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Section 11.4 Electron Configurations and Atomic Properties 1.To understand how the principal energy...

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Section 11.4 Electron Configurations and Atomic Properties 1. To understand how the principal energy levels fill with electrons in atoms beyond hydrogen 2. To learn about valence electrons and core electrons 3. To learn about the electron configurations of atoms 4. To understand the general trends in properties in the periodic table Objectives
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Page 1: Section 11.4 Electron Configurations and Atomic Properties 1.To understand how the principal energy levels fill with electrons in atoms beyond hydrogen.

Section 11.4

Electron Configurations and Atomic Properties

1. To understand how the principal energy levels fill with electrons in atoms beyond hydrogen

2. To learn about valence electrons and core electrons

3. To learn about the electron configurations of atoms

4. To understand the general trends in properties in the periodic table

Objectives

Page 2: Section 11.4 Electron Configurations and Atomic Properties 1.To understand how the principal energy levels fill with electrons in atoms beyond hydrogen.

Section 11.4

Electron Configurations and Atomic Properties

A. Electron Arrangements in the First 18 Atoms on the Periodic Table

• H atom – Electron configuration – electron arrangement – 1s1 – Orbital diagram – orbital is represented as a box with a

designation according to its sublevel. Contains arrow(s) to represent electrons (spin)

Page 3: Section 11.4 Electron Configurations and Atomic Properties 1.To understand how the principal energy levels fill with electrons in atoms beyond hydrogen.

Section 11.4

Electron Configurations and Atomic Properties

A. Electron Arrangements in the First 18 Atoms on the Periodic Table

• He atom – Electron configuration – 1s2 – Orbital diagram

Page 4: Section 11.4 Electron Configurations and Atomic Properties 1.To understand how the principal energy levels fill with electrons in atoms beyond hydrogen.

Section 11.4

Electron Configurations and Atomic Properties

A. Electron Arrangements in the First 18 Atoms on the Periodic Table

• Li atom – Electron configuration– 1s2 2s1 – Orbital diagram

Write the electron configuration and orbital diagrams for Boron, Nitrogen, Fluorine and Argon

Page 5: Section 11.4 Electron Configurations and Atomic Properties 1.To understand how the principal energy levels fill with electrons in atoms beyond hydrogen.

Section 11.4

Electron Configurations and Atomic Properties

A. Electron Arrangements in the First 18 Atoms on the Periodic Table

Write the full electron configuration of Neon and Sulfur

Draw an orbital diagram for Magnesium and Chlorine

Page 6: Section 11.4 Electron Configurations and Atomic Properties 1.To understand how the principal energy levels fill with electrons in atoms beyond hydrogen.

Section 11.4

Electron Configurations and Atomic Properties

A. Electron Arrangements in the First 18 Atoms on the Periodic Table

Classifying Electrons

• Valence electrons – electrons in the outermost (highest) principal energy level of an atom

• Core electrons – inner electrons • Elements with the same valence electron arrangement

(same group) show very similar chemical behavior.

Page 7: Section 11.4 Electron Configurations and Atomic Properties 1.To understand how the principal energy levels fill with electrons in atoms beyond hydrogen.

Section 11.4

Electron Configurations and Atomic Properties

• Electron configurations for K through Kr

B. Electron Configurations and the Periodic Table

Page 8: Section 11.4 Electron Configurations and Atomic Properties 1.To understand how the principal energy levels fill with electrons in atoms beyond hydrogen.

Section 11.4

Electron Configurations and Atomic Properties

Using a Noble Gas Shorthand

• We can abbreviate electron configurations by using the configuration of the previous noble gas to cover the first part of the list of orbitals

• Mg is 1s2 2s2 2p6 3s2 or [Ne] 3s2

• The noble gas portion is the equivalent to the group of core electrons

• Use the Noble Gas shorthand to show the electron configurations of Carbon and Zirconium

Page 9: Section 11.4 Electron Configurations and Atomic Properties 1.To understand how the principal energy levels fill with electrons in atoms beyond hydrogen.

Section 11.4

Electron Configurations and Atomic Properties

Order of Filling of Orbitals

Atoms fill their orbitals in the order of their energies:

Page 10: Section 11.4 Electron Configurations and Atomic Properties 1.To understand how the principal energy levels fill with electrons in atoms beyond hydrogen.

Section 11.4

Electron Configurations and Atomic Properties

• Orbital filling and the periodic table

B. Electron Configurations and the Periodic Table

Page 11: Section 11.4 Electron Configurations and Atomic Properties 1.To understand how the principal energy levels fill with electrons in atoms beyond hydrogen.

Section 11.4

Electron Configurations and Atomic Properties

B. Electron Configurations and the Periodic Table

Page 12: Section 11.4 Electron Configurations and Atomic Properties 1.To understand how the principal energy levels fill with electrons in atoms beyond hydrogen.

Section 11.4

Electron Configurations and Atomic Properties

C. Atomic Properties and the Periodic Table

Metals and Nonmetals • Metals tend to lose electrons to form positive ions. • Nonmetals tend to gain electrons to form negative ions.

Page 13: Section 11.4 Electron Configurations and Atomic Properties 1.To understand how the principal energy levels fill with electrons in atoms beyond hydrogen.

Section 11.4

Electron Configurations and Atomic Properties

C. Atomic Properties and the Periodic Table

Atomic Size

• Size tends to increase down a column. • Size tends to decrease across a row.

(close to scale)

Page 14: Section 11.4 Electron Configurations and Atomic Properties 1.To understand how the principal energy levels fill with electrons in atoms beyond hydrogen.

Section 11.4

Electron Configurations and Atomic Properties

C. Atomic Properties and the Periodic Table

Ionization Energies• Ionization Energy – energy (ΔH) required to remove an

electron from an individual atom (gas)

– Tends to decrease down a column – Tends to increase across a row – Changes in an opposite direction to atomic size

Page 15: Section 11.4 Electron Configurations and Atomic Properties 1.To understand how the principal energy levels fill with electrons in atoms beyond hydrogen.

Section 11.4

Electron Configurations and Atomic Properties

Ionization Energies

Page 16: Section 11.4 Electron Configurations and Atomic Properties 1.To understand how the principal energy levels fill with electrons in atoms beyond hydrogen.

Section 11.4

Electron Configurations and Atomic Properties

Electron Affinity

• Electron Affinity is defined as ΔH for the process:

X(g) + e- = X(g)-

   ΔH = Electron Affinity

Page 17: Section 11.4 Electron Configurations and Atomic Properties 1.To understand how the principal energy levels fill with electrons in atoms beyond hydrogen.

Section 11.4

Electron Configurations and Atomic Properties

Electronegativity

• Ionization Energy and Electron Affinity are combined to give Electronegativity – a measure of how well atoms compete for electrons in a bond


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