1. Unit I Electron configuration and periodicity
Lundquist

2. Unit I.1
No note quiz questions, follow along in your packet starting on p. 24

3. Coulomb’s Law The long distance relationship rule
The force of attraction between two objects is proportional to their charges, and inverse to the distance between them
The long distance relationship rule
Coulomb’s Law

4. Review with your table Questions Word Bank
Attraction
Repulsion
Neutral
Positive
Negative
Charge
Distance
Nucleus
Force
Energy
Coulomb’s Law
Describe the nature of interaction between protons and electrons in an atom.
Review with your table

5. Which will require more energy to separate?

6. Which will require more energy to separate?

7. How many e-?

8. How many p+?

9. Which of these e- Will be the easiest (require the least energy) to remove (ionize)? Why?

10. 3 2A 2C
How does that compare with these? Which will be easiest to ionize? Rank them

11. First ionization energy
Remove 1 e- in the gas phase of an element
𝑒𝑛𝑒𝑟𝑔𝑦+ 𝐴 𝑔 → 𝐴 𝑔 𝑒 −
First ionization energy

12. 𝑒𝑛𝑒𝑟𝑔𝑦+ 𝐴 𝑔 → 𝐴 𝑔 𝑒 −
𝐴 𝑔 1+
𝐴 𝑔
Which has less energy?

13. Why is this an endothermic (requires energy) process?
𝑒𝑛𝑒𝑟𝑔𝑦+ 𝐴 𝑔 → 𝐴 𝑔 𝑒 −
𝐴 𝑔 1+
𝐴 𝑔
Why is this an endothermic (requires energy) process?

14. 𝑒𝑛𝑒𝑟𝑔𝑦+ 𝐻 𝑔 → 𝐻 𝑔 𝑒 −
The value of the first ionization energy is 1312 𝑘𝐽 𝑚𝑜𝑙 . on the graph on the next page put a horizontal line to indicate the energy of each specie

15. 𝑒𝑛𝑒𝑟𝑔𝑦+ 𝐻 𝑔 → 𝐻 𝑔 𝑒 −
Why is it negative? What does the difference in the two lines represent?

16. Remember this analogy?
How does your explanation account for the relative charge on H and He the distance of electron(s) from the nucleus?
How would you explain the difference in the 1st ionization energy of H with He?

17. Draw the 1st ionization energy of H and He. PREDICT A VALUE FOR Li

18. 520

20. 496
738
789
1046
1297
1530

24. Review with your table Questions Word Bank
Nucleus
Electron
Distance
energy
Level
Proton
Shell
Arrangement
Attraction
repulsion
Positive
Negative
Charge
location
Describe the electron structure (location of e-) of the atom
Review with your table

25. Electrons in higher energy levels require less energy to remove

26. Shells Layers of electrons around the nucleus Energy levels
Based on distance from the nucleus
Shells

27. Bohr Models Show electrons in their shell
Shows nuclear charge and number of neutrons
Outer most shell is known as the valence shell
Bohr Models

28. Do p. 14 & 15

29. Do All electrons in the same energy level have the same energy??
To answer this we can look at photoelectric spectroscopy data
Do All electrons in the same energy level have the same energy??

30. Photoelectric Spectroscopy Data

31. PES data What does the x-axis symbolize?
What’s the relationship between the 1st ionization energy of H (1312 𝑘𝐽 𝑚𝑜𝑙 ) and the PES data?
PES data

32. He is next How many e- does He have in its first shell?
Predict what the PES would look like if
The same amount of energy was needed to remove an electron
Different amounts of energy were required to remove an electron
He is next He

33. What it actually looks like

34. Li

35. What it actually looks like

41. Lets see them all

43. Unit I.2
Electron Configuration

44. Orbitals & Subshells Subshells Electrons can be ANYWHERE
Probability distribution around the nucleus
Orbitals
Divisions of that distribution based on space and magnetism
Orbitals & Subshells

46. Rules for Electron Configuration
Aufbau Principle
Lower energy levels fill first
Follow the periodic table and you will be fine
Rules for Electron Configuration

47. Write the complete electron configuration for Cl Write the complete electron configuration for I
Practice

48. Noble gas notation Short cut
[previous noble gas] any other subshells & orbitals
Noble gas notation

49. 1. 2. 3. 4.
Note Quiz Questions

50. 6. 5. 7.
Note Quiz Questions

51. Ions The Universe is lazy
Noble gasses have the least energy, thus are inert
Nonmetals will gain e- to be like noble gasses
More e- = more (-)
Metals will loose e- to be like noble gasses
Less e- = more (+)
Ions

52. 8. 9.
Note Quiz Questions

53. Orbital Notation Diagram for showing the spin of an electron
Hund’s Rule
e- won’t double up unless they have to
Pauli’s Exclusion Principle
Two e- cannot spin in the same direction in the same place
Orbital Notation

54. Draw the orbital diagram for Cl Draw the orbital diagram for I
Practice

55. 10.
Note Quiz Questions

56. Do the top of p. 16

57. Magnetism Diamagnetic No unfilled subshells Paramagnetic
At least 1 unfilled subshell
Ferromagnetic
LOTS of unfilled subshells
Found in the middle of the d-block and f-block
Magnetism

58. Do the bottom of p. 16

59. Quiz Next Class Use and interrupt PES data
Write electron configurations
Draw an orbital diagram
Discuss ionization energy
Chem.
Quiz Next Class

60. Unit I.3
Periodic Trends

61. Periodic Trends

62. EXPLAINATIONS Right to left Top to Bottom
Increased effective nuclear charge (Zeff)
Increased principle energy level (number of shells)
EXPLAINATIONS

63. Atomic Radius Which would be smaller??
As nuclear charge increases there is more attraction for the nucleus so atoms get smaller
Atomic Radius

64. As you gain shells you move further from the nucleus
Atomic Radius

65. Atomic Radius Increases from top to bottom
Decreases from left to right

66. First ionization energy
REMEMBER Coulomb’s Law
Smaller elements
Larger elements
First ionization energy

67. First ionization energy
Decreases from top to bottom
Increases from left to right

68. Electronegativity Ability of an atom to attract an electron
Scale from 0-4
Same-ish as electron affinity
Electronegativity

69. Ionic Radius Cations (+) Anions (-) Positive ions Negative ions
Have LESS e-
Same charge in nucleus
Pull e- closer in
Group 1 – 13 (all metals)
Negative ions
Have MORE e-
More repulsion from more e-
Pushes e- further out
Groups 15-18
Ionic Radius

71. Ionic Radius