1. 1
   A museum is designing a historical display about the development of the Periodic Table, and wants to correctly describe how elements are ordered within it.

   (a)

   In the modern Periodic Table, elements are arranged in order of:

   [1 mark]

   • AIncreasing relative atomic mass only
   • BIncreasing proton number (atomic number)
   • CAlphabetical order of their names
   • DDecreasing melting point

   (b)

   The display also explains that elements are grouped into vertical columns and horizontal rows. What are these vertical columns called?

   [1 mark]

   • AGroups
   • BPeriods
   • CIsotopes
   • DSeries

   (c)

   Explain what information about an element's electronic configuration can be found from its group number and its period number in the Periodic Table.

   [2 marks]

   Total for question 1: 4 marks

2. 2
   A chemistry teacher shows the class an unfamiliar element, X, from Group II of the Periodic Table, and asks them to predict the charge on the ion it forms.

   (a)

   What charge would the ion of element X be expected to have?

   [1 mark]

   • A1+
   • B2+
   • C2−
   • D3+

   (b)

   The teacher then asks about an unfamiliar element, Y, from Group VI. What charge would the ion of element Y be expected to have?

   [1 mark]

   • A6+
   • B1−
   • C2−
   • D4+

   (c)

   Explain, in terms of electronic configuration, why elements in the same group of the Periodic Table tend to form ions with the same charge.

   [2 marks]

   Total for question 2: 4 marks

3. 3
   A materials scientist is investigating a newly isolated element, Z, and finds it has an electronic configuration of 2,8,7.

   (a)

   Using this information, identify the group and period the element belongs to, and explain your reasoning.

   [3 marks]

   (b)

   The scientist compares element Z with fluorine, which is in the same group but a period above. Predict, giving reasons based on their position in the Periodic Table, whether element Z would be more or less reactive than fluorine, and describe how the metallic or non-metallic character would be expected to change moving across Period 3 from element Z's group towards Group I.

   [4 marks]

   Total for question 3: 7 marks

4. 4
   In the 19th century, before several elements had been discovered, a chemist arranging elements into an early Periodic Table left gaps in the arrangement and used the pattern of properties in each group and period to predict the properties of the missing elements.

   (a)

   Explain how the position of a gap in the table (its group and period) can be used to predict properties such as reactivity, ion charge and metallic or non-metallic character of the missing element.

   [6 marks]

   (b)

   Suppose the gap left by the chemist was in Group I, between two known elements, one in the period above and one in the period below. Using the general trends known for Group I, predict and explain the melting point, density and reactivity of the missing element, relative to its known neighbours in the same group.

   [6 marks]

   Total for question 4: 12 marks

End of questions