Brainscape's Knowledge GenomeTM


Top Flashcards (Certified)
All Flashcards

Chemistry > Exercise Book > Flashcards

Exercise Book Flashcards

1
Q

What is an anode?

Chemistry

A

An anode is a positive electrode rod made of graphite (carbon) that attracts negative ions

Chemistry

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

What is a cathode?

Chemistry

A

A cathode is a negative electrode rod made of graphite (carbon) that attracts positive ions

Chemistry

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

What are electrodes?

Chemistry

A

Electrodes are rods made of graphite (carbon) that allows for the electrical flow to attract ions

Chemistry

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

What is a cation?

Chemistry

A

A cation is a positively charged ion that is attracted to an anode

Chemistry

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

What is an anion?

Chemistry

A

An anion is a negatively charged ion that is attracted to a cathode

Chemistry

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

What is an electrolyte?

Chemistry

A

An electrolyte is a solution with an ionic compound containing positive and negative ions

Chemistry

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

What is an ore?

Chemistry

A

An ore is a rock that contains a metal that can be extracted

Chemistry

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

What is extraction

Chemistry

A

extraction is where you separate a metal from its ore, this can be done through the process of electrolysis

Chemistry

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

What is cyrolite?

Chemistry

A

Cyrolite is an aluminium compound that can reduce an ionic compounds melting points

Chemistry

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

What is Bauxite?

Chemistry

A

Bauxite is the ore that aluminium is found in

Chemistry

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

What is oxidation?

Chemistry

A

Oxidation is where an element loses electrons and the gain of oxygen

Chemistry

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

What is reduction?

Chemistry

A

reduction is where an element gains electrons but loses oxygen

Chemistry

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

What is electrolysis used for?

Chemistry

A

Electrolysis is used to separate metals from gases in ionic compounds

Chemistry

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

What does the acronym “PANIC” stand for

Chemistry

A

P - positive
A- anode
N - negative
I - is
C - cathode

Chemistry

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

What is a balanced equation

Chemistry

A

where the amount of reactants and products are balanced on either side of the equation

Chemistry

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

What are the reactants

Chemistry

A

the substances you start with in a chemical reaction

Chemistry

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

what are the products

Chemistry

A

the products is what is produced after a chemical reaction

Chemistry

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

Write the equation for water as a word equation

Chemistry

A

Hydrogen + Oxygen –> Water

Chemistry

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

Write the equation for water as a symbol equation

Chemistry

A

H + O2 –> H2O

Chemistry

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

In a c_______ reaction atoms cannot be c______ or d_______

Chemistry

A

In a chemical reaction atoms cannot be created or destroyed.

Chemistry

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

In a b_______ equation it has the s____ amount of atoms either side

Chemistry

A

In a balanced equation it has the same amount of atoms either side

Chemistry

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

What is the state symbol (s)

Chemistry

A

solid

Chemistry

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

What is the state symbol (l)

Chemistry

A

liquids

Chemistry

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

What is the state symbol (g)

Chemistry

A

gas

Chemistry

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
What is the state symbol (aq) ## Footnote Chemistry
aqueous solutions ## Footnote Chemistry
26
Balance the equation: H2 + O2 --> H2O ## Footnote Chemistry
2H2 + O2 --> 2H2O ## Footnote Chemistry
27
Where can we find the relative atomic mass ## Footnote Chemistry
The top number on the element card in the periodic table ## Footnote Chemistry
28
What is the symbol of relative atomic mass ## Footnote Chemistry
Ar ## Footnote Chemistry
29
What does the symbol Ar mean ## Footnote Chemistry
Relative atomic mass ## Footnote Chemistry
30
What does the relative atomic mass (Ar) tell us ## Footnote Chemistry
The average mass of an atom ## Footnote Chemistry
31
How can we work out the number of neutrons in an atom ## Footnote Chemistry
Relative Atomic Mass (Ar) - Atomic Number Top number - Bottom number ## Footnote Chemistry
32
What is Mr ## Footnote Chemistry
Relative formula mass ## Footnote Chemistry
33
What is the relative formula mass (Mr) ## Footnote Chemistry
The total mass of a compound ## Footnote Chemistry
34
How do you work out the relative formula mass (Mr) ## Footnote Chemistry
add up the relative atomic mass (Ar) of each compound ## Footnote Chemistry
35
What is the relative formula mass (Mr) of Sulphuric acid (H2SO4) ## Footnote Chemistry
H2SO4 (1x2)+32+(16x4) 2+32+64 = 98 98 is the Mr of sulphuric acid ## Footnote Chemistry
36
What can Mr also be referred to ## Footnote Chemistry
relative molecular mass ## Footnote Chemistry
37
What number on the periodic table is the atomic number ## Footnote Chemistry
the bottom number ## Footnote Chemistry
38
What is an aqueous solution ## Footnote Chemistry
substances that can be dissolved in water ## Footnote Chemistry
39
What is a mole ## Footnote Chemistry
an amount of a substance ## Footnote Chemistry
40
A mole always contains the same number of a____, m_______ or i_____. ## Footnote Chemistry
A mole always contains the same number of atoms, molecules or ions. ## Footnote Chemistry
41
In an atom the subatomic particles of p______ and e________ are always the same unless it's an i____. ## Footnote Chemistry
In an atom the subatomic particles of protons and electrons are always the same unless its an ion. ## Footnote Chemistry
42
What is the different between an isotope and ion ## Footnote Chemistry
ion = different number of electrons isotopes = different number of neutrons ## Footnote Chemistry
43
How do we work out the number of moles using the relative atomic mass (Ar) ## Footnote Chemistry
number of moles = mass (g) / Ar ## Footnote Chemistry
44
How do we work out the number of moles using the relative formula mass (Mr) ## Footnote Chemistry
number of moles = mass (g) / Mr ## Footnote Chemistry
45
How many moles of sulphuric acid molecules are there in19.6g of sulphuric acid (H2SO4) to 2 significant figures? ## Footnote Chemistry
1) Work out the Mr of H2SO4 (1x2)+32+(16x4) 2+32+64=98 number of moles = mass (g) /Mr number of moles = 19.6/98 number of moles = 0.20 mol (2 sig fig) ## Footnote Chemistry
46
What is the unit used for moles ## Footnote Chemistry
mol ## Footnote Chemistry
47
What is the unit "mol" used for ## Footnote Chemistry
moles ## Footnote Chemistry
48
How do you work out the percentage by mass ## Footnote Chemistry
(atom/Ar)x100 = percentage ## Footnote Chemistry
49
Work out the percentage mass of C in CO2 ## Footnote Chemistry
1) Work out the Ar of CO2 12+(16x2)=44 C = 12 O = 16 2) put it into the equation (atom/Ar)x100 = percentage (12/44)x100 = 27.3% ## Footnote Chemistry
50
Work out the percentage mass of O in CO2 ## Footnote Chemistry
1) Work out the Ar of CO2 12+(16x2)=44 C = 12 O = 16 - there are 2 oxygen atoms so we have to do 16+16 to get 32 2) put it into the equation (atom/Ar)x100 = percentage (32/44)x100= 72.7% ## Footnote Chemistry
51
What are 2 methods to purify a salt ## Footnote Chemistry
Distillation Reverse Osmosis ## Footnote Chemistry
52
When do reactions occur between metals and acids ## Footnote Chemistry
when the metal is more reactive than hydrogen in the acid ## Footnote Chemistry
53
reactions only occur when the metal is m____ reactive than h______ in the acid ## Footnote Chemistry
reactions only occur when the metal is more reactive than hydrogen in the acid ## Footnote Chemistry
54
What happens when an acid is dissolved in water ## Footnote Chemistry
hydrogen ions are released ## Footnote Chemistry
55
hydrogen ions are released when.... ## Footnote Chemistry
the metal is more reactive than hydrogen in the acid ## Footnote Chemistry
56
All a______ contain h________ ## Footnote Chemistry
all acids contain hydrogen ## Footnote Chemistry
57
When an acid reacts with a metal.... ## Footnote Chemistry
salt is formed ## Footnote Chemistry
58
Complete the equation: carbonate + acid ---> ? + ? + ? ## Footnote Chemistry
acid + carbonate --> salt + water + carbon dioxide ## Footnote Chemistry
59
Complete the equation: alkali + acid ---> ? + ? ## Footnote Chemistry
alkali + acid ---> salt + water ## Footnote Chemistry
60
Complete the equation: metal + acid ---> ? + ? ## Footnote Chemistry
metal + acid ---> salt + hydrogen ## Footnote Chemistry
61
Complete the equation: base + acid ---> ? + ? ## Footnote Chemistry
base + acid ---> salt + water ## Footnote Chemistry
62
Why are not all elements on the table metals ## Footnote Chemistry
elements like carbon and hydrogen are on the metal reactivity table because they show which metals are more/less reactive than them ## Footnote Chemistry
63
How reactive are metals at the top of the metal reactivity table ## Footnote Chemistry
very reactive violent dangerous etc. alkali metals ## Footnote Chemistry
64
How does crystallisation work ## Footnote Chemistry
1) prepare a saturated solution by dissolving a soli5d in a solvent at a high temperature 2) allow the solution to cool and slowly form crystals 3) you can poke the crystals to encourage them to grow filter the solution to separate it from the crystals ## Footnote Chemistry
65
What is the acronym REDOX for ## Footnote Chemistry
REDuction OXidation ## Footnote Chemistry
66
What is reduction ## Footnote Chemistry
gains electrons, loses oxygen in a chemical reaction ## Footnote Chemistry
67
What is oxidation ## Footnote Chemistry
loses electrons, gains oxygen in a chemical reaction ## Footnote Chemistry
68
What are the 3 main types of acid ## Footnote Chemistry
Hydrochloric acid Sulfuric acid Nitric acid ## Footnote Chemistry
69
What will hydrogen become in a chemical reaction Hydrogen --> ? ## Footnote Chemistry
Hydrogen --> Hydroxide ## Footnote Chemistry
70
What will nitric become in a chemical reaction Nitric --> ? ## Footnote Chemistry
Nitric --> Nitrate ## Footnote Chemistry
71
What will oxygen become in a chemical reaction Oxygen --> ? ## Footnote Chemistry
Oxygen --> Oxide ## Footnote Chemistry
72
What will Sulfuric become in a chemical reaction Sulfuric --> ? ## Footnote Chemistry
Sulfuric --> Sulfate ## Footnote Chemistry
73
How is the air polluted ## Footnote Chemistry
through burning fossil fuels ## Footnote Chemistry
74
What are the 3 fossil fuels ## Footnote Chemistry
coal oil gas ## Footnote Chemistry
75
C________ C________ only happens when there is p_____ of o_______ ## Footnote Chemistry
Complete Combustion only happens when there is plenty of oxygen ## Footnote Chemistry
76
When does complete combustion occur when burning a hydrocarbon ## Footnote Chemistry
when there is plenty of oxygen ## Footnote Chemistry
77
What is the word equation for Complete Combustion ## Footnote Chemistry
Hydrocarbons + plenty of oxygen --> carbon dioxide + water ## Footnote Chemistry
78
I______ C_______ only happens when there is a l_____ supply of o______ ## Footnote Chemistry
Incomplete combustion only happens when there is a limited supply of oxygen ## Footnote Chemistry
79
What are 2 pollutant products of incomplete combustion ## Footnote Chemistry
carbon monoxide particulates (soot) ## Footnote Chemistry
80
What is the word equation for Incomplete Combustion ## Footnote Chemistry
Hydrocarbons + limited oxygen --> carbon monoxide + water ## Footnote Chemistry
81
What are the 4 main types of pollutants ## Footnote Chemistry
Carbon monoxide Soot Sulfur dioxide Nitric oxides ## Footnote Chemistry
82
How is carbon monoxide dangerous ## Footnote Chemistry
- diffuses into our blood bind to the haemoglobin causing less oxygen to be transported around the body - colourless, odourless, difficult to detect - death, fainting, comas ## Footnote Chemistry
83
How are particulates (soot) dangerous ## Footnote Chemistry
- can cause respiratory issues (soot in lungs) - global dimming ## Footnote Chemistry
84
What are particulates ## Footnote Chemistry
solid particles of carbon (like soot) ## Footnote Chemistry
85
How is sulfur dioxide (SO2) dangerous ## Footnote Chemistry
- sulfur oxides from hydrocarbon - respiratory issues - acid rain ## Footnote Chemistry
86
How is nitrogen oxide dangerous ## Footnote Chemistry
- nitrogen reacts with oxygen from air - acid rain - requires high temperatures ## Footnote Chemistry
87
Where does nitrogen oxide take place ## Footnote Chemistry
inside internal combustion engines like cars (that require high temperatures) ## Footnote Chemistry
88
the pH is the c_______ of h________ ions ## Footnote Chemistry
the pH is the concentration of hydrogen ions ## Footnote Chemistry
89
What is a strong acid ## Footnote Chemistry
- an acid from 0-3 on the pH scale - very acidic ## Footnote Chemistry
90
What is an acid ## Footnote Chemistry
an acid is a acidic solution ranging from 0-6 on the pH scale ## Footnote Chemistry
91
What is a weak acid ## Footnote Chemistry
- an acid from 4-6 on the pH scale ## Footnote Chemistry
92
What point is neutral on the pH scale ## Footnote Chemistry
7 on the pH scale ## Footnote Chemistry
93
What is an alkaline ## Footnote Chemistry
an alkaline is an alkali solution ranging from 8-14 on the pH scale ## Footnote Chemistry
94
What is a weak alkaline ## Footnote Chemistry
- an alkali from 8-10 on the pH scale ## Footnote Chemistry
95
What is a strong alkaline ## Footnote Chemistry
- an alkali from 11-14 on the pH scale - very alkaline ## Footnote Chemistry
96
What is an acid ## Footnote Chemistry
a substance that forms an aqueous solution with a pH of less than 7 ## Footnote Chemistry
97
on the pH scale how much does the scale increase/decrease by from going from pH 6 to pH 2 0, 1, 2, 3, 4, 5, 6, 7, 8, 9, 10, 11, 12, 13, 14 ## Footnote Chemistry
0, 1, 2, 3, 4, 5, 6, 7, 8, 9, 10, 11, 12, 13, 14 pH 2 <-- pH 6 x10000 higher ## Footnote Chemistry
98
on the pH scale how much does the scale increase/decrease by from going from pH 9 to pH 10 0, 1, 2, 3, 4, 5, 6, 7, 8, 9, 10, 11, 12, 13, 14 ## Footnote Chemistry
0, 1, 2, 3, 4, 5, 6, 7, 8, 9, 10, 11, 12, 13, 14 pH 9 --> pH 10 x10 lower ## Footnote Chemistry
99
A l_____ concentration means a solution is d______ ## Footnote Chemistry
A lower concentration means a solution is dilute ## Footnote Chemistry
100
What is concentration ## Footnote Chemistry
how much acid there is in a certain volume ## Footnote Chemistry
101
What is strength ## Footnote Chemistry
how much an acid dissociates ## Footnote Chemistry
102
At any given c________ a s_____ a______ will have a l______ pH ## Footnote Chemistry
At any given concentration a strong acid will have a lower pH ## Footnote Chemistry
103
If there is more concentration... ## Footnote Chemistry
If there is more concentration there will be more acid per unit ## Footnote Chemistry
104
What is electrolysis used for ## Footnote Chemistry
Electrolysis is a process used to extract metal from ionic compounds ## Footnote Chemistry
105
E________ is a process used to extract metal from i______ compounds ## Footnote Chemistry
Electrolysis is a process used to extract metal from ionic compounds ## Footnote Chemistry
106
What happens to ions when they reach the electrodes ## Footnote Chemistry
they turn back into atoms ## Footnote Chemistry
107
At which electrode does metals build up around ## Footnote Chemistry
cathode (negative electrode) ## Footnote Chemistry
108
At which electrode is gas released ## Footnote Chemistry
anode (positive electron) ## Footnote Chemistry
109
Name the 4 main parts of the process of electrolysis ## Footnote Chemistry
- battery cell - cathode (electrode) - anode (electrode) - electrolyte ## Footnote Chemistry
110
How can we reduce the melting point ## Footnote Chemistry
using a cryolite ## Footnote Chemistry
111
What are the benefits of using a cryolite ## Footnote Chemistry
- saves money -less energy is required ## Footnote Chemistry
112
What do cations (negative ions) move towards in electrolyte ## Footnote Chemistry
positive anode (electrode) ## Footnote Chemistry
113
What do anions (positive ions) move towards in electrolyte ## Footnote Chemistry
negative cathode (electrode) ## Footnote Chemistry
114
Ions can move f_____ in electrolyte ## Footnote Chemistry
Ions can move freely in electrolyte ## Footnote Chemistry
115
What is need for electrolysis to take place ## Footnote Chemistry
- a current to cause electrons in ions to move - needs to be molten or aqueous ## Footnote Chemistry
116
How can we extract aluminium ## Footnote Chemistry
through the process of electrolysis ## Footnote Chemistry
117
Where does aluminium oxide come from ## Footnote Chemistry
a mineral call bauxite ## Footnote Chemistry
118
how can we lower the melting point of aluminium oxide ## Footnote Chemistry
by mixing it with a cryolite ## Footnote Chemistry
119
What are the half equations in aluminium oxide ## Footnote Chemistry
Al3+ + 3e- --> Al 2O2 - 4e- --> O2 ## Footnote Chemistry
120
At the cathode, there are positive metal ions and hydrogen What will happen if the the metal is more reactive than hydrogen ## Footnote Chemistry
Hydrogen is produced ## Footnote Chemistry
121
At the cathode, there are positive metal ions and hydrogen What will happen if the the metal is less reactive than hydrogen ## Footnote Chemistry
metal is produced ## Footnote Chemistry
122
At the anode, What will happen if the the metal is a halogen (group 7) ## Footnote Chemistry
metal (halogen) is produced) ## Footnote Chemistry
123
At the anode, What will happen if the the metal is not a halogen (group 7) ## Footnote Chemistry
Oxygen is produced ## Footnote Chemistry
124
What is group 7 on the periodic table ## Footnote Chemistry
Halogens ## Footnote Chemistry
125
What group are Halogens ## Footnote Chemistry
group 7 ## Footnote Chemistry
126
What happens in the column of halogens (group 7) ## Footnote Chemistry
reactivity decreases ## Footnote Chemistry
127
What type of compounds undergo electrolysis ## Footnote Chemistry
ionic compounds ## Footnote Chemistry
128
what is an ionic compound ## Footnote Chemistry
where a non-metal and a metal are chemically combined together as a compound and can be separated ## Footnote Chemistry
129
Elements in Group 1 (alkali metals) typically ____ _ electron to form _ _ ## Footnote Chemistry
Elements in Group 1 (alkali metals) typically lose 1 electron to form + 1 ## Footnote Chemistry
130
Elements in Group 2 (alkaline earth metals) typically ____ _ electrons to form _ _ ## Footnote Chemistry
Elements in Group 2 (alkaline earth metals) typically lose 2 electrons to form + 2 ## Footnote Chemistry
131
Elements in Group 3 typically ____ _ electron to form _ _ ## Footnote Chemistry
Elements in Group 3 typically lose 3 electron to form + 3 ## Footnote Chemistry
132
Elements in Group 7 typically ____ _ electron to form _ _ ## Footnote Chemistry
Elements in Group 7 typically gain 1 electron to form - 1 ## Footnote Chemistry

Chemistry (91 decks)

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