Chapter 8: Problem 59
What is the oxidation number of carbon in \(\mathrm{C}_{3} \mathrm{O}_{2}\) (carbon suboxide)? (a) \(+4 / 3\) (b) \(+10 / 4\) (c) \(+2\) (d) \(+2 / 3\)
Short Answer
Expert verified
The oxidation number of carbon in \(\mathrm{C}_{3} \(\text{O}_{2}\)\) is \(+\frac{4}{3}\).
Step by step solution
01
- Understand rules for oxidation numbers
Understand the key rules for oxidation numbers: elements in their elemental form have an oxidation number of 0. Oxygen typically has an oxidation number of -2 (except in peroxides or when bonded to fluorine). The sum of oxidation numbers in a neutral compound is 0.
02
- Assign known oxidation numbers
Assign the typical oxidation number of -2 to oxygen. Since there are two oxygen atoms, their total contribution to the oxidation number is \(2 \times -2 = -4\).
03
- Calculate the oxidation number for carbon
Let \(x\) be the oxidation number of carbon. For the compound \(\mathrm{C}_{3} \mathrm{O}_{2}\), the total sum of oxidation numbers must be zero. So, for three carbon atoms: \(3x + 2(-2) = 0\). Solve for \(x\) to find the oxidation number of carbon.
04
- Solve for the oxidation number of carbon
Rearrange and solve the equation \(3x - 4 = 0\). Adding 4 to both sides gives \(3x = 4\), and dividing by 3 yields \(x = \frac{4}{3}\), which indicates the oxidation number of carbon in the compound.
Unlock Step-by-Step Solutions & Ace Your Exams!
-
Full Textbook Solutions
Get detailed explanations and key concepts
-
Unlimited Al creation
Al flashcards, explanations, exams and more...
-
Ads-free access
To over 500 millions flashcards
-
Money-back guarantee
We refund you if you fail your exam.
Over 30 million students worldwide already upgrade their learning with Vaia!
Key Concepts
These are the key concepts you need to understand to accurately answer the question.
Oxidation States
Oxidation states, also known as oxidation numbers, are a fundamental concept in chemistry that provide insight into the electron distribution of atoms within molecules and compounds. Understanding oxidation states is crucial for grasping redox reactions and chemical bonding patterns. In simple terms, the oxidation state indicates the degree of oxidation of an atom, often representing the number of electrons an atom has gained, lost, or appears to use when bonding with other atoms.
For instance, in a neutral molecule, the sum of all oxidation states equals zero, while in ions, the sum equals the ion's charge. Let's consider a practical example from an exercise: determining the oxidation number of carbon in \(\mathrm{C}_{3} \mathrm{O}_{2}\), carbon suboxide. By applying the rules, the known -2 oxidation state for oxygen is used to infer the less obvious state for carbon. Through a simple algebraic calculation, it is shown that the carbon atoms in carbon suboxide have an oxidation state of +4/3.
This exercise highlights the importance of recognizing the common oxidation states such as 0 for elemental forms and -2 for oxygen, with exceptions. By mastering the concept of oxidation states, students can predict the types of chemical bonding and the outcomes of chemical reactions with higher accuracy.
For instance, in a neutral molecule, the sum of all oxidation states equals zero, while in ions, the sum equals the ion's charge. Let's consider a practical example from an exercise: determining the oxidation number of carbon in \(\mathrm{C}_{3} \mathrm{O}_{2}\), carbon suboxide. By applying the rules, the known -2 oxidation state for oxygen is used to infer the less obvious state for carbon. Through a simple algebraic calculation, it is shown that the carbon atoms in carbon suboxide have an oxidation state of +4/3.
This exercise highlights the importance of recognizing the common oxidation states such as 0 for elemental forms and -2 for oxygen, with exceptions. By mastering the concept of oxidation states, students can predict the types of chemical bonding and the outcomes of chemical reactions with higher accuracy.
Chemical Bonding
Chemical bonding is key to understanding the structure and stability of compounds formed from atoms. At its core, chemical bonding involves the attraction between atoms that allows the formation of chemical substances. There are several types of chemical bonds, including ionic, covalent, and metallic bonds.
In the context of the oxidation states, chemical bonding relates to how atoms share or transfer electrons. For example, oxidation numbers can help us determine the type of bond between atoms: a higher difference in oxidation states suggests an ionic bond, while similar oxidation numbers indicate a covalent bond. In \(\mathrm{C}_{3} \mathrm{O}_{2}\), carbon and oxygen bond together which suggests a type of covalent bonding as they are both non-metals. However, the oxidation state of +4/3 for carbon in carbon suboxide hints towards an unconventional type of covalent bonding because it is not an integer, which is usually the case in simple covalent compounds.
Understanding these bonding types helps in predicting the properties of the compound such as melting and boiling points, conductivity, and solubility. Grasping the nuances of chemical bonding will enhance a student's ability to draw Lewis structures, predict molecular geometry, and understand the behavior of substances in different environments.
In the context of the oxidation states, chemical bonding relates to how atoms share or transfer electrons. For example, oxidation numbers can help us determine the type of bond between atoms: a higher difference in oxidation states suggests an ionic bond, while similar oxidation numbers indicate a covalent bond. In \(\mathrm{C}_{3} \mathrm{O}_{2}\), carbon and oxygen bond together which suggests a type of covalent bonding as they are both non-metals. However, the oxidation state of +4/3 for carbon in carbon suboxide hints towards an unconventional type of covalent bonding because it is not an integer, which is usually the case in simple covalent compounds.
Understanding these bonding types helps in predicting the properties of the compound such as melting and boiling points, conductivity, and solubility. Grasping the nuances of chemical bonding will enhance a student's ability to draw Lewis structures, predict molecular geometry, and understand the behavior of substances in different environments.
Redox Reactions
Redox reactions, short for reduction-oxidation reactions, encompass all chemical reactions in which atoms have their oxidation states changed. These reactions are characterized by the transfer of electrons between chemical species. The substance that gains electrons is reduced, and its oxidation state decreases, whereas the substance that loses electrons is oxidized, and its oxidation state increases.
In the exercise involving \(\mathrm{C}_{3} \mathrm{O}_{2}\), while we're not dealing with a redox reaction directly, the concept of assigning oxidation numbers is applied, which is fundamental to understanding redox processes. In redox reactions, the principles of conservation of charge and mass are applied, just as the sum of oxidation numbers in a compound is conserved and totals to zero for neutral compounds. For instance, when assigning oxidation states in redox couples, you can anticipate which species will be oxidized and which will be reduced during the reaction.
Recognizing redox reactions is vital since they play a key role in various biological processes, industrial applications, and even in our daily lives, such as in batteries and combustion. Proficiency in redox reactions not only aids in solving chemistry problems but also assists in explaining the mechanics behind phenomenon such as corrosion, energy production, and metabolic pathways.
In the exercise involving \(\mathrm{C}_{3} \mathrm{O}_{2}\), while we're not dealing with a redox reaction directly, the concept of assigning oxidation numbers is applied, which is fundamental to understanding redox processes. In redox reactions, the principles of conservation of charge and mass are applied, just as the sum of oxidation numbers in a compound is conserved and totals to zero for neutral compounds. For instance, when assigning oxidation states in redox couples, you can anticipate which species will be oxidized and which will be reduced during the reaction.
Recognizing redox reactions is vital since they play a key role in various biological processes, industrial applications, and even in our daily lives, such as in batteries and combustion. Proficiency in redox reactions not only aids in solving chemistry problems but also assists in explaining the mechanics behind phenomenon such as corrosion, energy production, and metabolic pathways.
