Question

Does each orbital have exactly the same amount of energy as another orbital? Explain.

Answer 1

No, they do not.
You have s, p, d, and f and so forth, orbitals....
The lower is \(s\) and increases as you go higher. However, the orbitals of each of those IS the same energy and it said to be "degenerate".

Answer 2

I did not understand this part. -->The lower is s and increases as you go higher. However, the orbitals of each of those IS the same energy and it said to be "degenerate".

Answer 3

Can you explain about it much more please?

Answer 4

Hmm, I don't know how in depth to get with this depending on the grade this is for.
But, ok. But let me try to simplify this because this is venturing into physical chemistry.

As I was saying, is that, if you recall back to your quantum numbers, \(n\), \(m_l\), and \(l\), all orbitals of the same velue of \(\color{red}{n}\) but different values of \(l\) and \(m_l\) have the same energy. But, this is true for hydrogenic atoms.
Because when you have more than one wavefunction, or \(\psi\), correspnding to the same energy, they are said to be degenerate. And by degenerate, which basically means orbitals which have the same energy in an atom.

When I was referring to s, p, and d-orbitals...i was referring to their subshells. There is a different name for the shells, and you use differnt letters.
an s-orbital takes on a spherical shape. The electron is free to float about it freely about it.
so it can give equal energy all aorund. However, the p-orbital subshell, has three shapes, in a coordinate system, x, y, and z.

Answer 5

Is this making a bit of sense to you?

Answer 6

Thanks a lot. You know about chemistry so much. I fan you to ask you my other questions in the future.

Answer 7

Last question. You meant that as orbitals increase. They have different energies right?

Answer 8

Yes. s-orbital has lowest energy, because you have a sphere. It is distributed equally. Then you have p-orbital, which is higher in energy than an orbital of s.

Answer 9

But a 2s orbital is higher than a 1s orbital in energy.

Answer 10

Ok. What about 2py, 2px, 2pz. I assume they have the same energy? right? Because they are all in the p orbital and in one energy level.

Answer 11

What course is this for?

Answer 12

Chemistry 11.

Answer 13

And yes, they are.
What is Chemistry 11?

Answer 14

chemistry grade 11 in highschool

Answer 15

Oh. Ok. Well, yeah. In that case, for high school, all you need to know is that the more you go up, the higher in energy it is.
I don't think you will go into d-orbitals at high school level. So do not worry about that.

Answer 16

We still have to know the electron configuration for them. @thadyoung I know I asked lots of questions from you and you deserve more than one medal. You mentioned that as we go up in higher energy level, the energy increases, so does it mean that the p orbitals in energy level 4 and 5 are different from each other in terms of the amount of energy?

Answer 17

Don't worry about anything above group 4, because it gets a little more complicated when you start diving into d-orbitals.
But if you must know, d-orbitals are actually lower in energy than p-orbitals.

Answer 18

As you increase from 1s \(\rightarrow\) 2s you do increase in energy because you're now entering a new subshell.
You're no longer adding electrons into the 1s orbital, rather a new 2s orbital. As you remember might recall from hunds rule, OR if you're curious about quantum chemistry, it is the pauli exclusion principle.

Answer 19

As you add electrons, you are also adding more protons, and the electrons are also becoming farther away from the nucleus of the atom.

Now, you move onto 2s