Between these orbitals: s, px, py, pz, dxy, dyz, dxz, dx2-y2, and dz2. Which of them absolutely cannot overlap, and why? If you can, please give me clear explanation (rather than their symmetry doesn't match, please say something like because this orbital approach in this plane/axis, which doesn't match with the one from the other orbital, etc).

Between these orbitals: s, px, py, pz, dxy, dyz, dxz, dx2-y2, and dz2. Which of them absolutely cannot overlap, and why? If you can, please give me clear explanation (rather than their symmetry doesn't match, please say something like because this orbital approach in this plane/axis, which doesn't match with the one from the other orbital, etc).

Organic Chemistry

8th Edition

ISBN:9781305580350

Author:William H. Brown, Brent L. Iverson, Eric Anslyn, Christopher S. Foote

Publisher:William H. Brown, Brent L. Iverson, Eric Anslyn, Christopher S. Foote

Chapter1: Covalent Bonding And Shapes Of Molecules

Section: Chapter Questions

Problem 1.63P: Draw the delocalized molecular orbitals for the following molecule. Are both bonds of the triple...

See similar textbooks

Similar questions

Draw the delocalized molecular orbitals for the following molecule. Are both bonds of the triple bond involved in the delocalized orbitals?
Predict whether the MO diagram S2 would show s-p mixing or not.
This molecule has [x overlapping atomic p orbitals that combine to make [y]. molecular pi orbitals.
Can i get help on this problem please
Specify the hybridization at the atom labeled a-d. For each atom enter one of the following: sp3, dsp2, sp3d, or sp.
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?
Please explain.
Draw an MO diagram to explain the existence of the trihydrogen cation (H3+). Hint: it forms a cyclic structure. Use individual 1s orbitals from H atoms to form your molecular orbitals (don’t worry about forming LGOs; determine the symmetries of the MOs using the projection operator method and sketch approximate wavefunctions for each). How many electrons are present in this molecule? What is the bond order? What type of bonding is this?
Draw the electron correlation diagram for O2. a. Identify which combinations of atomic orbitals form each molecular orbital and state whether this is the result of constructive or destructive interference between the electronic wavefunctions. b. Label the molecular orbitals based on their symmetry. c. What is the bond order of O2? O2+? O2-? d. List these three molecules in order of decreasing bond length. e. List them in order of decreasing bond energy. f. Which of these three molecules would be attracted to a magnetic field?
Consider a ring system made up of 6 atoms (each one contributing a p atomic orbital to make 6 pi molecular orbitals). If the system is filled with 8 electrons, there will ----orbitals containing pairs of electrons and------ orbitals containing single, unpaired electrons. Hint: Use a Frost Circle.
Show o versus R overlap for 2p orbitals Show R overlap for 2d orbitals- can d orbitals orientate for o overlap?
4. Molecular Orbital Theory Let's construct an MO diagram for KrBr*, the krypton bromide cation. Let's focus only on the n=4 valence shell in for both species. a) Which of the two atoms, Kr or Br, has a 4p electrons that are lower in energy? Justify your answer in terms of periodic trends. Also provide experimental evidence for your answer in terms of ionization energies (available online). b) Based on part (a), draw an MO diagram for KrBr*, reflecting the appropriate relative energies of the Kr/Br valence electrons. Connect the orbitals that mix/split with dashed lines. c) Populate the MO diagram with the appropriate number of valence electrons. What is the expected bond order?