1.Carbon monoxide is a toxic gas due to how it binds to the Fe in hemoglobin blocking the abilityfor oxygen to bind and be transported to cells in our body. Create an MO diagram for CO. After creatingthe diagram, label the HOMO and LUMO, and draw the specific orbital interactions for these two energystates.

MOs for CO can be created by using the balance shell electronic configuration of C atom and O atom.…

Answered: 1. Carbon monoxide is a toxic gas due…

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter10: Molecular Structure And Bonding Theories

Section: Chapter Questions

Problem 10.116QE

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Discuss the nature of the bonding in the nitrite ion (NO2) . Draw the possible Lewis resonance diagrams for this ion. Use the VSEPR theory to determine the steric number, the hybridization of the central nitrogen atom, and the geometry of the ion. Show how the use of resonance structures can be avoided by introducing a de-localized MO. What bond order does the MO model predict for the NO bonds in the nitrite ion?
Discuss the nature of the bonding in the nitrate ion (NO3) . Draw the possible Lewis resonance diagrams for this ion. Use the VSEPR theory to determine the steric number, the hybridization of the central N atom, and the geometry of the ion. Show how the use of resonance structures can be avoided by introducing a de-localized MO. What bond order is predicted by the MO model for the NO bonds in the nitrate ion?
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?
Why do we hybtidize atomic orbitals to explain the bonding in covalent compounds? What type of bonds form from hybrid orbitals: sigma or pi? Explain.
Lets look more closely at the process of hybridization. (a) What is the relationship between the number of hybrid orbitals produced and the number of atomic orbitals used to create them? (b) Do hybrid atomic orbitals form between different p orbitals without involving 5 orbitals? (c) What is the relationship between the energy of hybrid atomic orbitals and the atomic orbitals from which they are formed?
Nitric oxide (NO) is an important signaling molecule in biological systems. Two ions based on NO are also known: the nitrosonium cation (NO*) and the nitroxyl anion (NO). Construct the molecular orbital diagram for NO (Note: s-p mixing is significant in NO). To the side, sketch the combinations of AOs that contribute to each MO. b. Explain how your diagram illustrates the difference in electronegativity between N and O. Predict the bond order and number of unpaired electrons in NO. d. Predict the bond order and number of unpaired electrons in the ions NO* and NO". Which of the three species would you predict to have the shortest bond? Explain why. а. С.
Consider a heteronuclear diatomic molecule, AB, where A and B are period 2 elements. Using the following pieces of information, provide details on the molecular orbital diagram of AB: Clue 1: The MO diagram of AB does not contain non- bonding electrons. Clue 2: The s and p orbital energies of both atoms are quite close to one another that interactions between different orbital types occur. Clue 3: AB" is more stable than AB, but AB2 is less stable than AB". Clue 4: The potential energies of the atomic orbitals of A are higher than the potential energies of the atomic orbitals of B. Table 1. Atomic orbital energies of period 2 elements. Atom Orbital energy Orbital energy (2s) (2p) Li -5.45 Ве -9.30 B -14.0 -8.30 C -19.5 -10.7 -25.5 -13.1 -32.3 -15.9 F -46.4 -18.7 Ne -48.5 -21.5
Below is an incomplete molecular orbital diagram. Fill in the diagram for the diatomic molecule X2, where each atom of X has 6 valence electrons in s and p orbitals. w р S π р S Based on your diagram, [Select] substance would be expected to be [Select] bond(s) would be expected to form and the ?
92. The three most stable oxides of carbon are carbon monox- ide (CO), carbon dioxide (CO,), and carbon suboxide (C,O2). The space-filling models for these three com- pounds are For each oxide, draw the Lewis structure, predict the mo- lecular structure, and describe the bonding (in terms of the hybrid orbitals for the carbon atoms).
Considerthese following ions: 02 -, N -, Li2 + and O - a. Based on molecular orbital theory (MOT), which of the ion(s) exhibit(s) paramagnetism? b. For those ions that are paramagnetic, determine the number of unpaired electrons. Support your answers with appropriate molecular orbital energy diagram.
The next two questions investigate how Molecular Orbital Theory and Lewis Theory view carbon monoxide. —. Draw a molecular orbital energy diagram (showing all of the bonding and antibonding molecular orbitals and their respective energies) for CO. Use the Molecular Orbital energy levels for B2 , C2 and N 2 for the CO molecule. —. Calculate the bond order for CO from the molecular orbital energy diagram. —. Is CO paramagnetic or diamagnetic? ------------- b. Draw the Lewis structure for CO. —. Calculate the formal charge on each atom in CO. —. Draw the dipole for CO. —. Calculate the oxidation numbers for the carbon and oxygen atoms in CO. —. Formal charges, dipoles, and oxidation numbers are different ways of understanding the charges on covalently-bonded atoms. They tend to agree or be similar. At least in some ways, they disagree for CO. Formal charge guidelines assume that all bonding electrons are shared evenly between the two bonded atoms. Oxidation number guidelines assume that…
O CHEMICAL BONDING Recognizing typical LCAO molecular orbitals Heather V Stua, che following sketch of a molecular orbital (MO) in a homonuclear diatomic molecule. This MO was formed by combining one 2s atomic orbital from each atom. The dark dots in this sketch are the nuclei. do Now use the sketch to complete the table below. Write the symbol for this MO. O bonding Is this a bonding or antibonding MO? O antibonding On O higher O lower What is the energy of this MO, compared to the energy of a 2s orbital on one of the separate atoms? O the same o not enough information to decide Explanation Check O 2021 McGraw-Hill Education. All Rights Reserved. Terms of Use Privacy Accessibility

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