Using the molecular orbital energy ordering for second-row homonuclear diatomic molecules in which the 20 orbitals...

Using the molecular orbital energy ordering for second-row homonuclear diatomic molecules in which the 20 orbitals lie at a l

Using the molecular orbital energy ordering for second-row homonuclear diatomic molecules in which the 20 orbitals lie at a lower energy than the 02p, draw the MO energy diagrams and predict the bond order in a molecule or ion with each number of total valence electrons. Will the molecule or ion be diamagnetic or paramagnetic? a) 6 valence electrons b) 9 valence electrons c) 12 valence electrons

Expert Solution

Note that the molecules/ions given are not necessarily homonuclear molecules. They can be heteronuclear molecules as well. Also, they can be cationic or anionic. Please see the attached solution:

The * marked MO's are antibonding in nature, while others are bonding in nature.

If all the elctrons are paired, than the molecule/ion is diamagnetic, else paramagnetic.

queen_honey_blossom answered 2 years ago

Assuming that the molecular orbital energy level diagram for homonuclear diatomic molecules can be applied to...

Assuming that the molecular orbital energy level diagram for homonuclear diatomic molecules can be applied to heteronuclear diatomic molecules, arrange the NO, NO- and NO+ in order of decreasing bond length, from longest to shortest. Explain why that order is accurate using molecular orbital diagrams and what you know about how bond lengths behave.

Compare the energies of molecular orbitals of homonuclear diatomic molecules with the energies of the atomic...

Compare the energies of molecular orbitals of homonuclear diatomic molecules with the energies of the atomic orbitals with which they correlate. Both bonding and antibonding molecular orbitals lie lower in energy than the atomic orbitals. Both bonding and antibonding molecular orbitals are higher in energy than the atomic orbitals. Bonding orbitals are higher and antibonding orbitals are lower in energy than the atomic orbitals. Bonding orbitals are lower and antibonding orbitals are...

Consider the molecular orbital diagram shown below, a diagram that is often applied to the first row diatomic molecules.

Consider the molecular orbital diagram shown below, a diagram that is often applied to the first row diatomic molecules. Note that this diagram comprises orbitals derived from the n = 2 valence shell of orbitals (2s and 2p). Use this diagram to determine (1) if the following diatomic molecules or ions will be diamagnetic (all electrons paired) or paramagnetic (one or more unpaired electrons), and (2) for paramagnetic species, the number of unpaired electrons.O2, N2, CO, NO, NO-, NO+, CN-,...

Outline the rules of the building-up principle for homonuclear diatomic molecules.

5. Using boxes to represent orbitals, draw the molecular orbital energy level diagrams for the following...

5. Using boxes to represent orbitals, draw the molecular orbital energy level diagrams for the following molecules, with energy increasing vertically, putting electrons into the appropriate orbitals. For each indicate: the bond order and whether the molecule is paramagnetic or diamagnetic. a) B2 b) CN- c) NO d) NO+

9.5 Explain the concepts of the molecular orbital model and apply to diatomic molecules Define diamagnetism...

9.5 Explain the concepts of the molecular orbital model and apply to diatomic molecules Define diamagnetism and paramagnetism Determine if specific ions are paramagnetic or diamagnetic Explain what a molecular orbital is and how it is different from a hybrid orbital Explain the difference between an anti-bonding and a bonding as well as a sigma and pi molecular orbitals. Populate a molecular orbital diagram with the valence electrons of an atom or ion Determine the bond order and magnetic properties...

let us consider the case of a bonding electron in a diatomic molecule using molecular orbital...

let us consider the case of a bonding electron in a diatomic molecule using molecular orbital theory. Given that the probabilities of finding the electron in atomic orbitals ?A and ?B are 1/3 and 2/3, respectively, what is the LCAO-MO wavefunction for the electron? (Neglect the overlap integral as a simplifying approximation)

Suppose that you have 16 diatomic molecules or ions with the valence molecular orbital arrangement shown here (Figure 2)

Suppose that you have 16 diatomic molecules or ions with the valence molecular orbital arrangement shown here (Figure 2) , but with different numbers of valence electrons. Species 1 has one valence electron, species 2 has two valence electrons, etc. Classify them as diamagnetic or paramagnetic.

Subject: Physical Chemistry Topic: Molecular Orbital Theory Explain why the energy stabilization for bonding orbitals is...

Subject: Physical Chemistry Topic: Molecular Orbital Theory Explain why the energy stabilization for bonding orbitals is less than the destabilization energy for antibonding orbitals.

Which statement is not true of molecular orbitals? A)The number of molecular orbitals formed is always...

Which statement is not true of molecular orbitals? A)The number of molecular orbitals formed is always equal to the number of atomic orbitals combined. B)A molecular orbital can accommodate up to two electrons. C)When electrons are added to orbitals of the same energy, the most stable arrangement is predicted by Hund's rule. D)Low-energy molecular orbitals fill before high-energy molecular orbitals fill. E)Antibonding molecular orbitals are higher in energy than all of the bonding molecular orbital

Question