SCH3U Periodicity Test Review
Atomic Structure and the Periodic Table
Extra practice questions using the
online textbook are posted on the
website.
1. Which is greater in mass – a proton or an electron?
2. Where are the most reactive elements located in the periodic
Classroom textbook also has extra
table?
practice.
3. What is the periodic law?
These are random sample questions
4. What patterns can you identify within a typical period in the
periodic table? Describe a typical pattern. Be sure you name the to get you thinking!
groups involved.
5. Create a chart to distinguish between the differences between metals and non-metals.
6. Identify the properties and characteristics of different families and groups of the periodic table
(halogens, alkali metals, noble gases, transition metals, alkaline earth metals).
7. Rank each of the following elements, Cl, Mg, S, in order of increasing atomic size. Explain your
answer.
8. Compare the atoms, nitrogen, oxygen, and sulfur. Between oxygen and nitrogen, which atom
has a greater effective nuclear charge? How do you know?
9. Which is greater – the force on each electron in the sodium atom or in the sodium ion? How
does this affect the size of each?
10. Based on the trends of the periodic table, explain if a nitrogen atom or a nitrogen ion has a
larger radius. Explain your reasoning.
11. Rank each of the following elements, K, Ca, Kr, in order of decreasing ionization energy.
Explain your answer.
12. Which element in the following pair, O and Li, will have the lower electron affinity? Explain your
answer.
13. Write equations that represent ionization energy and electron affinity. How are they different?
14. In your words, describe and explain the periodic trend for electronegativity. Please provide
examples.
15. Use a drawing of your choice to show clearly the relationship among the following terms:
valence, stable octet, electron, energy level.
16. Compare the following characteristics between bromine and potassium: number of protons,
atomic radius, ionic radius, electron affinity, number of valence electrons, shielding effect, and
first ionization energy.
17. Give the reason for the decrease in the first ionization energy for the alkaline-earth metals
(group 2) when moving down the group from beryllium to radium.\Of all the elements
discovered so far, state which one probably has the largest atomic radius. Explain your
reasoning.
18. Describe the relationship between the group number and the electron configuration of the
elements in a group
19. Arrange the following elements in order of decreasing atomic radius: sulfur, chlorine, aluminum
and sodium. Explain if your arrangement shows a periodic trend or a group trend.
20. Choose which statement about the alkali metals lithium and cesium is correct:
a. As the atomic number increases, the electronegativity of the elements increases.
b. As the atomic number increases, the melting point of the element increases.
c. As the atomic number increases, the first ionization energy of the element increases.
d. As the atomic number increases, the atomic radius decreases.
e. As the atomic number increases, the electron affinity increases.
SCH3U Periodicity Test Review
21. The following elements and ions have the same number of electrons. Determine which of the
following shows the correct order of their increasing radii.
a. K+ > Ar > Ca2+
b. Ar > K+ > Ca2+
c. Ca2+ > K+ >Ar
d. Ca2+ > Ar > K+
e. They all have the same radii
22. Determine which element you would expect to have the lowest first ionization energy
a. Li
b. Cs
c. H
d. He
e. Ba
23. The following is a list of the usual charge found on the ions of a series of elements
YW2+
Z2V3+
X+
State which elements are most likely to be metals.
a. V, W, and X
b. V and W
c. X and Y
d. Y and Z
e. only X
24. Most noble gases do not react because their atoms already have complete valence shells.
However, large noble gas atoms can be made to form compounds.
a. Name a larger noble gas that may be able to react.
b. Name two elements that larger noble gases may be able to combine with. Explain your
choices.
c. Would a compound that contains a larger noble gas and another element follow the octet
rule? Explain.
d. Why do you think large noble gas atoms form compounds but small noble gas atoms do
not? Explain.
25. Explain the trend of reactivity in group 7 in terms of electron affinity. Provide diagrams and
examples to support your answer.
26. The first, second, and third ionization energies for a certain element are 0.736 MJ/mol, 1.45
MJ/mol, and 7.72 MJ/mol respectively.
a. State in which group of the periodic table you would expect to find this element. Explain
your answer.
b. Predict if the fourth ionization energy would be greater or smaller than 25 MJ/mol.
Explain your reasoning.
27. An element has the following successive ionization energies below. Predict and explain what
group the following element would occupy.
IE1 = 1.1 MJ
IE2 = 2.2 MJ
IE3 = 20.6 MJ
IE4 = 26.2 MJ
IE5 = 37.8 MJ
IE6 = 47.3 MJ