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Chapter 4: Problem 85

Consider the reaction between sodium metal and fluorine \(\left(\mathrm{F}_{2}\right)\) gas to form sodium fluoride. Using oxidation states, how many electrons would each sodium atom lose, and how many electrons would each fluorine atom gain? How many sodium atoms are needed to react with one fluorine molecule? Write a balanced equation for this reaction.

Short Answer

Expert verified
Each sodium atom loses one electron, and each fluorine atom gains one electron. Two sodium atoms are needed to react with one fluorine molecule. The balanced equation for the reaction is \(2 \mathrm{Na}(s) + \mathrm{F}_{2}(g) \rightarrow 2 \mathrm{NaF}(s)\).

Step by step solution

01

Determine the oxidation states of sodium and fluorine in their elemental forms.

Sodium is in its elemental form as a metal, and fluorine is in its elemental form as a diatomic molecule, F2. In their elemental forms, both sodium and fluorine have an oxidation state of 0.
02

Determine the oxidation states of sodium and fluorine in sodium fluoride.

Sodium fluoride is a binary ionic compound formed between sodium cations, Na+, and fluoride anions, F-. Sodium has a +1 oxidation state and fluorine has a -1 oxidation state in sodium fluoride.
03

Calculate the number of electrons lost by each sodium atom and gained by each fluorine atom.

To go from its elemental form to its combined form in sodium fluoride, each sodium atom loses an electron. The oxidation state of sodium increases from 0 to +1. Therefore, each sodium atom loses one electron. Each fluorine atom gains an electron to go from its elemental form to its combined form in sodium fluoride. The oxidation state of fluorine decreases from 0 to -1. Therefore, each fluorine atom gains one electron.
04

Determine the number of sodium atoms needed to react with one fluorine molecule.

Since each fluorine atom gains one electron and there are two fluorine atoms in a fluorine molecule, a fluorine molecule will gain a total of 2 electrons. To provide these 2 electrons, two sodium atoms are required, since each sodium atom can lose one electron.
05

Write a balanced equation for this reaction.

Now that we know that two sodium atoms are needed to react with one fluorine molecule to form two sodium fluoride molecules, we can write a balanced equation for this reaction: \[2 \mathrm{Na}(s) + \mathrm{F}_{2}(g) \rightarrow 2 \mathrm{NaF}(s)\] In summary, each sodium atom loses one electron, each fluorine atom gains one electron, and two sodium atoms are needed to react with one fluorine molecule. The balanced equation for the reaction between sodium metal and fluorine gas to form sodium fluoride is: \[2 \mathrm{Na}(s) + \mathrm{F}_{2}(g) \rightarrow 2 \mathrm{NaF}(s).\]

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What mass of solid aluminum hydroxide can be produced when \(50.0 \mathrm{~mL}\) of \(0.200 \mathrm{M} \mathrm{Al}\left(\mathrm{NO}_{3}\right)_{3}\) is added to \(200.0 \mathrm{~mL}\) of \(0.100 \mathrm{M} \mathrm{KOH} ?\)

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