Suppose that you have 16 diatomic molecules or ions with the valence molecular orbital arrangement shown here (Figure 1) , but with different numbers of valence electrons. Species 1 has one valence electron, species 2 has two valence electrons, etc. Classify each as diamagnetic or paramagnetic.
The bonding and anti – bonding interaction of the molecules can be explained with the help of a molecular orbital diagram. It also gives a detailed description of bonding in molecules. The diamagnetic and paramagnetic behavior of the molecules can be explained according to the arrangement of electrons.
Molecular orbital diagram:
The molecular orbital diagram consists of two types of bond. They are sigma bond and pi bond . The electrons first fill the lower energy level 2s and then moves to the higher energy level 2p. Also, the electrons first fill the bonding molecular orbital and then moves to anti – bonding molecular orbitals.
If the electrons in molecular orbitals are paired, then it is called diamagnetic. If the electrons in molecular orbitals are unpaired, then it is called paramagnetic.
Diamagnetic: 2, 4, 8, 10, 14, and 16
Paramagnetic: 1, 3, 5, 6, 7, 9, 11, 12, 13 and 15
Ans:Suppose that you have 16 diatomic molecules or ions with the valence molecular orbital arrangement shown...
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.Figure 2:
Using the molecular orbital energy ordering for second-row homonuclear diatomic molecules in which the π2p orbitals lie at lower energy than the σ2p, predict the bond order in a molecule or ion with each of the following numbers of total valence electrons.(Use the drawing MO energy diagrams) Will the molecule or ion be diamagnetic or paramagnetic? Part A Determine the bond order in a molecule or ion with 4 valence electrons. Part B Will this molecule or ion be diamagnetic...
The molecular orbital energy diagram for the valence orbitals of
the NO– ion is shown below. Use this diagram to answer the
following questions.
a) What is the bond order in NO– ? b) Is NO– diamagnetic, or is
it paramagnetic? How can you tell? c) Which has the larger bond
distance, NO– or NO?
* O2p T2p T2p G2s
13. (14 pts) MO Theory Draw the complete (core and valence) molecular orbital energy level diagram for the homonuclear diatomic molecule Be2. Use standard MO symbols to label the energy levels (That is: o, o, , or n*, as needed, with subscripts indicating which atomic orbitals formed them.) a. Sketch the molecular orbital formed when two 2p orbitals, one each on each Be atom, overlap to form a o antibonding MO b. Using your MO energy level diagram in (a),...
Match each of the following ions and molecules with its correct molecular Complete the Lewis structure of the chlorite ion, ClO2-, which is used as a bleaching agent. Complete only two resonance structure in which the formal charges are closest to zero. What is the valence molecular orbital configuration (according to MO theory) of homonuclear diatomic species where the atoms have an atomic number greater than seven? How many electrons are there in the pi antibonding orbitals of the following...
What kind of molecular orbital for a diatomic molecule is represented by the drawing shown? Select one: a. op ob. 02p C. Tt2p O d. tip e. 02 Which of the following molecules has bonding that can be described as an sp2-sp? o-overlap and one p-p 1-overlap using Valence Bond Theory? Do not consider bonds to hydrogen. Select one: a. N2 b. HCCH c. H2CCH2 d. Bez e. CO
Molecular orbitals. Consider the following diatomic molecules: H2*, H2, Li2, N2, O2. For each molecule, (A) determine the number of electrons N; (B) give the index i of the HOMO (1 is lowest energy orbital, 2 is next one up, etc); (C) sketch the shape of the HOMO, indicating the signs of the lobes; (D) indicate the symmetry of the HOMO (o, T, 6)
Molecular orbitals. Consider the following diatomic molecules: H2*, H2, Li2, N2, O2. For each molecule, (A)...
5. Some heteronuclear d energy levels like th heteronuclear diatomic molecules have energy levels like those in Figure 3, while others to ey levels like those in Figure 4 (e.g., CN, CN-, and CNT). Write the molecular orbital electron configurations for these three species. For example electron configuration for H, is (015) b. Arrange these species in increasing bond order, increasing bond length, and increasing bond energy
0.67/1 pts Question 15 Ad molecular orbital possesses electron density [Select [Select] the nuclei and electrons in the internuclear axis that orbital weaken the bond. Answer 1: above and below Answer 2 not between Answer 3: weaken 0/1 pts t Question 16 Considering only the valence s and pelectrons from the individual atoms, an F2 molecule contains how many electrons in all antibond ing molecular orbitals if it has a molecular orbital diagram as shown below?
0.67/1 pts Question 15...
please answer
question 7 using question 5 and the molecular orbital diagram
given.
5. Prepare a molecular orbital diagram for BN. You may consider valence orbitals only. Label the atomic orbitals for B and N with the appropriate potential energy. Decide which orbitals have the correct symmetry, orientation, and potential energies to interact (see the handout provided during class). Label the valence atomic orbitals with the appropriate potential energy. Should s-p mixing be considered for BN? How will the MO...