Answer:
a) Magnetic Quantum Number
b) Principal Quantum Number
c) Electron Spin Quantum Number
d) Orbital Angular Momentum Quantum Number
Explanations:
Quantum numbers are the number used to describe the energy levels available to atoms or molecules.
There are four types of quantum numbers in chemistry namely;
• Principal Quantum number (n)
,
• Angular momentum Quantum number(ℓ)
• Magnetic moment (mℓ) and;
,
• Electron spin quantum number (ms).
a) The orientation of the orbital space is classified under the Magnetic Quantum Number. This quantum number determines the number of orbitals and their orientation within a subshell. Its value also depends on the orbital angular momentum quantum number (l)
b) The size of the orbital is classified under the Principal Quantum number. This quantum number designates the principal electronic shells with a minimum ground state of n = 1. The state n = 1 designates the first principal shell (the innermost shell). Note that n cannot be equal to zero because there is no atom with zero or a negative amount of energy levels/principal shells. n = 2 connotes the second principal shell and so on.
c) The magnetic moment is classified under the Electron Spin Quantum Number. This quantum number does not depend on another quantum number.
This quantum number connotes the direction of the electron spin. It may have a spin of +1/2, represented by an arrow pointing upwards ↑(spin-up), or –1/2, represented by a downward arrow ↓ (spin down).
d) The shape of the orbital is classified under the Orbital Angular Momentum Quantum Number. This quantum number determines the shape of an orbital and the angular distribution. The angular node is known to be equal to the angular momentum quantum number (l).
Each value of "l" indicates a specific s, p, d, f subshell and is dependent on the principal quantum number "n". The value of "l" can be equal to zero and a positive integer compared to the principal quantum number "n" that cannot be equal to zero