Which of the following statements about molecular orbital (MÔ) theory are untrue? **select all that apply destructive overlap of atomic orbitals produces antibonding MOS paramagnetic molecules will not align in a magnetic field bond order equals the number of bonding electrons minus the number of antibonding electrons antibonding MOs are lower in energy than bonding MOs constructive overlap of atomic orbitals produces bonding MOS diamagnetic molecules do not have any half-filled MOs Moving to the next question prevents changes to this answer.

Which of the following statements about molecular orbital (MÔ) theory are untrue? **select all that apply destructive overlap of atomic orbitals produces antibonding MOS paramagnetic molecules will not align in a magnetic field bond order equals the number of bonding electrons minus the number of antibonding electrons antibonding MOs are lower in energy than bonding MOs constructive overlap of atomic orbitals produces bonding MOS diamagnetic molecules do not have any half-filled MOs Moving to the next question prevents changes to this answer.

Chemistry by OpenStax (2015-05-04)

1st Edition

ISBN:9781938168390

Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Chapter8: Advanced Theories Of Covalent Bonding

Section: Chapter Questions

Problem 19E: Strike-anywhere matches contain a layer of KClO3 and a layer of P4S3. The heat produced by the...

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Strike-anywhere matches contain a layer of KClO3 and a layer of P4S3. The heat produced by the friction of striking the match causes these two compounds to react vigorously, which sets fire to the wooden stem of the match. KCIO3 contains the ClO3 ion. P4S3 is an unusual molecule with the skeletal structure. (a) Write Lewis structures for P4S3 and the ClO3 ion. (b) Describe the geometry about the P atoms, the S atom, and the Cl atom in these species. (c) Assign a hybridization to the P atoms, the S atom, and the Cl atom in these species. (d) Determine the oxidation states and formal charge of the atoms in P4S3 and the ClO3 ion.
Consider these following ions: O2-, 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 draw appropriate molecular orbital energy diagram.
rotation is possible around sigma bonds but not around pi bonds because pi bonds are always made from hybridized orbitals pi bonds are stronger and resist rotation sigma bonds occur above and below the internuclear axis while pi bonds are only along the internal axis or sigma bonds maintain orbital overlap during rotation while rotation would break orbital overlap between pi orbitals
Draw the molecular orbital (MOs) that results from combining the following atomic orbitals. Recall that, depending on the phases and orientation of the orbitals, you may have: a. constructive overlap to form a bonding orbital b. destructive overlap to form an antibonding orbital c. no overlap (equal amounts constructive and destructive). In this case, write “non-bonding” instead of drawing an orbital
Which of the following statements true about the bonds in the figure above? a. Only sigma bonds use hybridized orbitals to overlap in forming the bonds b. Sigma bonds form from the end-to-end overlap of two hybridized s and p orbitals c. Pi bonds for from the side-to-side overlap of hybridized sp, sp2, sp3 orbitals d. The maximum number of sigma and pi bonds between two atom are different, but the energy level of the two bonds
The basis of the VSEPR model of molecular bonding is ________. Select one: a. atomic orbitals of the bonding atoms must overlap for a bond to form b. regions of electron density on an atom will organize themselves so as to maximize s-character c. regions of electron density in the valence shell of an atom will arrange themselves so as to maximize overlap d. electron domains in the valence shell of an atom will arrange themselves so as to minimize repulsions e. hybrid orbitals will form as necessary to, as closely as possible, achieve spherical symmetry Clear my choice
It might seem that a square-planar geometry of four electron domains around acentral atom would be more favorable than a tetrahedron. Can you rationalize whythe tetrahedron is preferred, based on angles between electron domains?
A MO scheme for CO2 is shown below. Fill in the electrons for both the atoms and the molecule. Notice that since there are 2 oxygens, there are six p orbitals and two s orbitals associated with the right hand column of the MO scheme. Determine which orbitals are bonding vs. nonbonding, vs. antibonding and calculate the bond order. Notice that the names of the MO’s are no longer s and p - they have other names. (Hint: bonding vs. antibonding vs. nonbonding can be figured out based on the energy of the MOs and the positioning of the dashed lines.) Compare the bond order to the valence bond picture of CO2, [O=C=O]. How are they related?
Which statement is true concerning molecular orbital (MO) theory? A. Atomic orbitals overlap to form bonds B. Atomic orbitals combine to form both bonding and anti-bonding orbitals C. Atomic orbitals through VSEPR can determine the geometric shapes of molecules D. Atomic orbitals on the same atom combine with each other to make hybrid orbitals.
Which of the following statements about a p* antibonding molecular orbital is true? A pi* antibonding molecular orbital is formed when two p orbitals of similar phase overlap. A pi* antibonding molecular orbital is formed when two p orbitals of opposite phase overlap. A pi* antibonding molecular orbital is a higher-energy molecular orbital than a pi bonding molecular orbital. Both the statements “a pi* antibonding molecular orbital is formed when two p orbitals of opposite phase overlap” and “a pi* antibonding molecular orbital is a higher-energy molecular orbital than a pi bonding molecular orbital” are true.
Consider a NF molecule a. Draw orbitals of each atorn and find possible interactions among them. b. Draw atomic orbitals. using the potential energy information c. Draw molecular orbitals from the atomic orbitals of N and F. d. What is the band order of this molecule? e. Specify the types of molecular orbitals, or (NF,NF? Which of the three has the longest bond length -NF, NF, and NF ? Explain your answer.
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.