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WorksheetsAQA Trilogy Chemistry Paper 1 Basics
Total questions: 69
Worksheet time: 35mins
Name
Class
Date
1.
What are the 3 sub-atomic particles called?
a)
potions, neutrons and electrons
b)
protons, neurons and electrons
c)
protons, neutrons and elections
d)
protons, neutrons and electrons
2.
What is the mass number?
a)
Number of protons plus neutrons
b)
Number of protons plus electrons
c)
Number of neutrons plus electrons
3.
What is the atomic number?
a)
Number of protons plus electrons
b)
Number of protons
c)
Number of protons plus neutrons
d)
Number of protons, neutrons and electrons
4.
What is the charge on a proton?
a)
positive 1
b)
0
c)
negative 1
5.
What is the charge on a neutron?
a)
positive 1
b)
0
c)
negative 1
6.
What is the charge on an electron?
a)
positive 1
b)
0
c)
negative 1
7.
How many protons, neutrons and electrons does a lithium atom have?
a)
p=3 n=4 e=3
b)
p=3 n=7 e=3
c)
p=3 n=4 e=4
8.
Where are the protons and neutrons found?
a)
In isotopes
b)
In ions
c)
In the nucleus
d)
In shells
9.
Where are the electrons found?
a)
In isotopes
b)
In ions
c)
In the nucleus
d)
In shells
10.
How mant electrons fill each shell?
a)
2, 4, 6....
b)
2, 4, 8....
c)
8, 8, 8....
d)
2, 8, 8....
11.
An isotope is an atom with the same number of....
a)
protons and neutrons but a different number of electrons.
b)
neutrons and electrons but a different number of protons.
c)
protons and electrons but a different number of neutrons.
12.
In what order are elements on the modern periodic table?
a)
Mass number
b)
Atomic Mass
c)
Atomic number
d)
Relative Atomic Mass
13.
Which is NOT a property of metals.
a)
good electrical conductor
b)
good electrical insulator
c)
good thermal conductor
d)
high melting & boiling point
14.
Which is NOT a property of non-metals?
a)
low density
b)
good electrical conductor
c)
brittle
d)
good thermal insulator
15.
How did Mendeleev arrange the periodic table?
a)
Grouped elements with similar properties. Left gaps for undiscovered elements.
b)
Grouped elements with different properties. Left gaps for undiscovered elements.
16.
Lithium + water ->
a)
lithium oxide + hydrogen
b)
lithium hydroxide + water
c)
lithium hydroxide + hydrogen
17.
What would you NOT see if potassium reacted with water?
a)
Metal would sink
b)
Metal moves along surface of water
c)
Lilac flame
d)
Fizzing
18.
Sodium chloride + fluorine -->
a)
Sodium chloride + fluorine
b)
Sodium + chlorine
c)
Sodium fluoride + chlorine
19.
Why are Group 0/Noble gases unreactive?
a)
They are gases
b)
Full outer shell of electrons
c)
Too many protons
20.
Why is fluorine more reactive than bromine?
a)
Fluorine has less shells so attraction between nucleus and outer electrons is stronger
b)
Fluorine has more shells so attraction between nucleus and outer electrons is stronger
21.
Why is potassium more reactive than sodium?
a)
Potassium has more shells so attraction between nucleus and outer electrons is stronger
b)
Potassium has more shells so attraction between nucleus and outer electrons is weaker
22.
From which alkali metal is it easiest to remove the outer electron?
a)
Li
b)
Na
c)
K
23.
Which halogen is it easiest to give an outer electron?
a)
F
b)
Cl
c)
Br
24.
What type of structure & bonding is in H2O?
a)
Simple molecular covalent
b)
Giant covalent
c)
Giant ionic
d)
Giant metallic
25.
What type of bonding is in graphine?
a)
Simple molecular covalent
b)
Giant covalent
c)
Giant ionic
d)
Giant metallic
26.
What type of bonding is in magnesium chloride?
a)
Simple molecular covalent
b)
Giant covalent
c)
Giant ionic
d)
Giant metallic
27.
What type of bonding is in calcium?
a)
Simple molecular covalent
b)
Giant covalent
c)
Giant ionic
d)
Giant metallic
28.
What type of bonding is in sodium chloride?
a)
Simple molecular covalent
b)
Giant covalent
c)
Giant ionic
d)
Giant metallic
29.
What type of bonding is in silicon dioxide?
a)
Simple molecular covalent
b)
Giant covalent
c)
Giant ionic
d)
Giant metallic
30.
Why are alloys harder than pure metals?
a)
Distorted structure. Layers can not slide.
b)
Distorted structure. Layers can slide.
31.
Why does sodium chloride have a high melting point?
a)
Lots of energy needed to break the strong electrostatic forces between positive metal ions and electrons.
b)
Lots of energy needed to break the strong electrostatic forces between oppositely charged ions.
32.
Why can ionic compounds only conduct electricity when molten or in a solution?
a)
Ions are free to move so can carry charge through the structure.
b)
Electrons are free to move so can carry charge through the structure.
33.
Why is methane a gas at room temperature?
a)
Weak intermolecular forces between molecules, so little energy needed to break.
b)
Weak bonds, so little energy needed to break.
34.
Why is diamond hard?
a)
4 strong covalent bonds between carbons.
b)
4 weak covalent bonds between carbons.
35.
Why does anything conduct electricity?
a)
Charged particles can move
b)
Charged particles can flow throughout the structure
36.
How many elements are in (NH4)2CO3?
a)
4
b)
7
c)
2
d)
3
37.
How many atoms are in (NH4)2CO3?
a)
14
b)
4
c)
13
d)
9
38.
Calculate the Mr of H2O. (H=1, O=16)
a)
3
b)
17
c)
16
d)
18
39.
1.50 moles of concentration of 5.00 mol/dm3. What is the volume in dm3?
a)
7.5
b)
0.3
c)
3.33
40.
Find the anomally in the following results: 33, 28, 16, 29, 31.
a)
33
b)
28
c)
16
d)
29
41.
Find the mean of the following results: 33, 28, 16, 29, 31.
a)
30
b)
31
c)
27
d)
34
42.
Place the metals in order of reactivity (most reactive to least reactive)
a)
Magnesium, iron, copper, gold, potassium
b)
Potassium, gold, magnesium, iron, copper
c)
Magnesium, potassium, iron, copper, gold
d)
Potassium, magnesium, iron, copper, gold
43.
Metal + Acid ->
a)
Salt + Hydrogen
b)
Salt + Water + Carbon dioxide
c)
Salt + Water
44.
Metal oxide + Acid ->
a)
Salt + Hydrogen
b)
Salt + Water + Carbon dioxide
c)
Salt + Water
45.
Metal hydroxide + Acid ->
a)
Salt + Hydrogen
b)
Salt + Water + Carbon dioxide
c)
Salt + Water
46.
Metal carbonate + Acid ->
a)
Salt + Hydrogen
b)
Salt + Water + Carbon dioxide
c)
Salt + Water
47.
Why can lead be extracted by displacement using carbon?
a)
Lead is less reactive than carbon.
b)
Carbon is less reactive than lead.
48.
What does reduction mean?
a)
Loss of oxygen, gain of electrons
b)
Gain of oxygen, loss of electrons
49.
What does oxidation mean?
a)
Loss of oxygen, gain of electrons
b)
Gain of oxygen, loss of electrons
50.
Sodium oxide + sulfuric acid ->
a)
Sodium sulfate + water
b)
Sodium sulfate + hydrogen
c)
Sodium sulfate + water + carbon dioxide
51.
Calcium carbonate + hydrochloric acid ->
a)
Calcium chloride + water
b)
Calcium chloride + hydrogen
c)
Calcium chloride + water + carbon dioxide
52.
Which would you NOT do if you prepared dry crystals of copper sulfate?
a)
Add excess copper oxide
b)
Boil it until dry
c)
Add sulfuric acid to beaker
d)
Filter
53.
What does electrolysis mean?
a)
Breaking down of covalent compounds using electricity.
b)
Breaking down of ionic compounds using electricity.
54.
Which ion goes to the negative electrode and why?
a)
Positive ion, opposites attract.
b)
Negative ion, opposites attract.
55.
Which ion goes to the positive electrode and why?
a)
Positive ion, opposites attract.
b)
Negative ion, opposites attract.
56.
In which situations are ions free to move and can carry charge.
a)
Solid
b)
Liquid (molten)
c)
Aqueous (solution)
57.
What products are produced at which electrode when molten lead bromide (PbBr2) undergoes electrolysis?
a)
Positive electrode= lead ; Negative electrode= bromine
b)
Positive electrode= bromine ; Negative electrode= lead
58.
What products are produced at which electrode when molten aluminium oxide (Al2O3) undergoes electrolysis?
a)
Positive electrode= aluminium; Negative electrode= oxygen
b)
Positive electrode= oxygen ; Negative electrode= aluminium
59.
What ions are in water?
a)
H+ and OH-
b)
H2O
c)
H+ and O2-
60.
What products are produced when aqueous sodium chloride (NaCl) undergoes electrolysis?
a)
chlorine, hydrogen
b)
chlorine, sodium
c)
chlorine, hydrogen, sodium hydroxide
61.
What products are produced when aqueous copper sulfate (CuSO4) undergoes electrolysis?
a)
copper, oxygen, sulphuric acid
b)
copper, sulphur
62.
What temperature change would you expect in an exothermic reaction?
a)
Increase
b)
Decrease
63.
What temperature change would you expect in an endothermic reaction?
a)
Increase
b)
Decrease
64.
What does activation energy mean?
a)
The minimum amount of energy needed for particles to react.
b)
The maximum amount of energy needed for particles to react.
65.
Define exothermic reaction.
a)
Gives out energy to the surroundings.
b)
Takes in energy from the surroundings.
66.
Define endothermic reaction.
a)
Gives out energy to the surroundings.
b)
Takes in energy from the surroundings.
67.
Choose an exothermic reaction.
a)
thermal decomposition
b)
ice packs for injuries
c)
combustion
68.
Choose an endothermic reaction.
a)
thermal decomposition
b)
hand warmers
c)
combustion
69.
Calculate the temperature change if the initial temperature is 23°C and the final temperature is 18°C.
a)
23
b)
18
c)
51
d)
5
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