1. The arrangement of pure matter
Periodic Table
The arrangement of pure matter

2. Disappearing Spoon – Sam Kean
Sam Kean on the topic of the periodic table.
“Of Course, part of the frustration you might remember about the periodic table could flow from the fact that, despite its being freely available to fall back on, a gigantic and fully sanctioned cheat sheat, it remained less than frickin’ helpful.”

3. Disappearing Spoon – Sam Kean
“On the one hand, the periodic table seemed organized and honed, almost German engineered for maximum scientific utility. On the other hand, it was such a jumble of long numbers, abbreviations, and what looked for all the world like computer error Messages ([Xe]6s2 4f145d1), it was hard not to feel anxious. And although the periodic table had something to do with other sciences, such as biology and physics, it wasn’t clear what exactly.”

4. The Beginning Alchemy – Chemistry
Need to organize elements
Before modern technology elements identified by their physical properties
Primarily metals
After 1750 systematic process for testing chemical properties
Number of element discoveries increased

5. Antoine Lavoisier Antoine Lavoisier—”father of modern chemistry”
Frenchman lived during the late 1700’s
Discovery of more elements
Four categories:
Metals
Non-metals
Gases
Earths

6. Building the Table 1871 Dmitri Mendeleev a Russian Chemist
Arranged by increasing atomic mass
Final Arrangement
Grouped elements with similar properties in columns
Each column increased in mass from top to bottom

7. Mendeleev’s Periodic Table
Dmitri Mendeleev

8. Importance… Firsts… Evidence
Properties of element related to location on the periodic table
Left gaps for future elements to be discovered
Predicted the discovery of elements
Evidence
Decades later discovered elements confirmed the usefulness of Mendeleev’s table

9. The Modern Periodic Table
Arranged by increasing atomic number
Number of protons
Mendeleev was not aware that elements have different numbers of protons
Periods
Each row on the periodic table
Depends on the number of available orbitals for electrons

10. The World of Periodic Tables

11. Spiral Periodic Table http://www.youtube.com/watch?v=qhg2uOSb-LA

12. Links to Periodic Tables
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13. The Periodic Table
Period
Group or Family
Group or family
Period

14. “Electrons drive the periodic table” Sam Kean
Column on the periodic table
Elements in a group have similar properties
Properties of elements repeat predictably when atomic number is used to arrange groups
Similar electron configurations
Pattern of repeating properties is known as periodic law
Gilbert Lewis’ work on bonding

15. Valence Electrons
Valence electrons are the electrons that are in the outermost energy level of an atom
Valence electrons determine how an element will bond with other elements
Examples:
Na, O, Cl, N, B, Al, Si

16. Valence Electrons Cont…

17. Group 1A Alkali Metals Highly reactive 1 Valence electron
All elements in Group 1
Highly reactive
Not usually found in nature
Increases down the periods
1 Valence electron
Easily lose valence electron (Reducing agents)
React violently with water
React with halogens to form salts
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18. Group 2A Alkaline Earth Metals Reactivity increases from top to bottom
All elements in group 2
harder than group 1
Reactivity increases from top to bottom
2 valence electrons

19. Groups 3-6A Boron Family Carbon Family Nitrogen Family Oxygen Family
Elements in group 3
3 valence electrons
Carbon Family
Elements in group 4
4 valence electrons
Increasingly metallic from top to bottom
Nitrogen Family
All elements in group 5
5 valence electrons
Oxygen Family
Elements in group 6
6 valence electrons

20. Group 7A The Halogens At room temperature different states
Elements in group 7
Elements have 7 valence electrons
At room temperature different states
Similar chemical properties
Highly reactive
Fluorine is most reactive

21. Group 8A The Noble Gases Stable electron configuration
Elements in group 8
Stable electron configuration
All elements want this type of configuration
Colorless, odorless, and extremely unreactive
Because of stable electron configuration

22. Classes of Elements Metals Transition Metals
Good conductors of heat and electricity
Malleable
Ductile
High tensile strength
Luster
Transition Metals
Elements in groups 3-12
Properties can vary

23. Examples of Metals
Potassium, K reacts with water and must be stored in kerosene
Copper, Cu, is a relatively soft metal, and a very good electrical conductor.
Zinc, Zn, is more stable than potassium
Mercury, Hg, is the only metal that exists as a liquid at room temperature

24. Classes of Elements Non-Metals Metalloids
Very poor conductors of heat and electricity
Tend to be brittle
Low melting and boiling points
Many are gases at room temperature
Metalloids
Elements that have both metallic and non-metallic properties
Properties can vary depending on the environmental conditions
Semiconductors of electricity

25. Examples of Nonmetals
Microspheres of phosphorus, P, a reactive nonmetal
Sulfur, S, was once known as “brimstone”
Graphite is not the only pure form of carbon. Diamond is also carbon; the color comes from impurities caught within the crystal structure

26. Silicon, Si – A Metalloid
Silicon has metallic luster
Silicon is brittle like a nonmetal
Silicon is a semiconductor of electricity
Other metalloids include:
Boron, B
Germanium, Ge
Arsenic, As
Antimony, Sb
Tellurium, Te