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4.3 Review Questions 1. Give the oxidation state for the underlined element in each of the following species: (a) CaBr2 (e) S2O32–
(b) OF2
(f) BaH2
(c) C6H12O6
(g) ClO–
(d) K2O2
(h) S8
2. Complete and balance each of the following reactions. (States are not required.) Indicate which involve electron transfer. (a) Ca + O2 ➝
(b) CaO + H2O ➝
(c) Ca + H2O ➝
(d) Ca(OH)2 + HCl ➝
3. (a) What is an oxidizing agent?
(b) What is a reducing agent?
(c) How would you expect electronegativity to be related to the strength of each?
4. For each of the following reactions, indicate the species being oxidized and reduced and show the oxidation states above their symbols.
(a) 2 KClO3(s) ➝ 2 KCl(s) + 3 O2(g)
(b) Mg(s) + 2 AgNO3(aq) ➝ Mg(NO3)2(aq) + 2 Ag(s)
(c) P4(s) + 5 O2(g) ➝ 2 P2O5(g)
(d) NH4NO3(s) ➝ N2O(g) + 2 H2O(l)
5. In which chemical family would you expect to find: (a) the most readily oxidized elements? Explain.
(b) the most readily reduced elements? Explain.
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Chapter 4 Expressing and Measuring Chemical Change 187