How to draw a molecular orbital (MO) diagram for F$_2^+$?

Which of these species has a longer bond, $\mathrm{B}_2$ or $\mathrm{B}_2$ ? Explain in terms of molecular orbital theory.

How to draw a molecular orbital (MO) diagram for B$_2$?

Use the drawing of the mo energy diagram to predict the bond order of $\ce{Li2+}$.

In molecular orbital theory, what is a non bonding orbital?

Construct the orbital diagram of the $\mathrm{F^-}$ ion. A neutral fluorine atom has 9 electrons. How many electrons does a $\mathrm{F^-}$ ion have?

Write the symbol for the ion of each of the following:

a. fluorine

b. barium

c. sodium

d. iodine

Some species with two oxygen atoms only are the oxygen molecule, $\mathrm{O}_2$, the peroxide ion, $\mathrm{O}_2{ }^{2-}$, the superoxide ion, $\mathrm{O}_2^{-}$, and the dioxygenyl ion, $\mathrm{O}_2^{+}$. Draw an $\mathrm{MO}$ diagram for each, rank them in order of increasing bond length, and find the number of unpaired electrons in each.

Construct the MO energy level diagram for the cyanide ion, keeping in mind that the more electronegative element has orbitals lower in energy than the less electronegative element. What is the bond order in this ion? Compare the valence bond and molecular orbital descriptions of bonding in this ion.

Molecular nitrogen, carbon monoxide, and cyanide ion are isoelectronic,

Draw an MO diagram for each,

Write orbital diagrams for each ion and determine if the ion is diamagnetic or paramagnetic.

a. $\ce{Cd^{2+}}$
b. $\ce{Au^+}$
c. $\ce{Mo^{3+}}$
d. $\ce{Zr^{2+}}$

For each of the following metals, write the electronic configuration of the atom and its 3+ ion: Mo. Draw the crystal-field energy-level diagram for the d orbitals of an octahedral complex, and show the placement of the d electrons for each 3+ ion, assuming a weak-field complex. How many unpaired electrons are there in each case?

Some species with two oxygen atoms only are the oxygen molecule, O2, the peroxide ion, O22-, the superoxide ion, O2- and the dioxygenyl ion, O2+. Draw an MO diagram for each, rank them in order of increasing bond length, and find the number of unpaired electrons in each.

Which of the following has the list of compounds in the correct order of decreasing density (higher density > lower density)?

a. $\ce{CH2Cl2 > CH2Br2 > CH2I2}$
b. $\ce{CH2Cl2 > CH2I2 > CH2Br2}$
c. $\ce{CH2I2 > CH2Br2 > CH2Cl2}$
d. $\ce{CH2I2 > CH2Cl2 > CH2Br2}$