803) Said atoms where solid spheres and there was a different sphere for each element
What did John Dalton do?
81
# C4 - The Periodic Table
(1897) That atoms weren't solid spheres and there were negatively charged particles - electrons. Theory was called the "Plum Pudding Model".
What did J.J Thomson discover?
82
# C4 - The Periodic Table
(1911) Theory of the Nuclear Atom - Gold Foil experiment found that the positive nucleus was surrounded by negative electrons after positive particles passed through the gold, rather than be deflected.
How did Rutherford describe the atom?
83
# C4 - The Periodic Table
(1913) Electrons had fixed orbits and fixed energy which prevented the electrons being attracted to the positive nucleus. They orbited in shells.
What did Niels Bohr describe?
84
# C4 - The Periodic Table
Typically dissolve in water, conduct electricity when in a solution/molten, have very high melting points and their structures are described as giant ionic lattices.
What are the properties of ionic compounds?
85
# C4 - The Periodic Table
A shared pair of electrons
What is a covalent bond?
86
# C4 - The Periodic Table
lithium hydroxide + hydrogen (2Li + 2H₂O → 2LiOH + H₂)
lithium + water
87
# C4 - The Periodic Table
sodium hydroxide + hydrogen (2Na + 2H₂O → 2NaOH + H₂)
sodium + water
88
# C4 - The Periodic Table
potassium hydroxide + hydrogen (2K + 2H₂O → 2KOH + H₂)
potassium + water
89
# C4 - The Periodic Table
Because potassium is able to lose its outer electron easier than lithium because the larger radius means that the force of attraction from the nucleus is weaker.
Why is potassium more reactive than lithium?
90
# C4 - The Periodic Table
Red or crimson
What colour flame does lithium produce?
91
# C4 - The Periodic Table
Orange
What colour flame does sodium produce?
92
# C4 - The Periodic Table
Purple or lilac
What colour flame does potassium produce?
93
# C4 - The Periodic Table
Wash the nichrome wire to clean and make compound stick. Dip into metal compound and hold in Bunsen Burner to produce coloured flame. Repeat with different metal compound.
What is the method for the flame test?
94
# C4 - The Periodic Table
Salt formers' - they (Group 7s) react with Group 1 to make salts
What are halogens?
95
# C4 - The Periodic Table
potassium chloride (2K + Cl₂ → 2KCl)
Potassium + chlorine
96
# C4 - The Periodic Table
sodium chloride (2Na + Cl₂ → 2NaCl)
Sodium + chlorine
97
# C4 - The Periodic Table
potassium bromide (2K + Br₂ → 2KBr )
Potassium + bromine
98
# C4 - The Periodic Table
2NaCl + Br₂ an example of a displacement reaction
Complete and what is this an example of: Cl₂ + 2NaBr
99
# C4 - The Periodic Table
Non metals. E.g. Hydrogen (H₂) or Carbon Dioxide (CO₂)
What elements are bonded by covalent bonds?
100
# C4 - The Periodic Table
A metal and a non metal. E.g. Magnesium and oxygen forms magnesium oxide.
Which elements are bonded ionically?
101
# C4 - The Periodic Table
Low melting point and boiling point. Low density (lithium, sodium and potassium float on water). Very soft - can be cut with a knife.
What are the properties of Group 1 Metals?
102
# C4 - The Periodic Table
Fairly reactuve, poisonous green gas (low boiling point)
Describe chlorine at room temperature...
103
# C4 - The Periodic Table
A dense, poisonous orange liquid
Describe bromine at room temperature...
104
# C4 - The Periodic Table
A dark grey crystalline solid (high boiling point)
Describe iodine at room temperature...
105
# C4 - The Periodic Table
High tensile strength makes them hard to break. Can be hammered to different shapes because they are malleable.
Why are metals strong and able to bend into different shapes?
106
# C4 - The Periodic Table
With strong metallic bonds. Strong bond between delocalised electrons and positive ions. Outer electrons of each atom can move freely - delocalised and makes them good conductors of heat and electricity.
How are metals bonded?
107
# C4 - The Periodic Table
Catalysts - e.g. Iorn is used in Haber Process and nickel is used in hydrogenation of alkenes (making margarine).
What can transition metals be used for?
108
# C4 - The Periodic Table
USUALLY: Iron (II) = light green Iron (III) = orange/brown Copper = blue
What colour are iron and copper compounds?
109
# C4 - The Periodic Table
A metal oxide and carbon dioxide - usually results in a colour change
What do transition metal carbonates usually thermally decompose into?
110
# C4 - The Periodic Table
Where two solutions react and as solid forms in the solution
What is a precipitate?
111
# C4 - The Periodic Table
Barium chloride - if a white precipitate forms then sulphate ions are present
What solution is used to test for sulphate ions?
112
# C4 - The Periodic Table
Silver nitrate solution - a coloured precipitate will form if chloride, bromide, or iodide ions are present.
What solution is used to test halide ions?
