Determining Oxidation States

Oct 13, 2025 by magicalceylontours.com 90 views

Introduction

Oxidation states are a fundamental concept in chemistry that help us understand the distribution of electrons within a chemical compound. In this article, we will delve into the world of covalently bonded compounds, specifically the acetate ion ($$CH_3COO^-$$), and explore the oxidation states of its constituent atoms.

What are Oxidation States?

Oxidation states are a way to describe the number of electrons an atom has gained or lost in a chemical compound. They are denoted by a positive or negative sign, with positive indicating a loss of electrons and negative indicating a gain of electrons. The sum of the oxidation states of all atoms in a compound is equal to the charge on the compound.

The Acetate Ion: A Covalently Bonded Compound

The acetate ion ($$CH_3COO^-$$) is a covalently bonded compound consisting of two carbon atoms, three hydrogen atoms, and two oxygen atoms. The acetate ion has a charge of -1, indicating that it has gained one electron.

Determining Oxidation States

To determine the oxidation states of the carbon atoms in the acetate ion, we need to consider the bonds between the atoms. The carbon atom bonded to the three hydrogen atoms is in a sp3 hybridization state, indicating that it has a tetrahedral geometry. This carbon atom is bonded to the oxygen atom through a single covalent bond, which is a sigma bond.

The other carbon atom is bonded to the oxygen atom through a double covalent bond, which is a sigma and a pi bond. This carbon atom is also bonded to the oxygen atom through a single covalent bond, which is a sigma bond.

Calculating Oxidation States

To calculate the oxidation states of the carbon atoms, we need to consider the bonds between the atoms. The carbon atom bonded to the three hydrogen atoms has a bond order of 1 with the oxygen atom, while the other carbon atom has a bond order of 2 with the oxygen atom.

Using the bond order, we can calculate the oxidation states of the carbon atoms. The carbon atom bonded to the three hydrogen atoms has an oxidation state of +1, while the other carbon atom has an oxidation state of +3.

Conclusion

In conclusion, the two carbon atoms in the acetate ion ($$CH_3COO^-$$) have different oxidation states. The carbon atom bonded to the three hydrogen atoms has an oxidation state of +1, while the other carbon atom has an oxidation state of +3.

Answer

The correct answer is:

A. +1 and +3

Discussion

The acetate ion is a covalently bonded compound that consists of two carbon atoms, three hydrogen atoms, and two oxygen atoms. The oxidation states of the carbon atoms are determined by the bonds between the atoms. The carbon atom bonded to the three hydrogen atoms has an oxidation state of +1, while the other carbon atom has an oxidation state of +3.

References

Atkins, P. W., & De Paula, J. (2010). Physical chemistry (9th ed.). Oxford University Press.
Brown, T. E., & LeMay, H. E. (2014). Chemistry: The Central Science (13th ed.). Pearson Education.

Additional Resources

Khan Academy: Oxidation States
Chemistry LibreTexts: Oxidation States
Purdue University: Oxidation States
Frequently Asked Questions: Oxidation States in Covalently Bonded Compounds ====================================================================

Q: What is the difference between oxidation states and oxidation numbers?

A: Oxidation states and oxidation numbers are often used interchangeably, but technically, oxidation numbers refer to the charge on an atom in a compound, while oxidation states refer to the number of electrons an atom has gained or lost.

Q: How do I determine the oxidation state of an atom in a covalently bonded compound?

A: To determine the oxidation state of an atom in a covalently bonded compound, you need to consider the bonds between the atoms. You can use the following steps:

Determine the total charge on the compound.
Calculate the charge on each atom in the compound using the bond order and the electronegativity of the atoms involved.
Add up the charges on each atom to determine the oxidation state of the atom.

Q: What is the bond order, and how is it used to determine oxidation states?

A: The bond order is a measure of the number of bonds between two atoms. It is used to determine the oxidation state of an atom in a covalently bonded compound. The bond order is calculated by counting the number of bonds between the atoms and then dividing by 2.

Q: How do I calculate the oxidation state of a carbon atom in a covalently bonded compound?

A: To calculate the oxidation state of a carbon atom in a covalently bonded compound, you need to consider the bonds between the carbon atom and the other atoms in the compound. You can use the following steps:

Determine the bond order between the carbon atom and the other atoms in the compound.
Calculate the charge on the carbon atom using the bond order and the electronegativity of the atoms involved.
Add up the charges on each atom to determine the oxidation state of the carbon atom.

Q: What is the difference between a sigma bond and a pi bond?

A: A sigma bond is a type of covalent bond that involves the overlap of two atomic orbitals along the bond axis. A pi bond is a type of covalent bond that involves the overlap of two atomic orbitals perpendicular to the bond axis.

Q: How do I determine the oxidation state of an oxygen atom in a covalently bonded compound?

A: To determine the oxidation state of an oxygen atom in a covalently bonded compound, you need to consider the bonds between the oxygen atom and the other atoms in the compound. You can use the following steps:

Determine the bond order between the oxygen atom and the other atoms in the compound.
Calculate the charge on the oxygen atom using the bond order and the electronegativity of the atoms involved.
Add up the charges on each atom to determine the oxidation state of the oxygen atom.

Q: What is the significance of oxidation states in covalently bonded compounds?

A: Oxidation states are significant in covalently bonded compounds because they help us understand the distribution of electrons within the compound. They also help us predict the reactivity of the compound and its ability to form bonds with other atoms.

Q: How do I apply the rules for determining oxidation states to a complex covalently bonded compound?

A: To apply the rules for determining oxidation states to a complex covalently bonded compound, you need to follow these steps:

Determine the total charge on the compound.
Calculate the charge on each atom in the compound using the bond order and the electronegativity of the atoms involved.
Add up the charges on each atom to determine the oxidation state of the atom.
Use the oxidation states to predict the reactivity of the compound and its ability to form bonds with other atoms.

Q: What are some common mistakes to avoid when determining oxidation states?

A: Some common mistakes to avoid when determining oxidation states include:

Failing to consider the bond order between atoms.
Failing to calculate the charge on each atom using the bond order and electronegativity.
Failing to add up the charges on each atom to determine the oxidation state of the atom.
Failing to consider the electronegativity of the atoms involved in the bond.

Q: How do I verify the oxidation states of a covalently bonded compound?

A: To verify the oxidation states of a covalently bonded compound, you can use the following steps:

Calculate the total charge on the compound.
Calculate the charge on each atom in the compound using the bond order and electronegativity.
Add up the charges on each atom to determine the oxidation state of the atom.
Compare the calculated oxidation states with the expected oxidation states based on the compound's structure and properties.

Q: What are some real-world applications of oxidation states in covalently bonded compounds?

A: Some real-world applications of oxidation states in covalently bonded compounds include:

Predicting the reactivity of a compound and its ability to form bonds with other atoms.
Understanding the distribution of electrons within a compound.
Designing new compounds with specific properties.
Developing new materials with unique properties.

Q: How do I use oxidation states to predict the reactivity of a covalently bonded compound?

A: To use oxidation states to predict the reactivity of a covalently bonded compound, you can follow these steps:

Determine the oxidation state of each atom in the compound.
Use the oxidation states to predict the reactivity of the compound based on its ability to form bonds with other atoms.
Consider the electronegativity of the atoms involved in the bond.
Use the predicted reactivity to design new compounds with specific properties.

Q: What are some common misconceptions about oxidation states in covalently bonded compounds?

A: Some common misconceptions about oxidation states in covalently bonded compounds include:

Assuming that oxidation states are the same as oxidation numbers.
Failing to consider the bond order between atoms.
Failing to calculate the charge on each atom using the bond order and electronegativity.
Failing to add up the charges on each atom to determine the oxidation state of the atom.

Q: How do I use oxidation states to design new compounds with specific properties?

A: To use oxidation states to design new compounds with specific properties, you can follow these steps:

Determine the oxidation state of each atom in the compound.
Use the oxidation states to predict the reactivity of the compound based on its ability to form bonds with other atoms.
Consider the electronegativity of the atoms involved in the bond.
Use the predicted reactivity to design new compounds with specific properties.

Q: What are some real-world examples of compounds with specific properties designed using oxidation states?

A: Some real-world examples of compounds with specific properties designed using oxidation states include:

Designing new materials with unique electrical properties.
Developing new catalysts with specific reactivity.
Creating new compounds with specific optical properties.
Designing new compounds with specific thermal properties.