Electron configuration and hybridisation Flashcards
How would an electron shift from one orbital to another?
If it gained or lost energy
What do s, p, d, and f refer to?
Subshells
Each orbital can fit ___ electrons
2
How many electrons can the s subshell fit?
2
How many electrons can the p subshell fit?
6
How many electrons can the d subshell fit?
10
How many electrons can the f subshell fit?
14
What do (as examples) px and dxz refer to?
Orbitals
What is required for two electrons to occupy the same orbital?
They must have opposite spins - the Pauli Exclusion Principle
In electron configuration notation, what do the numbers refer to, what are they called, and what letter is used to represent them?
The numbers are called principal quantum numbers, they are represented by the letter n, and they refer to energy fields aka shells
Electrons in the outermost shells have ______ energy than those in the innermost shell.
Higher
Remember: The negatively charged electron is attracted to the positively charged proton. It takes more energy to send it further away from the proton.
What formula is used to predict how many electrons can fit into a given shell/energy level?
2n2
How many sub-levels does each energy level have?
The same number as the principal quantum number. So energy level 1 has 1 sub-level, energy level 2 has 2 sub-levels, etc.
What are the levels of electron configuration from broadest to narrowest?
- Energy level/shell
- Sub-level/sub-shell
- Orbital
How many orbitals is in each sublevel?
s = 1
p = 3
d = 5
f = 7
How many electrons can fit in each sublevel?
s - 2
p - 6
d - 10
f - 14
What is the Pauli Exclusion Principle?
That two electrons occupying the same orbital must have opposite spin
In electron configuration, what do arrows pointing up or down indicate?
Electrons spinning in one or the other direction
In which order are orbitals filled (up to 5d)
1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 4f, 5d
How else are the different energy levels sometimes notated?
1 = K
2 = L
3 = M
4 = N
5 = O
6 = P
7 = Q
What is the Aufbau principle?
The principle that electrons fill lower energy fields before higher energy fields (and therefore determines how we determine electron configuration)
What is Hund’s rule?
Before a second electron can be placed in any orbital, all the orbitals of a sub-level must have at least one electron and all must have the same spin.
Write the electron configuration of Bromine (z = 35) in both notation styles
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p5
[Ar] 4s2 3d10 4p5
From electron configuration notation, how can you figure out how many valence electrons an element has?
These will be the electrons noted separately in noble gas notation.
e.g. Silicon = [Ne]3s23p2 = 4 valence electrons