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Chapter 22: Problem 97

Indicate the oxidation state for the element noted in each of the following: a. \(\mathrm{H}\) in \(\mathrm{CaH}_{2}\) b. \(\mathrm{H}\) in \(\mathrm{H}_{2} \mathrm{O}\) c. \(\operatorname{Cin} \mathrm{CH}_{4}\) d. \(\mathrm{S}\) in \(\mathrm{H}_{2} \mathrm{SO}_{4}\)

Short Answer

Expert verified
a. H is -1; b. H is +1; c. C is -4; d. S is +6.

Step by step solution

01

Identify Oxidation States in Compounds

To determine oxidation states, recall the standard rules: Hydrogen is usually +1, but is -1 when bound to less electronegative elements (like metals). Oxygen is usually -2. The sum of oxidation states in a neutral compound must equal zero.
02

Determine Oxidation State of H in CaH2

In calcium hydride (\( \mathrm{CaH}_{2} \)), calcium (\( \mathrm{Ca} \)) is a metal that typically has an oxidation state of +2. Since there are two hydrogen atoms, and the compound is neutral, hydrogen must have an oxidation state of -1 each: \( 2(-1) + 2 = 0 \).
03

Determine Oxidation State of H in H2O

In water \( (\mathrm{H}_{2} \mathrm{O}) \), oxygen usually has an oxidation state of -2. There are two hydrogen atoms, which must balance this by having a +1 oxidation state each: \( 2(+1) - 2 = 0 \).
04

Determine Oxidation State of C in CH4

Consider methane \( (\mathrm{CH}_{4}) \): Hydrogen has a +1 oxidation state, so the four hydrogens contribute +4. Carbon's oxidation state must counterbalance these as the compound is neutral, resulting in \( \mathrm{C} = -4 \): \( -4 + 4(+1) = 0 \).
05

Determine Oxidation State of S in H2SO4

In sulfuric acid \( (\mathrm{H}_{2} \mathrm{SO}_{4}) \), hydrogen is +1 for each and there are two hydrogen atoms, contributing +2. Oxygen is -2 and there are four oxygen atoms contributing -8. Sulfur (\( \mathrm{S} \)) must balance them by having an oxidation state of +6: \( 2(+1)+\mathrm{S}+4(-2) = 0 \), hence \( \mathrm{S} = +6 \).

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Calcium Hydride and Oxidation State of Hydrogen
Calcium hydride, represented chemically as \( \mathrm{CaH}_{2} \), is a compound where calcium, a metal, is paired with hydrogen. In this compound, it is crucial to determine the oxidation states. For calcium hydride, we must consider the rules of oxidation states:
  • Elements in a compound strive to attain a stable electronic structure, often determined by their group in the periodic table.
  • Metals like calcium typically possess a positive oxidation state, commonly +2 due to their tendency to lose electrons.
  • Hydrogen, however, can have a more unique role, especially when bound to metals, as it takes an oxidation state of -1.
In \( \mathrm{CaH}_{2} \), hydrogen's role switches from its usual +1 to -1 because of calcium's higher electronegativity. By solving the equation \( 2(-1) + (+2) = 0 \), we find the oxidation state of hydrogen in calcium hydride is -1. This reversal of hydrogen's oxidation state signifies the formation of hydrides, a specialized type of chemical bonding.
Oxidation State of Hydrogen in Water
Water, known chemically as \( \mathrm{H}_{2}\mathrm{O} \), is a simple yet vital molecule in chemistry. It consists of two hydrogen atoms bonded to one oxygen atom. To grasp the concept of oxidation states:
  • Oxygen, in most compounds, holds an oxidation state of -2 since it is highly electronegative and tends to gain electrons.
  • Hydrogen, when combined with non-metals like oxygen, usually maintains a +1 oxidation state.
Using these guidelines, we can determine that in water, each hydrogen takes on a +1 oxidation state, while oxygen carries a -2. Balancing the equation \( 2(+1) + (-2) = 0 \), shows that the molecules neutralize each other out, making water a stable compound with a net charge of zero. This illustrates hydrogen's flexibility in oxidation states based on its bonding partners.
Understanding Methane and Carbon's Oxidation State
Methane, \( \mathrm{CH}_{4} \), is a simple hydrocarbon and a primary component of natural gas. Here, we look into the oxidation state of carbon:
  • Hydrogen, when it pairs with more electronegative elements like carbon, holds a +1 oxidation state.
  • In methane, there are four hydrogen atoms, so their combined contribution is \( 4(+1) \).
  • To balance this, carbon must have an oxidation state that offsets +4, making it \( -4 \).
The equation \( -4 + 4(+1) = 0 \) confirms that the compound is neutral, revealing carbon's oxidation state as -4. This example underscores the importance of understanding the role of electronegativity and electron sharing in covalent bonds.
Sulfuric Acid and Sulfur's Oxidation State
Sulfuric acid, or \( \mathrm{H}_{2}\mathrm{SO}_{4} \), is a significant and widely used chemical in many industrial applications. Determining the oxidation state of sulfur involves:
  • Each hydrogen has an oxidation state of +1, with two hydrogen atoms contributing +2.
  • Oxygen, common as a strong oxidizing element, has an oxidation state of -2, with four atoms contributing a total of -8.
  • To balance these, sulfur must have an oxidation state that counteracts these charges.
The calculation \( 2(+1) + \mathrm{S} + 4(-2) = 0 \) leads us to deduce \( \mathrm{S} = +6 \), ensuring the neutrality of the compound. Understanding the oxidation state of sulfur in sulfuric acid is vital for comprehending its reactivity and role in various chemical reactions.

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Most popular questions from this chapter

How is sodium hypochlorite prepared? Give the balanced chemical equation.

What are the oxidation numbers of sulfur in each of the following? a. \(\mathrm{S}_{8}\) b. \(\mathrm{CaS}\) c. \(\mathrm{CaSO}_{4}\) d. \(\mathrm{SCl}_{4}\)

Xenon tetrafluoride, \(\mathrm{XeF}_{4}\), is a colorless solid. Give the Lewis formula for the \(\mathrm{XeF}_{4}\) molecule. What is the hybridization of the xenon atom in this compound? What geometry is predicted by the VSEPR model for this molecule?

Baking powders contain sodium (or potassium) hydrogen carbonate and an acidic substance. When water is added to a baking powder, carbon dioxide is released. One kind of baking powder contains \(\mathrm{NaHCO}_{3}\) and sodium aluminum sulfate, \(\operatorname{NaAl}\left(\mathrm{SO}_{4}\right)_{2}\). Write the net ionic equation for the reaction that occurs in water solution.

Write equations for each of the following. a. reaction of \(\mathrm{H}_{2} \mathrm{~S}\) with \(\mathrm{SO}_{2}\) b. oxidation of \(\mathrm{SO}_{2}\) with \(\mathrm{Cr}_{2} \mathrm{O}_{7}^{2-}(a q)\) to \(\mathrm{SO}_{4}^{2-}\) c. reaction of hot, concentrated \(\mathrm{H}_{2} \mathrm{SO}_{4}\) with \(\mathrm{Cu}\) d. reaction of sulfur with \(\mathrm{Na}_{2} \mathrm{SO}_{3}\)
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