Transcript Section 11.4 Electron Configurations and

Section 11.4
Electron Configurations and Atomic Properties
Objectives
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
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)
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
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
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
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.
Section 11.4
Electron Configurations and Atomic Properties
B. Electron Configurations and the Periodic Table
• Electron configurations for K through Kr
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
Section 11.4
Electron Configurations and Atomic Properties
Order of Filling of Orbitals
Atoms fill their orbitals in
the order of their energies:
Section 11.4
Electron Configurations and Atomic Properties
B. Electron Configurations and the Periodic Table
• Orbital filling and the periodic table
Section 11.4
Electron Configurations and Atomic Properties
B. Electron Configurations and the Periodic Table
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.
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)
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
Section 11.4
Electron Configurations and Atomic Properties
Ionization Energies
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
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