Chapter 9

Evaluate Write a balanced chemical equation for the reaction of aluminum with oxygen to produce aluminum oxide.

A single-replacement reaction occurs between copper and silver nitrate. When 63.5 g of copper reacts with 339.8 g of silver nitrate, 215.8 g of silver is produced. Write a balanced chemical equation for this reaction. What other product formed? What is the mass of the second product?

Complete the following problems in scientific notation. Round off to the correct number of significant figures. (Chapter 2) a. \(\left(5.31 \times 10^{-2} \mathrm{cm}\right) \times\left(2.46 \times 10^{5} \mathrm{cm}\right)\) b. \(\left(6.42 \times 10^{-2} \mathrm{g}\right) \div\left(3.21 \times 10^{-3} \mathrm{g}\right)\) c. \(\left(9.87 \times 10^{4} \mathrm{g}\right)-\left(6.2 \times 10^{3} \mathrm{g}\right)\)

Differentiate between electron configuration and electron-dot structure. (Chapter 5)

Write the electron configuration for the element fitting each description. (Chapter 6) a. a metalloid in group 13 b. a nonmetal in group 15, period 3

Describe the formation of positive and negative ions. (Chapter 7)

Write the formula for the compounds made from each of the following pairs of ions. (Chapter 7) a. copper(I) and sulfite b. tin(IV) and fluoride c. gold(III) and cyanide d. lead(II) and sulfide

Balance Equations Create a flowchart describing how to balance a chemical equation