The image at right shows electron density solutions for the molecule H₂ in panels a-e and an energy diagram for the atomic and molecular orbitals in the bottom right panel. The two hydrogen nuclei are shown as circles within the electron density solution images. The images a-e correspond to the 01s molecular orbital. Each depiction shows the contour of the 01s orbital at different electron density cutoffs. The cutoffs, in order from a to e, are, in units of electron/a³, 0.10, 0.15, 0.20, 0.25, and 0.30. (ao is the characteristic size of the hydrogen atom, called the Bohr radius.) The images show the locations of electron density at or above these values. How many electrons are found in H₂? Select one: O 1 O 2 O 3 O 4 Impossible to tell (a) (c) (e) (b) (d) 0.8 Eo*--. E Es Eot H 1s *0 0₁ 1s

The image at right shows electron density solutions for the molecule H₂ in panels a-e and an energy diagram for the atomic and molecular orbitals in the bottom right panel. The two hydrogen nuclei are shown as circles within the electron density solution images. The images a-e correspond to the 01s molecular orbital. Each depiction shows the contour of the 01s orbital at different electron density cutoffs. The cutoffs, in order from a to e, are, in units of electron/a³, 0.10, 0.15, 0.20, 0.25, and 0.30. (ao is the characteristic size of the hydrogen atom, called the Bohr radius.) The images show the locations of electron density at or above these values. How many electrons are found in H₂? Select one: O 1 O 2 O 3 O 4 Impossible to tell (a) (c) (e) (b) (d) 0.8 Eo--. E Es Eot H 1s 0 0₁ 1s

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 10.100QE: The molecular orbital diagram of NO shown in Figure 10.47 also applies to the following species....

See similar textbooks

Similar questions

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 p*2p orbitalsof the carbon monoxide molecule. This is calledd@p 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 carbonnearest the M. The CO bond axis should be on the x-axis.(c) Draw the CO p*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 p*2p orbital of CO? (e) What kind of bond is being madewith the orbitals between M and C, s or p ? (f) Predict whatwill happen to the strength of the CO bond in a metal–COcomplex compared to CO alone.
The photoelectron spectrum of HBr has two main groupsof peaks. The first has ionization energy 11.88 eV. Thenext peak has ionization energy 15.2 eV, and it is followedby a long progression of peaks with higher ionizationenergies. Identify the molecular orbitals corresponding tothese two groups of peaks.
The diagram that follows shows the highest-energy occupiedMOs of a neutral molecule CX, where element X is in thesame row of the periodic table as C. (a) Based on the numberof electrons, can you determine the identity of X? (b) Wouldthe molecule be diamagnetic or paramagnetic? (c) Considerthe π2p MOs of the molecule. Would you expect them to havea greater atomic orbital contribution from C, have a greateratomic orbital contribution from X, or be an equal mixtureof atomic orbitals from the two atoms?
Indicate whether each statement is true or false. (a) s orbitalscan only make s or s* molecular orbitals. (b) The probabilityis 100% for finding an electron at the nucleus in a p* orbital.(c) Antibonding orbitals are higher in energy than bondingorbitals (if all orbitals are created from the same atomic orbitals).(d) Electrons cannot occupy an antibonding orbital.
esonance Theory? Sate five c we main oxnorimonte that w
A O The quantum numbers for last electron -3 * ?of vanadium is it c- n=4 , I=3 , ml=+2 , ms= -1/2 b- n=4 , 1=2 , ml=+2 , ms=+1/2 O a- n=3 , l=2, ml=0 , ms=+1/2 * ?Bond order of Cl2 is -4 c. 1 a. 2 O b. 3 O * ?Bond order of B2 is -5 а. 1 с. 3 b. 2 صفحة 3 من 4 II
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.
From your knowledge of molecular orbital diagrams, what is the correct set of relationships between the ionization energies of molecular hydrogen to that of atomic hydrogen, and molecular oxygen to that of atomic oxygen? IEĦ, ?IEH;IEo, ?IEo where [? =>, IEo O IEH, > IEH; IE0, IEH; IE0, > IEo O IEH, = IEH; IE0, = IEo
Given the following molecule, on which part of the molecule is the electron density the | greatest? O=C=O on the oxygen atom to the left O It is evenly distributed. O on the oxygen atom to the right on the C O on the two oxygen atoms
4. Describe thelocation of the maximumelectron density of o- and n-bonds. How is the difference in the spatial arrangementof the electron density of these bonds reflected on their strength?
How many orbitals are allowed in asub shell if 2 B5 An organic flavoring agent extraoted fram A PePPer mint oil.it contains c, Hr and o. in o ne combus tion amlysis) 0:0100g of the Substance yields 0.01153 g H,o and 0,02816g co . what is the empirical formula and mdecular formula of this f lvorng agent is the molar mass is 156l 9 Imol
The photoelectron spectrum of HBr has two main groups of peaks. The first has ionization energy 11.88 eV. The next peak has ionization energy 15.2 eV, and it is followed by a long progression of peaks with higher ionization energies. Identify the molecular orbitals corresponding to these two groups of peaks.