What is the role of wave interference in determining whether a molecular orbital is bonding or antibonding? Match the words in the left column to the appropriate blanks in the sentences on the right. constructive an increased a diminished higher opposite phases the same phase particles waves destructive lower Reset Help The electrons in orbitals behave like waves therefore the bonding molecular orbital arises from the constructive interference between the atomic orbitals, because orbitals have the same phase ; the antibonding molecular orbital arises from the destructive interference between the atomic orbitals, because the interacting orbitals have opposite phases. The bonding orbital has higher electron density in the internuclear region and, therefore, lower energy. The antibonding orbital has a node in the internuclear region and, therefore, higher in energy than atomic orbitals.

What is the role of wave interference in determining whether a molecular orbital is bonding or antibonding? Match the words in the left column to the appropriate blanks in the sentences on the right. constructive an increased a diminished higher opposite phases the same phase particles waves destructive lower Reset Help The electrons in orbitals behave like waves therefore the bonding molecular orbital arises from the constructive interference between the atomic orbitals, because orbitals have the same phase ; the antibonding molecular orbital arises from the destructive interference between the atomic orbitals, because the interacting orbitals have opposite phases. The bonding orbital has higher electron density in the internuclear region and, therefore, lower energy. The antibonding orbital has a node in the internuclear region and, therefore, higher in energy than atomic orbitals.

Organic Chemistry: A Guided Inquiry

2nd Edition

ISBN:9780618974122

Author:Andrei Straumanis

Publisher:Andrei Straumanis

Chapter17: Conjugation And Molecular Orbital (mo) Theory

Section: Chapter Questions

Problem 8CTQ

See similar textbooks

Similar questions

Enter in order the hybridization and coordination number (CN) of the central atom for each substance
What property of molecules allows them to change their threedimensionalshape?
Mixing changes the bonding–antibonding nature of some orbitals. Explain?
Antibonding molecular orbitals can be used to make bondsto other atoms in a molecule. For example, metal atomscan use appropriate d orbitals to overlap with the π*2p orbitalsof the carbon monoxide molecule. This is calledd-π backbonding. (a) Draw a coordinate axis system inwhich the y-axis is vertical in the plane of the paper andthe x-axis horizontal. Write “M” at the origin to denote ametal atom. (b) Now, on the x-axis to the right of M, drawthe Lewis structure of a CO molecule, with the carbon nearest the M. The CO bond axis should be on the x-axis.(c) Draw the CO π*2p orbital, with phases (see the “CloserLook” box on phases) in the plane of the paper. Two lobesshould be pointing toward M. (d) Now draw the dxy orbitalof M, with phases. Can you see how they will overlap withthe π*2p orbital of CO? (e) What kind of bond is being madewith the orbitals between M and C, σ or π ? (f) Predict whatwill happen to the strength of the CO bond in a metal–COcomplex compared to CO alone.
The following is part of a molecular orbital energy-level diagramfor MOs constructed from 1s atomic orbitals. (a) What labels do we use for the two MOs shown? (b) Forwhich of the following molecules or ions could this be theenergy-level diagram:H2, He2, H2+, He2+, or H2-?(c) What is the bond order of the molecule or ion? (d) If anelectron is added to the system, into which of the MOs will itbe added? [
How are the following similar, and how do they differ? (a) molecular orbitals and molecular orbitals (b) for an atomic orbital and for a molecular orbital (c) bonding orbitals and antibonding orbitals
The following sketches show the atomic orbital wave functions(with phases) used to construct some of the MOs ofa homonuclear diatomic molecule. For each sketch, determinethe type of MO that will result from mixing theatomic orbital wave functions as drawn. Use the same labelsfor the MOs as in the “Closer Look” box on phases.
The table below shows some physical properties of halogenatedliquids. Which of the following statements best explains these data?(a) The larger the dipole moment, the stronger the intermolecularforces, and therefore the boiling point is lowest for themolecule with the largest dipole moment. (b) The dispersionforces increase from F to Cl to Br; since the boiling point alsoincreases in this order, the dispersion forces must make a fargreater contribution to intermolecular interactions thandipole-dipole interactions. (c) The trend in electronegativityis F > Cl > Br; therefore, the most ionic compound (CH2F2)has the lowest boiling point, and the most covalent compound(CH2Br2) has the highest boiling point. (d) Boiling point increaseswith molecular weight for these nonpolar compounds.
How are the following similar, and how do they differ?(a) σ molecular orbitals and π molecular orbitals(b) ψ for an atomic orbital and ψ for a molecular orbital(c) bonding orbitals and antibonding orbitals
Which of the following statement(s)regarding stable heteronuclear diatomic molecules is(are) CORRECT? a. Their molecular orbital diagram are more symmetrical than those of homonuclear diatomic molecules. b. The greater is the difference in energy between two overlapping atomic orbitals, the more polar the resulting bond is, due to electrons occupying the resulting bonding molecular orbital. c. All have bond orders greater than zero. d. The antibonding molecular orbitals have more of the character of the more electronegative element than the more electropositive element.
The cutoff off says that is most paramagnetic
How to determine the si or re side of flatvin??