I hope everyones studying is going well. I was doing Kaplan FL #1, and I think I may have misunderstood the concept or question. In any regards, my concern is the following:
I know that the s orbital is lower in energy than the p-orbital. Thus the more the s character, the lower the energy. Thus, sp would be considered the lowest energy. This is where I become confused. I always thought that the sp bond would be the highest energy, and strongest. That the triple bond would be the highest energy.
I dont understand the connection, if someone could please clear this up for me. Also, how do the C-H energy levels compare in sp3, sp2, and sp. For those that have kaplan, its question:
Molecular orbitals in hydrocarbons are formed between the 1s atomic orbital of H and sp, spy, and sp3 orbitals of C. Which correctly lists the energy levels of C-H bonds.
Benzene, ethyne, and methane.
Thanks in advance.
I know that the s orbital is lower in energy than the p-orbital. Thus the more the s character, the lower the energy. Thus, sp would be considered the lowest energy. This is where I become confused. I always thought that the sp bond would be the highest energy, and strongest. That the triple bond would be the highest energy.
I dont understand the connection, if someone could please clear this up for me. Also, how do the C-H energy levels compare in sp3, sp2, and sp. For those that have kaplan, its question:
Molecular orbitals in hydrocarbons are formed between the 1s atomic orbital of H and sp, spy, and sp3 orbitals of C. Which correctly lists the energy levels of C-H bonds.
Benzene, ethyne, and methane.
Thanks in advance.