Study the following sketch of a molecular orbital (MO) in a homonuclear diatomic molecule. This MO was formed by combining one 3s atomic orbital from eachatom.The dark dots in this sketch are the nuclei.Now use the sketch to complete the table below.Write the symbol for this MO.Is this a bonding or antibonding MO?bondingWhat is the energy of this MO, compared to theenergy of a 3s orbital on one of the separateatoms?antibondinghigherlowerthe samenot enough informationto decideσΠхG

Step 1: The answers are numbered from top to bottom Step 2: Step 3: Step 4:

Answered: Study the following sketch of a…

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 10.97QE

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Similar questions

Compare and contrast the molecular orbital and ionic bonding descriptions of LiF.
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?
Identify the hybrid orbitals used by antimony in SbCl5 and in SbCl6, the ion formed from the reaction of SbCl5 and Cl. Explain your choices.
When two amino acids react with each other, they form a linkage called an amide group, or a peptide link. (If more linkage. are added, a protein or polypeptide is formed.) (a) What are the hybridizations of the C and N atoms in the peptide linkage? (b) Is the structure illustrated the only resonance structure possible for the peptide linkage? If another resonance structure is possible. compare it with the o ne shown. Decide which is the more important structure. (c) The computer-generated structure shown here, which contains a peptide linkage, shows that this linkage is flat. This is an important feature of proteins. Speculate on reasons that the CONH linkage is planar. What are the sites of positive and negative charge in this dipeptide?
Why is the concept of hybridization required in valence bond theory?
Electrons in bonding molecular orbitals are most likely to be found in the region between the two bonded atoms. Why does this arrangement favor bonding? In a antibonding orbital, where are the electrons most likely to be found in relation to the nuclei in a bond?
In the molecular orbital mode l, compare and contrast bonds with bonds. What orbitals form the bonds and what orbitals form the bonds? Assume the z-axis is the internuclear axis.
7.59 What type of hybrid orbital is generated by combining the valence s orbital and all three valence p orbitals of an atom? How many hybrid orbitals result?
Draw the Lewis structure for HCN. Indicate the hybrid orbitals, and draw a picture showing all the bonds between the atoms, labeling each bond as or .
Use Figs. 4-54 and 4-55 to answer the following questions. a. Would the bonding molecular orbital in HF place greater electron density near the H or the F atom? Why? b. Would the bonding molecular orbital have greater fluorine 2p character, greater hydrogen 1s character, or an equal contribution from both? Why? c. Answer the previous two questions for the antibonding molecular orbital in HF.
If you have three electron regions around a central atom, how can you have a triangular planar molecule? An angular molecule? What bond angles are predicted in each case?
Explain why an electron in the bonding molecular orbital in the H2 molecule has a lower energy than an electron in the 1s atomic orbital of either of the separated hydrogen atoms.

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