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Types of Chemical Reactions
Chemical reactions are happening all around you: bread rising and baking in the oven, the leaves changing color in the fall, even the digestion of food in your own body. All are chemical reactions. In a chemical reaction, one or more things, called reactants, change into one or more new things, called products.
Chemical reactions can be written as a word equation or in shorthand. A word equation would look like oxygen + hydrogen = water. Shorthand, this would look like O2 + H = H2 O. The things reacting are on the left side of the equation, and the products are on the right. Reactions can require energy or give off energy, but matter is always conserved. What that means is that however much you start with in reactants, you end with the exact same amount in products.
There are five types of chemical reactions: combination, decomposition, single-replacement, double-replacement and combustion.
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- 1:09 Combination Reaction
- 1:50 Decomposition Reaction
- 2:20 Single-Replacement Reaction
- 2:52 Double-Placement Reaction
- 3:29 Combustion Reaction
- 4:27 Lesson Summary
A combination reaction is when two or more substances react to form one new substance; essentially, when A + B = AB, as in the example of hydrogen and oxygen combining to make water. The reactants can be either two elements, as in the water example, or two compounds AB + CD = ABCD, such as when magnesium oxide combines with carbon dioxide to make magnesium carbonate (MgO + CO2 = MgCO3). Or, even one element and one compound: A + BC = ABC.
A decomposition reaction, as you can guess, is the opposite of a combination reaction. This is a chemical change in which a single compound breaks down into two or more products (AB = A + B). Most decomposition reactions require energy in the form of heat or light. An example is when mercury oxide, with the addition of heat, breaks down into mercury and oxygen (2HgO + heat = 2Hg + O2).
Single-replacement reactions start getting a bit trickier. This is a chemical reaction in which one reactant replaces a second one (AB + C = AC + B). In this type of reaction, both the reactant and product consist of one element and one compound. One example is when you put potassium into water to form potassium hydroxide plus hydrogen gas. Very explosive! (2K + 2H2 O = 2KOH + H2).
A double-replacement reaction is a chemical reaction involving the exchange of positive ions between two compounds. An ion is an electrically charged atom. It is charged because there are unequal numbers of protons and electrons. A positive ion has fewer electrons than protons, so it has a positive charge. The reaction looks like this: A+B- + C+D- = A+D- + C+B-. So, the positively charged ions changed places.
And, lastly is the combustion reaction. In a combustion reaction, an element or compound reacts with oxygen, usually producing energy as heat or light. A combustion reaction always involves oxygen as a reactant. An example is methane + oxygen = carbon dioxide + water (CH4 + 2O2 = CO2 + 2H2 O).
Predicting Chemical Reactions
You can predict the products of a chemical reaction by knowing the reactants. For instance, if you have positive ions, then it will be a double-replacement reaction. An element plus a compound making another element and compound is probably a single-replacement reaction. Two elements adding together to make a compound - that's a combination reaction. One compound breaking apart to make two elements - that's a decomposition reaction. Lastly, if oxygen is involved as a reactant, it is probably a combustion reaction.
The five common types of chemical reactions are the following:
Combination reaction: A + B = AB
Decomposition reaction: AB = A + B
Single-replacement reaction: AB + C = AC + B
Double-replacement reaction: A+B- + C+D- = A+D- + C+B-
Combustion: AB + O2 = AO + B
After watching this video lesson, you'll be able to:
- Explain what a chemical reaction is
- Describe the five common types of chemical reactions: combination, decomposition, single-replacement, double-replacement and combustion reactions
- Predict the products of a chemical reaction
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Common Chemical Reactions and Energy Change
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