1. Putting Atoms Together

2. The OCTET RULE & IONS electrons valence 8
The octet rule is a simple chemical theory that states that atoms gain, lose, or share _____________ so that they have eight electrons in their outer_________ shells, similar to the noble gases.
In simple terms, atoms are more stable when the outer shells of their atoms have _____ electrons.
hydrogen & helium only need to fill the 1st energy level (2 electrons) to become stable.
electrons
valence 8

3. When an atom loses or gains electrons (in order to have 8 valence electrons), it becomes charged and is known as an ______.
Atoms that gain electrons become _________ charged ions or _______.
Atoms that lose electrons become _________ charged ions or ________.
Ions have _____ outer shells and are ________.
ion
negatively
anions
positively
cations
full
stable

4. ALKALI METALS
e) How many positive charges (protons) are there in Li+? ________
How many negative charges (electrons) are there in Li+? ________
What is the total charge on the stable Li+ ion? ________
f) How many positive charges (protons) are there in Na+? ________
How many negative charges (electrons) are there in Na+?________
What is the total charge on the stable Na+ ion? ________
g) What is the charge on ions of the ALKALI METALS? ________ 3+ 2- 1+
11+
10- 1+ 1+

5. ALKALI METALS
 2. a) Describe the chemical reactivity of the ALKALI METALS.
Very reactive
b) Draw Bohr-Rutherford diagrams for Li, Na, and K.
Li Na K 3 11 19

6. ALKALI METALS
 c) Why are the ALKALI METALS reactive (why are they not stable)?
  They do not have a full outer shell
It is easier for the atoms of the alkali metals to ___________electrons in order to get a full outer energy level.
How many electrons should the ALKALI METALS lose from their outer shell to be stable? _______
lose 1

7. HALOGENS
d) How many positive charges (protons) are there in F-? ________
How many negative charges (electrons) are there in F-? ________
What is the total charge on the stable F- ion? ________
f) How many positive charges (protons) are there in Cl-? ________
How many negative charges (electrons) are there in Cl-? ________
What is the total charge on the stable Cl- ion? ________
What is the charge on ions of the HALOGENS? ________ 9+
10- 1-
17+
18- 1- 1-

8. HALOGENS 3. a) Describe the chemical reactivity of the HALOGENS.
Very reactive
b) Draw Bohr-Rutherford diagrams for F and Cl.
F Cl 9 17

9. HALOGENS
 c) Why are the HALOGENS reactive (why are they not stable)?
  They do not have a full outer shell
d) It is easier for the atoms of the halogens to ___________electrons in order to get a full outer energy level. How many electrons should the HALOGENS gain for their outer shell to be stable? _______
gain 1

10. NOBLE GASES a) Describe the chemical reactivity of the NOBLE GASES.
very stable / not reactive
Draw Bohr-Rutherford diagrams for He, Ne, and Ar.
He Ne Ar
c) Why are the NOBLE GASES stable and unreactive? 2 10 18
  They all have full outer shells