Now, an orbital can hold a maximum of 2 electrons that have opposite spins according to the Pauli exclusion principle. It states that no two electrons found within an orbital can have the same electron spin. One has to spin up and one has to spin down. When we talk about this electron spin, it concerns the rotational spin of an electron inside an atomic orbital. We start out filling an orbital with an electron that points up, followed by the next one pointing down. If we were to fill out this orbital, we would use arrows to depict the electrons within it: one would point up and one would point down. They have opposite spins inside the same orbital. Realize here that the electron that points up has an electron spin value of plus one-half. Pointing up, it spins clockwise, and an electron that points down has an electron spin value of minus a half. Pointing down means that it spins counterclockwise. So, just remember, plus a half is synonymous with clockwise, and negative a half is synonymous with counterclockwise in relation to an electron spin.
Electronic Structure: Electron Spin - Online Tutor, Practice Problems & Exam Prep
Electron Spin deals with the rotational spin (up or down) of an electron inside an orbital.
Electronic Structure:Electron Spin
Electronic Structure: Electron Spin Concept 1
Video transcript
Electronic Structure: Electron Spin Example 1
Video transcript
Here it says to provide the n value, subshell letter, and electron spin for the highlighted electron in a third principle level. Alright. So here when we're talking about the 3rd principle level, we're talking about the energy level or shell number. So here this means that n equals 3 because, remember, energy level, shell number, principal level, all referring to the n value. That means the answer is either b or d. Next, we have an image here of 3 orbitals. You have to think about which subshell letter has 3 orbitals. Remember, s only has 1, p is the one that has 3, d has 5. Alright. So we're dealing with p. So the subshell letter is p. So far it's still b or d. Now we look at the electron within that particular orbital. Which way is it pointing? Is it pointing up or is it pointing down? We can see that the electron that's highlighted is pointing down. That means its electron spin would be minus a half. So that would mean that option would be our correct answer.
Which of the following can represent the highlighted electron in a set of 5d orbitals.