Textbook Question
What is the coordination number of the metal in each of the following complexes?
(d) [ZrF8]4-
(e) [Fe(EDTA)(H2O)]-
Ch.21 - Transition Elements and Coordination Chemistry
McMurry8th EditionChemistryISBN: 9781292336145
Not the one you use?Change textbookSelect a different textbook
Table of contents
- Ch.1 - Chemical Tools: Experimentation & Measurement143
- Ch.2 - Atoms, Molecules & Ions134
- Ch.3 - Mass Relationships in Chemical Reactions149
- Ch.4 - Reactions in Aqueous Solution157
- Ch.5 - Periodicity & Electronic Structure of Atoms92
- Ch.6 - Ionic Compounds: Periodic Trends and Bonding Theory73
- Ch.7 - Covalent Bonding and Electron-Dot Structures47
- Ch.8 - Covalent Compounds: Bonding Theories and Molecular Structure51
- Ch.9 - Thermochemistry: Chemical Energy104
- Ch.10 - Gases: Their Properties & Behavior138
- Ch.11 - Liquids & Phase Changes43
- Ch.12 - Solids and Solid-State Materials56
- Ch.13 - Solutions & Their Properties98
- Ch.14 - Chemical Kinetics79
- Ch.15 - Chemical Equilibrium107
- Ch.16 - Aqueous Equilibria: Acids & Bases94
- Ch.17 - Applications of Aqueous Equilibria125
- Ch.18 - Thermodynamics: Entropy, Free Energy & Equilibrium66
- Ch.19 - Electrochemistry130
- Ch.20 - Nuclear Chemistry73
- Ch.21 - Transition Elements and Coordination Chemistry122
- Ch.22 - The Main Group Elements155
- Ch.23 - Organic and Biological Chemistry43
Chapter 21, Problem 58
Do you expect a compound with vanadium in the +2 oxidation state to be an oxidizing or a reducing agent? Explain.
Verified step by step guidance1
Understand the concept of oxidation states: The oxidation state of an element in a compound indicates the degree of oxidation (loss of electrons) of that element. A positive oxidation state means the element has lost electrons.
Identify the oxidation state of vanadium: In this problem, vanadium is in the +2 oxidation state, meaning it has lost two electrons.
Determine the tendency of vanadium in the +2 state: A species with a lower oxidation state (like +2) has the potential to lose more electrons, but it can also gain electrons to reach a higher oxidation state.
Consider the role of reducing and oxidizing agents: A reducing agent donates electrons to another species and is itself oxidized. An oxidizing agent accepts electrons from another species and is itself reduced.
Analyze vanadium's behavior: Since vanadium in the +2 oxidation state can gain electrons to reach a higher oxidation state, it is more likely to act as a reducing agent, donating electrons to other species.
Verified video answer for a similar problem:
This video solution was recommended by our tutors as helpful for the problem above.
Was this helpful?
Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Oxidation States
Oxidation states indicate the degree of oxidation of an atom in a compound. In this context, vanadium in the +2 oxidation state means it has lost two electrons. Understanding oxidation states is crucial for predicting the behavior of elements in redox reactions, as they determine whether a species can gain or lose electrons.
Recommended video:
Guided course
02:42
Oxidation Numbers
Reducing Agents
A reducing agent is a substance that donates electrons in a chemical reaction, causing another species to be reduced. When a compound has a lower oxidation state, like vanadium in +2, it is often a good reducing agent because it can easily lose more electrons to achieve a higher oxidation state, thus facilitating the reduction of other substances.
Recommended video:
Guided course
01:01Oxidizing and Reducing Agents
Redox Reactions
Redox (reduction-oxidation) reactions involve the transfer of electrons between two species, where one is oxidized and the other is reduced. The ability of a compound to act as an oxidizing or reducing agent is determined by its oxidation state and electron affinity. In this case, vanadium in the +2 state is likely to act as a reducing agent, as it can donate electrons to other species.