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253 Terms
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1
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What are all substances made from?
atoms
2
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What is the smallest part of an element that
can exist?
an atom
3
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Approximately how many different
elements are there?
100
4
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Where are all of the elements shown?
The Periodic Table
5
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What are formed from elements by
chemical reactions?
compounds
6
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What do chemical reactions always involve?
The formation of new substances
7
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What is this the definition of:
Substances containing two or more
elements chemically combined in fixed
proportions
compound
8
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What is this the definition for:
Something consisting of two or more
elements or compounds not chemically
combined together.
mixture
9
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Which processes can be used to separate
mixtures?
Filtration, Crystallisation, Distillation, Chromatography, Fractional Distillation
10
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Before the discovery of electrons what were
atoms thought to be?
Tiny spheres that could not be divided
11
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Which model was created due to the
discovery of the electron?
The Plum-Pudding model
12
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What does the plum pudding model suggest
about the atom?
That it is a ball of positive charge with negative electrons embedded in it
13
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What did the results from the alpha particle
scattering experiment show?
That the mass of an atom was concentrated at the centre (nucleus) and the nucleus was
charged
14
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How did Niels Bohr adapt the nuclear model
He suggested that electrons orbit the nucleus at specific distances
15
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What is the name given to small positively
charged particles in the nucleus?
protons
16
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What did the experimental work of James
Chadwick provided the evidence for?
neutrons
17
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What is the relative charge of the proton?
+1
18
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What is the relative charge of a neutron
0
19
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What is the relative charge of an electron
-1
20
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In an atom the number of electrons is equal
to the number of
protons
21
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What is the atomic number of an element?
the number of protons
22
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All atoms of a particular element have the
same number of?
protons
23
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Atoms of different elements have different
numbers of
protons
24
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What is the radius of an atom?
0.1nm (1x10-^10m)
25
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How many times smaller is the radius of the
nucleus compared to the atom
10,000
26
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What is the relative mass of a proton?
1
27
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What is the relative mass of a neutron?
1
28
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What is the relative mass of an electron?
Very small (1/2000)
29
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What is the mass number of an atom?
the sum of protons and neutrons
30
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What do we call atoms of the same element
with different numbers of neutrons
isotopes
31
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Isotopes of an element have a different
number of?
neutrons
32
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What is the relative atomic mass of an
element?
The average values of the abundance of the isotopes of the element
33
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What is the maximum number of electrons
that can be found on the lowest energy
level?
2
34
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What is the maximum number of electrons
that can be found on the second energy
level?
8
35
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How are the elements in the periodic table
arranged?
In order of atomic number
36
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What do we call a column in the periodic
table?
groups
37
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What do we call rows in the periodic table?
periods
38
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What do elements in the same group in the
periodic table have in common?
The same number of electrons in their outer shell
39
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Before the discovery of protons, neutrons
and electrons how did scientists classify the
elements?
Arranging them in order of their atomic weights
40
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How did Mendeleev overcome problems
with creating a periodic table?
By leaving gaps for undiscovered elements
41
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Elements that react to form positive ions
are
metals
42
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Elements that do not form positive ions are
non-metals
43
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The majority of elements are
metals
44
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Where are metals found on the periodic
table?
To the left and bottom
45
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Where are non-metals found on the
periodic table?
To the right and top
46
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What do we call the elements in Group 0?
The noble gases
47
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Why are Group 0 elements unreactive and
do not easily form molecules?
They have stable arrangements of electrons
48
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How many electrons do the noble gases
have in their outer shell (excluding Helium)
8
49
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What happens to the boiling point of the
noble gases as you go down the group?
It increases
50
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Which noble gas has 2 electrons in the
outer shell?
Helium
51
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What are the elements in Group 1 know as?
The alkali metals
52
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How many electrons are there in the outer
shell of the alkali metals?
1
53
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How does the reactivity of the elements in
Group 1 change as you go down the group?
It increases
54
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What is the general equation for the
reaction of an alkali metal with chlorine?
Alkali metal + Chlorine → Metal chloride
55
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What is the general equation for the
reaction of an alkali metal with water?
Alkali metal + Water → Metal hydroxide + Hydrogen
56
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What is the general equation for the
reaction of an alkali metal with oxygen?
Alkali metal + Oxygen → Metal oxide
57
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What are the elements in group 7 known
as?
the Halogens
58
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How many electrons do the Group 7
elements have in their outer shell?
7
59
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How are the halogens found?
In pairs of atoms
60
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As you go down Group 7 what happens to
the boiling points of the elements?
It increases
61
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As you go down Group 7 what happens to
the relative molecular mass of the
elements?
It increases
62
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As you go down Group 7 what happens to
the reactivity of the elements?
It decreases
63
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What will a more reactive halogen do to a
less reactive halogen when in an aqueous
solution of its salt?
Displace it
64
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What transition element is used in the
Harber process?
Iron
65
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What transition element increases the
decomposition of hydrogen peroxide to
oxygen and water?
Manganese (IV) oxide
66
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What can the transition elements form?
Coloured compounds
Ions with different charges
67
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What colour does Iron(II) hydroxide, Fe(OH)2
Pale green
68
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What colour does Iron(III) hydroxide, Fe(OH)3
Orange- brown
69
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What colour does Iron(III) oxide, Fe2O3
Red-brown
70
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What can the transition elements be used as?
Catalysts
71
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What are the transition elements?
Metals
72
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What are the main transition elements?
Chromium, Manganese, Cobalt, Nickle, Copper
73
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How should the transition elements be
simplified as?
Cr, Mn, Fe, Co, Ni, Cu
74
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What do the transition elements have in
common?
They have similar properties
75
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How do the transition elements differ from
Group 1 metals?
-higher melting points
- higher densities
-Stronger and harder
-Reactivity with oxygen, water and halogen
Conducts electricity
76
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What type of bonding occurs between
oppositely charged ions?
ionic bonding
77
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What type of bonding occurs between
atoms which share pairs of electrons?
covalent bonding
78
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Which type of bonding is found in atoms
which share delocalised electrons?
Metallic bonding
79
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Which type of bonding occurs in
compounds formed from metals combined
with non-metals?
Ionic bonding
80
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Which type of bonding occurs in most non-
metallic elements?
Covalent bonding
81
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Which type of bonding occurs in
compounds of non-metals?
Covalent bonding
82
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Which type of bonding occurs in alloys?
Metallic bonding
83
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What is transferred in ionic bonding?
electrons
84
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When a metal atom becomes positively
charged what has it lost?
electrons
85
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What would be the charge of an ion formed
from a Group 1 element?
+1
86
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What would be the charge of an ion formed
from a Group 2 element?
+2
87
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What would be the charge of an ion formed
from a Group 6 element?
-2
88
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What would be the charge of an ion formed
from a Group 7 element?
-1
89
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What is an ionic compound?
a giant structure of ions
90
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What holds ionic compounds together?
Strong electrostatic forces of attraction between oppositely charged ions
91
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Name 2 covalently bonded substances with
giant covalent structures
Diamond, Silicon dioxide
92
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Some covalently bonded substances have
very large molecules, such as
polymers
93
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How are the atoms arranged in metals?
In a regular pattern
94
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What are the electrons in the outer shell of
metal atoms like?
Delocalised
95
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What does delocalised electrons mean?
Electrons that are free to move around
96
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What are the three states of matter?
solid, liquid, gas
97
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What takes place at the melting point?
melting and freezing
98
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What takes place at the boiling point?
Boiling and condensing
99
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How does the strength of the forces
between particles affect the boiling point?
The stronger the forces between the particles the higher the boiling point
100
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What are the limitations of the particle
model?
- There are no forces
- All particles are represented as spheres
- The spheres are solid
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