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Here are the answers to a Questions on First Year Honors Hybridization.
1) # of atomic orbital "in" = # of hybridized orbital "out"
2a) # of outside atoms bonded to central atom
2c) # of LP (Lone Pairs) on central atoms
3) Look at the list of atomic orbitals (s,p,p,p,d,d,d,d,d: did not include subscripts) and count from L to R the number from Question 2. Then put them together. For example, if Q2 answer is 3, then you have sp<sup>2</sub> hybridized(counted s,p,p) orbitals.
4) Since exceeding Rule of 8 would need greater than 4 hybridized orbitals then you needed greater than 4 atomic orbitals. Since the s and p atomic orbitals only gives you 4, then you need to use d atomic orbitals. d orbitals only exist for elements that are in the 3rd energy level or greater.
left to right (R)