Atomic orbitals and electronic config

Question 1

What are the different shapes of orbitals?

Answer 1

s,p,d and f

Question 2

Name all of the quantum numbers, giving their letters

Answer 2

principal quantum number, n
angular momentum quantum number, l
magnetic quantum number, ml
spin magnetic quantum number, ms

Question 3

principal quantum number n indicates

Answer 3

the main energy level for an electron and is related to the size of the orbital

Question 4

the angular momentum number l determines

Answer 4

the shape of the subshell and can have values from 0 to n-1

Question 5

The magnetic number ml determines

Answer 5

the orientation of the orbital and can have values between -l and +l

Question 6

The spin magnetic quantum number ms determines

Answer 6

the direction of spin and can have values of -1/2 or +1/2

Question 7

What is the Aufbau principle?

Answer 7

electrons fill up orbitals in order of increasing energy

Question 8

What is Hund’s rule?

Answer 8

when degenerate orbitals are available, electrons fill each singly, keeping their spins parallel before spin pairing starts

Question 9

What is the Pauli exclusion principle?

Answer 9

No two electrons in an atom can have the same set of 4 quantum numbers, therefore, no orbital can hold more than 2 electrons and these 2 electrons must have opposite spin

Question 10

There is a special stability associated with

Answer 10

half-filled and full subshells

Question 11

Electron pair repulsions decrease in strength in the order:

Answer 11

non bonding pair/non bonding pair >non bonding pair/bonding pair>bonding pair/bonding pair