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Types of Chemical Reactions

Doing chemical reactions is the main focus of chemistry because that's where the action is. That's when something gets made, changed, or destroyed. So a lot of emphasis is placed on chemical reactions.

Chemical reactions can be understood by these three areas of focus. A reaction is basically shuffling around the building blocks of chemistry (atoms/ions/molecules/electrons). Force & energy is what decides if the reaction occurs and how fast. Mathematics helps you keep an inventory of all the starting and ending materials.

As mentioned, chemical reactions mostly focuses on the building blocks. More specifically, how they are put together, how they dissassemble, and ways to rearrange them.

Types of Chemical Reactions
Synthesis (Combination)
Single Replacement/Displacement
Double Replacement/Displacement
Oxidation (Combustion)

Chemical reactions are often classified into these five categories. Let's go through them one by one.

Synthesis (Combination)

Medicines / Drugs
Man-made Jewels

Synthesis is the making of some compound such as a drug, a flavoring, a plastic, a jewel.

If atoms were big enough to pick up, we could easily make all kinds of interesting materials. Of course, they are extremely small and it's not that easy, but the concept is just as easy.

The synthesis reaction is normally represented by the letters "A" and "B" forming a compound represented by "AB". "A" and "B" could represent just two different elements, or they could be compounds (2 or more elements). (roll cursor over image for animation)

FLAVORINGS (example of synthesis):

Many articificial flavorings are made from combining an alcohol with an organic acid. An alcohol has an "OH" group. An organic acid has a carboxylic acid group (COOH). The questions marks means there is more attached to these groups. Depending what is attached, a different flavor is synthesized.

When the alcohol and organic acid combine, water is released. Below you will see some of the reactions that make the flavors you see here.

Below is the synthesis of pear flavoring. It starts with propyl alcohol (similar to rubbing alcohol) and acetic acid. As these join, water is released and pear flavoring is synthesized.
Notice that I show three ways of representing the molecules involved. The top are called "space-filled" models because they show the space that each atom takes up. You can see that the hydrogen atoms are smaller than the carbon or oxygen atoms. The middle models are structural formulas that help show the structure of the molecule. The bottom are skeletal structural formulas that indicate carbon atoms by a bend in a line. Carbon atoms are also at the end of line if there's no other element indicated.

Below is the synthesis reaction for apple flavoring. Here we start with ethanol (a two carbon alcohol) and butyric acid (it gives rancid butter that bad odor). When combined they form ethyl butyrate. The name "ethyl" is used when there are a small chain of two carbon atoms attached. "Butyrate" is the butyric acid without its acidic hydrogen.

Below is the synthesis reaction for pineapple flavoring. When potatoes are fermented to make alcohol (ethanol), there's also some amyl alcohol produced (5 carbon alcohol). The smell or taste of amyl alcohol will make people instantly nauseated. The other reactant is salicylic acid, which is the active ingredient in many wart removers and anti-dandruff shampoos. Salicylic acid dissolves skin; however, when these two nasty chemicals are combined, they make a nice pineapple flavoring that you eat.

Decomposition Reactions:

Speed up decomposition
   * Toxic waste
   * Waste
   * Fats
   * Explosives
Slow down decomposition

Decomposition Reactions:

We are interested in decomposition reactions for two different reasons. Sometimes we want to speed up decomposition and other times we want to slow down decomposition.

Here's an example of decomposition of turkey waste. We don't eat turkey feathers, heads, feets, and guts, so there's a need to get rid of this waste. Some companies have figured out ways to break down all of this waste into an oil. Remember most tissue (muscles, protein, etc.) in animals are made with very long chains of carbon. The process is to break down these long chains to about 10 to 20 carbon atoms long. That makes an oil similar to diesel or biodiesel.

The general formula for decomposition is shown here. This could mean two atoms that are bonded fly apart, or it can mean a larger molecule with multiple atoms coming apart. (roll cursor over image to see animation)

Potassium perchlorate is shown. When it decomposes it releases oxygen. That oxygen is used to speed up the combustion of material it's in contact with. For example, potassium perchlorate is used in fireworks. Other material such as paper or sawdust mixed with it will explode because of this source of oxygen.

Here's a fun decomposition reaction. The starting compound is ammonium dichromate. When heated, it begins to decompose into nitrogen gas, water vapor and powdered chromium (III) oxide. It looks like a volcano with ash being spread all over the place.

This looks like the compound is burning, but looking at the chemical equation we see no oxygen is being consumed. So the flame it produces does not need oxygen. So you can't put out this kind of "fire" by smothering it like most fires.

Here is ammonium dichromate again but this time showing a molecule of ammonium dichromate decomposing. (roll cursor over image to see animation).

Whenever you see gases in the products realize that the reaction can be dangerous because it can build up pressure and cause an explosion.

Single Replacement:
Another type of reaction is called single replacement (or single displacement). One element that is not bonded to any other element (A) comes in to take the place of another element that is bonded to something (B). Element (B) is now freed.

Sacrificial metal:
An example of a single replacement reaction is when one metal is sacrificed to save another metal. For example, concrete pillars have iron rebar in them for strength. However, salt water can quickly react with the iron to form iron (II) chloride. To prevent this, a metal like zinc or magnesium is attached to the rebar and will protect the iron. Here's the reaction:
Zn + FeCl2 -> Fe + ZnCl2

Notice the zinc metal becomes zinc chloride and the iron that had reacted with the chlorine becomes metallic iron. This preserves the iron rebar. In a similar manner the aluminum in boats are preserved by a piece of zinc or magnesium. See the person pointing to a plug of magnesium that is in embedded in the boat's rudder? That keeps the salt water from dissolving the aluminum; the magnesium dissolves in aluminum's place.

Double Replacement/Displacement: This kind of reaction is represented by one compound (represented by "AB") combining with another compound (represented by "CD"). The reaction happens when "A" and "C" swap places. Remember these letters represent any element. For example, let's say you have a pond that is poisoned with dissolved barium. This can be remedied with a double replacement reaction. That's because when barium chloride and magnesium sulfate come in contact with each other, the barium and magnesium atoms swapped places. This reaction doesn't really occur with solid barium chloride and solid magnesium sulfate. They need to be dissolved. See description under image.

The bottom equation above shows that the ions of barium, chlorine, magnesium, and sulfate are all in water indicated with the (aq) subscript. In water the ions with the same charge will stay away from each other, but those with opposite charges attract each other. So the 2+ magnesium ion will be attracted to the negative 1 chloride ions. They come together but water will pull them apart. Likewise the 2+ barium ion will be attracted to the negative sulfate ion. This time the attraction is so strong that water cannot pull them apart. So they form solid barium sulfate particles that sink to the bottom of the pond. Even if stirred up, solid barium sulfate is not dangerous to drink because the barum is bonded so tightly with sulfate that it want come apart to poison someone.

Neutralizing corrosive lye (sodium hydroxide).

Let's say you were using some drain opener (sodium hydroxide) and accidentally spilled some on the carpet. Lye is very dangerous and will cause blindness if gotten in the eye and will dissolve skin. The corrosive part of sodium hydroxide is the hydroxide. Notice that if you could replace the sodium in NaOH with hydrogen, you would get HOH, which is water. A weak acid like vinegar can supply that hydrogen. Below is the full reaction. Notice the water in the vinegar will dissolve the sodium hydroxide. The neutralization takes place when the H+ from the acetic acid bumps into the OH- from the sodium hydroxide. At that point they form water (HOH or written as H2O).

Oxidation reactions:

As the lists states, we are interested in oxidation reactions for two opposite reasons. Sometimes we want to speed it up and sometimes slow it down.

Combustion (a type of oxidation):
Hot air balloons use large propane torches to heat the air in the balloon. Unfortunately, that much flame can cause a catastrophic fire (see bottom image). Fortunately, the 11 people in this balloon survived.
All hydrocarbons (like propane) produce carbon dioxide and water as the combustion products. The unbalanced combustion reaction for propane is:
C3H8 + O2 --> CO2 + H2O
Since propane has 3 carbons, it makes 3 carbon dioxide molecules. Since it has 8 hydrogen atoms, it will make four H2O molecules. Let's show that:
C3H8 + O2 --> 3CO2 + 4H2O
Now we need to balance the oxygen on the left side. On the right side there are 6 oxygen atoms in the 3 carbon dioxide molecules and 4 oxygen atom in the 4 water molecules. That's a total of 10 oxygen atoms. Since oxygen travels as O2, we need five O2 molecules to give us 10 oxygen atoms. So our final balanced equation is:
C3H8 + 5O2 --> 3CO2 + 4H2O
A + B -> AB (synthesis)
AB -> A + B (decomposition)
A + BC -> B + AC
(single replacement)
AB + CD -> AC + BD
(double replacement)
Hydrocarbon + oxygen -> CO2 + H2O
Identifying the type of chemical reaction is easy. It's all about what you can do with building blocks. In other words, you can stick atoms together (synthesis), pull them apart (decomposition), replace one atom with another (single replacement), switch the positions of two atoms from two different compunds (double-replacement) and use oxygen atoms to combine with carbon and hydrogen atoms (combustion/oxidation).
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Since April 12, 2008