1. Introduction to the Periodic Table

3. Periodic Table
Dmitri Mendeleev – constructed the 1st periodic table by listing the elements in columns in order of increasing atomic mass.
He then rearranged the columns so that the elements with the most similar properties were side by side.

4. Periodic Table
Henry Moseley determined the atomic number of atoms of the element.
He arranged the elements in order of increasing atomic number.

5. Periodic Law
When elements are arranged in order of increasing atomic number.
An important consequence is that the elements with similar chemical and physical properties end up in the same column.

6. Key to the Periodic Table
Elements are organized on the table according to their atomic number, usually found near the top of the square.
The atomic number refers to how many protons an atom of that element has.
For instance, hydrogen has 1 proton, so it’s atomic number is 1.
The atomic number is unique to that element. No two elements have the same atomic number.

7. Atomic Mass Unit (AMU)
The unit of measurement for an atom is an AMU. It stands for atomic mass unit.
One AMU is equal to the mass of one proton.

9. Properties of Metals
Metals are good conductors of heat and electricity.
Metals are shiny.
Metals are ductile (can be stretched into thin wires).
Metals are malleable (can be pounded into thin sheets).
A chemical property of metal is its reaction with water which results in corrosion.

10. Properties of Non-Metals
Non-metals are poor conductors of heat and electricity.
Non-metals are not ductile or malleable.
Solid non-metals are brittle and break easily.
They are dull.
Many non-metals are gases.
Sulfur

11. Properties of Metalloids
Metalloids (metal-like) have properties of both metals and non-metals.
They are solids that can be shiny or dull.
They conduct heat and electricity better than non-metals but not as well as metals.
They are ductile and malleable.
Silicon

12. Arrangement of Periodic Table
Horizontal rows/Periods
There are 7 periods.
The period number corresponds to the number of energy levels an atom of that element has.
The elements in a period increase by one proton and one electron as you go from left to right.
Properties within a period change as you move across from element to element.

13. Arrangement of Periodic Table
Vertical columns/Groups or Families
Each group are numbered 1-18
Each group is numbered a second time with a Roman numeral (I-VIII/1-8) and the letter A or B.
The Roman numeral corresponds to the number of valence electrons—the number of electrons in the outer most energy level.
Exception to Rule is Helium.
Elements in each group have similar properties.

14. Group Names to Know Group 1 (IA) — Alkali Metals
Group 2 (IIA) — Alkaline Earth Metals
Group 17 (VIIA) — Halogens, “salt-formers”
Group 18 (VIIIA) — Noble Gases also called inert gases because they undergo very few chemical reactions.

15. Representative Elements
Representative Elements are the groups with the letter A next to their Roman numeral.
Groups 1, 2, and 13—18
Group A elements exhibit a wide range of physical and chemical properties.

17. Alkali Metals
The alkali family is found in the first column of the periodic table.
Atoms of the alkali metals have a single electron in their outermost level, in other words, 1 valence electron.
They are shiny, have the consistency of clay, and are easily cut with a knife.

18. Alkali Metals They are the most reactive metals.
They react violently with water.
Alkali metals are never found as free elements in nature. They are always bonded with another element.

19. Alkaline Earth Metals They are never found uncombined in nature.
They have two valence electrons.
Alkaline earth metals include magnesium and calcium, among others.

20. Transition Metals
Transition Elements include those elements in the B families.
These are the metals you are probably most familiar: copper, tin, zinc, iron, nickel, gold, and silver.
They are good conductors of heat and electricity.

21. Halogen Family
The elements in this family are fluorine, chlorine, bromine, iodine, and astatine.
Halogens have 7 valence electrons, which explains why they are the most active non-metals. They are never found free in nature.
Halogen atoms only need to gain 1 electron to fill their outermost energy level.
They react with alkali metals to form salts.

22. Noble Gases
Noble Gases are colorless gases that are extremely un-reactive.
One important property of the noble gases is their inactivity. They are inactive because their outermost energy level is full.
Because they do not readily combine with other elements to form compounds, the noble gases are called inert.
The family of noble gases includes helium, neon, argon, krypton, xenon, and radon.
All the noble gases are found in small amounts in the earth's atmosphere.

23. Rare Earth Elements
The thirty rare earth elements are composed of the lanthanide and actinide series.
One element of the lanthanide series and most of the elements in the actinide series are called trans-uranium, which means synthetic or man-made.

24. Dmitri Mendeleev, the original, periodic table (1869).

25. Alternative Periodic Tables The periodic spiral of Professor Thoedor Benfey.  

26. Alternative Periodic Tables Triangular long form by Emil Zmaczynski

27. Alternative Periodic Tables Dr
Alternative Periodic Tables Dr. Timmothy Stowe's physicists periodic table.  

28. Alternative Periodic Tables Albert Tarantola's orbital periodic table.