Practice 3.2 Periodic trends with authentic IB Chemistry exam questions for both SL and HL students. This question bank mirrors Paper 1A, 1B, 2 structure, covering key topics like atomic structure, chemical reactions, and organic chemistry. Get instant solutions, detailed explanations, and build exam confidence with questions in the style of IB examiners.
Which metal has the strongest metallic bond?
State the meaning of the term mass number (A). State the difference between mass number and atomic number (Z). Show how these numbers can be used to determine the number and types of particles in an atom.
State the electronic configuration for a carbon atom. Calculate the number of protons, electrons and neutrons in a carbide ion, 12C4-, and state their relative positions in the ion.
Chlorine consists of 35Cl and 37Cl atoms. If the relative atomic mass, Ar, of chlorine is 35.5, calculate the percentage of 35Cl in a sample, given Ar(35Cl) = 35.0 and Ar(37Cl) = 37.0. In terms of their electronic structure, state two ways in which atoms of 35Cl are similar to 37Cl. Besides the difference in the mass and the number of neutrons, state one way in which compounds containing 35Cl differ from compounds containing 37Cl atoms.
Trends in atomic radii of elements are given in Table 8 of the Data Booklet. Account for the trend in atomic radii of the halogens (F → At) and the period 2 elements (Li → Ne).
Write the equation for the first ionisation of magnesium, including the states. With reference to its electronic configuration, account for the ionisation energy values for magnesium in the table below:
Energy (kJ mol-1) required to remove: 1st electron | 2nd electron | 3rd electron 740 | 1450 | 7740
Explain the general increase in trend in the first ionization energies of the period 3 elements, Na to Ar.
Which of the following is the electron configuration of a metallic element?
Which property shows a general increase from left to right across period 2, Li to F?
Which of the following properties of the halogens increase from F to I? I. Atomic radius II. Melting point III. Electronegativity
Which series represents atoms in order of decreasing atomic radius?
Properties of elements and their compounds can be related to the position of the elements in the periodic table.
Explain the decrease in atomic radius from K to Br.
Explain why the radius of the potassium ion, , is smaller than the radius of the oxide ion, .
Sketch a graph to show the relative values of the successive ionization energies of beryllium.
Predict, giving your reasons, whether or is likely to have a more exothermic enthalpy of hydration.
Which oxide dissolves in water to give a solution with a pH below 7?
What is the electron configuration of vanadium?