1. Announcement Homework is due at the beginning of class.
Put it on your desk during the first two minutes.
HW detentions ed at the beginning of class.
You will need a “homework detention rescinding form” signed (after class!) if you didn’t complete your HW by the first two minutes of class.

2. Review
Review subatomic particles, mass number, atomic number, average atomic mass

3. The Periodic Table of the Elements

4. Dmitri Mendeleev (1869)
Organized the elements by atomic mass and other properties
Looked for repeating patterns
When arranged by increasing atomic mass, similarities in chemical properties appeared at regular intervals.
Periodic: things that repeat at regular intervals

5. The Periodic Table is Born
Mendeleev then created a table where elements with similar properties were grouped together: the first periodic table of the elements (1869)

6. The First Periodic Table

7. Atomic mass
Always increasing?
Empty spaces
Predicted they would be filled by elements with certain properties
By 1886 these spaces were filled, by elements with those properties!

8. Another Contribution
Henry Moseley arranged elements by their atomic number, not by atomic mass
Periodic Law: the physical and chemical properties of the elements are periodic functions of their atomic numbers
Periodic functions: repeating patterns
Related to the number and location of electrons

9. Increasing Atomic Number (and, more or less, atomic mass)

10. Periods (across rows)
Groups (down columns)

11. Group Numbers 1 18 2 13 14 15 16 17

12. Elements in the same group have similar chemical and physical properties.

13. Areas of the PTE
Non-metals
Metals

14. A quick tour of the periodic table

15. Metals Solid at room temperature Conduct electricity Shiny
Ductile and malleable: can be made into wires and beaten into sheets

16. Group 1: Alkali Metals Extremely reactive Why?
Don’t exist alone naturally

17. sodium
potassium
cesium (l)
rubidium

18. http://video. google. com/videoplay

19. Group 2: Alkaline Earth Metals
Very reactive

20. Non-Metals Liquids or gases at room temperature
Don’t conduct electricity

21. Group 17: Halogens Very reactive non-metals
Need only one electron to fill valence shell
All exist as diatomic molecules
Cl2, Br2, I2 (all colored)

22. Halogens – colored diatomic molecules
fluorine
pale yellow gas
chlorine
yellow-green gas
bromine
red-brown liquid
iodine
black-purple liquid
purple gas

23. Group 18: Noble Gases Not reactive Gases at room temperature
Stable electron arrangement

24. The Giant Periodic Table Project6 C
12.01

25. The Giant Periodic Table Project
Be neat
Be bold! We need to be able to read this from anywhere in the room!
Be creative, but not cluttered.
Be accurate.
Atomic mass to TWO digits (Ex: 12.01) is ideal.

26. Electron Configuration
The arrangement of electrons in an atom
Each element’s atoms are different
How do we figure out what the electron configuration looks like?

27. So where are the electrons?
Electrons do NOT orbit like planets.

28. Energy Levels Major shells (layers) around the nucleus
lower levels filled before higher levels are filled
1st: 2 electrons
2nd: 8 electrons
3rd: 8 electrons

29. Practice with Simple Electronic StructureHe B Mg Li Be O Ne Cl

30. Electron Apartment Building

31. Electronic Structure Energy levels Sub-levels Orbital
Two electrons per orbital

32. Inside energy levels…
Each energy level has one or more sub-level made from different shaped orbitals.
Energy Level
Number of Sub-levels 1
1 (s) 2
2 (s, p) 3
3 (s, p, d) 4
4 (s, p, d, f)

33. Sub-levels are made up of one or more orbitals

34. What is an orbital?
Orbital: An area where you expect to find the electron.

36. Sub-levels Different shapes s – sphere one orbital p – figure eight
three orbitals
d –
five orbitals
f –
seven orbitals

37. p Sub-level
p sub-level has three orbitals
px, py, pz

38. Energy Level Types of sub-levels Total orbitals 1 4 3 9
Electron capacity
(orbitals x2) 1 s 2
s, p
1+3= 4 8 3
s, p, d
1+3+5= 9 18
s, p, d, f
=16 32

41. How do we figure out where the electrons are?
1. Figure out the energy levels of the orbitals
2. Add electrons to the orbitals according to three rules
Three Rules for Electron Configuration

42. 1: Aufbau Principle
An electron goes to the lowest-energy orbital that can take it.

43. 2: Pauli Exclusion Principle
No two electrons can have exactly the same configuration description
Can have the same orbital, but must have opposite spins.

44. 3. Hund’s Rule
Orbitals of equal energy are each occupied by one electron before any orbital is occupied by a second electron
All electrons that are by themselves in an orbit must have the same spin.

46. Energies of sub-levels

50. Multiple choice practice

51. Who arranged the periodic table by atomic number?
Dmitri Mendeleev
Henry Mosley
Ernest Rutherford
Democritus

52. Which property is not increasing from left to right on the periodic table?
Atomic mass
Atomic number
Number of electrons
Reactivity

53. Which is not a property of the metals?
Shiny
Gas at room temperature
Conduct electricity
Solid at room temperature

54. Which is a property of non-metals?
Conduct electricity
Gas or liquid at room temperature
To the left of the staircase line
Malleable and Ductile

55. Which is not a property of the alkali metals?
Solid at room temperature
Not reactive
Extremely reactive
Never exist alone in nature

56. Which accurately describes the maximum number of electrons in each energy level?
2, 8, 8
8, 8, 8
2, 2, 8
8, 2, 2

57. Which lists the sublevels in the correct order?
d, p, s, f
s, p, f, d
p, s, f, d
s, p, d, f

58. What is the name of the following orbital shape?d f

59. How many electrons can fit in the s sub-level/orbital?1 2 3
Eight million

60. How many electrons can fit in any single orbital?1 2 3
Eight million

61. How many electrons total can fit in the p sub-level?2 4 6 14

62. How many d orbitals make up the d sub-level?2 3 5 7

63. How many f orbitals make up the entire f sub-level?2 3 5 7

64. How many electrons total can fit in the entire d sub-level?2 6 10 14

65. Which rule states that the lower energy levels are filled before the higher ones?
Aufbau Principle
Pauli Exclusion Principle
Hund’s Rule

66. Which rule states that electrons are alone unless there is no space left, and then they can be with another electron?
Aufbau Principle
Pauli Exclusion Principle
Hund’s Rule

67. Which rule states that no two electrons can have the same configuration (that is, be in the same space at the same time)?
Aufbau Principle
Pauli Exclusion Principle
Hund’s Rule

68. Take these notes on Orbital Notation paper

69. What do the orbitals/sub-levels "look like" when you put them all together?

70. 1: Aufbau Principle
An electron goes to the lowest-energy orbital that can take it.

71. 2: Pauli Exclusion Principle
No two electrons can have exactly the same configuration description
Can have the same orbital, but must have opposite spins.

72. 3. Hund’s Rule
Orbitals of equal energy are each occupied by one electron before any orbital is occupied by a second electron
All electrons that are by themselves in an orbit must have the same spin.

75. How do we write electron configurations?
Orbital Notation
Electron Configuration Notation
Noble Gas Notation (shorthand)
All ways to communicate where the electrons are in any atom.

76. s – sphere
one orbital – 2 electrons
p – figure eight
three orbitals – 6 electrons
d –
five orbitals – 10 electrons
f –
seven orbitals – 14 electrons

77. Orbital Notation Electron configuration goes below a line or box
Arrows representing electrons go on the lines or in the boxes
1s 2s p s p s

78. Be, Si, Ne, Cl

79. Write the orbital notation Homework notebook!Ne Na S Zn I

80. Electron Configuration Notation
Main energy level Sub-levelElectrons
Carbon (6 electrons) 1s22s22p2
Aluminum (13 electrons)
1s22s22p63s23p1
Oxygen
Argon
Copper
Zirconium

81. Noble Gas Notation (Shorthand)
Noble gasses have totally filled outer orbitals.
If Ne (a noble gas) is 1s22s22p6, we can abbreviate Na (Sodium) as [Ne]3s1.
Sodium has one more electron than Neon, so its Noble Gas Notation is Neon plus one electron in the s sublevel of the third energy level.

82. Practice Fe (Iron) Electron Configuration Notation Noble Gas Notation
K (Potassium)
Li (Lithium)
Be (Beryllium)

83. Orbital Notation Boron 1s22s22p1 Atomic Number? How many electrons?

84. Aufbau Principle: start with 1s and work up in energy level
Pauli Exclusion Principle: No two elements can have the same arrangement of electrons
Hund’s Rule: Fill in one electron per orbital first, then go back.

85. s, p, d and f blocks of the periodic table

86. “Long form” periodic table
groups
periods

87. Electronic structures are related to the position of the elements on the periodic table
s-block: s orbitals are filled
p-block: p orbitals are filled
etc.