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Chapter 3: Problem 58

Write balanced equations for the reaction of aluminum metal with the following nonmetals: (a) sulfur (b) bromine (c) nitrogen (d) oxygen (forming \(\mathrm{O}^{2-}\) ions) (e) oxygen (forming \(\mathrm{O}_{2}{ }^{2-}\), or peroxide ions)

Short Answer

Expert verified
(a) \(2\mathrm{Al} + 3\mathrm{S} \rightarrow \mathrm{Al}_{2}\mathrm{S}_{3}\) (b) \(2\mathrm{Al} + 6\mathrm{Br} \rightarrow 2\mathrm{AlBr}_{3}\) (c) \(2\mathrm{Al} + \mathrm{N}_{2} \rightarrow 2\mathrm{AlN}\) (d) \(4\mathrm{Al} + 3\mathrm{O}_{2} \rightarrow 2\mathrm{Al}_{2}\mathrm{O}_{3}\) (e) \(2\mathrm{Al} + 3\mathrm{O}_{2} \rightarrow \mathrm{Al}_{2}(\mathrm{O}_{2})_{3}\)

Step by step solution

01

(a) Reaction of aluminum with sulfur

First, we need to determine the compound formed by combining aluminum and sulfur. Aluminum has a charge of +3, and sulfur has a charge of -2. To balance the charges, the formula for the compound is Al2S3. Now, we must balance the equation: \(2\mathrm{Al} + 3\mathrm{S} \rightarrow \mathrm{Al}_{2}\mathrm{S}_{3}\)
02

(b) Reaction of aluminum with bromine

Aluminum has a charge of +3, and bromine has a charge of -1. So, the compound formed by combining them is AlBr3. Now, we must balance the equation: \(2\mathrm{Al} + 6\mathrm{Br} \rightarrow 2\mathrm{AlBr}_{3}\)
03

(c) Reaction of aluminum with nitrogen

Aluminum and nitrogen combine to form aluminum nitride. Aluminum has a charge of +3, and nitrogen has a charge of -3. So, the formula of the compound is AlN. Now, we must balance the equation: \(2\mathrm{Al} + \mathrm{N}_{2} \rightarrow 2\mathrm{AlN}\)
04

(d) Reaction of aluminum with oxygen (forming \(\mathrm{O}^{2-}\) ions)

Aluminum and oxygen combine to form aluminum oxide. Aluminum has a charge of +3, and oxygen (as \(\mathrm{O}^{2-}\) ions) has a charge of -2. The formula for the compound is Al2O3. Now, we must balance the equation: \(4\mathrm{Al} + 3\mathrm{O}_{2} \rightarrow 2\mathrm{Al}_{2}\mathrm{O}_{3}\)
05

(e) Reaction of aluminum with oxygen (forming \(\mathrm{O}_{2}{ }^{2-}\), or peroxide ions)

Aluminum and oxygen can also combine to form aluminum peroxide. In this case, oxygen has a charge of -1, as it forms peroxide ions (\(\mathrm{O}_{2}{ }^{2-}\)). The formula for aluminum peroxide is Al(O2)3. Now, we must balance the equation: \(2\mathrm{Al} + 3\mathrm{O}_{2} \rightarrow \mathrm{Al}_{2}(\mathrm{O}_{2})_{3}\)

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Most popular questions from this chapter

A 5.025-g sample of calcium is burned in air to produce a mixture of two ionic compounds, calcium oxide and calcium nitride. Water is added to this mixture. It reacts with calcium oxide to form \(4.832 \mathrm{~g}\) of calcium hydroxide. How many grams of calcium oxide are formed? How many grams of calcium nitride?

All the fertilizers listed below contribute nitrogen to the soil. If all these fertilizers are sold for the same price per gram of nitrogen, which will cost the least per 50 -lb bag? urea, \(\left(\mathrm{NH}_{2}\right)_{2} \mathrm{CO}\) ammonia, \(\mathrm{NH}_{3}\) ammonium nitrate, \(\mathrm{NH}_{4} \mathrm{NO}_{3}\) guanidine, \(\mathrm{HNC}\left(\mathrm{NH}_{2}\right)_{2}\)

When three moles of a metal oxide, \(\mathrm{MO}_{2}\), react with ammonia gas, the metal (M), water, and nitrogen gas are formed. (a) Write a balanced equation to represent the reaction. (b) When \(13.8 \mathrm{~g}\) of ammonia react with an excess of metal oxide, \(126 \mathrm{~g}\) of \(\mathrm{M}\) are formed. What is the molar mass for \(\mathrm{M}\) ? What is the identity of \(\mathrm{M} ?\)

Lead is a heavy metal that remains in the bloodstream, causing mental retardation in children. It is believed that \(3 \times 10^{-7} \mathrm{~g}\) of \(\mathrm{Pb}\) in \(1.00 \mathrm{~mL}\) of blood is a health hazard. For this amount of lead (a) how many atoms of lead are there in one \(\mathrm{mL}\) of a child's blood? (b) how many moles of lead are in \(1.00 \mathrm{~L}\) of blood?

Suppose that the atomic mass of \(\mathrm{C}-12\) is taken to be \(5.000 \mathrm{amu}\) and that a mole is defined as the number of atoms in \(5.000 \mathrm{~kg}\) of carbon-12. How many atoms would there be in one mole under these conditions? (Hint: There are \(6.022 \times 10^{23} \mathrm{C}\) atoms in \(12.00 \mathrm{~g}\) of \(\mathrm{C}-12 .\) )
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