What is bond order of O2?

Question

Answer

2

Answer

See i will give you short trick for such question.
First calculate the total electron . And keep in mind when total electron is 14 then bond order 3 and by increasing or decressing of electron then bond order decreese by .5
See in O2 total electron is 16 so you find bond order i 2

Answer

Bond order means no. of bonded electrons , as in O2 the no of bonded electrons are 2 . please upvote and follow me.

Answer

Bond Order of O2:

Oxygen (O2) is a diatomic molecule, meaning it consists of two oxygen atoms bonded together. The bond order of O2 is a measure of the stability of the molecule and is defined as the difference between the number of bonding and antibonding electrons divided by two.

Determining Bond Order:

To determine the bond order of O2, we need to follow the following steps:

1. Calculate the total number of electrons:
- Oxygen has 8 electrons in its outermost shell (valence electrons).
- Since there are two oxygen atoms in O2, the total number of valence electrons is 8 * 2 = 16.

2. Draw the molecular orbital diagram:
- In the molecular orbital diagram, we represent the atomic orbitals of each oxygen atom and their resulting molecular orbitals.
- The molecular orbitals are formed by combining the atomic orbitals through constructive or destructive interference.
- The two molecular orbitals formed are the bonding (σ) and antibonding (σ*) orbitals.

3. Fill in the electrons:
- Starting with the lowest energy molecular orbital, we fill in the electrons according to the Aufbau principle and Hund's rule.
- The bonding orbital is filled first, followed by the antibonding orbital.

4. Count the number of bonding and antibonding electrons:
- The bonding electrons are those present in the bonding orbital.
- The antibonding electrons are those present in the antibonding orbital.

5. Calculate the bond order:
- Bond order = (number of bonding electrons - number of antibonding electrons) / 2.

Molecular Orbital Diagram of O2:

The molecular orbital diagram of O2 can be represented as follows:

- σ* (Antibonding orbital)
- σ (Bonding orbital)

Bond Order Calculation for O2:

In the molecular orbital diagram of O2, we can fill in the electrons as follows:

- σ: ↑↓ ↑↓ ↑↓ ↑ (4 electrons)
- σ*: ↑↓ (2 electrons)

The number of bonding electrons is 4, and the number of antibonding electrons is 2.

Using the bond order formula, we can calculate the bond order as:

Bond order = (4 - 2) / 2 = 2 / 2 = 1

Bond Order of O2:

The bond order of O2 is 1. A bond order of 1 indicates a stable molecule, as there is one net bonding electron. This means that O2 has a double bond between the two oxygen atoms, resulting in a stable, symmetric molecule.

Importance of Bond Order:

The bond order provides valuable information about the nature of the bond between two atoms. A higher bond order indicates a stronger and more stable bond. In the case of O2, its bond order of 1 indicates a relatively stable molecule with a double bond between the oxygen atoms.

The bond order also affects various properties of molecules, such as bond length and bond energy. A higher bond order generally corresponds to a shorter bond length and a higher bond energy.

Understanding the bond order helps in predicting the reactivity, stability, and physical properties of molecules, as well as their behavior in chemical reactions.

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