Concept explainers
Interpretation: The existence of the
Concept introduction: The electronic configuration for multi-electron diatomic molecule is written using the molecular orbitals, derived from the
The bond order is calculated by difference between the anti-bonding electrons and the bonding electrons by two. This can be stated as,
As the bond order increases, the stability also increases. The bond order is directly proportional to the bond energy and inversely proportional to the bond length.
To determine: The explanation regarding the existence and the dissociation of the
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Chemistry: An Atoms First Approach
- Use MO theory to predict the bond order and the number of unpaired electrons in the super-oxide ion, , and the peroxide ion, .arrow_forwardThe bond dissociation energies for the species NO, CF , and CF+ are ordered as CF+NOCF . Use MO theory to explain this ordering.arrow_forwardConsider the molecule E2, where E is the element with atomic number 5. [If the atomic number were 8, the molecule would be O2.] What is the bond order for the molecule? This is the answer to put in the answer box. Show the calculation and also support your answer with an energy level diagram (MO diagram).arrow_forward
- Construct an approximate molecular orbital energy diagram for a hypothetical planar form of NH3. From a consideration of the atomic energy levels, place the N and H3 orbitals on either side of a molecular orbital energy-level diagram. Then use your judgement about the effect of bonding and anti bonding interactions and energies of the parent orbitals to construct the molecular orbital energy levels in the centre of your diagram and draw lines indicating the contributions of the atomic orbitals to each molecular orbital. Ionization energies are I(H1s) = 13.6 eV, I(N2s) = 26.0 eV, and I(N2p)=13.4 eV.arrow_forwardGiven that the following MO-energy-level diagram (see attached image) applies to the the diatomic molecular cation BO+, match the letter label of each energy level with the corresponding orbital descriptor. Match the letter on the daigram (a, b, c, d, etc) to the given below: O2p σ2p σ2s* π2p σ2p* B+2s π2p* σ2s O2s B+2parrow_forwardUse sketches of orbitals to show how VB theory explains the bonding in the Cl2 molecule. Illustrate with appropriate orbital diagrams as well. Use these to determine the number of orbitals that overlap in the Cl2 molecule. How many orbitals overlap in Cl2? Choose answer that aplies. a. Bonding will be similar to the bonding in F2, because fluorine and chlorine are in the same group of the periodic table. b. One 3p orbital of each chlorine atom will participate in the bonding in the Cl2 molecule. c. One 2p orbital of each chlorine atom will participate in the bonding in the Cl2 molecule. d. Two sp7 molecular orbitals will participate in the bonding in Cl2 molecule. d. Bonding will be similar to the bonding in F2, because fluorine and chlorine are in the same period of the periodic table.arrow_forward
- A MO scheme for CO2 is shown below. Fill in the electrons for both the atoms and the molecule. Notice that since there are 2 oxygens, there are six p orbitals and two s orbitals associated with the right hand column of the MO scheme. Determine which orbitals are bonding vs. nonbonding, vs. antibonding and calculate the bond order. Notice that the names of the MO’s are no longer s and p - they have other names. (Hint: bonding vs. antibonding vs. nonbonding can be figured out based on the energy of the MOs and the positioning of the dashed lines.) Compare the bond order to the valence bond picture of CO2, [O=C=O]. How are they related?arrow_forwardWhat is the primary difference between valence bond theory (VB) and molecular orbital theory (MO)? A) VB determines the summation of mixed wave functions as hybrid orbitals; MO determines the sum of atomic orbital energy as energy level diagrams. B) VB determines the summation of mixed wave functions as energy level diagrams; MO determines the sum of atomic orbital energy as hybrid orbitals. C) MO determines the summation of mixed wave functions as energy level diagrams; VB determines the sum of atomic orbital energy as hybrid orbitals. D) MO determines the summation of mixed wave functions as hybrid orbitals; VB determines the sum of atomic orbital energy as energy level diagrams.arrow_forwardSketch the antibonding molecular orbital that results from the linear combination of two 1s orbitals. Indicate the region where interference occurs and state the kind of interference (constructive or destructive).arrow_forward
- (a) Dihydrogen cation H2+ is commonly found in interstellar space. It can be generated by ionization of dihydrogen molecule H2. What electromagnetic radiation can be used to generate the H2+ cation? (b) Construct an energy level diagram for the molecular orbitals of the H2+ cation. What is the bond order of the HH bond in the H2+ cation? (c) Suggest a spectroscopic method for differentiation of H2 gas and the H2+ cation. Explain your answers.arrow_forwardBased on molecular orbital theory, is it correct to say that when a diatomic molecule loses an electron, the bond energy always decreases (that is, that the bond is always weakened)? Explain and provide examples to prove your case.arrow_forwardWhich one of the following statements is false? Valence bond theory and molecular orbital theory can be described as two different views of the same thing. When one considers the molecular orbitals resulting from the overlap of any two specific atomic orbitals, the bonding orbitals are always lower in energy than the antibonding orbitals. Molecular orbitals are generally described as being more delocalized than hybridized atomic orbitals. One of the shortcomings of molecular orbital theory is its inability to account for a triple bond in the nitrogen molecule, N2. One of the shortcomings of valence bond theory is its inability to account for the paramagnetism of the oxygen molecule, O2.arrow_forward
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