Which of the following statements about molecularorbital theory is incorrect?a) Bonding molecular orbitals result from theconstructive interference of atomic orbitals.b) Antibonding molecular orbitals have higherenergy than the corresponding bonding orbitals.c) Electrons in antibonding orbitals stabilize themolecule.d) The number of molecular orbitals formed equalsthe number of atomic orbitals combined.

Options a, b and d are correct asa. Bonding molecular orbitals result from the constructive…

Answered: Which of the following statements about…

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter7: Chemical Bonding And Molecular Structure

Section: Chapter Questions

Problem 7.57PAE: 7.57 What observation about molecules compels us to consider the hybridization of atomic orbitals?

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Similar questions

Aspartame is a compound that is 200 times sweeter than sugar and is used extensively (under the trade name NutraSweet) in diet soft drinks. The skeleton structure of the atoms in aspartame is (a) Complete the Lewis structure and give the number of and bonds in aspartame. (b) What is the hybridization about each carbon atom that forms a double bond with an oxygen atom? (c) What is the hybridization about each nitrogen atom?
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?
Why is the concept of hybridization required in valence bond theory?
What hybrid orbitals would be expected for the central atom in each of the following molecules or ions?
Compare and contrast the molecular orbital and ionic bonding descriptions of LiF.
Based on the discussion so far, identify a characteristic that is common to all situations where electron-region geometry and molecular geometry are the same for a molecule or a polyatomic ion.
7.96 Consider the hydrocarbons whose structures are shown below. Which of these molecules would be planar, meaning that all of the atoms must lie in the same plane? Explain your answer in terms of orbital hybridizations.
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?
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?
Do lone pairs about a central atom affect the hybridization of the central atom? If so, how?
Numerous molecules are detected in deep space. Three of them are illustrated here. (a) Are these compounds isomers? (b) Indicate the hybridization of each C atom in each molecule. (c) What is the value of the HCH angle in each of the three molecules? (d) Which of these molecules is/are polar? (e) Which molecule should have the strongest carbon-carbon bond? The strongest carbon-oxygen bond?
a) Identify atomic orbital #1 and #2. Indicate the number of radial and angular nodes for both b) What type of molecular orbital (σ, π, or no interaction) will be formed when these orbitals approach each other along the x axis? Describe the orbital overlap if applicable. Assume that the atomic orbitals are at appropriate energy levels to mix.

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