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Atomic Structure
Question Paper 1
Level
IGCSE
Subject
Chemistry (4402)
Exam Board
AQA
Unit
C2
Topic
Sub-Topic
Atomic Structure; Analysis and Quantitative
Chemistry
Atomic Structure
Booklet
Question Paper 1
Time Allowed:
55
Score:
/ 55
Percentage:
/100
minutes
Grade Boundaries:
Page 1
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Q1.This question is about magnesium.
(a)
(i)
The electronic structure of a magnesium atom is shown below.
Use the correct answer from the box to complete each sentence.
electrons
neutrons
protons
shells
The nucleus contains protons and ..................
The particles with the smallest relative mass that move around the nucleus are
called ..................
Atoms of magnesium are neutral because they contain the same number of
electrons
and ..................
(3)
(ii)
A magnesium atom reacts to produce a magnesium ion.
Which diagram shows a magnesium ion?
Tick ( ) one box.
Page 2
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(1)
(b)
Magnesium and dilute hydrochloric acid react to produce magnesium chloride
solution and hydrogen.
Mg(s) + 2 HCl(aq)
(i)
MgCl2(aq) + H2(g)
State two observations that could be made during the reaction.
1 ............................................................................................................
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2 ............................................................................................................
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(2)
(ii)
In this question you will be assessed on using good English, organising
information clearly and using specialist terms where appropriate.
Describe a method for making pure crystals of magnesium chloride from
magnesium and dilute hydrochloric acid.
In your method you should name the apparatus you will use.
You do not need to mention safety.
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Page 3
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(6)
(Total 12 marks)
Q2.This question is about atoms.
Atoms contain electrons, neutrons and protons.
(a)
(i)
Which of these particles has a positive charge?
Tick ( ) one box.
Electron
Neutron
Proton
(1)
(ii)
Which of these particles does not have an electrical charge?
Tick ( ) one box.
Electron
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Neutron
Proton
(1)
(b)
How are the elements in the periodic table arranged?
Tick ( ) one box.
In order of increasing atomic number
In order of increasing mass number
In order of increasing reactivity
(1)
(c)
The diagram shows the arrangement of the electrons in an atom of fluorine.
(i)
How many protons are in an atom of fluorine?
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Tick ( ) one box.
2
7
9
(1)
(ii)
The boiling point of fluorine is −188 °C.
What is the state of fluorine at room temperature?
Tick ( ) one box.
Solid
Liquid
Gas
(1)
(d)
Fluorine reacts with copper to form an ionic compound.
(i)
Explain, in terms of electrons and electronic structure, what happens to a
fluorine atom when it reacts with copper.
Use the diagram above to help you to answer this question.
Page 6
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(2)
(ii)
Describe a chemical test which would show that a solution contains copper(II)
ions.
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(2)
(Total 9 marks)
Q3.Some students were investigating the rate at which carbon dioxide gas is produced when
metal carbonates react with an acid.
One student reacted 1.00 g of calcium carbonate with 50 cm 3, an excess, of dilute
hydrochloric acid.
The apparatus used is shown in Diagram 1.
Diagram 1
Page 7
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Dilute hydrochloric acid
(a)
Complete the two labels for the apparatus on the diagram.
(2)
(b)
The student measured the volume of gas collected every 30 seconds.
The table shows the student’s results.
Time in
seconds
Volume of carbon
dioxide
collected in cm3
30
104
60
(i)
90
198
120
221
150
232
180
238
210
240
240
240
Diagram 2 shows what the student saw at 60 seconds.
Diagram 2
Page 8
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What is the volume of gas collected?
Volume of gas = .................... cm3
(1)
(ii)
Why did the volume of gas stop changing after 210 seconds?
...............................................................................................................
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(1)
(c)
Another student placed a conical flask containing 1.00 g of a Group 1 carbonate
(M2CO3) on a balance.
He then added 50 cm3, an excess, of dilute hydrochloric acid to the flask and
measured the mass of carbon dioxide given off.
The equation for the reaction is:
M2CO3 + 2HCl
2MCl + H2O + CO2
The final mass of carbon dioxide given off was 0.32 g.
(i)
Calculate the amount, in moles, of carbon dioxide in 0.32 g carbon dioxide.
Relative atomic masses (Ar): C = 12; O = 16
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Moles of carbon dioxide = .................... moles
(2)
Page 9
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(ii)
How many moles of the metal carbonate are needed to make this number of
moles of carbon dioxide?
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Moles of metal carbonate = .................... moles
(1)
(iii)
The mass of metal carbonate used was 1.00 g.
Use this information, and your answer to part (c) (ii), to calculate the relative
formula mass (Mr) of the metal carbonate.
If you could not answer part (c) (ii), use 0.00943 as the number of moles of
metal carbonate. This is not the answer to part (c) (ii).
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Relative formula mass (Mr) of metal carbonate = ....................
(1)
(iv)
Use your answer to part (c) (iii) to calculate the relative atomic mass (Ar) of the
metal in the metal carbonate (M2CO3) and so identify the Group 1 metal in the
metal carbonate.
If you could not answer part (c) (iii), use 230 as the relative formula mass of
the metal carbonate. This is not the answer to part (c) (iii).
To gain full marks, you must show your working.
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Relative atomic mass of metal is .........................................................
Identity of metal .....................................................................................
(3)
Page 10
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(d)
Two other students repeated the experiment in part (c).
(i)
When the first student did the experiment some acid sprayed out of the flask
as the metal carbonate reacted.
Explain the effect this mistake would have on the calculated relative atomic
mass of the metal.
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(3)
(ii)
The second student used 100 cm3 of dilute hydrochloric acid instead of 50 cm3.
Explain the effect, if any, this mistake would have on the calculated relative
atomic mass of the metal.
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(3)
(Total 17 marks)
Q4.(a)
Figure 1 shows an atom of element G.
Page 11
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Figure 1
Draw a ring around the correct answer to complete each sentence.
(i)
Label A shows
an electron
an ion
a nucleus
(1)
(ii)
The particle labelled B is
an isotope
a molecule
a neutron
(1)
(iii)
The mass number of element G is
5
6
11
(1)
(iv)
Use the periodic table to identify element G.
Element G is
boron
carbon
sodium
(1)
(b)
Figure 2 shows a compound of G and hydrogen.
Figure 2
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Draw a ring around the correct answer to complete each sentence.
(i)
The formula of the compound in Figure 2 is
GH3
G3H
3HG
(1)
(ii)
The type of bonding shown in Figure 2 is
covalent
ionic
metallic
(1)
(Total 6 marks)
Q5.(a)
The symbols for seven different elements are shown in Figure 1.
Figure 1
He
Be
Na
S
Ca
Fe
Choose the correct symbol from Figure 1 to answer each question.
You may use each symbol once, more than once or not at all.
Write the symbol that represents:
Page 13
Ar
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(i)
a Group 1 element
............................................................
(1)
(ii)
a transition metal
............................................................
(1)
(iii)
an element with electrons in the same number of energy levels as an atom of
argon (Ar)
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(1)
(iv)
an element which forms an oxide that dissolves in water to form an acidic
solution
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(1)
(v)
an element that forms a chloride with the formula XCl
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(1)
(b)
A teacher put a cube of sodium metal into water containing universal indicator, as
shown in Figure 2.
Figure 2
The equation for the reaction is:
Page 14
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(i)
2Na(s)
+
2H2O(l)
2NaOH (aq)
+
H2(g)
sodium
+
water
sodium
hydroxide
+
hydrogen
The sodium floated on the surface of the water. The universal indicator turned
purple.
Give three other observations that would be seen during the reaction.
1 ............................................................................................................
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2 ............................................................................................................
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3 ............................................................................................................
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(3)
(ii)
Name the ion that made the universal indicator turn purple.
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(1)
(c)
Figure 3 represents the electronic structure of a sodium atom.
Figure 3
In the space below, draw the electronic structure of a sodium ion. Include the charge
on the ion.
Page 15
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(2)
(Total 11 marks)
Page 16