Naming Compounds

There are 3 types of compounds that one should know: Type 1, Type 2 and Type 3.

Type 1
Type 1 compounds are ionic. There is a cation (group 1 and 2, Al, Zn, Ag, and Cd on the periodic table)
 and there is an anion (non-metal/polyatomic ion).
The first thing you need to do is write the name of the cation. Then, change the ending of the anion to "-ide". For example, oxygen = oxide, sulfur = sulfide, ect.
Never change the name of a polyatomic ion.

Example of a Type 1: potassium + chlorine
                                        K+          Cl-      =KCL
                                 =potassium chloride

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Type 2
The most important thing to remember about Type 2 compounds is this: DO NOT TRUST THE PERIODIC TABLE!
Mn SO4 =  manganese (II) sulfate
Mn2 (SO4)3 = manganese (III) sulfate
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Type 3
Uses prefixes to tell how many each element there are in the compound. (don't use mono on the first element in the compound)
1: mono
2: di
3: tri
4: tetra
5: penta
6: hexa
7: hepta
8: octa
9: nona
10: deca
Remember to change the ending of the last element to "-ide"

Examples:
H4C2 = tetrahydogren  dicarbon
CO =carbon monoixde
P2O4CL3 = diphosphorus tetraoxygen trichloride

Chemistry Games

I was online one day looking for some help with the periodic table. Lo and behold, I find a site dedicated to chemistry games that actually help!

Here is the website address: http://www.sheppardsoftware.com/Elementsgames.htm

Molecular Formula

Every molecular formula is a whole number multiple of the empirical formula.
In order to find the molecular formula, find the multiplier:

Here is an example on finding the molecular formula:

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I do have one question relating to molecular formula; how can compound be a molecular and empirical formula at the same time:

For example:

 Why is the answer E?

Empirical Formula

The definition of an empirical formula is to take a molecule and put it into the simplest whole number ratio. Be sure to remember that ionic compounds are usually already in empirical formula.

Here is an example: C2 H6 ----------------> CH3

The 2 IN C2H6 is the molecular formula (tells you what and how many are in a molecule). We'll get to the molecular formula later.

The 1 in CH3 is the empirical formula (simplest whole number ratio).

Here are two more examples to finding the E.F.:

C9H16 ----------> C9H16
C62H4O12 ---------> C31H2O6
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Finding the empirical formula is easy, you just have to follow some steps.
First, go from percent to mass
Second, mass to moles
Third, divide by the smallest
Fourth, multiply until it's whole

Here is an example by using the steps above in order to find the E.F.:

And there is how to solve E.F. in a nutshell!

Christmas Tree Story

I was listening to Science Friday on NPR one day and found myself listening to this really cool interview called 'Chemistry Keeps Christmas Tree Alive, For Longer'. The subject of the interview was to explain how and why trees lose their needles. At the Nova Scotia's Christmas Tree Research Center, researchers are trying to find a way to extend the life of Christmas Trees.

Here is the website to listen/read the interview: http://www.npr.org/2010/12/10/131967516/Chemistry-Keeps-Christmas-Trees-Alive-For-Longer