Unit 1 – Metallic Bonding
Unit 1 - Jan 2009
Q1.
 (a)  (i)   Complete the electronic configuration of the magnesium atom.
(1)
1s2
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(ii)   Complete the electronic configuration of the chlorine atom.
(1)
1s2
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(b)  (i)   Write the equation, including state symbols, for the reaction of magnesium with chlorine.
(2)

(ii)  Name the type of bonding present in magnesium chloride.
(1)
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(iii)   Draw a diagram (using dots or crosses) to show the bonding in magnesium chloride.  Include ALL the electrons in each species and the charges present.
(3)

(c)  State the type of bonding that exists in solid magnesium.
(1)
Type
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*(d)  Explain fully why the melting temperature of magnesium is higher than that of
         sodium.
(3)
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(Total for question = 12 marks)

Unit 1 - Jun 2009
Q2.
 The graph shows the variation in melting temperatures of the elements across Period 3
 (Na to Ar) of the Periodic Table.

(a)  Complete the table below to show the type of structure and bonding for the elements
       shown.
(3)

(b)  Explain why silicon has a much higher melting temperature than sulfur.
(2)
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*(c)  Explain why the melting temperature increases from sodium to aluminium.
(2)
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 (d)  Magnesium forms the basic oxide magnesium oxide, MgO.  This oxide is almost insoluble in water.  On gentle warming with dilute sulfuric acid, magnesium oxide reacts to form aqueous magnesium sulfate solution.
*(i)  Describe how you would use the above reaction to prepare a pure sample of magnesium sulfate.
(5)
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(ii)  Suggest what action should be taken if a pupil spilt a small quantity of dilute sulfuric acid on a laboratory bench.
(1)
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(e)  The data in the table below will be useful when answering this question.

Magnesium carbonate reacts with dilute sulfuric acid.

(i)  Explain why the reaction between strontium carbonate and dilute sulfuric acid stops after a few seconds.
(1)
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(ii)  Strontium sulfate is produced when aqueous sodium sulfate is added to aqueous strontium chloride.
       Give the ionic equation for the reaction, including state symbols.
(2)

(Total for question = 16 marks)
Unit 1 - Jan 2010
Q3.
The bonding in magnesium oxide, MgO, is
   A      ionic.
   B      metallic and ionic.
   C      ionic and covalent.
   D      metallic and covalent.
(Total for question = 1 mark)

Unit 1 - Jun 2010
Q4.
Which of these statements is incorrect?
   A   The atomic radius of metals increases down a Group.	
   B   The trend in the melting temperature of successive elements across Period 2 is similar to that in Period 3.
   C   A metallic structure is held together by attractions between metal atoms and delocalized electrons.
   D   Na+ and O2- ions are isoelectronic.
(Total for question = 1 mark)

Unit 1 - Jan 2011
Q5.
 Metals usually have high melting temperatures and boiling temperatures because there are
   A     strong attractions between the ions.
   B     strong attractions between the delocalised electrons.
   C     strong attractions between the ions and the delocalised electrons.
   D     strong intermolecular forces.
(Total for question = 1 mark)

Unit 1 - Jun 2011
Q6.
Metals are good conductors of heat and electricity and usually have high melting temperatures and boiling temperatures.
(a) (i)   Describe the structure of a metal.
(2)

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      (ii)   Describe the bonding in a metal.
(2)

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(b) Explain why the melting temperature of magnesium (650 °C) is much higher than that of sodium (98 °C).
(3)
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(c) Explain how metals conduct electricity.
(2)
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(Total for Question = 9 marks)

Unit 1 - Jan 2012
Q7.
* The melting temperatures of the elements of Period 3 are given in the table below. Use these values to answer the questions that follow.

(a) Explain why the melting temperature of sodium is very much less than that of
             magnesium.
(3)
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(b) Explain why the melting temperature of silicon is very much greater than that of white phosphorus.
(3)
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 (c) Explain why the melting temperature of argon is the lowest of all the elements of Period 3.
(1)
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(d) Explain why magnesium is a good conductor of electricity whereas sulfur is a non-conductor.
(2)
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 (Total for question = 9 marks)

Unit 1 - Jan 2013
Q8.
 Metals are good conductors of electricity because
   A     metal atoms are arranged in a regular lattice.
   B     metal ions are very close to each other.
   C     metal ions are free to move through the lattice.
   D     electrons are free to move through the lattice.
(Total for question = 1 mark)

Unit 1 - Jun 2013
Q9.
(a)  In a mass spectrometer being used to determine relative atomic masses, gaseous atoms are ionized. The ions are then accelerated and deflected before being detected.

(i)  Explain how atoms are ionized in a mass spectrometer.
(1)
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(ii)  How are the ions accelerated in a mass spectrometer?
(1)
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(iii)  How are the ions deflected in a mass spectrometer?
(1)
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(b)  The following data were obtained from the mass spectrum of a sample of platinum.

Calculate the relative atomic mass of platinum in this sample. Give your answer to one decimal place.
(2)

(c)  In which block of the Periodic Table is platinum found?
(1)
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(d)  Most solids exist as lattice structures.

(i)  Complete the table, using a tick () if the substance conducts electricity or a cross () if the substance does not conduct electricity.
(2)

*(ii)  Explain the electrical conductivities of sodium and of sodium oxide in the solid and liquid states.
(3)
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(Total for Question = 11 marks)

Unit 1 - Jun 2014
Q10.
 Naturally occurring samples of potassium contain three isotopes, 39K, 40K and 41K.
(a)  The isotopes can be separated in a mass spectrometer.
(i)  In the diagram below, particles are ionized at A and detected at D.

Name the processes occurring in the mass spectrometer at B and C.
(2)
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C  ...................................................................................................................................... 

(ii)  A sample of potassium has the following composition.

Calculate the relative atomic mass of this sample of potassium, giving your answer to two decimal places.
(2)

(iii)  Complete the table below to show the numbers of sub-atomic particles in an atom of each of the isotopes 39K and 41K.
(1)

(iv)  Complete the electronic configuration for an atom of 39K.
(1)
1s2 ........................................................................................................................... 

(v)  Why is potassium placed after argon in the Periodic Table, even though it has a smaller relative atomic mass?
(1)
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*(vi)  Explain why a potassium ion is smaller than a potassium atom.
(2)
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(b)  The type of bonding in potassium is metallic.
Draw a labelled diagram to illustrate the metallic bonding in potassium.
(2)

(c)  The graph shows the variation of first ionization energy with atomic number for six successive elements in the Periodic Table, including potassium. The letters used to label the elements are not their symbols.

(i)  Define the term first ionization energy.
(3)
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(ii)  Identify, with a reason, which element is potassium.
(2)
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(Total for question = 16 marks)
Q11.
his question concerns the Periodic Table.
(a)  An atom of argon has mass number 40. Complete the table below showing the numbers of sub-atomic particles in this atom of argon. Use the Periodic Table as a source of data.
(1)

(b)  An atom of potassium has mass number 39. Explain why argon is placed before potassium in the modern Periodic Table.
(1)
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(c)  In the context of the Periodic Table, explain what is meant by the term periodicity.
(2)
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(d)  The graph shows the variation in melting temperatures of the elements across Period 3 (Na to Ar) of the Periodic Table.

(i)  Name one of the elements above that is composed of simple molecules at room temperature and pressure.
(1)
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(ii)  Silicon has a giant atomic structure. Explain how this structure results in the high melting temperature shown on the graph.
(2)
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(iii)  Explain why the melting temperature of magnesium is higher than that of sodium.
(3)
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(Total for question = 10 marks)