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Solving Problems: A Chemistry Handbook
Chemistry: Matter and Change
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SOLVING PROBLEMS:
A CHEMISTRY HANDBOOK
CHAPTER 6
normally form chemical bonds). These atoms are small and can gain
only one or two electrons to have a stable noble-gas configuration.
Therefore, when these elements form a chemical bond, their attraction for electrons is large.
Electronegativities generally increase across a period and
decrease down through a group.
Practice Problems
21. For each of the following pairs, predict which atom has the
higher electronegativity.
a. Mg, Na
d. Ca, Ba
b. Na, Al
e. S, O
c. Cl, I
f. Se, Br
Chapter 6 Review
22. Explain why the word periodic is applied to the table of elements.
23. Why do elements in a group in the periodic table exhibit similar
chemical properties?
24. What chemical property is common to the elements in group 18
of the periodic table? Why do these elements have this
property?
25. In terms of electron configurations, what does the group
number of the representative elements in the periodic table
tell you?
26. Describe the group and period trends in the following
atomic properties.
a. atomic radius
b. electronegativity
c. first ionization energy
d. ionic radius
27. Describe the relationship between the electronegativity value of
an element and the tendency of that element to gain or lose
electrons when forming a chemical bond.