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WorksheetsChemistry Paper 1 GCSE (9-1)
Total questions: 108
Worksheet time: 53mins
Name
Class
Date
1.
What is the Top Number?
a)
Mass Number
b)
Atomic/Proton Number
2.
What is the Bottom Number?
a)
Mass Number
b)
Atomic/Proton Number
3.
Carbon has an Atomic Number of 6: Is Carbon-12 Stable?
a)
Yes
b)
No
4.
Carbon has an Atomic Number of 6: Is Carbon-14 Stable?
a)
Yes
b)
No
5.
Carbon has an Atomic Number of 6: Caron-14 has 8 what?
a)
Protons
b)
Neutrons
c)
Electrons
6.
Does Mr Have Multiple Elements?
a)
Yes
b)
No
7.
Does Ar Have Multiple Elements?
a)
Yes
b)
No
8.
NH3
a)
Ammonia
b)
Calcium Chloride
c)
Sodium Carbonate
d)
Sulfuric Acid
e)
Methane
9.
CaCl2
a)
Ammonia
b)
Calcium Chloride
c)
Sodium Carbonate
d)
Sulfuric Acid
e)
Methane
10.
Na2CO3
a)
Ammonia
b)
Calcium Chloride
c)
Sodium Carbonate
d)
Sulfuric Acid
e)
Methane
11.
CH4
a)
Ammonia
b)
Calcium Chloride
c)
Sodium Carbonate
d)
Sulfuric Acid
e)
Methane
12.
H2SO4
a)
Ammonia
b)
Calcium Chloride
c)
Sodium Carbonate
d)
Sulfuric Acid
e)
Methane
13.
Simple Distillation
a)
Solutions
b)
Mixtures
14.
Fractional Distillation
a)
Solutions
b)
Mixtures
15.
Solutions
a)
Simple Distillation
b)
Fractional Distillation
16.
Mixtures
a)
Simple Distillation
b)
Fractional Distillation
17.
Group 1 Up
a)
Less Reactive
b)
More Reactive
18.
Group 1 Down
a)
Less Reactive
b)
More Reactive
19.
Group 7 Up
a)
Less Reactive
b)
More Reactive
20.
Group 7 Down
a)
Less Reactive
b)
More Reactive
21.
Most Elements are?
a)
Metals
b)
Non-Metals
22.
Group 1
a)
Metals
b)
Non-Metals
23.
Group 1
a)
Alkali Metals
b)
Transition Metals
c)
Halogens
d)
Noble Gases
24.
Group 3
a)
Alkali Metals
b)
Transition Metals
c)
Halogens
d)
Noble Gases
25.
Group 7
a)
Alkali Metals
b)
Transition Metals
c)
Halogens
d)
Noble Gases
26.
Group 0
a)
Alkali Metals
b)
Transition Metals
c)
Halogens
d)
Noble Gases
27.
Group 1 Down
a)
Lower Boil
b)
Higher Boil
28.
Group 1 Up
a)
Lower Boil
b)
Higher Boil
29.
Group 1 With Water
a)
Hydrogen Gas and Metal Oxide
b)
Metal Chloride Salts
c)
Metal Oxide
30.
Group 1 With Chlorine
a)
Hydrogen Gas and Metal Oxide
b)
Metal Chloride Salts
c)
Metal Oxide
31.
Group 1 With Oxygen
a)
Hydrogen Gas and Metal Oxide
b)
Metal Chloride Salts
c)
Metal Oxide
32.
Hydrogen Gas and Metal Oxide
a)
Group 1 With Water
b)
Group 1 With Chlorine
c)
Group 1 With Oxygen
33.
Metal Chloride Salts
a)
Group 1 With Water
b)
Group 1 With Chlorine
c)
Group 1 With Oxygen
34.
Metal Oxide
a)
Group 1 With Water
b)
Group 1 With Chlorine
c)
Group 1 With Oxygen
35.
Halogens
a)
Colour
b)
No Colour
36.
Alkali Metals
a)
Colour
b)
No Colour
37.
Group 7 Down
a)
Lower Boil
b)
Higher Boil
38.
Group 7 Up
a)
Lower Boil
b)
Higher Boil
39.
Group 1
a)
Forms Positive Ions
b)
Forms Negative Ions
40.
Group 3
a)
Forms Positive Ions
b)
Forms Negative Ions
41.
Group 5
a)
Forms Positive Ions
b)
Forms Negative Ions
42.
Group 7
a)
Forms Positive Ions
b)
Forms Negative Ions
43.
Metalic Bonding
a)
Metal + Metal
b)
Metal + Non-Metal
c)
Non Metal + Non Metal
44.
Ionic Bonding
a)
Metal + Metal
b)
Metal + Non-Metal
c)
Non Metal + Non Metal
45.
Covalent Bonding
a)
Metal + Metal
b)
Metal + Non-Metal
c)
Non Metal + Non Metal
46.
Metal + Metal
a)
Metalic Bonding
b)
Ionic Bonding
c)
Covalent Bonding
47.
Metal + Non-Metal
a)
Metalic Bonding
b)
Ionic Bonding
c)
Covalent Bonding
48.
Non Metal + Non Metal
a)
Metalic Bonding
b)
Ionic Bonding
c)
Covalent Bonding
49.
Ionic Bonding
a)
One Loses, One Gains
b)
They Share
c)
Delocalised Electrons
50.
Covalent Bonding
a)
One Loses, One Gains
b)
They Share
c)
Delocalised Electrons
51.
Metalic Bonding
a)
One Loses, One Gains
b)
They Share
c)
Delocalised Electrons
52.
Diamond
a)
Each Carbon is Covalented 4 Times
b)
Each Carbon is Covalented 3 Times in a Hexagon
c)
One Sheet of Graphite
d)
Hollow Ball of Carbon
53.
Graphite
a)
Each Carbon is Covalented 4 Times
b)
Each Carbon is Covalented 3 Times in a Hexagon
c)
One Sheet of Graphite
d)
Hollow Ball of Carbon
54.
Graphene
a)
Each Carbon is Covalented 4 Times
b)
Each Carbon is Covalented 3 Times in a Hexagon
c)
One Sheet of Graphite
d)
Hollow Ball of Carbon
55.
Fullerenes
a)
Each Carbon is Covalented 4 Times
b)
Each Carbon is Covalented 3 Times in a Hexagon
c)
One Sheet of Graphite
d)
Hollow Ball of Carbon
56.
Avogadro Constant = 6.02*10^What?
a)
23
b)
24
c)
25
d)
26
e)
27
57.
Acid + Base
a)
Salt + Water
b)
Salt + Water + Carbon Dioxide
c)
Salt + Hydrogen
d)
Metal Hydroxide + Hydrogen
58.
Acid + Metal Carbonate
a)
Salt + Water
b)
Salt + Water + Carbon Dioxide
c)
Salt + Hydrogen
d)
Metal Hydroxide + Hydrogen
59.
Acid + Metal
a)
Salt + Water
b)
Salt + Water + Carbon Dioxide
c)
Salt + Hydrogen
d)
Metal Hydroxide + Hydrogen
60.
Metal + Water
a)
Salt + Water
b)
Salt + Water + Carbon Dioxide
c)
Salt + Hydrogen
d)
Metal Hydroxide + Hydrogen
61.
Acid + Metal Oxide/Hydroxide
a)
Salt + Water
b)
Salt + Water + Carbon Dioxide
c)
Salt + Hydrogen
d)
Metal Hydroxide + Hydrogen
62.
Salt + Water
a)
Acid + Base
b)
Acid + Metal Carbonate
c)
Acid + Metal
d)
Metal + Water
63.
Salt + Water + Carbon Dioxide
a)
Acid + Base
b)
Acid + Metal Carbonate
c)
Acid + Metal
d)
Metal + Water
64.
Salt + Hydrogen
a)
Acid + Base
b)
Acid + Metal Carbonate
c)
Acid + Metal
d)
Metal + Water
65.
Metal Hydroxide + Hydrogen
a)
Acid + Base
b)
Acid + Metal Carbonate
c)
Acid + Metal
d)
Metal + Water
66.
Losing Electrons
a)
Oxidation
b)
Reduction
67.
Gaining Electrons
a)
Oxidation
b)
Reduction
68.
Gaining Charge
a)
Oxidation
b)
Reduction
69.
Losing Charge
a)
Oxidation
b)
Reduction
70.
Oxidation
a)
Losing Electrons
b)
Gaining Electrons
71.
Reduction
a)
Losing Electrons
b)
Gaining Electrons
72.
Oxidation
a)
Losing Charge
b)
Gaining Charge
73.
Reduction
a)
Losing Charge
b)
Gaining Charge
74.
Reduction
a)
Negative Electrode
b)
Positive Electrode
75.
Oxidation
a)
Negative Electrode
b)
Positive Electrode
76.
Electrolysis
a)
Spilting Up
b)
Putting Together
77.
F (Floride)
a)
Halide
b)
Not Halide
78.
Cl (Chlorine)
a)
Halide
b)
Not Halide
79.
Br (Bromine)
a)
Halide
b)
Not Halide
80.
I (Iodine)
a)
Halide
b)
Not Halide
81.
Mg (Magnesium)
a)
Halide
b)
Not Halide
82.
C (Carbon)
a)
Halide
b)
Not Halide
83.
Ar (Argon)
a)
Halide
b)
Not Halide
84.
H (Hydrogen)
a)
Halide
b)
Not Halide
85.
The Negative Electrode
a)
Less Reactive than Hydrogen (Metal) or Hydrogen
b)
More Reactive than Hydrogen (Metal) or Hydrogen
c)
Halite If Possible or Oxygen and Water
d)
Oxygen and Water then Halites
86.
The Positive Electrode
a)
Less Reactive than Hydrogen (Metal) or Hydrogen
b)
More Reactive than Hydrogen (Metal) or Hydrogen
c)
Halite If Possible or Oxygen and Water
d)
Oxygen and Water then Halites
87.
pH of Water
a)
6
b)
7
c)
8
d)
9
e)
10
88.
Cm^3 to Dm^3
a)
/1000
b)
/100
c)
*1
d)
*100
e)
*1000
89.
Dm^3 to Cm^3
a)
/1000
b)
/100
c)
*1
d)
*100
e)
*1000
90.
When a reaction is at Equilibrium the Reactants and Products are always Equal
a)
true
b)
false
91.
Moles =
a)
Mass(g) / Mr
b)
Mr / Mass(g)
c)
Mr * Mass(g)
92.
1
a)
Using a Pipette and Pipette filler, add a set volume of the alkali to a conical flask. Add 2 or 3 drops of indicator as well.
b)
Use a funnel to fill a burette with acid of known concentration. Record the initial volume of acid in the burette.
c)
Using the burette, add the acid to the alkali, a drop at a time and keep swirling.
d)
When there is a sudden change in colour, stop dropping acid.
e)
Record the final volume of acid in the burette, and start the chemical calculation.
93.
2
a)
Using a Pipette and Pipette filler, add a set volume of the alkali to a conical flask. Add 2 or 3 drops of indicator as well.
b)
Use a funnel to fill a burette with acid of known concentration. Record the initial volume of acid in the burette.
c)
Using the burette, add the acid to the alkali, a drop at a time and keep swirling.
d)
When there is a sudden change in colour, stop dropping acid.
e)
Record the final volume of acid in the burette, and start the chemical calculation.
94.
3
a)
Using a Pipette and Pipette filler, add a set volume of the alkali to a conical flask. Add 2 or 3 drops of indicator as well.
b)
Use a funnel to fill a burette with acid of known concentration. Record the initial volume of acid in the burette.
c)
Using the burette, add the acid to the alkali, a drop at a time and keep swirling.
d)
When there is a sudden change in colour, stop dropping acid.
e)
Record the final volume of acid in the burette, and start the chemical calculation.
95.
4
a)
Using a Pipette and Pipette filler, add a set volume of the alkali to a conical flask. Add 2 or 3 drops of indicator as well.
b)
Use a funnel to fill a burette with acid of known concentration. Record the initial volume of acid in the burette.
c)
Using the burette, add the acid to the alkali, a drop at a time and keep swirling.
d)
When there is a sudden change in colour, stop dropping acid.
e)
Record the final volume of acid in the burette, and start the chemical calculation.
96.
5
a)
Using a Pipette and Pipette filler, add a set volume of the alkali to a conical flask. Add 2 or 3 drops of indicator as well.
b)
Use a funnel to fill a burette with acid of known concentration. Record the initial volume of acid in the burette.
c)
Using the burette, add the acid to the alkali, a drop at a time and keep swirling.
d)
When there is a sudden change in colour, stop dropping acid.
e)
Record the final volume of acid in the burette, and start the chemical calculation.
97.
Can you remeber 10 elements in the Reactivty Series, in order? (Including Carbon and Hydrogen)
a)
Yes
b)
No
98.
Steps in a Fuel Cell: 1
a)
The Electrolyte is Potassium Hydroxide, the Electrodes are often porous Carbon with a catalyst, H goes into -, O goes into +
b)
At the – Electrode, Hydrogen loses electrons to Make H+ ions
c)
At the + Electrode, Oxygen gains electrons to Make O- ions
d)
The H+ ions and O- ions join to make water.
e)
The Electrons from through an external circuit from the + to the -, this is the electric current.
99.
Steps in a Fuel Cell: 2
a)
The Electrolyte is Potassium Hydroxide, the Electrodes are often porous Carbon with a catalyst, H goes into -, O goes into +
b)
At the – Electrode, Hydrogen loses electrons to Make H+ ions
c)
At the + Electrode, Oxygen gains electrons to Make O- ions
d)
The H+ ions and O- ions join to make water.
e)
The Electrons from through an external circuit from the + to the -, this is the electric current.
100.
Steps in a Fuel Cell: 3
a)
The Electrolyte is Potassium Hydroxide, the Electrodes are often porous Carbon with a catalyst, H goes into -, O goes into +
b)
At the – Electrode, Hydrogen loses electrons to Make H+ ions
c)
At the + Electrode, Oxygen gains electrons to Make O- ions
d)
The H+ ions and O- ions join to make water.
e)
The Electrons from through an external circuit from the + to the -, this is the electric current.
101.
Steps in a Fuel Cell: 4
a)
The Electrolyte is Potassium Hydroxide, the Electrodes are often porous Carbon with a catalyst, H goes into -, O goes into +
b)
At the – Electrode, Hydrogen loses electrons to Make H+ ions
c)
At the + Electrode, Oxygen gains electrons to Make O- ions
d)
The H+ ions and O- ions join to make water.
e)
The Electrons from through an external circuit from the + to the -, this is the electric current.
102.
Steps in a Fuel Cell: 5
a)
The Electrolyte is Potassium Hydroxide, the Electrodes are often porous Carbon with a catalyst, H goes into -, O goes into +
b)
At the – Electrode, Hydrogen loses electrons to Make H+ ions
c)
At the + Electrode, Oxygen gains electrons to Make O- ions
d)
The H+ ions and O- ions join to make water.
e)
The Electrons from through an external circuit from the + to the -, this is the electric current.
103.
Neutralisation is an example of a xxxxx Reaction.
a)
Endothermic
b)
Exothermic
104.
Combustion is an example of a xxxxx Reaction.
a)
Endothermic
b)
Exothermic
105.
Citric acid + Sodium Hydrogencarbonate is an example of a xxxxx Reaction.
a)
Endothermic
b)
Exothermic
106.
Thermal Decomposition is an example of a xxxxx Reaction.
a)
Endothermic
b)
Exothermic
107.
Can you define Activation Energy?
a)
Yes
b)
No
108.
Group 8
a)
Alkali Metals
b)
Transition Metals
c)
Halogens
d)
Noble Gases
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