1. Electron Shells First Shell, maximum 2 electrons
Third shell, max # 8 electrons, (in this
case, the last, so
called the Valence
Shell.)
Second Shell,
Maximum 8 electrons

2. Charges The outer electrons on an atom are called: Valence electrons.
Atoms want an ASCVI Diagram that looks like a Noble Gas because…
Noble Gases have the most stable structure.
Usually, this means the atom ends up with a Charge.

3. Ions
Ion= a Charged atom in which the number of ELECTRONS (-) is different from the number of PROTONS (+).
Ionic Charge= is the number of positive (+) or negative (-) Charges on an atom. Ex: Mg+2

4. Groups Mg
Be (Berylium)

5. So…
Even though each element has a different # of PROTONS and ELECTRONS, each element in a group has a similar Bohr-Rutherford Diagram.
This means they want to gain or lose the same number of Electrons.
It also means elements in a Group will react similarly in Chemical Reactions.

6. Group Name and Number Akali Metals Akaline Earth Metals Noble Gases
Halogens
Transition metals

7. Cl & Na Chlorine Gas is poisonous.
In terms of electrons, what does Chlorine want to do?
-Gain an electron. So what would the Charge be?
Would you eat Na?
In terms of electrons, what does Sodium want to do?
Lose an electron. So what would the Charge be?

8. Cl & Na, cont’d What would happen if we put Na and Cl together?
We get NaCl, a.k.a.:
SALT!

9. Na + Cl Na+1 + electron + Cl
Salt, what has Happened?
Sodium (Na) gave up its Valence electron to the Chlorine (Cl).
Na + Cl Na+1 + electron + Cl
Na+1 + Cl NaCl
Why do you think they are now written together? Why are there no Charges?

10. Ionic Bonding
Positives will be attracted to Negatives. The force of the attraction between a Positively Charged Ion and a Negatively Charged Ion is called an IONIC BOND.
When two Ions Bond, they form an Ionic Compound. Ex. NaCl
Check your new textbook…

11. Ionic Compounds Positive Ion is called a CATION.
Negative Ion is called an ANION.
Write down 2 other cations and anions that you think would fit together

12. Ionic Compounds Notice the cross over of Charges
The Cation is always written FIRST, Anion Second.
Ionic compounds are made up of metals and non-metals, the metal is written FIRST.

13. Formation of Ionic Compounds Crossing Rule
Ca+2 + Cl-1
CaCl2

14. Ionic Structure
Ionic Compounds: Compounds made up of positive and negative ions that have resulted from the transfer of electrons from a metal to a non-metal.

15. Naming Ionic Compounds
Regular names:
Write the name of the metal first
Replace the ending of the non-metal with –ide
eg. Mg3P2 → Magnesium Phosphide

16. Naming Ionic Compounds
Transition Metals:
When a metal can form more than one type of ion
State the charge using a Roman numeral
eg. CuBr → Copper I Bromide
Eg. CuO → Copper II Oxide

17. Naming Ionic Compounds
Acids:
Recognized by the H+ ion out front (but not like in water, H2O, that’s covalent)
Name it using the non-metal, but with the ending -ic
eg. HCl → Hydrochloric acid
Eg. HF → Hydrofluoric acid
Try HI
→ Hydroiodic acid