Chapter 5 Flashcards
Order the following: shells, subshells and orbital services
Shells made of subshells
Subshells made of orbitals
How many electrons per orbital
2 paired electrons
How many orbitals in s subshell
1
How many orbitals in p subshell
3
How many orbitals in d subshell
5
Subshells in shell 1
Only s
Subshells in shell 2
S and p
Subshells in shell 3
S,p and d
Subshells in shell 4
S,p,d and f
Number of electrons per shell number
2,8,18,32
What does this mean:
3P subscript 6
Shell number 3
Orbital p
6 electrons in those orbitals
Shape of s orbital?
S orbital shape of higher shells?
Sphere
Higher shells are larger in volume but same shape
Why do higher shell orbitals have higher volume
Higher shell electrons have more energy so on average they are further away from the nucleus
What do the orbitals actually represent?
What are the chances of finding an electron in the orbital?
The area around a nucleus where there is a high chance of finding an electron
but they move randomly and we have no idea of the electron’s direction or speed so theoretically they can be anywhere in the universe
95%
Shape of p orbital
Two lobes of same size which align with axes that they are named for. 3 orbitals in x y and z axis so perpendicular to each other. All three are equal energy
Dumbell shape
Shape of d orbital
4 lobes and one very strange shape all with equal energy
Why do two electrons in same orbital have opposite spin
Same charge so repel
What is an electron cloud
An orbital where an electron can potentially be found
How would you arrange 4 electrons in a p orbital
2 paired electron in first square
And 1 each in the other two squares
How do you remember order of energy
1s
2s 2p
3s 3p 3d
4s 4p 4d 4f
Diagonally down
Why does copper and chromium only have 1 electron in 4s orbital?
Stability because having full orbitals or half full sets of orbitals is more stable and favourable energetically
1s2 2s2 2p6 3s2 3p6 4s2 3d2
This atom becomes an ion and loses 2 electron
What is its config or from which orbital is the electron lost
4s2 orbital loses both electrons because of first in first out rule
When filling 4s is lower in energy so filled first but once filled it becomes higher energy so it is lost before 3d
3/4 rules of electron config in the orbitals
Fill electron with lowest energy level first
Only 2 electron in an orbital with opposite spins
Each orbital has 1 electron before 2nd is introduced or paired
What is shorthand rule
Any example?
Using previous noble gas and then add in outer electron subshells as normal
Na = Ne in square brackets then 3s1
