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Mobile App Chapter 3: Problem 4
The oxidation number of \(\mathrm{V}\) in \(\mathrm{Cs}_{4} \mathrm{Na}\left(\mathrm{HV}_{10} \mathrm{O}_{28}\right)\) is: (a) \(+2\) (b) \(+5\) (c) \(-2\) (d) \(+3\)
Short Answer
Expert verified
+5
Step by step solution
01
Understanding the Compound
Identify the components of the compound \(\mathrm{Cs}_{4}\mathrm{Na}(\mathrm{HV}_{10}\mathrm{O}_{28})\). It consists of cesium (Cs), sodium (Na), hydrogen (H), vanadium (V), and oxygen (O). The compound is neutral, so the sum of oxidation states must equal zero.
02
Assign Oxidation Numbers for Known Elements
Assign oxidation numbers to the elements with known values. For alkali metals in compounds, both cesium (Cs) and sodium (Na) have an oxidation number of +1. Oxygen (O) usually has an oxidation number of -2. The hydrogen (H) attached to the non-metal (oxygen in this case) has an oxidation number of +1.
03
Calculate Oxidation Numbers
Set up the equation based on the sum of the oxidation numbers multiplying by their subscripts and equal it to zero for the neutral compound: \[4(1) + 1(1) + 10(x) + 28(-2) + 1(1) = 0\], where x is the oxidation number of vanadium (V).
04
Solve for the Oxidation Number of Vanadium
Solve the equation for x: \[4 + 1 + 10x - 56 + 1 = 0\] which simplifies to \10x = 50\. Then, \[x = \frac{50}{10}\], which yields \[x = 5\].
05
Conclude the Oxidation Number
The oxidation number of vanadium (V) in the given compound is +5.
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Key Concepts
These are the key concepts you need to understand to accurately answer the question.
Chemistry Education
Mastering concepts like oxidation number calculation is essential in chemistry education, providing a strong foundation for understanding various chemical processes. Grasping these concepts requires familiarity with the electronic structure of atoms and their interactions in compounds.
Oxidation numbers represent the theoretical charge an atom would have if all bonds to atoms of different elements were completely ionic. By understanding oxidation numbers, students can predict the products of chemical reactions, balance redox equations, and comprehend the transfer of electrons.
Teachers aiming to enhance chemistry education should emphasize the importance of rules used to determine oxidation states, making use of examples and practice exercises to clarify these rules. Educational resources should incorporate visual aids and offer hands-on activities that cater to different learning styles, ensuring that all students, regardless of their background knowledge, can achieve a comprehensive understanding of oxidation numbers and their significance in chemistry.
Oxidation numbers represent the theoretical charge an atom would have if all bonds to atoms of different elements were completely ionic. By understanding oxidation numbers, students can predict the products of chemical reactions, balance redox equations, and comprehend the transfer of electrons.
Teachers aiming to enhance chemistry education should emphasize the importance of rules used to determine oxidation states, making use of examples and practice exercises to clarify these rules. Educational resources should incorporate visual aids and offer hands-on activities that cater to different learning styles, ensuring that all students, regardless of their background knowledge, can achieve a comprehensive understanding of oxidation numbers and their significance in chemistry.
Redox Reactions
Redox reactions, or oxidation-reduction reactions, are processes where electrons are transferred between substances. They are fundamental to various chemical and biological systems, such as cellular respiration and rust formation.
In redox reactions, oxidation refers to the loss of electrons, while reduction describes the gain of electrons. The substance that donates electrons undergoes oxidation and is termed the reducing agent. Conversely, the substance that accepts electrons is reduced and acts as the oxidizing agent.
To understand these reactions, identifying the changes in oxidation numbers is crucial. For instance, when a metal undergoes corrosion, its oxidation number increases as it loses electrons to oxygen. Therefore, teaching these concepts should involve applying oxidation states to monitor electron flow and deduce which substance is oxidized or reduced, strengthening the learner's ability to analyze and predict the outcomes of redox reactions.
In redox reactions, oxidation refers to the loss of electrons, while reduction describes the gain of electrons. The substance that donates electrons undergoes oxidation and is termed the reducing agent. Conversely, the substance that accepts electrons is reduced and acts as the oxidizing agent.
To understand these reactions, identifying the changes in oxidation numbers is crucial. For instance, when a metal undergoes corrosion, its oxidation number increases as it loses electrons to oxygen. Therefore, teaching these concepts should involve applying oxidation states to monitor electron flow and deduce which substance is oxidized or reduced, strengthening the learner's ability to analyze and predict the outcomes of redox reactions.
Oxidation States
The oxidation state, or oxidation number, indicates the degree of oxidation of an atom in a chemical compound. Conventionally, the oxidation state is an integer value that can be positive, negative, or zero, based on hypothetical ionic charge.
Assigning oxidation states is based on a set of rules, including: alkali metals (group 1) have an oxidation state of +1, alkaline earth metals (group 2) have +2, oxygen typically has -2 (except in peroxides and when bonded to fluorine), and hydrogen has +1 when bonded to non-metals and -1 when bonded to metals.
It's worth noting that oxidation states do not necessarily represent the actual charges on atoms in molecules or complexes. However, they are incredibly useful for understanding the electronic structure and for balancing redox reactions. When teaching oxidation states, it is beneficial to examine both simple ions and more complex molecules to elucidate how these states are determined, and as seen in the step by step solution, how they contribute to understanding the overall chemical behavior of a substance.
Assigning oxidation states is based on a set of rules, including: alkali metals (group 1) have an oxidation state of +1, alkaline earth metals (group 2) have +2, oxygen typically has -2 (except in peroxides and when bonded to fluorine), and hydrogen has +1 when bonded to non-metals and -1 when bonded to metals.
It's worth noting that oxidation states do not necessarily represent the actual charges on atoms in molecules or complexes. However, they are incredibly useful for understanding the electronic structure and for balancing redox reactions. When teaching oxidation states, it is beneficial to examine both simple ions and more complex molecules to elucidate how these states are determined, and as seen in the step by step solution, how they contribute to understanding the overall chemical behavior of a substance.
