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What are the electronic configuration of O2+ and O2 species as per molecular orbital theory?
O2+ is more stable than O2-. Because According to molecular orbital theory O2+ has 15 electrons has one electron in antibonding orbital. In the case of O2- 17 electrons are present &3 electrons are present in antibonding orbitals. If number of electrons more in antibonding orbital the molecule become unstable.
What is O2+ ion?
The dioxygenyl ion, O + 2, is a rarely-encountered oxycation in which both oxygen atoms have a formal oxidation state of +12. It is formally derived from oxygen by the removal of an electron: O2 → O +
How many molecular orbitals are in O2?
Each oxygen bonds to the other with its 1s, 2s, and 2p orbitals. These 5 atomic orbitals combine to form 10 molecular orbitals.
What are the electronic configuration of O2+ and O2 species as per molecular orbital theory compare the bond energy and magnetic character of O2+ and O2 species?
According to molecular orbital theory electronic configurations of O 2 + and O 2 – species are as follows : Higher bond order of O 2 + shows that it is more stable than O 2 – . Both the species have unpaired electrons. So both are paramagnetic in nature.
What is Bond order O2+?
Bond order for both NO+ and NO− is 2.
What is bond length O2+?
Molecular Parameters – Oxygen – Selenium Compounds
| Molecular Formula | Name | Bond Length (Å) |
|---|---|---|
| O2 | oxygen | O-O 1.208 |
| [O2]+ | O-O 1.1227 | |
| [O2]-(s) | O-O 1.28 (s=0.01) | |
| [O2]2-(s) | O-O 1.49 (s=0.009) |
What is Bond order o2+?
Which one of the two O2+ and O2 has higher bond order explain?
According to the molecular orbital theory, the general molecular orbital configuration will be, As there are 8 electrons in oxygen. From this we conclude that the bond order from lowest to highest will be, Hence, posses highest bond order.