1. 1.1 Atoms, Elements and the Periodic Table

2. The Periodic Table and the Elements
What is the periodic table ?
What information is obtained from the table ?
How can elemental properties be predicted base on the PT ?

3. Dmitri Mendeleev (1869)
In 1869 Mendeleev and Lothar Meyer (Germany) published nearly identical classification schemes for elements known to date. The periodic table is base on the similarity of properties and reactivities exhibited by certain elements. Later, Henri Moseley ( England, ) established that each elements has a unique atomic number, which is how the current periodic table is organized.

4. The periodic table is the most important tool in the chemist’s toolbox!

5. The Periodic Table A map of the building block of matter.

6. Periodic Table Expanded View
The way the periodic table usually seen is a compress view, placing the Lanthanides and actinides at the bottom of the stable.

7. The Periodic Law
Periodic Law- States that chemical and physical properties of the elements repeat in regular, periodic patterns when they are arranged according to their atomic number. Periodic Trends – Repeating patterns that arise by organizing elements according to their atomic number

8. Lewis Diagrams
Lewis Diagrams- are models of the atom showing the chemical symbol and only the valence electrons for that element.
Bohr-Rutherford Diagram
Lewis Dot Diagram

9. Valence Electrons- Octet Rule- RULE:
∙ ∙ ∙ ∙ ∙∙ ∙∙ ∙∙ ∙∙
Li Be∙ B∙ ∙C∙ ∙N∙ ∙O: ∙F: :Ne:
∙ ∙ ∙ ∙∙ ∙∙ ∙∙
RULE:
Electrons are added one at a time starting at 12 o’clock then 3, 6, 9 o’clock. Electrons do not pair until the 5th electron which is back to 12 o’clock.
Valence Electrons-
electrons in the valence shell (outer most shell)
Octet Rule-
when the maximum number of 8 electrons is achieved in their valence shell.

10. Periodic Table: Metallic arrangement
Layout of the Periodic Table: Metals vs. nonmetals
Nonmetals
Metals

11. Periodic Table: electron behavior
The periodic table can be classified by the behavior of their electrons

12. Reading the Periodic Table: Classification
Nonmetals, Metals, Metalloids, Noble gases

13. Across the Periodic Table
Periods/Rows: Are arranged horizontally across the periodic table (rows 1-7)
These elements have the same number of valence shells.
2nd Period
6th Period

14. Down the Periodic Table
Groups/Family: Are arranged vertically down the periodic table (columns or group, or 1-8 A,B)
These elements have the same number of electrons in the outer most shells, the valence shell.
Alkali Family:
1 e- in the valence shell
Halogen Family:
7 e- in the valence shell

15. Infamous Families of the Periodic Table
Notable families of the Periodic Table and some important members:
Alkali
Alkaline (earth)
Transition Metals
Noble Gas
Halogen

16. Important members - the Elements
Individual members of selected Elements & their characteristics H He Li Na K Ca Mg Fe I Cl F P S Si O N C Al Zn Cu Ag Br

17. Summary Periodic Table: Map of the Building block of matter
Type: Metal, metalloid and Nonmetal
Groupings: Representative or main, transition and Lanthanide/Actanides
Family: Elements in the same column have similar chemical property because of similar valence electrons
Alkali, Alkaline, chalcogens, halogens, noble gases
Period: Elements in the same row have valence electrons in the same shell.

18. Periodic Table e- configuration from the periodic periodic table The Periodic Table can be arrange by subshells. The s-block is Group IA and & IIA, the p-block is Group IIIA - VIIIA. The d-block is the transition metals, and the f-block are the Lanthanides and Actinide metals H
1s1 He
1s2 Li
2s1 Be
2s2 B
2p1 C
2p2 B
2p1 N
2p3 O
2p4 F
2p5 Ne
2p6 Na
3s1 Mg
3s2 Al
3p1 Si
3p2 P
3p3 S
3p4 Cl
3p5 Ar
3p6 K
4s1 Ca
4s2 Sc
3d1 Ti
3d2 V
3d3 Cr
4s13d5 Mn
3d5 Fe
3d6 Co
3d7 Ni
3d8 Cu
4s13d10 Zn
3d10 Ga
4p1 Ge
4p2 As
4p3 Se
4p4 Be
4p5 Kr
4p6 Rb
5s1 Sr
5s2 Y
4d1 Zr
4d2 Nb
4d3 Mo
5s14d5 Tc
4d5 Ru
4d6 Rh
4d7 Ni
4d8 Ag
5s14d10 Cd
4d10 In
5p1 Sn
5p2 Sb
5p3 Te
5p4 I
5p5 Xe
5p6 Cs
6s1 Ba
6s2 La
5d1 Hf
5d2 Ta
5d3 W
6s15d5 Re
5d5 Os
5d6 Ir
5d7 Ni
5d8 Au
6s15d10 Hg
5d10 Tl
6p1 Pb
6p2 Bi
6p3 Po
6p4 At
6p5 Rn
6p6 Fr
7s1 Ra
7s2 Ac
6d1 Rf
6d2 Db
6d3 Sg
7s16d5 Bh
6d5 Hs
6d6 Mt
6d7

19. The Number of Electrons in Each Energy Level:
Max # of electrons 1
1s2 = 2 2
2s22p6 =8 3
3s23p63d10 =18 4
4s24p64d104f14=32

20. Atomic Orbitals

21. electrons occupy lowest energy levels available
Basic Principle:
electrons occupy lowest energy levels available

22. Aufbau Principle -- “Bottom Up Rule”22

23. Pauli exclusion principle
An orbital can contain a maximum of 2 electrons,
and they must have the opposite “spin.”
Hund’s Rule
You must fill all subshells of an orbital
before doubling up arrows.
Example:
Determine the electron configuration and orbital notation for the ground state neon atom. 23

24. 2 ways to write electron configurations
spdf Notation 1 s
value of energy level
sublevel
no. of
electrons
spdf NOTATION
for H, atomic number = 1
Orbital Box Notation
Arrows show electron spin
(+½ or -½)
ORBITAL BOX NOTATION
for He, atomic number = 2 1s 2  24

25. Shorthand notation practice
[Noble Gas Core] + higher energy electrons
Examples
● Aluminum: 1s22s22p63s23p [Ne]3s23p1
● Calcium: 1s22s22p63s23p64s2
[Ar]4s2
● Nickel: 1s22s22p63s23p64s23d8
[Ar]4s23d8 {or [Ar]3d84s2}
● Iodine: [Kr]5s24d105p5 {or [Kr]4d105s25p5}
● Astatine (At): [Xe]6s24f145d106p5
{or [Xe]4f145d106s26p5}

26. Basic Principle: electrons occupy lowest energy levels available
Rules for Filling Orbitals
Bottom-up
(Aufbau’s principle)
Fill orbitals singly before doubling up
(Hund’s Rule)
Paired electrons have opposite spin
(Pauli exclusion principle) 26

27. Full Configuration: 1s22s22p63s23p3 Valence Configuration: 3s23p3
Phosphorus
Symbol: P
Atomic Number: 15
Full Configuration: 1s22s22p63s23p3
Valence Configuration: 3s23p3
Shorthand Configuration: [Ne]3s23p3     1s 2s 2p 3s 3p
Box Notation 27

28. Identify examples of the following principles:
1) Aufbau 2) Hund’s rule 3) Pauli exclusion

29. READ SECTION 1.1, pp.10-12 PRACTICE PROBLEMS Page 14, #1,2,4,6.
WORK SESSION 
READ SECTION 1.1, pp.10-12
PRACTICE PROBLEMS
Page 14, #1,2,4,6.