4 - Quantum Numbers

Proverbs 16:3

Quantum numbers

______ cover the part of quantum mechanics that talks about energy and location of electrons

Orbital

[QUANTUM NUMBER]

An _____ is a space that accommodates 2 electrons.

2 electrons

[QUANTUM NUMBER]

An ORBITAL is a space that accommodates _____ electrons

Spin

[QUANTUM NUMBER]

An ORBITAL is a space that accommodates 2 electrons and these are held by what we called _____

Node

[QUANTUM NUMBERS]

A _____ is a section of the orbital that cannot hold electrons.

Subshell/ sublevel

[QUANTUM NUMBERS]

Multiple orbitals can be grouped in a __________, and multiple subshells constitute a whole energy shell /level

Energy shell /level

[QUANTUM NUMBERS]

Multiple orbitals can be grouped in a subshell/ sublevel and Multiple subshells constitute a whole________

Subshell / Sublevel

[QUANTUM NUMBERS]

Energy shell have a smaller portion known as ______.

1-7 orbitals

[QUANTUM NUMBERS]

Subshell / Sublevel can have as much as ____ orbitals

Subshell / Sublevel

[QUANTUM NUMBERS]

Multiple orbitals can be grouped in a ______.

Energy shell / Energy level

[QUANTUM NUMBERS]
Multiple subshells constitute a whole _____

Type (symbol)	Represents	Numbers
Principal (n)	Energy level/shell	1, 2, 3, 4, and so on
Azimuthal / Angular (l)	1) Shape of orbital 2) Sublevel/subshell	0, 1, 2, 3
Magnetic (ml)	Orientation of an orbital	s = 0 only p = -1, 0, +1 d = -2, -1, 0, +1, +2 and so on
Spin (ms)	Spin of an electron inside an orbital	+1/2 (up arrow) -1/2 (down arrow)

Type of Quantum Numbers [4]

Part of a Quantum Number

Principal Quantum Number (n)

[QUANTUM NUMBERS]

Energy level / Energy shell of an orbital

Azimuthal / Angular Quantum Number (I)

[QUANTUM NUMBERS]

• Shape of orbital

• Sublevel/ Subshell

Magnetic Quantum Number (m_l)

[QUANTUM NUMBERS]

Orientation of an orbital

Spin Quantum Number (m_s)

[QUANTUM NUMBERS]

Spin of an elecron inside an orbital

Azimuthal / Angular Quantum Number (l)

[QUANTUM NUMBERS]

__________ represents both the number and shape of orbitals per sublevel/subshell

ℓ (Azimuthal Quantum Number)	Orbital Type (Subshell)	Number of Orbitals	Shape of Orbitals	Maximum Number of Electrons
0	s	1	Sphere	2
1	p	3	Dumbbell	6
2	d	5	Four-leaf clover	10
3	f	7	Complex	14

[QUANTUM NUMBERS]
Table 6. Azimuthal Quantum Number Interpretations

Degenerate

[QUANTUM NUMBERS]

Starting from the p-subshell , multiple orbitals of the same subshell have the same energies and are called _____.

• Aufbau Principle (Madelung Rule)

• Hund’s Rule (Maximum Multiplicity Rule)

[QUANTUM NUMBERS]

There are principles concerned mainly with the principal and azimuthal number such as ____ [2]

Madelung rule

[QUANTUM NUMBERS]

Aufbau principle is also known as ____

Maximum Multiplicity Rule

[QUANTUM NUMBERS]

Hund’s rule is also known as _____

Aufbau principle (Madelung Rule)

[QUANTUM NUMBERS]
In an atom with multiple energy levels and/or sublevels, the electrons are filled up from 1st onward in a predictable fashion by order of increasing energy

a. Aufbau principle

b. Hund’s rule

c. Pauli exclusion principle

Hund’s rule (Maximum Multiplicity Rule)

[QUANTUM NUMBERS]

Electrons fill up degenerate orbitals singly first (+1/2) before pairing up

a. Aufbau principle

b. Hund’s rule

c. Pauli exclusion principle

Pauli exclusion principle

[QUANTUM NUMBERS]

Once the magnetic and spin quantum numbers are considered, the ______ enters, which states that every electron in an atom is unique

a. Aufbau principle

b. Hund’s rule

c. Pauli exclusion principle

Pauli exclusion principle

Example:

[QUANTUM NUMBERS]

No two electrons have the same set of four quantum numbers.Because they are all unique (or “exclusive)

a. Aufbau principle

b. Hund’s rule

c. Pauli exclusion principle

Electronic configuration

[QUANTUM NUMBERS]
Assume that every electron in an atom is placed in a specific orbital in a specific shell. When all of them are considered, an atom’s ______ can now be written.

Electronic configuration:

TRUE

[QUANTUM NUMBERS]

TRUE OR FALSE:

Electron Configuration is usually written in the complete form, but if the element is large, it’s fine to use the abbreviated form

Example:

Complete Form (Strontium) = 1s² 2s² 2p⁶ 3s² 3p⁶ 3d¹⁰ 4s² 4p⁶ 5s²

Abbreviated Form (Strontium) = [Kr] 5s²

(Context: Kr = 1s² 2s² 2p⁶ 3s² 3p⁶ 3d¹⁰ 4s² 4p⁶)

[QUANTUM NUMBERS]

Example of Electron Configuration of Sulfur:

Valence

[QUANTUM NUMBERS]

Outermost (applies to shells, subshells, or electrons)

Core

[QUANTUM NUMBERS]

Inner electrons (anything except the valence)

Octet Rule

[QUANTUM NUMBERS]

According to ______ rule

• For smaller atoms, valence electrons of s and p block elements must be eight (8; octa-) to be stable

TRUE

[QUANTUM NUMBERS]

TRUE OR FALSE:

• The smaller atoms refer to most non metals in organic compounds , since s and p orbitals are all they have.

TRUE

[QUANTUM NUMBERS]

TRUE OR FALSE:

• The larger atoms with d orbitals can attains stability without needing to follow the octet rule.