Drawing Arrangement Flashcards
Why can two electrons occupy the same orbital
Because of electron spin
Define electron spin, and explain why they don’t repel
Electron spin is caused by the momentum that an electron has, two electrons in the same orbital have opposite spins. This is why they don’t repel
What are the three golden rules of Electron Configuration
1.Electrons fill up from the lowest energy level first
2. Fill up orbitals singularly, before they start sharing
3.When forming ions you add or remove electrons to or from the highest occupied sub-shell
When you have p-orbitals, whats the rule on filling the 3 p-orbitals.
Start with Px then Py then Pz. add one electron to the first of every box, this is because they’re have the same energy level, so you cant fill one and leave one empty
What’s the rule of adding or removing electrons on p,d and f-orbitals when drawing ions
You add or remove electrons from occupied boxes with the highest energy level first.
What is the exception to rule 1 of electron configuration
The one exception is that 4s has a lower energy level than 3d.
In sub-shell notation how to you represent the amount of electrons in each box
You either add ² is the box if full (2 electrons) or ¹ if the box isnt full. For example 1s², 2s¹, This shows that theres 3 electrons meaning its the element Lithium. For orbitals that have 3 or 5 different parts you subscript the full amount of orbitals so if a p orbital had 5 electrons you will do 1s²,2s²,2p⁵
For s and p block elements, how are the electrons changed to become ions
Electrons are removed from or added to the highest sub shell
When you have a 4s and 3d ion, which box changed first when the electron count is changed.
As long as each of the 5 3d orbitals are half full, the electron is added or removed from the 4s orbital first. However, you still write the 5 3d orbitals before the 4s.
