Use molecular orbital theory to explain why the bond energy of an O2 molecule is less...

Use molecular orbital theory to explain why the bond energy of an O₂ molecule is less than that of a O₂⁺ ion.

Expert Solution

First calculate the total number of electrons present in the atom and draw the molecular orbital diagram.

The M O diagram for a molecule with electrons < 14 is different from that of a molecule having electrons > 14.

In the case of electrons < 14 the (pi 2px) ( pi 2py) orbitals are lower in energy than the ( sigma 2px) whereas in case of electrons > 14 its vice versa. This is because in case of electrons < 14 sp mixing takes place ( sp mixing takes place when the 2s and 2p orbitals have similar energies ) and in case of electrons > 14 the difference in energy between the s and p orbitals is greater and hence sp mixing does not take place.

Fill the electrons in the molecular orbitals following the general rules of electron filling.

Calculate the bond order using the formula, Bond order = 1/2 ( electrons in BMO - electrons in ABMO )

and the bond energy ( measure of bond strength) is directly proportional to the bond order.

queen_honey_blossom answered 1 year ago

Create a Molecular orbital diagram for O2- . What is the bond order of this molecule?

Prepare a molecular orbital diagram for the BeH2 molecule. Assume in orbital potential energy of 4.0...

Prepare a molecular orbital diagram for the BeH2 molecule. Assume in orbital potential energy of 4.0 eV for the 2p orbitals of Be and -9.3eV for the 2s orbital. Assume that both the 2p and the 2s of Be interact with the two group orbitals of the hydrogens.

Subject: Physical Chemistry Topic: Molecular Orbital Theory Explain why the energy stabilization for bonding orbitals is...

Subject: Physical Chemistry Topic: Molecular Orbital Theory Explain why the energy stabilization for bonding orbitals is less than the destabilization energy for antibonding orbitals.

Apply molecular orbital theory to predict which species has the strongest bond. Apply molecular orbital theory...

Apply molecular orbital theory to predict which species has the strongest bond. Apply molecular orbital theory to predict which species has the strongest bond. O+2 O−2 O2 All bonds are equivalent according to molecular orbital theory.

Molecular Orbital Theory -- Homodiatomics Use the molecular orbital model to fully describe the bonding in...

Molecular Orbital Theory -- Homodiatomics Use the molecular orbital model to fully describe the bonding in O2+, O2, O2-, and O22-. Determine which of the following statements are true and which are false. The electron configuration of O2- is (σ2s)2(σ2s*)2(σ2p)2(π2p)4(π2p*) The electron configuration of O2+ is (σ2s)2(σ2s*)2(σ2p)2(π2p)4(π2p*) The number of unpaired electrons in O2+ and O22- is, respectively, 1 and 2. The bond lengths increase in the order: O2+ < O2 < O2- < O22-. The bond order in O2+...

Consider the species (O2)2- and (O2)2+. According to molecular orbital theory, which of these species will...

Consider the species (O2)2- and (O2)2+. According to molecular orbital theory, which of these species will be diamagnetic? (O2)2+ and (O2)2- (O2)2+ (O2)2- neither is diamagnetic The magnetic property can only be determined for molecules, not ions.

1. Draw the molecular orbital diagram for NO. What is the bond order? Is the molecule...

1. Draw the molecular orbital diagram for NO. What is the bond order? Is the molecule paramagnetic or diamagnetic? 2. Draw the molecular orbital diagram and Lewis structure for the diatomic oxygen, N2. What is the bond order for according to MO diagram and according to Lewis structure? Is the molecule paramagnetic or diamagnetic? 3. Methionine, CH3SCH2CH2CH(NH2)CO2H, is an amino acid found in proteins. The Lewis structure of this compound is shown below. What is the hybridization type of each...

Question

Use molecular orbital theory to explain why the bond energy of an O2 molecule is less...

Solutions

Expert Solution

Related Solutions