Chemical Nomenclature - Oct 2 Class

In the beginning of class, Mr. Doktor showed us an example of electrolysis. He used pickles, water, and a battery charger. He then touched the pickle with the two wires, and you could see smoke come out and the pickle being electricuted. He then touched the water with the wires and smoke came out as well. You could see the hydrogen and oxygen as the smoke and you could smell this funky burning smell. You should not try this experiment at home due to dangerous results such as being electricuted or starting a fire.



Here is a video of an example of electrolysis.

http://www.youtube.com/watch?v=Or22ktW8btc&feature=related
This is a quick video that shows how hydrogen and oxygen atoms blow up a balloon. In my assumption, i believe that the balloon blew up due to evaporating water.



After that experiment in class, Mr. Doktor gave us examples and questions about naming compounds. Here are the examples done in class:
Name:
1. PbS2 - Lead (IV) Sulphide
2. MgO - Magnesium Oxide
3. CuCl2 - Copper (II) Chloride
4. Cr2O3 - Chromium (III) Oxide

Chemical Nomenclature
- Naming chemical compounds has been a very difficult task and different systems have been used through the centuries.
- Today the most common system is IUPAC for most chemicals.
- Ions
* Binary Ionic
- Polyatomic Ions
- Molecular Compounds
- Acids



Chemical Formulas
Be aware of the differences between ion and compound formulas.
Zn²+ - ion charge
BaCl2 - number of ions (Subscript)

Naming Ions
- For metals, use the name of the element and add ion
Eg. Al³+ = Aluminium Ion
- For non-metals, remove the original ending and add -ide
Eg. F- = Fluorine -> Fluoride

Polyatomic Ions have special names.

Binary Ionic
Steps:
1. Write the formula for the cation first and then the formula for the anion. (Cation = positive because "cat" = "pussytive" & Anion = Negative)
2. Criss cross charges moving the numbers below.
3. Reduce ion numbers to lowest common multiples, omit 1 and omit charges.
Eg.


Example
- Write the chemical formulas of:
Aluminum Fluoride = AlF3
Sodium Oxide = Na2O
Iron (III) Sulphide = Fe2S3

Multivalent Ions
- Some elements can form more than one Ion
Eg. Iron -> Fe³+ or Fe²+ / Copper -> Cu²+ or Cu¹+
- The more common ion is the top one of the P.T.
- IUPAC uses roman numerals in the parenthesis to show the charge.
- Classical (ie old) systems uses latin names of elements and the suffixes -ic (larger charge) and -ous (smaller charge)
FeO -> Ferrous Oxide
Fe2O3 -> Ferric Oxide

Other Classical Names
- Ferr = Iron
- Cupp = Copper
- Mercur = Mercury
- Stann = Tin
- Aunn = Gold
- Plumb = Lead
Chemical Formula: Sodium Nitrate -> NaNO3 (Na+/NO3-)
Barium Phosphate -> Ba3(PO4)2