1. Electron Configurations and Periodic Trends

3. Review What information can we get from the Periodic Table?
How can we classify elements on the Periodic Table?
What model of the atom do we use today? What does an atom look like?

4. Electron Configurations
The ways in which electrons are arranged in various orbitals around the nuclei of atoms are called electron configurations.
These will tell you where we can expect to find electrons based upon their energy.
Lowest energy = closer to the nucleus
Higher energy = further away

5. Orbitals
Each energy sublevel corresponds to an orbital of a different shape, which describes where the electron is likely to be found.
s, p, d, and f orbitals

6. S orbitals

7. P orbitals

8. S with p orbitals

9. d orbitals

10. f orbitals

11. Review

12. Electron Configurations
3 rules to finding Electron Configurations 1. Aufbau Principle: electrons occupy the orbitals of lowest energy first. 2. Pauli Exclusion Principle: only two electrons per atomic orbital. 3. Hund’s rule: electrons occupy orbitals of the same energy in a way to maximize the total spin.

13. Practice
Carbon Argon Nickel Silicon Sulfur Selenium

15. Independent Practice

16. What trends do you see with the electron configurations?
Now, I’ll teach you a short cut based on these trends.

17. Periodic Trends Atomic size Size of its ion Ionization energy
Electronegativity

18. Atomic Size
Measured as half the distance between two nuclei of the same atom when they are joined.
In general, the size increases from top to bottom within a group and decreases left to right across a period.

19. Practice with Atomic size
Give the larger of the two atoms
Carbon or Nitrogen?
Phosphorus or Arsenic?
2. Put the following elements in order of increasing atomic size: potassium, calcium, sodium and magnesium

20. Ionic size trends? Same as atomic size
Which ion would be larger: sodium or magnesium? Sulfur or selenium?
Put the following ions in order of decreasing size: sodium, magnesium, sulfur and selenium.

21. Trends in Ionization Energy
Remember: electrons can move to higher energy levels
Sometimes, enough energy is gained to remove the electron completely (ionization energy).
Tends to decrease from top to bottom within a group and increase from left to right across a period.

24. Trends in Electronegativity
Ability to attract electrons
In general, electronegativity decreases from top to bottom and increase across a period left to right. (same as ionization energy)

25. Practice
Which would have more affinity to attract electrons: Fluorine or chlorine? Which atom would lose an electron easier: lithium or sodium?

26. Open Note Check Quiz
How does atomic size change within groups and across periods?
When do ions form?
How does electronegativity vary on the periodic table?
Arrange these elements in order of decreasing atomic size: sulfur, chlorine, aluminum, and sodium.
Which element in each pair has the larger first ionization energy?
Sodium, potassium
Magnesium, phosphorus

27. Independent Practice Electron configurations and Periodic Trends
Finish notes with questions and a summary
Update glossary with all key terms thus far!
Key Terms: anion, cation, ion, electronegativity, ionization energy, electron configuration, atom, atomic number, electron, proton, neutron, isotopes, group, period, nucleus