1. Patterns and the Periodic Table
The periodic table is set up such that metals are found on the left side and non-metals on the right. Properties of metals and non-metals can be found below.
METALS
Solid, Shiny, Maleable, Conductor (Example: Nickel)
NON-METALS
Solid/Liquid/Gas, Dull, Brittle, Insulators (Example: Bromine)

2. The periodic table also categorizes elements into periods and groups
The periodic table also categorizes elements into periods and groups. Each row of elements on the periodic table is called a period. Each column is a group of elements with similar properties.

3. Four best-known groups of elements are:
Group 1: Alkali Metals – shiny, silvery metals (Li, Na); form compounds that are mostly white solids and very soluble in water.
Group 2: Alkaline Earth Metals – shiny, metals (Mg, Ca); form compounds that are often insoluble in water.
Group 17: Halogens – non-metallic (F, Cl); poisonous elements that react readily with sodium and other alkali elements.
Group 18: Noble Gases – far right of the periodic table (He, Ne); very stable, do not form compounds.

4. The Periodic Table

5. This is an example of a Bohr Diagram:
Atoms and Ions
This is an example of a Bohr Diagram:

6. Atoms are composed of 3 types of subatomic particles:
Protons – positive charge, weighs the same as a neutron, located in nucleus, number of protons is equal to the atomic number of an element on periodic table.
Neutrons – neutral, weighs the same as a proton, located in nucleus.
Electrons – negative charge, have no mass, located outside the nucleus – circle the nucleus at different energy levels (orbits/shells).
**The number of electrons equals the number of protons. (# p = # e-)**

7. To understand the formation of compounds, you have to understand the arrangement of electrons.
The farther away an electron is from the nucleus, the greater its energy and more likely the element will be involved in a chemical change – therefore, electrons in outer orbits are involved in bonding.
The outer orbit is called the valence shell and the electrons in this orbit are called valence electrons.

8. Bohr Diagram for Lithium
Bohr diagrams represent the arrangement of electrons in various orbits.
The first orbit can have a maximum of 2 electrons
The second orbit a maximum of 8 electrons, and for elements up to 20 electrons
The third orbit has a maximum of 8 electrons.
Bohr Diagram for Lithium
Atomic #
AtomicMass

9. Bohr Diagram for Fluorine
Atomic #
Atomic mass

10. Noble Gases Noble gases do not form compounds. Why?
Because their valence shell is stable.
Bohr Diagram for Helium
Bohr Diagram for Neon

11. When elements form compounds, changes occur in the electron arrangement. In some compounds, electrons are transferred from one atom to another so that atoms can have stable electron arrangements (full valence shells).
If Lithium loses 1 electron, when it forms a compound it then becomes stable. However, now it is no longer neutral (the protons no longer equal the electrons). Therefore, Li forms an ION, which is charged atom – the amount of electrons do not equal the amount of protons.

12. Ion – a charged particle that results when an atom gains or loses one or more electrons. Ionic Charge – the numeric value of the electric charge with a plus or minus sign. Therefore, Lithium’s ionic charge is +1 because it now has 3 protons and 2 electrons. It will be written as Li+1
Lithium as an ATOM has 3 Electrons and 3 Protons
Lithium as an ION has 2 Electrons and 3 Protons

13. Draw the Bohr diagram for a Calcium ion.
Draw the Bohr diagram for Calcium and state how many electrons Calcium would gain or lose and what its ionic charge is and how it would be written.
Draw the Bohr diagram for a Calcium ion.

14. Draw the Bohr diagram for Sulphur
Draw the Bohr diagram for a Sulphur ion. Sulphur can’t lose 6 electrons so it wants to gain 2 electrons to form a stable ion. S2- is an anion.

15. Naming Ions A positive ion is called a CATION
A negative ion is called an ANION.
The name of a positive ion is the same as the name of the element: calcium forms calcium ions.
The name of a negative ion is determined by adding “ide” to the stem of the name. For example, oxygen forms oxide ions, phosphorus forms phosphide ions, and sulphur forms sulphide ions.