1. Periodic Table and Compounds

2. Periodic Table Interactive Periodic Table
The Periodic Table was developed in 1869 by a Russian chemist called Dmitri Mendeleev.

3. Periodic Table Element- contains only one type of atom
In Each element’s square:
Name
Atomic Number- the number of protons and electrons (P=E)
Atomic Symbol- Abbreviation for the element
Atomic Mass- average mass of an atom of that element
Subtract the number of protons from atomic mass to get the neutrons.

4. Periodic Table
Mercury and Bromine are the only two liquids on the periodic table.
Mercury is a liquid Metal!

5. Periodic Table
Group (Family)- a column of elements on the periodic table
Special Groups:
Alkali Metals
Alkali Earth Metals
Transition Metals (Except La, Ac, Uub, Uuu)
Nonmetals (Except Al, Ga, Ge, In, Sn, Sb, Tl, Pb, Bi, Po)
Halogens
Noble Gases

6. Family
Families have something in common. They all have the same number of electrons in their outer shell…what is that…you will see!
Other things they have in common…
Metals- easily conduct electricity.
Nonmetals- Do NOT conduct electricity easily
Gases- Do not form compounds easily

7. Period Period- A row of elements on the periodic table
As you go across the row, each element’s atomic number increases by one.

8. We are Family!
Sodium
Rubidium
Potassium
Cesium

9. Microscopic view of the atoms of
the element argon (gas phase).
Elements
Elements (atoms) are arranged by energy shells. The number of electrons on the periodic table is the number of electrons in the energy shells.
1st shell- 2 electrons
2nd shell- 8 electrons
3rd shell- 18 electrons (Could have 8)
4th shell- 32 electrons
                       

10. Compound-Made of two or more elements (atoms).
                       
Compound-Made of two or more elements (atoms).
Ex. Water - H2O – always 2-H and 1-O
Compounds can have properties that are different from the elements from which they are made.
The smallest part of a compound is a molecule.
Molecule- a group of atoms held together by the energy of a chemical bond.

11. Ion- Positively or negatively charged atom.
More or less electrons cause atoms to have a charge.

13. Compounds Ionic Compound- Opposite ions attract to TAKE electrons
Two types of Compounds:
Ionic Compound- Opposite ions attract to TAKE electrons
Ex. NaCl

14. Compounds
Covalent Compound- Bond that forms when outer electrons are shared
Ex. H2O
Most covalent compounds do not dissolve in water