Chemical Reactions

     In our chemistry class we were given a lab on chemical reactions. We had to do eight reactions from five different categories which were synthesis, decomposition, single-replacement, double-replacement and combustion.
     If you do not know what this categories are here are the meanings:

Synthesis: Makes or creates two or more substances joined together to make a third thing.               
                     General form: A + X -> AX

Decomposition: To take apart or break down.(substances is broken down into two different substances.)
                   General form: AX -> A + X

Single-Replacement: An element replaces a similar element in a compound usually take place in aqueous solution.
                    General form: A + Bx(aq) -> Ax + B

Double-Replacement: Ions of two compounds that changes places. Usually takes place in aqueous solution. one product is usually soluble (aq) and the other forms such as gas or sometimes water.
                                General Form: Ax(aq)+ BY(aq) -> AY + Bx

Combustion: A substance( usually hydrocarbon) combined with oxygen releasing a large amount of heat and light.
                A complete Combustion: Hydrocarbon + Oxygen -> Carbon dioxide + water
                                                        C3H3 + O2 -> CO2(g) + H2O(l) + Energy

                  Out of all the reactions my group completed my favorite reaction was Double-Replacement. It was really easy to complete and it had a fast reaction. This is how I did it:

1.Measure 10 ml of Iron Sulfate into a beaker.
2. Measure 1 teaspoon of aluminum metal. Set aside
3. Now drop the aluminum metal into the iron sulfate beaker and wait around 2-4 minutes to see the reaction of the chemicals.

The reaction should create some sort of bubbles or white liquid at the bottom of the beaker. That is because the iron sulfate is dissolving the aluminum metal.

Chem Formula

Not good at naming ions? No worries! With these few simple tricks you will be a pro shortly!

Step 1: Determine whether the compound is ionic or covalent.

• An ionic compound will have one non-metal element and one metal element
• Ex:  NaCl (Sodium is a metal and Chloride is a non-metal)
• A covalent compound (often referred to as molecular) has two non-metal elements
• Ex: CO (Carbon and Oxygen are both non-metals)

Step 2:  Ionic compounds must have a net charge of 0.

• Using the periodic table, determine the charge of each ion.
• Ex: Alkali metals (Lithium, Potassium) have a +1 charge.  Alkaline earth metals (Magnesium, Calcium) have a +2 charge.
• For NaCl we know that Na has a +1 charge and Cl has a -1 charge.
• Determine whether or not a roman numeral must be used.
• Ex: Fe (Iron) has a +2 and +3 charge, which is important to note when used in a compound.
• Determine if multiples of an ion or element are required to balance out the net charge.
• Ex: (Li)3PO4 means that the Lithium ion must be multiplied by three to balance the Phosphates -3 charge.  In the case of Potassium permanganate, the charges balance out (a +1 and a -1) so no multiplication is needed.

Step 3:  Covalent compounds use a special prefix system for naming.

• Determine the charges of each ion 
• Ex: ClF (Chlorine has a -1 charge and Fluorine has a -1 charge)
• Based on the molecular formula, name the molecule based of the number of elements.
• Ex: Cl2O would be named Dichlorine monoxide, di- for two chlorines and mono- for one oxygen.  N2O5 would be named Dinitrogen pentoxide, di- for two nitrogens and penta- for five oxygens.

Numerical Prefixes

mono: 1

di: 2

tri: 3

tetra: 4

penta: 5

hexa: 6

hepta: 7

octa: 8

nona: 9

deca: 10