IBDP Official Exam Material
FREE Past paper Questions by Topic
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Topic 3: Periodicity
For both SL and HL students
1. [1 mark]
Which elements are considered to be metalloids?
I. Gallium
II. Germanium
III. Arsenic
A. I and II only
B. I and III only
C. II and III only
D. I, II and III
2. [1 mark]
Which property of elements increases down a group but decreases across a period?
A. Atomic radius
B. Electronegativity
C. Ionic radius
D. Ionization energy
3. [1 mark]
Which gases are acidic?
I. nitrogen dioxide
II. carbon dioxide
III. sulfur dioxide
II. carbon dioxide
III. sulfur dioxide
A. I and II only
B. I and III only
C. II and III only
D. I, II and III
4. [1 mark]
Which of the following is the electron configuration of a metallic element?
A. [Ne] 3s2 3p2
B. [Ne] 3s2 3p4
C. [Ne] 3s2 3p6 3d3 4s2
D. [Ne] 3s2 3p6 3d10 4s2 4p5
5. [1 mark]
Three elements, X, Y, and Z are in the same period of the periodic table. The relative sizes of their atoms are represented by the diagram.
6. [1 mark]
Which element is found in the 4th group, 6th period of the periodic table?
A. Selenium
B. Lead
C. Chromium
D. Hafnium
7. [1 mark]
State, giving a reason, whether carbon or nitrogen is the most electronegative element.
8. [1 mark]
The nitride ion and the magnesium ion are isoelectronic (they have the same electron configuration). Determine, giving a reason, which has the greater ionic radius.
9. [2 marks]
Suggest two reasons why atoms are no longer regarded as the indivisible units of matter.
10. [2 marks]
Electrons are arranged in energy levels around the nucleus of an atom.
Explain why the first ionization energy of calcium is greater than that of potassium.
11. [1 mark]
Which combination describes the acid–base nature of aluminium and phosphorus oxides?
12. [1 mark]
Which trend is correct, going down group 1?
A. Melting point increases
B. Reactivity decreases
C. First ionisation energy increases
D. Electronegativity decreases
13. [1 mark]
Which property increases down group 1?
A. atomic radius
B. electronegativity
C. first ionization energy
D. melting point
14. [1 mark]
Which is a d-block element?
A. Ca
B. Cf
C. Cl
D. Co
15. [2 marks]
Explain the general increase in trend in the first ionization energies of the period 3 elements, Na to Ar.
16. [2 marks]
The properties of elements can be predicted from their position in the periodic table.
Explain why Si has a smaller atomic radius than Al.
17. [2 marks]
Explain the decrease in radius from Na to Na+.
18. [1 mark]
Which of the following shows a general increase across period 3 from Na to Cl?
A. Ionic radius
B. Atomic radius
C. Ionization energy
D. Melting point
19. [1 mark]
Which oxide will dissolve in water to give the solution with the lowest pH?
A. P4O10
B. SiO2
C. Al2O3
D. MgO
20. [2 marks]
Outline why the chlorine atom has a smaller atomic radius than the sulfur atom.
21. [1 mark]
Comment on how international cooperation has contributed to the lowering of CFC emissions responsible for ozone depletion.
22. [1 mark]
Which property shows a general increase from left to right across period 2, Li to F?
A. Melting point
B. Electronegativity
C. Ionic radius
D. Electrical conductivity
26. [1 mark]
Which is an f-block element?
A. Sc
B. Sm
C. Sn
D. Sr
27. [9 marks]
(a) i. Define the term first ionization energy. (2)
ii. Write an equation, including state symbols, for the process occurring when measuring the first ionization energy of aluminium. (1)
(b) Explain why the first ionization energy of magnesium is greater than that of sodium. (3)
(c) Lithium reacts with water.
Write an equation for the reaction and state two observations that could be made during the reaction. (3)
28. [9 marks]
(a) The general trend in ionisation energy. (2)
(b) Any exceptions to the general trend. (4)
(c) The trend in the acid–base character of the oxides of the elements. (3)
29. [11 marks]
The graph of the first ionization energy plotted against atomic number for the first twenty elements shows periodicity
(a) Define the term first ionization energy and explain what is meant by the term periodicity. (2)
(b) Explain how the data from this graph provides evidence for the existence of principal energy levels and sub-levels within atoms. (4)
(c) State what is meant by the term second ionization energy. (1)
(d) Sketch and explain the shape of the graph obtained for the successive ionization energies of potassium against the number of electrons removed.
(Use a logarithmic scale for ionization energy on the y-axis) (4)
If you need the markscheme, including the examiners' reports for each question, and more exam and teaching materials on this topic, contact me through the contact page