Interpretation:
The element being oxidized and reduced in the given reaction should be determined.
Concept Introduction:
The oxidation state is defined as the charge(s) that an atom would have when electron(s) were transferred completely from a molecule or ion.
The element being oxidized is the one whose oxidation increases in the reaction whereas the reduced element is the one whose oxidation number decreases in the reaction.
Interpretation:
The element being oxidized and reduced in the given reaction should be determined.
Concept Introduction:
The oxidation state is defined as the charge(s) that an atom would have when electron(s) were transferred completely from a molecule or ion.
The element being oxidized is the one whose oxidation increases in the reaction whereas the reduced element is the one whose oxidation number decreases in the reaction.
Interpretation:
The element being oxidized and reduced in the given reaction should be determined.
Concept Introduction:
The oxidation state is defined as the charge(s) that an atom would have when electron(s) were transferred completely from a molecule or ion.
The element being oxidized is the one whose oxidation increases in the reaction whereas the reduced element is the one whose oxidation number decreases in the reaction.
Interpretation:
The element being oxidized and reduced in the given reaction should be determined.
Concept Introduction:
The oxidation state is defined as the charge(s) that an atom would have when electron(s) were transferred completely from a molecule or ion.
The element being oxidized is the one whose oxidation increases in the reaction whereas the reduced element is the one whose oxidation number decreases in the reaction.
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Introductory Chemistry: A Foundation
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- Xenon trioxide, XeO3, reacts with aqueous base to form the xenate anion, HXeO4. This ion reacts further with OH to form the perxenate anion, XeO64, in the following reaction: 2HXeO4(aq)+2OH(aq)XeO64(aq)+Xe(g)+O2(g)+2H2O(l) Identify the elements that are oxidized and reduced in this reaction. You will note that the equation is balanced with respect to the number of atoms on either side. Verify that the redox part of this equation is also balanced, that is, that the extents of oxidation and reduction are also equal.arrow_forwardThree reactions very important to the semiconductor industry are The reduction of silicon dioxide to crude silicon, SiO2(s) + 2 C(s) → Si(s) + 2 CO(g) ΔrH° = 689.9 kJ/mol The formation of silicon tetrachloride from crude silicon, Si(s) + 2 Cl2(g) → SiCl4(g) ΔrH° = −657.01 kJ/mol The reduction of silicon tetrachloride to pure silicon with magnesium, SiCl4(g) + 2 Mg(s) → 2 MgCl2(s) + Si(s) ΔrH° = −625.6 kJ/mol Calculate the overall enthalpy change when 1.00 mol sand, SiO2, changes into very pure silicon by this series of reactions.arrow_forwardConsider the reaction between oxygen (O2) gas and magnesium metal to form magnesium oxide. Using oxidation states, how many electrons would each oxygen atom gain, and how many electrons would each magnesium atom lose? How many magnesium atoms are needed to react with one oxygen molecule? Write a balanced equation for this reaction.arrow_forward
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