Atomic orbitals, electronic configurations and the periodic table

Question 1

Principal quantum number, symbol n, determines what?

Answer 1

the main energy level and it can have values n = 1, 2, 3, 4, etc. The numbers determine the size and energy of the shell.

Question 2

Angular momentum quantum number, symbol ℓ, determines what?

Answer 2

the shape of the sub-shell and is labelled as s, p, d, f. This can have values from zero to ( n -1).
value 0 labelled as ‘s’ subshell;
value 1 labelled as ‘p’ subshell;
value 2 labelled as ‘d’ subshell;
value 3 labelled as ‘f’ subshell.

Question 3

Magnetic quantum number (also known as magnetic quantum number), symbol mℓ, relates to what?

Answer 3

the orientation in space of the orbital eg if ℓ = 2 (labelled as a ‘d’ orbital)
mℓ could have the value +2, +1, 0, -1, -2

Question 4

Spin magnetic quantum number: determines what?

Answer 4

the direction of spin. It is therefore called the spin quantum number, ms. It has values of +12 or −12

Question 5

the aufbau principle

Answer 5

electrons fill orbitals in order of increasing energy

Question 6

Hund’s rule

Answer 6

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

Question 7

Pauli exclusion principle

Answer 7

no two electrons in one atom can have the same set of
four quantum numbers, therefore, no orbital can hold more than two electrons and
these two electrons must have opposite spins

Question 8

what is a dative covalent bond?

Answer 8

atoms can provide pair of non bonding electrons that form the covalent bond