40 use the following mo diagram to find the bond order for o2.

Welcome to Sarthaks eConnect: A unique platform where students can interact with teachers/experts/students to get solutions to their queries. Students (upto class 10+2) preparing for All Government Exams, CBSE Board Exam, ICSE Board Exam, State Board Exam, JEE (Mains+Advance) and NEET can ask questions from any subject and get quick answers by subject teachers/ experts/mentors/students. "O"_2 is well-known to be paramagnetic, and it is one of the successes of molecular orbital theory. You can see that "CO" is not (as it has zero unpaired electrons), but "NO" is (it has one unpaired electron). Well, the MO diagram for "O"_2 is: The bond order is already calculated in the diagram.

The bond order varies from one molecule to another. Oxygen is a diatomic molecule. Let us first know what is meant by bond order. Bond order. The bond order may be defined as half the difference between the number of electrons in bonding molecular orbitals (Nonbonding) and the number of electrons in the antibonding molecular orbital. Formula ...

Use the following mo diagram to find the bond order for o2.

Without 2s-2p mixing With 2s-2p mixing CK :O r 25 20 2s AO MO AO AO MO AO A MO energy levels for O Fa. and Ne B MO energy levels for Ba Cz and Ng 0.5 This problem has been solved! See the answer See the answer See the answer done loading Solution. , The electrons in the highest occupied molecular orbital are unpaired therefore it is paramagnetic in nature. Also, the bond order can be calculated as [N b. ]/2=[10−6]/2=2. Therefore there is a double bond present as O=O. The bond order tells us the average number of bonds between the bonded atoms. In a diatomic molecule such as `O_2`, the bond order simply tells the number of bonds between the two atoms. The bond order can be interpreted from MO diagrams using the following formula: `"Bond Order" = 1/2 [("Bonding "e^-)-("Antibonding " e^-)]`

Use the following mo diagram to find the bond order for o2.. Electron Configurations and Bond Orders Just as with atoms, we can write a molecular electron configuration for O2 σ2σ*2σ2π4π*2 We can also calculate the O–O bond order: BO 1 2 # bonding e # anti-bonding e 1 2 8 4 2 LCAO MO theory also predicts (correctly) that O2has two unpaired electrons. A polyatomic ion is composed of multiple covalently bonded atoms. CO₃²⁻ is a polyatomic ion composed of a carbon atom and three oxygen atoms. Predict the chemical formula for the ionic compound formed by Au³⁺ and HSO₃⁻. Au (HSO3)3. Predict the chemical formula for the ionic compound formed by NH₄⁺ and PO₄³⁻. (NH4)3PO4. Explanation: In a molecule, there are total 16 electrons. The molecular orbital configuration of molecule is as follows.. The formula for bond order is as follows. Bond order = There are 10 bonding and 6 non-bonding electrons in the orbitals according to the molecular orbital configuration. 2) Stability of molecules in terms of bond order. Bond order is defined as half of the difference between the number of electrons present in the bonding and antibonding orbitals. Bond Order = ½ ( N b – Na) The molecule is stable if N b > Na ie. bond order is positive. The molecule is unstable if N b < Na i.e. the bond order is negative or zero.

The bond order tells us the average number of bonds between the bonded atoms. In a diatomic molecule such as `O_2`, the bond order simply tells the number of bonds between the two atoms. The bond order can be interpreted from MO diagrams using the following formula: `"Bond Order" = 1/2 [("Bonding "e^-)-("Antibonding " e^-)]` Solution. , The electrons in the highest occupied molecular orbital are unpaired therefore it is paramagnetic in nature. Also, the bond order can be calculated as [N b. ]/2=[10−6]/2=2. Therefore there is a double bond present as O=O. Without 2s-2p mixing With 2s-2p mixing CK :O r 25 20 2s AO MO AO AO MO AO A MO energy levels for O Fa. and Ne B MO energy levels for Ba Cz and Ng 0.5 This problem has been solved! See the answer See the answer See the answer done loading

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