1. PERIODIC TABLE OF ELEMENTS

2. The Elements

3. Naming Elements Most elements were named in latin
Symbols for the elements are derived from latin name
Determined by the International Union of Pure and Applied Chemistry (IUPAC)
New elements are given a temporary 3 letter symbol until IUPAC decides on an appropriate 2 letter symbol
This committee names new elements based on where they were discovered or to pay tribute to a notable scientist

4. Common Elements and Symbols

5. A Brief History

6. Johann Dobereiner (1829)
Noted a similarity among the physical and chemical properties of several groups of three elements
Middle element had mass about halfway between the atomic masses of the other two – LAW OF TRIADS

7. John Newlands (1864)
Arranged all known elements in order of increasing atomic mass
Law of Octaves
Noticed repeating physical and chemical properties every 8 elements

8. Mendeleev (1869)
Dmitri Ivanovitch Mendeleev created the first accepted version of the periodic table.
He grouped elements according to their atomic mass; elements with similar properties appeared in same column
Blank spaces were left to add elements
First periodic law: elements arranged according to increasing atomic mass show a periodic recurrence of properties at regular intervals 

9. Mendeleev’s Periodic Table

10. Modern Periodic Law
When the internal structure of atoms was discovered, Mendeleev’s periodic law was revised
Elements arranged according to increasing atomic number show a periodic recurrence of properties at regular intervals

11. Features of the P.T.

14. Groups Periods Columns of elements are called groups or families.
Elements in each family have similar but not identical properties.
For example, lithium (Li), sodium (Na), potassium (K), and other members of group 1 are all soft, white, shiny metals.
All elements in a family have the same number of valence electrons.
Each horizontal row of elements is called a period.
The elements in a period are not alike in properties.
In fact, the properties change from metallic to non-metallic as you go across

15. Staircase line
Divides metals on left from non-metal on right

16. State of Matter Indicated by colour of the symbol Black = solid
Blue = liquid
Red = gas

17. Families

19. Hydrogen
The hydrogen square sits atop Family 1, but it is not a member of that family. Hydrogen is in a class of its own.
It’s a gas at room temperature.
It has one proton and one electron in its one and only energy level.
Hydrogen only needs 2 electrons to fill up its valence shell.

21. Alkali Metals Group 1 metals One valence electron
Most reactive metals, react violently with water to make a base
soft, silver, solids
alkali metals in water

24. Alkaline Earth Metals Group 2 metals two valence electrons.
React slowly with water
Solid, react with air to form oxides
React with H to form hydrides (except Be)

26. Transition Metals Groups 3 - 12 Strong, hard metals
High melting points
good conductors of heat and electricity.
React with O to make oxides
Some react with acids
Form multivalent ions

28. Halogens Group 17 non-metals 7 valence electrons
Extremely reactive with hydrogen and metals
Solid, liquid or gas
Dull, do not conduct electricity

30. Noble Gases Group 18 non-metals Full valence shell
gases that are extremely un-reactive (stable)
Low melting and boiling points

31. Lanthanides (rare earth metals)
Atomic #
Belong to period (row) # 6 on the periodic table

32. Actinides Atomic # 89 - 102 Belong to the 7th period
Include the transuranic elements (elements with atomic #93 or greater – synthetic)