Which of the following statements is incorrect? 9. Which of the following statements is incorrect?A. Based on its Lewis structure, oxygen molecule should be diamagnetic.B. Delta (8) orbitals can be formed by overlapping two d., or two d2,2 orbitals in parallel planes.C. The donor atom is carbon in most carbonyl (CO) coordination compounds.D. N; has a triple bond according to both the Lewis and the molecular orbital models.E. To form an MO, energies of the atomic orbitals must be identical.

Answered: Image /qna-images/answer/9d9b9bbd-aec1-491f-a561-48a9fdb473a0.jpg

Which of the following statements is incorrect? A. Based on its Lewis structure, oxygen molecule should be diamagnetic. B. Delta (8) orbitals can be formed by overlapping two d, or two da,2 orbitals in parallel planes. C. The donor atom is carbon in most carbonyl (CO) coordination compounds. D. N; has a triple bond according to both the Lewis and the molecular orbital models. E. To form an MO, energies of the atomic orbitals must be identical.

Which of the following statements is incorrect? A. Based on its Lewis structure, oxygen molecule should be diamagnetic. B. Delta (8) orbitals can be formed by overlapping two d, or two da,2 orbitals in parallel planes. C. The donor atom is carbon in most carbonyl (CO) coordination compounds. D. N; has a triple bond according to both the Lewis and the molecular orbital models. E. To form an MO, energies of the atomic orbitals must be identical.

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter9: Covalent Bonding: Orbitals

Section: Chapter Questions

Problem 41E: Consider the following molecular orbitals formed from the combination of two hydrogen 1s orbitals:...

See similar textbooks

Similar questions

According to the valence bond theory, which of the following statements is/are incorrect? (79Au) I- The hybrid type of an outer orbital complex cannot be sp3. II- Square plane compounds are more stable than tetrahedral compounds. In the III- Octahedral, high spin d5 complex, the number of single electrons is 1. IV- Tetrachloroaurate(III) ion is diamagnetic.
1. Consider the bonding of two boron atoms using MO theory. How many bonds will form based on the filling of its molecular orbitals? 2.T/F p orbitals always interact to form Pi or Pi* orbitals.
Show how Mn2+ and Gd3+ are paramagnetic.
NiCl4]2- and Ni(CO)4 have sp3 or dsp2 hybridization? Explain. What type of hybridization is shown by (i) inner and (ii) outer orbital octahedral complexes?
Draw the hybridization for the metal centre of the complex below. You need to determine the geometry before you start, [RhMe(PPh3)3] [RhMe(PMe3)4]
1.What are the dominant energy terms that are responsible for cesium fluoride occurring as an ionic solid and hydrogen fluoride occurring as a diatomic gas at standard conditions? 2.Explain why the energy separation between the t2g and eg d molecular orbitals in Mo(OCH3)6 is smaller than the value for Mo(CO)6 even though the average Mo-OCH3 bond dissociation enthalpy is more than twice the M-CO
Many compounds of the transition-metal elements contain direct bonds between metal atoms. We will assume that the z-axis is defined as the metal–metal bond axis. (a) Which of the 3d orbitals (Figure 6.23) can be used to make a σ bond between metal atoms? (b) Sketch the bonding and σ3d* antibonding MOs.(c)With reference to the “Closer Look” box on the phases of orbitals, explain why a node is generated in the σ3d* MO. (d) Sketch the energy-level diagram for the Sc2 molecule, assuming that only the 3d orbital from part (a) is important. (e)What is the bond order in Sc2?
What type of geometry (according to valence bond theory) does Mn exhibit in the complex ion, [Mn(NH3)4]2+?
Describe the bonding in NO+, NO, and NO, using both the localized electron and molecular orbital models. Account for any discrepancies between the two models.
Consider the following molecular orbitals formed from the combination of two hydrogen 1s orbitals: a. Which is the bonding molecular orbital and which is the antibonding molecular orbital? Explain how you can tell by looking at their shapes. b. Which of the two molecular orbitals is lower in energy? Why is this true?
Bromine forms a number of oxides of varying stability. (a) One oxide has 90.90% Br and 9.10% O. Assuming its empirical and molecular formulas are the same, draw a Lewis structure of the molecule and specify the hybridization of the central atom (O). (b) Another oxide is unstable BrO. Assuming the molecular orbital diagram in Figure 9. 16 applies to BrO, write its electron configuration (where Br uses 45 and 4p orbitals). What is the highest occupied molecular orbital (HOMO) for the molecule?
A useful solvent that will dissolve salts as well as organic compounds is the compound acetonitrile, H3CCN. It is present in paint strippers. (a) Write the Lewis structure for acetonitrile, and indicate the direction of the dipole moment in the molecule. (b) Identify the hybrid orbitals used by the carbon atoms in the molecule to form bonds. (c) Describe the atomic orbitals that form the n bonds in the molecule. Note that it is not necessary to hybridize the nitrogen atom.