I may have solved it.
d orbital hybridization, what is this?
In answer to your query, yes this is for homework. The textbook states nothing about d orbital hybridization. I did finally work out a solution that correlates with the solutions given on the internet. I'll describe the method:
1. Draw 4 o's and one p in the centre.
2. Draw a pair of electrons in between all four Os and the P.
3. Draw the remaining electrons around each O leaving 6 electrons around each Oxygen atom, and a bond between each oxygen-phosphorus pair.
This is where I got confused:
4. Since eight electrons were placed around the P, and P only brought 5 electrons to begin with...the P has a charge of 3-...since each O now has 7 electrons associated with its charge and it originally brought 6, the charge on each O is 1-.
8. To simplify this, we need to carry one pair of electrons from one of the O's and place it with the already existent bond. This results in a double bond.
9. Now when we figure out the charges....we get....5 electrons on the P that are associated with the charge (i.e. not including the other valence in the pair)...since P originally brought 5, this atom is neutral. each single-bonded O is still 1- since we haven't changed anything with them...the double bonded O now has 6 electrons associated with its charge (i.e. not including the other valence in the pair) which is exactly what it had originally....thus it too is neutral.
10. So we have one phosphorus atom in the centre, surrounded by three oxygen anions with a charge of 1- single bonded, and 1 oxygen atom double bonded with no charge.
Is this correct? It may also be incorrect due to typos, grammatical errors etc.
What is d orbital hybridization? Sounds interesting.
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