1.6 CHEMICAL EQUATIONS – part two

When performing chemical equations you will encounter four basic types of reactions. Combination reactions, decomposition reactions, single and double replacement reactions.

1. Combination Reactions
The format for these reactions is A + B = AB. Combination reactions are simply the combination of 2 or more reactants to form a single product.
(from now on, instead of using = between reactants and products, we’ll use the arrow system. The need for this will be evident later on).

An example of a combination reaction would be:

chem reactions 2 ex 2

Another example would be:

chem reactions 2 ex 1

2. Decomposition Reactions
The format for these is AB  A + B. Decomposition reactions are simply the result of one reactant becoming 2 or more products. An example would be:

chem reactions 2 ex 3

Another example would be:

chem reactions 2 ex 4

3. Single Replacement Reactions
The format for these is A + BC  AB + C. Single displacement reactions occur when a reactant swaps places with another reactant. An example would be:

chem reactions 2 ex 5

As you can see above, Zinc swaps places with H. Another example would be:

chem reactions 2 ex 6

In the above single replacement reaction, Fe takes Cu’s place.

4. Double Replacement Reactions
The format for these is AB + CD → CB + AD. Double displacement reactions occur when both reactants swap partners. An example would be:

chem reactions 2 ex 8The Ag swapped partners with Na. Therefore Ag went from being with NO3 to being with Cl. And Na left Cl to be with NO3.

Another example would be:

chem reactions 2 ex 7
 Before moving onto the next tutorial, we suggest you try the sample questions for this tutorial. Have fun!

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