Arrange the following in order of decreasing stability. A blank molecular orbital diagram (Part A 1 figure) has been provided to help you.
Rank the fluorine species from most to least stable. To rank items as equivalent, overlap them. F2, F2+, F2-
F^+2,F2,F2-
F2+, F2, F2- is the correct answer as stated by "..."
I have no idea what the diagram looks like. BUT wouldn't you expect the F2 atom to be MUCH more stable than either of the others. You will need the diagram to rank the other two. Fit the F^+2 and the F^-2 into the diagram.
The neutral species is not necessarily the most stable
To determine the stability of the fluorine species, we need to consider their molecular orbital diagrams. Here's how you can analyze and rank them:
Step 1: Understand the basics of molecular orbital theory
Molecular orbital theory describes the behavior of electrons within molecules using molecular orbitals (MOs). MOs are formed by combining atomic orbitals (AOs) from each atom in the molecule.
Step 2: Sketch the molecular orbital diagram
Start by drawing a blank molecular orbital diagram with two energy levels: one for the F2 molecule and the other for F2+ and F2-. Label the energy levels as σ1s, σ1s*, σ2s, σ2s*, π2p, π2p*, etc., based on the atomic orbitals involved.
Step 3: Determine electron configuration and placement
For F2, fill the molecular orbitals with electrons according to the Aufbau principle, which states that electrons occupy the lowest energy orbitals first. Since fluorine has nine electrons, you will place one electron in each AO until they are all filled. The σ1s and σ1s* orbitals will be filled, leaving the π2p level empty.
For F2+ (fluorine cation), remove one electron from F2. You can do this by removing the least stable electron from the π2p orbital.
For F2- (fluorine anion), add one electron to F2. Add this electron to the most stable orbital available, which is the π2p* orbital.
Step 4: Compare stability based on the electron configuration
The stability of the fluorine species can be determined by comparing their electron configurations and the filling of molecular orbitals. The more stable a species, the lower its energy level.
Based on the analysis of molecular orbitals:
1. F2: This molecule has a filled σ1s and σ1s* orbital, making it the least stable since it has the highest energy level.
2. F2+: This cation is formed by removing one electron from F2. It loses an electron from the anti-bonding π2p orbital, making it more stable than F2 but less stable than F2-.
3. F2-: This anion is formed by adding one electron to F2. It occupies the anti-bonding π2p* orbital, making it the most stable of the three fluorine species due to the electron-electron repulsion being minimized.
Therefore, the ranked fluorine species from most stable to least stable are F2-, F2+, F2.
By analyzing the molecular orbital diagrams and considering electron configurations, you can determine the relative stability of different species.