(a) Consider the gaseous molecule BN-. At home, construct the molecular orbital diagram that is consistent with the known order of filling of molecular orbitals in the second period and with BN- being stable and paramagnetic.

What is the bond order of BN-?
(c) What ion of BN is isoelectronic with N2?

(d) Do you expect your answer to part c to be less stable, more stable, or equally stable as BN- from part a?

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bond order is 2.5

Thank you for the help.

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To answer these questions, let's break them down step by step:

(a) Constructing the molecular orbital diagram for BN-:
1. Start by considering the electronic configuration of the individual atoms. Boron (B) has an atomic number of 5, indicating that it has 5 electrons, while Nitrogen (N) has an atomic number of 7, indicating it has 7 electrons. Since BN- carries an extra electron, the total number of valence electrons will be 13 (5 from B + 7 from N + 1 for the negative charge).
2. Next, arrange the atomic orbitals based on their increasing energy levels. In the second period, there are 2s and 2p atomic orbitals available.
3. Fill the molecular orbitals using the Aufbau principle, which states that lower energy molecular orbitals are filled before higher energy ones. Each molecular orbital can accommodate a maximum of 2 electrons with opposite spins (Pauli exclusion principle).
4. The order of filling for the second period is: 2s -> 2s* -> 2px -> 2py -> 2pz -> 2px* -> 2py* -> 2pz*.
5. Distribute the 13 valence electrons into the molecular orbitals, starting with the lowest energy molecular orbital and filling up to the highest energy orbital until all electrons are utilized.
6. In order for BN- to be stable and paramagnetic, it must have unpaired electrons. Determine the number of unpaired electrons by considering the filling of electrons in the molecular orbitals.

(b) Calculating the bond order of BN-:
1. The bond order (BO) is calculated as the difference between the number of bonding electrons and the number of antibonding electrons, divided by 2. The bond order indicates the stability and strength of a bond.
2. Count the number of electrons in bonding molecular orbitals (MOs) and antibonding MOs.
3. Subtract the number of antibonding electrons from the number of bonding electrons.
4. Divide the difference by 2 to obtain the bond order.

(c) Finding the ion of BN that is isoelectronic with N2:
1. Isoelectronic species are those that have the same number of electrons.
2. Find the total number of electrons in the N2 molecule: nitrogen (N) has 7 electrons, and there are two nitrogen atoms, so the total count is 7 x 2 = 14 electrons.
3. Look for the BN ion that also has 14 electrons.

(d) Determining the relative stability of the ion from part (c) compared to BN-:
1. Compare the electron configuration and the electron distribution in bonding and antibonding MOs.
2. Consider factors like the electronegativity and atomic size of the atoms involved to determine relative stability.
3. Based on these considerations, make a judgment about the relative stability of the ion compared to BN-.

By following these steps, you should be able to construct the molecular orbital diagram, calculate the bond order of BN-, find the isoelectronic ion of BN, and determine its relative stability.