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Chapter 10: Problem 3

In methane, \(\mathrm{CH}_{4}\), (a) Assign an oxidation state to each atom in the molecule. (Hint: Draw a dot diagram first.) (b) How many electrons does the \(C\) atom own by oxidation-state electron bookkeeping? (c) How many more or fewer valence electrons are assigned to the \(\mathrm{C}\) atom here than are present in a free \(C\) atom?

Short Answer

Expert verified
The oxidation state of Carbon (C) in $\mathrm{CH}_{4}$ is -4, and each Hydrogen (H) atom has an oxidation state of +1. The Carbon atom in methane owns 8 electrons by oxidation-state electron bookkeeping. The Carbon atom in methane has 4 more valence electrons than a free Carbon atom.

Step by step solution

01

Draw the Lewis Dot Structure

To draw the Lewis Dot Structure of methane, we first need to determine the number of valence electrons each atom has. Carbon (C) has 4 valence electrons, and each Hydrogen (H) atom has 1 valence electron. In methane, the carbon atom shares one electron with each of the four hydrogen atoms, forming a covalent bond. The Lewis Dot Structure will look like this: H | H - C - H | H Step 2: Assign Oxidation State to Each Atom
02

Assign Oxidation State

In covalent compounds, oxidation states are assigned based on the more electronegative element. In the case of CH₄, Hydrogen is the more electronegative element compared to Carbon. Therefore, the oxidation state of Carbon (C) is -4, and each Hydrogen (H) atom has an oxidation state of +1. Step 3: Find the Number of Electrons Owned by the Carbon Atom by Oxidation-State Electron Bookkeeping
03

Determine the Number of Electrons Owned by Carbon

According to the oxidation-state electron bookkeeping, the number of valence electrons owned by the carbon atom is equal to the number of its valence electrons in the free state (4) minus its oxidation state (-4). Electrons owned by C = Valence Electrons of Free C - Oxidation State of C in CH₄ Electrons owned by C = 4 - (-4) Electrons owned by C = 4 + 4 Electrons owned by C = 8 So, the number of electrons owned by the Carbon atom in methane by oxidation-state electron bookkeeping is 8. Step 4: Determine the Difference in Valence Electrons in Methane's Carbon Atom Compared to a Free Carbon Atom
04

Calculate the Difference in Valence Electrons

To find the difference in valence electrons assigned to the Carbon atom in Methane compared to a free Carbon atom, we calculate the difference between the number of electrons owned by Carbon in both states: Difference = Electrons owned by C in Methane - Valence electrons of free C Difference = 8 - 4 Difference = 4 Thus, in methane, the Carbon atom has 4 more valence electrons assigned to it than a free carbon atom.

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Most popular questions from this chapter

If you put a piece of iron in an aqueous solution of blue \(\mathrm{Cu}^{2+}\) ions, the spontaneous redox reaction \(\mathrm{Fe}+\mathrm{Cu}^{2+} \rightarrow \mathrm{Fe}^{2+}+\mathrm{Cu}\) will occur. An aqueous solution of \(\mathrm{Fe}^{2+}\) ions is red-brown. (a) What is oxidized? (b) What is reduced? (c) What is the oxidizing agent? (d) What is the reducing agent? (e) What will happen to the piece of iron over time? (f) Do the electrons move from the oxidizing agent to the reducing agent or from the reducing agent to the oxidizing agent? (g) How could you use this reaction to make a battery? (Explain and show your battery in a diagram, using a nail and a penny as your source of iron and copper, respectively.)

Lithium is a very active metal, so active that it reacts with water to make flammable hydrogen gas. \(\mathrm{Li}(s)+\mathrm{H}_{2} \mathrm{O}(l) \rightarrow \mathrm{LiOH}(s)+1 / 2 \mathrm{H}_{2}(g)\) (a) What metal would you use in combination with Li to make a battery having the highest voltage? (Consult the EMF series.) (b) Too rapid a discharge of a lithium battery (which can occur if there is a short circuit) can overheat a lithium battery and cause it to explode and catch fire. Why is trying to put out such a fire with water a bad idea? (c) Would lithium be the anode or cathode in a lithium ion battery? Explain.

In the upper atmosphere, sunlight can convert oxygen to ozone: \(2 \mathrm{O}_{2} \rightarrow \mathrm{O}_{3}+\mathrm{O}\) Ozone Is this a redox reaction? Completely justify your answer.

Hydrogen gas burns very well in the presence of oxygen to give water: \(2 \mathrm{H}_{2}+\mathrm{O}_{2} \rightarrow 2 \mathrm{H}_{2} \mathrm{O}\) In principle, should it be possible to use this chemical reaction to produce electricity? Explain.

Which of the following are electron-transfer reactions? For those that are, indicate which reactant is the reducing agent and which reactant is the oxidizing agent. (a) \(\mathrm{PF}_{3}+3 \mathrm{H}_{2} \mathrm{O} \rightarrow \mathrm{H}_{3} \mathrm{PO}_{3}+3 \mathrm{HF}\) (b) \(\mathrm{H}_{2}+\mathrm{Cl}_{2} \rightarrow 2 \mathrm{HCl}\) (c) \(2 \mathrm{Cr}_{2} \mathrm{O}_{3}+3 \mathrm{Si} \rightarrow 4 \mathrm{Cr}+3 \mathrm{SiO}_{2}\) (d) \(\mathrm{HCl}+\mathrm{NaOH} \rightarrow \mathrm{NaCl}+\mathrm{H}_{2} \mathrm{O}\)
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