1. What is an ion?
A charged particle that results from the LOSS or GAIN of electrons
Positively charged  cation
Negatively charged  anion
Atoms gain/lose electrons in order to obtain a stable valence e- configuration like the noble gases
The Octet Rule: All other elements want a full valence shell of 8 e- like the noble gases (except for He which is stable with 2 valence e-) 1

2. Chemical Properties of Metals and NMs1
Metals tend to LOSE electrons and become positively charged ions
Non-metals tend to GAIN electrons and become negatively charged ions

3. Have one valence electron Highly reactive with water
Group 1: Alkali Metals
Have one valence electron
Highly reactive with water
Lose one electron to become +1 charged ions 1

4. Group 2: Alkaline Earth Metals Have two valence electrons
Reactive with water
**Elements in Groups 1 and 2 are so reactive that they are never found alone in nature (only found in stable compounds)
Lose two electrons to become +2 charged ions 1

5. Transition Metals Groups 3-12: Transition Metals
Can have multiple oxidation states
Colored ions must be transition metals 1

6. Inner Transition Metals (Rare Earth Metals)
Lanthanide series: an extension of period 6
Actinide series: an extension of period 7 1

7. The Halogens Have 7 valence electrons
Group 17- The Halogens
Have 7 valence electrons
Gain one electron to become -1 charged ions 1
Start here period 5 on Friday

8. The Noble (Inert) Gases
Group 18- Noble (Inert) Gases
Stable/ Non-reactive
Have a complete valence shell of 8 e- (except He which has 2 valence e-) 1