Ch.22 - The Main Group Elements
McMurry8th EditionChemistryISBN: 9781292336145
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TOC.tableOfContents
- Ch.1 - Chemical Tools: Experimentation & Measurement170
- Ch.2 - Atoms, Molecules & Ions160
- Ch.3 - Mass Relationships in Chemical Reactions169
- Ch.4 - Reactions in Aqueous Solution199
- Ch.5 - Periodicity & Electronic Structure of Atoms102
- Ch.6 - Ionic Compounds: Periodic Trends and Bonding Theory92
- Ch.7 - Covalent Bonding and Electron-Dot Structures61
- Ch.8 - Covalent Compounds: Bonding Theories and Molecular Structure59
- Ch.9 - Thermochemistry: Chemical Energy122
- Ch.10 - Gases: Their Properties & Behavior155
- Ch.11 - Liquids & Phase Changes54
- Ch.12 - Solids and Solid-State Materials73
- Ch.13 - Solutions & Their Properties120
- Ch.14 - Chemical Kinetics98
- Ch.15 - Chemical Equilibrium125
- Ch.16 - Aqueous Equilibria: Acids & Bases110
- Ch.17 - Applications of Aqueous Equilibria147
- Ch.18 - Thermodynamics: Entropy, Free Energy & Equilibrium86
- Ch.19 - Electrochemistry154
- Ch.20 - Nuclear Chemistry96
- Ch.21 - Transition Elements and Coordination Chemistry156
- Ch.22 - The Main Group Elements187
- Ch.23 - Organic and Biological Chemistry51
Capitolo 22, Problema 10
Consider the following oxoacids: HClO, HClO2, HClO3, and HClO4. In which oxoacid does chlorine have an oxidation state of +5? Which oxoacid is the strongest?
(LO 22.17)
(a) HClO has a Cl oxidation state of +5, and HClO4 is the strongest acid.
(b) HClO2 has a Cl oxidation state of +5, and HClO is the strongest acid.
(c) HClO3 has a Cl oxidation state of +5, and HClO4 is the strongest acid.
(d) HClO4 has a Cl oxidation state of +5, and HClO is the strongest acid.
Guida verificata passo dopo passo1
Step 1: Determine the oxidation state of chlorine in each oxoacid. Use the formula: Oxidation state of Cl = (Total charge of the compound) - (Sum of oxidation states of other elements).
Step 2: For HClO, assign oxidation states: H is +1, O is -2. Solve for Cl: +1 + Cl - 2 = 0.
Step 3: For HClO2, assign oxidation states: H is +1, each O is -2. Solve for Cl: +1 + Cl + 2(-2) = 0.
Step 4: For HClO3, assign oxidation states: H is +1, each O is -2. Solve for Cl: +1 + Cl + 3(-2) = 0.
Step 5: For HClO4, assign oxidation states: H is +1, each O is -2. Solve for Cl: +1 + Cl + 4(-2) = 0.
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Concetti chiave
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Oxidation State
The oxidation state of an element in a compound indicates the degree of oxidation or reduction of that element. It is a theoretical charge that an atom would have if all bonds were ionic. In oxoacids, the oxidation state of the central atom (like chlorine in HClO, HClO2, HClO3, and HClO4) can be determined by considering the number of oxygen atoms and the overall charge of the molecule.
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Oxidation Numbers
Oxoacids Strength
The strength of oxoacids is influenced by the number of oxygen atoms bonded to the central atom. Generally, as the number of oxygen atoms increases, the acid strength increases due to greater resonance stabilization of the conjugate base. In this case, HClO4, with four oxygen atoms, is the strongest acid among the given oxoacids.
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Resonance Structures
Resonance structures are different ways of drawing the same molecule that illustrate the delocalization of electrons. In oxoacids, resonance can stabilize the conjugate base formed after deprotonation. The more resonance structures available, the more stable the conjugate base, which typically correlates with stronger acid behavior, as seen in HClO4 compared to the other oxoacids.
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