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Understanding Electron Configuration and Orbital Diagrams in Atomic Structure, Lecture notes of Chemistry

An explanation of electron configuration in the Quantum Mechanical Model of the Atom, using relatable analogies and diagrams. It covers the concept of energy levels, sublevels, orbitals, and the rules governing their occupation by electrons. The document also includes exercises for drawing orbital diagrams for specific elements.

What you will learn

  • How do you draw orbital diagrams for specific elements?
  • What is the difference between the Bohr model and the Quantum Mechanical Model of the Atom?
  • What are the rules governing the occupation of orbitals by electrons?
  • How do energy levels, sublevels, and orbitals relate to each other in atomic structure?
  • What determines how elements bond and react with other elements?

Typology: Lecture notes

2021/2022

Uploaded on 09/12/2022

ekanga
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Electron Configuration
Arrangements in the Quantum
Mechanical Model
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pfa
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Electron Configuration

Arrangements in the Quantum

Mechanical Model

Electrons are important because they

determine how elements will bond and react

with other elements.

Bohr versus the REAL

THING:

Electron Configuration

Tells us the probable location of an

element’s electrons.

If YOU were an electron….

  • Atom = school
  • Energy Levels = hallways
  • Sub levels = classrooms
  • Orbitals = desks
  • Electrons = students

Energy Levels

give the general distance from the nucleus

E N E R G Y

1s

2s

3s

4s

1s

5s

6s

7s

2 p

3 p

4 p

5 p

6 p

7 p

3 d

4 d

5 d

6 d

4f

5f

Color YOUR Periodic Table!

Electron Configuration

1s

Energy Level –

Principal Quantum #

(possibilities are 1-7)

Sublevel

(s, p, d, or f)

of electrons

s: 1 or 2

p: 1-

d: 1-

f: 1-

If you add up all of the electrons, it should equal the atomic #

of the element

3 Main Rules of Orbital Diagrams

1) Aufbau Principle –

Electrons fill orbitals of the lowest energy

first.

The location of the
electron with the
highest energy will
help you identify
the element

Example:

1s

2

2s

2

2p

6

3s

2

3p

6

4s

2

3d

6

Highest energy electron

Element = Iron

3 Main Rules of Orbital Diagrams

2) Hund’s Rule –

Each orbital must have 1 e

before any can

have 2 e

2p

3 Main Rules of Orbital Diagrams

2) Hund’s Rule –

Each orbital must have 1 e

before any can

have 2 e

3) Pauli Exclusion Principle –

Only 2 e

can be found in each orbital, and

they must be spinning opposite directions.

Now write the electron

configuration:

  • Fe
  • O
  • Pb

1s

2

2s

2

2p

6

3s

2

3p

6

4s

2

3d

6

1s

2

2s

2

2p

6

3s

2

3p

6

4s

2

3d

10

4p

6

5s

2

4d

10

5p

6

6s

2

4f

14

5d

10

6p

2

1s

2

2s

2

2p

4

Lewis Dot Structures – show only

the valence electrons.

  • Valence Electrons – outershell electrons
  • You can count valence electrons by looking

at the group #.

Lewis Dot Structures – show only

the valence electrons.

  • Valence Electrons – outershell electrons
  • You can count valence electrons by looking

at the group #.

Remember Hund’s Rule when drawing Lewis

Dots BUT draw all “s” electrons (the first 2)

together on the right.

Lewis Dot Structures

Carbon:

C

4 valence e

-

= 4 dots