Electron Structure Flashcards
How are electrons arranged in an atom?
Electrons are arranged in shells which are split into 4 sub shells.
How many electrons fit into one orbital?
2
How many orbitals does the s subshell have?
1 (can hold 2 e-)
How many orbitals does the p subshell have?
3 (can hold 6 e-)
How many orbitals does the d subshell have?
5 (can hold 10 e-)
How many orbitals does the f subshell have?
7 (can hold 14 e-)
What happens if electrons are in higher shells?
They are further from the nucleus and have a higher energy.
What is the shape of the s orbital?
Spherical. It has one orbital and the 2 e- can move anywhere in that sphere.
What is the shape of the p orbital?
It has 3 dumbbell shaped orbitals, each at 90 degrees to each other. Each can hold 2 e- that can move anywhere within the entire shape.
What is spin paring?
2 electrons in one orbital spin in opposite directions.
What do you do for the elctronic configuration of ions?
Add or remove the electrons from the highest energy level
What is an orbital?
A region of space around the nucleus that contains uo to 2 electrons
Why do electrons fill up separate orbitals before pairing in the same one?
Because they repel eachother
Why don’t paired electrons jump to a higher orbital due to their repulsion?
The energy required to jump to a higher energy orbital is greater than inter electron repulsion
What are the exceptions to the Aufbau principle (rules of electronic configuration)?
Chromium and copper have the following electron configurations:
Cr is [Ar] 3d5 4s1 NOT [Ar] 3d4 4s2
Cu is [Ar] 3d10 4s1 NOT [Ar] 3d9 4s2
This is because the [Ar] 3d5 4s1 and [Ar] 3d10 4s1 configurations are energetically favourable.
By promoting an electron from 4s to 3d, these atoms achieve a half full or full d-subshell, respectively
