General Knowledge Flashcards
1
Q
Metallic Bonding
A
The sharing of electrons between 2 metals
2
Q
HN03
HCL
H2SO4
A
HN03- Nitric Acid
HCL- Hydrochloric acid
H2SO4- Sulphuric acid
3
Q
Why can metals conduct electricity
A
Deloсaliased electrons carry electrical charge through the metal
4
Q
Name key terms associated with electrolysis
A
Electrolyte, Cathode, Cation, Anion, Anode
5
Q
Why do simple covalent compounds have low melting + boiling points
A
Weak intermolecular forces
6
Q
Why do simple covalent compounds have low melting + boiling points
A
Weak intermolecular forces
7
Q
What are the 2 Non-Metals on the reactivity series
A
Carbon and Hydrogen
8
Q
What side of the periodic table are metals found?
A
Left
9
Q
What is displacement
A
More reactive element replaces a less reactive element in a compound
10
Q
What ion is present in acids?
A
Hydrogen
11
Q
Compare strong + weak acids
A
Strong acids dissociate completely, weak acids dissociate partially
12
Q
What is a cation
A
Ion with a positive charge
13
Q
What is an Anion
A
Ion with a negative charge
14
Q
What is corrosion
A
When metal degrades due to reaction with the environment
15
Q
Define metallic bonding
A
Sharing of electrons between 2 metals
16
Q
Why are life cycle assessments necessary
A
Helps work out the environmental impact of a product, from raw materials to disposal of the product
17
Q
What is an electrolyte
A
An ionic compound that breaks up into ions when it is dissolved in water or body fluids
18
Q
Define electrolysis
A
Process of using electricity to split water into hydrogen and oxygen
19
Q
Are metal ions positively or negatively charged
A
Positively charged
20
Q
What happens during the electrolysis of copper sulphate
A
Copper ions gain electrons and deposited as metal coppers
21
Q
Why is carbon dioxide a gas even at low temperatures
A
Weak intermolecular form low energy required to break them
22
Q
What happens to the reactivity in a group 1 alkali metal
A
Increases further down the group
23
Q
What happens to the reactivity in a group 7 halogen
A
Increases further up the group
24
Q
Why does reactivity increase furthers down the group 1 alkali metals
A
The outer electron is getting further away from the nucleus
25
In a group 1 alkali metal is the attraction higher or lower
Lower
26
In a group 1 alkali metal is the outer electron easier to gain or lose
Lose
27
What happens when a halogen reacts with an alkali metal
Called a halide
28
What is an ion
An atom or group of atoms that has an electrical charge
29
What is electrostatic interaction
Attractive force between objects with opposite electrical charges
30
Why do giant ionic substances have high melting points and boiling points
Large amounts of energy needed to break the many bonds
31
Why can’t giant ionic substances conduct electricity as a solid
No as ions can’t move
32
Why can giant ionic substance conduct electricity when melted and dissolved
Ions are free to move
33
What force hold ions together in a giant ionic substance
Electrostatic
34
What are 2 properties of giant ionic substances
Strong bonds, High melting points
35
Ionic bonding
Donation of electrons from a metal to a non metal , the electrostatic for between 2 opposites
36
What is a covalent bond
The sharing of electrons between 2 non metals
37
What is a neutralisation reaction
Acid and alkali react
38
Name the 6 stages of titration
1. Use a pipette to measure a fixed volume of alkali and put in a flask
2. Add a few drops of indicator into the flask and put flask on a white tile
3. Fill a burette with a dilute acid of a known concentration
4. Add acid from the burette and swirl the flask
5. Repeat
6. Write down the volume
39
What is collision theory
Explains how reactions happen
Particles must collide with enough activation energy to react
More particles that have activation energy more frequent and successful collisions there will be + higher rate of reaction
40
What is an endothermic reaction
A chemical proved that absorbs heat from its surroundings with a decreasing temperature
41
What is an exothermic reaction
A chemical reaction that releases energy by light or heat with an increasing temperature
42
What is the difference between chemical and physical changes in reactions
Physical alters the state size or shape of a substance a reversible change
Chemical creates a new substance by combining existing substances irreversible changes
43
what does the term equilibrium mean
A state in which opposing forces are balanced
44
What 3 things happen when hydrocarbon chains get longer
Boiling point increases
Thickness increases
Flammability decreases
45
Alkanes burn completely in oxygen to form which 2 products
Hydrogen
Carbon dioxide
46
Are alkanes saturated or unsaturated
Saturated
47
What’s the general formula of an alkane with an example
CnH2n+2 propane
48
Are alkenes saturated or unsaturated and what is the general formula with an example
Unsaturated
CnH2n, ethane
49
What does cracking mean
Breaking down long hydrocarbons into smaller more shorter molecules with heat and a catalyst
50
What is the process by which we separate crude oil into useful components
Fractional distillation
51
Stages of crude oil making
1. Heat it until it turns into a gas
2.Gas rises into fractionating column
3. Separate due to diverse boiling points
4. Condense at different temperatures
52
Why do atoms have no overall charge
Have the same number of protons and electrons
Protons positive and electrons negative
53
How to tell atomic number
Number of protons and electrons (bottom number)
54
How to work out number of neutrons
Mass number (top)- number of protons
55
What is an isotope
Same atomic number but different mass number
56
Which number is the relative atomic mass
The larger one
57
What is the composition of the atmosphere today
Nitrogen 78%
Oxygen 21%
Other gases 1%
58
2 ways the amount of co2 has decreased from the early atmosphere
Photosynthesis
Sedimentary rocks
59
1 way the amount of O2 increased from the early atmosphere
Photosynthesis by plants and algae
60
Name 3 greenhouse gases
Co2, Methane and Water Vapur.
61
2 human activities that have increased the amount of greenhouse gases in the atmosphere
Deforestation
Burning fossil fuels
62
3 ways carbon footprint can be reduced
Walk or bike to work
Insulate your house
Buy meat and fish from a sustainable source
63
What are the 5 stages of the greenhouse effect
1. The sun emits short wavelength radiation which passes through the atmosphere to earth
2. The earth absorbs the short wave length radiation
3. The earth remits long wavelength radiation
4. Greenhouse gases absorb the long wavelength radiation
5. Greenhouse gases re- radiate the long wavelength radiation in all directions
64
What is an ion and how is it formed
An atom or group of atoms that has an electrical charge and must gain or lose an electron
65
What is the formula for :
Magnesium chloride
Calcium sulphide
Lithium oxide
Mgcl2
CaS
Li2O
66
What holds the ions together in a giant ionic lattice
Strong ionic bond and electrostatic forces
67
Why do ionic compounds have high MPs and BPs
Large amounts of energy is needed to break the many strong bonds
68
Why can ionic compounds only conduct electricity when molten or dissolved in water
The ionic lattice is broken down allowing the ions to move freely
69
What does the Haber process produce and why is it so important around the world
Ammonia, which is used as fertiliser in industries worldwide.
70
What is the pressure needed for the Haber process
200 atmospheres (ATM)
71
Why is the Haber Process a reversible reaction.
An equilibrium is achieved and the arrow is there
72
What are the 2 starting chemicals in the Haber Processs and where do we get them from
Nitrogen (extracted from the air)
Hydrogen (obtained by natural gas)
73
What temperature is needed for the Haber Process
450 °C
74
What is the catalyst needed for the Haber Process
Iron
75
What is a greenhouse gas
Gases in earths atmosphere that trap heat
76
What problems do sulphur dioxide and nitrous oxide cause
Acid rain and smog
77
What are ionic bonds between
Metal and non metal
78
What are covalent bonds between
2 Non metals
79
What happens during Ionic bonding
Metal donates an electron to a non metal
80
Colours of universal indicator
Red/ orange in acid
Green in neutral
Blue/ purple in alkali
81
Colours of methyl orange
Red in acid
Orange in neutral
Yellow in alkali
82
Phenolphthalein colours
Colourless in acid
Colourless in neutral
Pink in alkali
83
What are the metals called in hydrochloric, sulphuric and nitric acid
Metal chlorides
Metal sulphates
Metal nitrates
84
What best describes what happens during electrolysis
Ionic compounds are decomposed
85
If you complete electrolysis with a powder rather than a solution why won’t it work
No current will flow as ions can’t move in a lattice
86
How could a pure dry sample of a precipitate be obtained from a mixture in a test tube
Filter the mixture then clean the solid with distilled water then let sit
87
How is the electronic configuration of chlorine linked to its period in the periodic table
Chlorine has 3 shells so chlorine is in period 3, the number of shells is the period number
88
How to find number of Protons, Neutrons and electrons
Number of protons= atomic number (bottom number)
Number of electrons= atomic number (bottom number)
Number of neutrons= atomic number - mass number (top)
89
Why would you use a polystyrene cup instead of a glass beaker
Polystyrene is a poor conductor of heat so reduces energy transfer
90
Over the past 3 billions years has the average surface temperature of earth increased or decreased
Decreased
91
Why has there been a decrease in water vapour since 3 billion years ago
Water vapour formed clouds which produced bodies of water
92
What test would show that a gas is oxygen
Put a glowing splint into the gas and it relights
93
What name is given to group 7 elements
Halogens
94
What’s a molecule
Two or more atoms joined together by a covalent bond
95
How can hydrogen chloride be converted into hydrochloric acid
Dissolve in water
96
What happens when you use a more concentrated acid in an experiment?
Speeds the reaction up
97
Why are some metals in group 1 of the periodic table
1 electron in their outer shell
98
What are 2 properties of a group 1 metal
Soft enough to be cut by a knife and low melting point
99
What’s a cathode
Negatively charged electrode
100
What’s an anode
Positively charged electrode
101
Reduction
Where a substance gains electrons
102
Oxidation
A reaction where a substance loses electrons, gains oxygen or loses hydrogen
103
What Is inert
Unreactive or inactive
104
Where are the 3 places natural resources come from
The earth, atmosphere and oceans
105
Why is recycling metals better than mining and extracting new metals
Uses less energy than metal production
106
How can metals be recycled
Melting the metal down
107
Why is recycling with glass easy
Can be endlessly recycled without losing quality
108
What are the 4 stages of a life cycle assessment
Getting the raw material
Manufacturing and packaging
Using the product
Product disposal
109
What are the problems with a life cycle assessment
Usingg data that will produced the company’s preferred answer
110
Desalinationn process
Sea water heated by a Bunsen burner untill it boils
Salt remains in the liquid
Steam is cooledd and condensed to make potable water
111
why is carbon used to extract some metals from their ores
because it's a more reactive chemical agent than many metals, allowing it to displace the metal from its oxide
112
How to make a soluble salt from an insoluble base
Chose an acid
Chose an insoluble base
Warm the acid
Add the insoluble base to the acid until there is no further reaction
Freeze the mixture
Heat the solution to evaporate the water
Crystals of salt will start to form
