Unit One, Chapter Two - Shapes Of Atomic Orbitals And Quantum Numbers Flashcards
How to find quantum number Ms?
Either +1/2 or -1/2 (no two electrons occupying the same orbital can have the same spin)
How to find quantum number Ml?
Range of values between positive and negative forms of I (e.g. L-2 , Ml = - 2, - 1, 0,+1,+2)
How to find quantum number l?
s-orbital = 0
p-orbital= 1
d-orbital = 2
f-orbital = 3
How to find quantum number n?
Number of shells
Which shells have d-orbitals?
All except for first and second
Which shells have p-orbitals?
All except the first
Which shells have an s-orbital?
All shells
In what order do the orbitals fill with elections?
s → p → d
The diameter of s-orbitals…
… Increases as the shell number increases
What are orbitals?
regions where there is a high probability of finding an electron
What does a d-orbital look like?
Four tear drop shapes in a cross (+)
What does a p-orbital look like?
Two tear drop shapes opposite each other (symmetricaI)
What does an s-orbital look like?
A sphere
What are the four types of orbitals?
s, p, d, and f
How many elections can one orbital hold?
Two (max)
What is a standing wave?
Waves that vibrate in time but do not move in space
In an isolated atom…
… The orbitals within each shell are said to be degenerate
What is Ms?
Spin magnetic quantum number (opposite to Ml for paired electrons)
What is Ml?
Magnetic quantum number (representing orientation)
What is l?
Angular momentum quantum number (representing shape)
What is n?
Principal quantum number (representing energy)
