chemical reaction assignment

Types of Chemical Reactions

A chemical reaction is a process or chemical change that transforms one set of substances ( the reactants ) into another set of substances (the products ). The process involves breaking chemical bonds between atoms and forming new bonds, so the number and type of atoms are the same for both reactants and products. The chemical change is described by a chemical equation . There are several types of chemical reactions. Here is look at the four main types of chemical reactions, plus additional key reaction types.

4 Main Types of Chemical Reactions

Keep in mind, there are different names for the reaction types. The four main types of chemical reactions are:

• Synthesis or combination reactions
• Decomposition or analysis reactions
• Single replacement, single displacement , or substitution reactions
• Double replacement , double displacement, or metathesis reactions

There are many other types of reactions, though. This table summarizes some key points of the main types of chemical reactions:

Let’s take a closer look at the types of reactions and get examples:

Synthesis or Direct Combination Reaction

In a synthesis, direct combination, or composition reaction, two (or more) reactants combine to form a more complex product. The general form of the reaction is: A + B → AB An example of a synthesis reaction is the combination of iron and sulfur to form iron(II) sulfide: 8 Fe + S 8  → 8 FeS

Here are other examples of synthesis reactions:

• 2 Na(s) + Cl 2 (g) → 2 NaCl(s)
• C(s) + O 2 (g) → CO 2 (g)
• S(s) + O 2 (g) → SO 2 (g)
• 2 Fe(s) + O 2 (g) → 2 FeO(s)
• 2 SO 2  + O 2  → 2 SO 3
• 6 C + 3 H 2  → C 6 H 6
• 4 Na + 2 C + 3 O 2  → 2 Na 2 CO 3

Decomposition or Analysis Reaction

A compound breaks or decomposes into smaller pieces in a chemical decomposition or analysis reaction. The general form of the reaction is: AB → A + B An example of a decomposition reaction is the electrolysis of water to form oxygen and hydrogen: 2 H 2 O → 2 H 2  + O 2

Here are additional examples of decomposition reactions:

• CaCO 3  → CaO + CO 2
• 2 KClO 3  → 2 KCl + 3 O 2
• Na 2 CO 3  → Na 2 O + CO 2

Single Replacement, Single Displacement, or Substitution Reaction

A single replacement, single displacement, or substitution reaction is when one element is displaced from a reactant to form a compound with another element. The reaction has the general form: A + BC → AC + B An example of a single replacement reaction is when zinc combines with hydrochloric acid to form zinc chloride and hydrogen. The zinc replaces or displaces the hydrogen in hydrochloric acid: Zn + 2 HCl → ZnCl 2  + H 2

Double Replacement, Double Displacement, or Metathesis Reaction

When the reactant cations and anions “swap partners” the reaction is called a double replacement, double displacement, or metathesis reaction. The general form for a double replacement reaction is: AB + CD → AD + CB An example of a double replacement reaction is the reaction between sodium chloride and silver nitrate to yield sodium nitrate and silver chloride: NaCl(aq) + AgNO 3 (aq) → NaNO 3 (aq) + AgCl(s)

Combustion Reaction

A combustion reaction is the reaction between a fuel and oxygen to form one or more oxides. Because many fuels are carbon-based, carbon dioxide (CO 2 ) is often a product. Sometimes water (H 2 O) is a product.

Here are examples of combustion reactions and their balanced equations :

• C 10 H 8  + 12 O 2  → 10 CO 2  + 4 H 2 O
• H 2  + O 2  → 2 H 2 O
• C 6 H 12 O 6  + 6 O 2  → 6 CO 2  + 6 H 2 O
• 2 Fe 2 S 3  + 9 O 2  → 2 Fe 2 O 3  + 6 SO 2
• 2 Al 2 S 3  + 9 O 2  → 2 Al 2 O 3  + 6 SO 2
• P 4  + 5 O 2  → 2 P 2 O 5

Acid-Base or Neutralization Reaction

An acid-base reaction is a type of double replacement reaction that occurs between an acid and a base. The H +  ion in the acid reacts with the OH –  ion in the base to form water and an ionic salt: HA + BOH → H 2 O + BA The reaction between hydrobromic acid (HBr) and sodium hydroxide is an example of an acid-base reaction: HBr + NaOH → NaBr + H 2 O

Oxidation-Reduction or Redox Reaction

Redox stands for reduction and oxidation . The two processes occur together. This type of reaction involves electron transfer between reactants and a change in oxidation number. An example is the reduction of I 2 to form  I –  and oxidation of S 2 O 3 2-  (thiosulfate anion) to form S 4 O 6 2- :

2 S 2 O 3 2− (aq) + I 2 (aq) → S 4 O 6 2− (aq) + 2 I − (aq)

Isomerization Reaction

In an isomerization reaction, the structural arrangement of a compound is changed but its net atomic composition remains the same.

For example:

CH 3 CH 2 CH 2 CH 3 (n-butane) → CH 3 CH(CH 3 )CH 3 (i-butane)

Hydrolysis Reaction

A hydrolysis reaction is a reaction in which one or more water molecules is added to a substance. In some cases, this causes both the substance and water molecule to split. The general form of a hydrolysis reaction is: X – (aq) + H 2 O(l) ↔ HX(aq) + OH – (aq)

The reverse reaction is a condensation reaction. In a condensation reaction, water is removed from a substance.

How Many Types of Chemical Reactions Are There?

Technically, there are hundreds or even thousands of different types of chemical reactions. However, chemistry students usually learn to classify them as 4 main types, 5 main types, or 6 main types. The four main types of chemical reactions are synthesis, decomposition, single displacement, and double displacement. But, remember, some people use different names for these reactions. Other important types of reactions are combustion, acid-base, redox reactions, and condensation reactions . It gets even more complicated in organic chemistry, where many reactions have special names. However, these other types of reactions also fit into one of the four main categories!

Types of Chemical Reactions Worksheet

Practice identifying the four main types of chemical reactions with this worksheet. Download and print the PDF worksheet and answer key.

[ Types of Chemical Reactions Worksheet ] [ PDF Answer Key ]

• Atkins, Peter W.; Julio de Paula (2006). Physical Chemistry (4th ed.). Weinheim: Wiley-VCH. ISBN 978-3-527-31546-8.
• IUPAC (1997). “Chemical Reaction”. Compendium of Chemical Terminology (2nd ed.) (the “Gold Book”). doi: 10.1351/goldbook.C01033
• Myers, Richard (2009). The Basics of Chemistry . Greenwood Publishing Group. ISBN 978-0-313-31664-7.
• Wiberg, Egon; Wiberg, Nils; Holleman, Arnold Frederick (2001). Inorganic Chemistry . Academic Press. ISBN 978-0-12-352651-9.

Related Posts

What is a Chemical Reaction?

Instructions, simulations.

Youtube ID: 7UUnRtwQPlc

Lesson Summary Video for teachers

Note: This video is designed to help the teacher better understand the lesson and is NOT intended to be shown to students. It includes observations and conclusions that students are meant to make on their own.

Key Concepts:

• A physical change, such as a state change or dissolving, does not create a new substance, but a chemical change does.
• A chemical change is the result of a chemical reaction.
• In a chemical reaction, the atoms and molecules that interact with each other are called reactants .
• In a chemical reaction, the atoms and molecules produced by the reaction are called products .
• In a chemical reaction, only the atoms present in the reactants can end up in the products. No new atoms are created, and no atoms are destroyed.
• In a chemical reaction, reactants contact each other, bonds between atoms in the reactants are broken, and atoms rearrange and form new bonds to make the products.

The teacher will use a small candle flame to demonstrate a chemical reaction between the candle wax and oxygen in the air. Students will see a molecular animation of the combustion of methane and oxygen as a model of a similar reaction. Students will use atom model cut-outs to model the reaction and see that all the atoms in the reactants show up in the products.

Students will be able to explain that for a chemical reaction to take place, the bonds between atoms in the reactants are broken, the atoms rearrange, and new bonds between the atoms are formed to make the products. Students will also be able to explain that in a chemical reaction, no atoms are created or destroyed.

Be sure you and the students wear properly fitting goggles. Be careful when lighting the candle. Be sure that the match and candle are completely extinguished when you are finished with the demonstration.

Materials for the Demonstration

• Tea light candle or other small stable candle
• Glass jar, large enough to be placed over the candle

Materials for Each Student

• Atom cut-outs from the activity sheet
• Sheet of colored paper or construction paper
• Colored pencils
• Glue or tape

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Standards Alignment

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Step 1 Review what happens during a physical change and introduce the idea of chemical change.

Tell students that in previous chapters they have studied different aspects of physical change. When atoms and molecules speed up or slow down, that is a physical change. When they change state from liquid to solid or from gas to liquid, that is a physical change. When a substance is dissolved by water or some other solvent, a new substance has not really been formed. The ions or molecules can still come back together to form the original substance.

Let students know that in this chapter they will explore what happens during a chemical change. In a chemical change, the atoms in the reactants rearrange themselves and bond together differently to form one or more new products with different characteristics than the reactants. When a new substance is formed, the change is called a chemical change .

Step 2 As a demonstration, light a candle and explain what is happening using the terms reactants , products , and chemical reaction .

Explain that in most chemical reactions, two or more substances, called reactants, interact to create different substances called products . Tell students that burning a candle is an example of a chemical reaction.

• Carefully light a tea light candle or other small candle.
• Keep the candle burning as you ask students the questions below. You will put the candle out in the second part of the demonstration

Expected Results

The wick will catch on fire and the flame will be sustained by the chemical reaction.

The following question is not easy, and students are not expected to know the answer at this point. However, thinking about a candle burning in terms of a chemical reaction is a good place to start developing what it means when substances react chemically.

Ask students:

• What do you think are the reactants in this chemical reaction? Wax and oxygen from the air are the reactants.

Students often say that the string or wick is burning. It is true that the string of the wick does burn but it’s the wax on the string and not so much the string itself that burns and keeps the candle flame burning. Explain that the molecules that make up the wax combine with oxygen from the air to make the products carbon dioxide and water vapor.

Point out to students that this is one of the major characteristics of a chemical reaction:

In a chemical reaction, atoms in the reactants combine in new and different ways to form the molecules of the products.

Students may be surprised that water can be produced from combustion. Since we use water to extinguish a fire, it may seem strange that water is actually produced by combustion. You may want to let students know that when they metabolize or “burn” food in their bodies, they also produce carbon dioxide and water.

Step 3 Place a jar over the candle to help students realize that oxygen is a reactant in the burning of a candle.

Remind students that air is a mixture of gases. Explain that when something burns, it reacts with the oxygen in the air.

Ask students to make a prediction:

• Will the candle still burn if one of the reactants (wax or oxygen) is no longer available? Students may guess that the candle will not burn because both reactants are required for the chemical reaction to continue.

• Carefully place a glass jar over the lit candle.

The flame goes out.

• Why do you think the flame goes out when we put a jar over the candle? Placing a jar over the candle limits the amount of oxygen in the air around the candle. Without enough oxygen to react with the wax, the chemical reaction cannot take place and the candle cannot burn.
• When a candle burns for a while, it eventually gets smaller and smaller. Where does the candle wax go? When a candle burns, the candle wax seems to “disappear.” It doesn’t really disappear: It reacts chemically, and the new products go into the air.

Note : Some curious students may ask what the flame is made of. This is a great question and not trivial to answer. The flame is burning wax vapor. The light of the flame is caused by a process called chemiluminescence. Energy released in the chemical reaction makes electrons from different molecules move to a higher energy state. When the electrons come back down, energy is released in the form of light.

Step 4 Introduce the chemical equation for the combustion of methane and explain that atoms rearrange to become different molecules.

Explain to students that wax is made of long molecules called paraffin and that paraffin is made up of only carbon atoms and hydrogen atoms bonded together. Molecules made of only carbon and hydrogen are called hydrocarbons . Tell students that you will use the simplest hydrocarbon (methane) as a model to show how the wax, or any other hydrocarbon, burns.

Project the image Methane and Oxygen React .

Show students that there is methane and oxygen on the left side of the chemical equation and carbon dioxide and water on the right side. Explain that the molecules on the left side are the reactants and the ones on the right side are the products . When the candle was burning, the paraffin reacted with oxygen in the air to produce carbon dioxide and water, similar to the chemical reaction between methane and oxygen.

Explain to students that the chemical formula for methane is CH 4 . This means that methane is made up of one carbon atom and four hydrogen atoms. Show students that the other reactant is two molecules of oxygen gas. Point out that each molecule of oxygen gas is made up of two oxygen atoms bonded together. It can be confusing for students that oxygen the atom, and oxygen the molecule, are both called oxygen . Let students know that when we talk about the oxygen in the air, it is always the molecule of oxygen, which is two oxygen atoms bonded together, or O 2 .

• Where do the atoms come from that make the carbon dioxide and the water on the right side of the equation? The atoms in the products come from the atoms in the reactants. In a chemical reaction, bonds between atoms in the reactants are broken and the atoms rearrange and form new bonds to make the products.

Note : Leave this equation projected throughout the activity in the Explore section of this lesson. Students will need to refer to it as they model the chemical reaction.

Give each student an activity sheet.

• Lesson 6.1 Student Activity Sheet  PDF  |  DOCX  |  Google Doc
• Lesson 6.1 Activity Sheet Answers  PDF  |  DOCX  |  Google Doc

Download the student activity sheet, and distribute one per student.

All Downloads

The activity sheet will serve as the “Evaluate” component of each 5-E lesson plan. The activity sheets are formative assessments of student progress and understanding. A more formal summative assessment is included at the end of each chapter.

Students will record their observations and answer questions about the activity on the activity sheet. The Explain It with Atoms and Molecules and Take It Further sections of the activity sheet will either be completed as a class, in groups, or individually, depending on your instructions. Look at the teacher version of the activity sheet to find the questions and answers.

Step 5 Have students make a model to show that in a chemical reaction the atoms of the reactants rearrange to form the products.

Question to Investigate

Where do the atoms in the products of a chemical reaction come from?

• Atom model cut-outs (carbon, oxygen, and hydrogen)

Prepare the Atoms

• Color the carbon atoms black, the oxygen atoms red, and leave the hydrogen atoms white.
• Use scissors to carefully cut out the atoms.

Build the Reactants

• On a sheet of paper, place the atoms together to make the molecules of the reactants on the left side of the chemical equation for the combustion of methane.
• Write the chemical formula under each molecule of the reactants. Also draw a “+” sign between the reactants.

After you are sure that students have made and written the formula for the reactant molecules, tell students that they will rearrange the atoms in the reactants to form the products.

Build the Products

• Draw an arrow after the second oxygen molecule to show that a chemical reaction is taking place.
• Rearrange the atoms in the reactants to make the molecules in the products on the right side of the arrow.
• Write the chemical formula under each molecule of the products. Also draw a “+” sign between the products.

Tell students that in a chemical reaction, the atoms in the reactants come apart, rearrange, and make new bonds to form the products.

Represent the Chemical Equation

• Have students use their remaining atoms to make the reactants again to represent the chemical reaction as a complete chemical equation.
• Glue or tape the atoms to the paper to make a more permanent chemical equation of the combustion of methane.

Step 6 Help students count the number of atoms on each side of the equation.

Project the animation Combustion of Methane .

Combustion of Methane

Show students that the atoms in methane and oxygen need to come apart like in their models. Also point out that the atoms arrange themselves differently and rebond to form new products. This is also like their model. Be sure that students realize that the atoms in the products only come from the reactants. There are no other atoms available. No new atoms are created, and no atoms are destroyed.

Note: Explain to students that chemical reactions are more complicated than the simplified model shown in the animation. The animation shows that bonds between atoms in the reactants are broken, and that atoms rearrange and form new bonds to make the products.

In reality, the reactants need to collide and interact with each other in order for their bonds to break and rearrange. Also, the animation shows all of the atoms in the reactants coming apart and rearranging to form the products. But in many chemical reactions, only some bonds are broken, and groups of atoms stay together as the reactants form the products.

Read more about the combustion of methane in Teacher Background.

• Lesson 6.1 Teacher Background  PDF

Guide students as you answer the following question together:

• How many carbon, hydrogen, and oxygen atoms are in the reactants compared to the number of carbon, hydrogen, and oxygen atoms in the products? Show students how to use the big number (coefficient) in front of the molecule and the little number after an atom of the molecule (subscript) to count the atoms on both sides of the equation. Explain to students that the subscript tells how many of a certain type of atom are in a molecule. The coefficient tells how many of a particular type of molecule there are. So if there is a coefficient in front of the molecule and a subscript after an atom, you need to multiply the coefficient times the subscript to get the number of atoms. For example, in the products of the chemical reaction there are 2H 2 O. The coefficient means that there are two molecules of water. The subscript means that each water molecule has two hydrogen atoms. Since each water molecule has two hydrogen atoms and there are two water molecules, there must be 2 x 2 = 4 hydrogen atoms. 

Note : The coefficients indicate the ratios of the numbers of molecules in a chemical reaction. It is not the actual number as in two molecules of oxygen and one molecule of methane since there are usually billions of trillions of molecules reacting. The coefficient shows that there are twice as many oxygen molecules as methane molecules reacting. It would be correct to say that in this reaction there are two oxygen molecules for every methane molecule.

Step 7 Explain that mass is conserved in a chemical reaction.

• Are atoms created or destroyed in a chemical reaction? No.
• How do you know? There are the same number of each type of atom on both the reactant side and the product side of the chemical equation we explored.
• In a physical change, like changing state from a solid to a liquid, the substance itself doesn’t really change. How is a chemical change different from a physical change? In a chemical change, the molecules in the reactants interact to form new substances. In a physical change, like a state change or dissolving, no new substance is formed.

Explain that another way to say that no atoms are created or destroyed in a chemical reaction is to say, “Mass is conserved.”

Project the image Balanced Equation . 

Explain that the balance shows the mass of methane and oxygen on one side exactly equals the mass of carbon dioxide and water on the other. When an equation of a chemical reaction is written, it is “balanced” and shows that the atoms in the reactants end up in the products and that no new atoms are created, and no atoms are destroyed.

Step 8 Introduce two other combustion reactions and have students check to see whether or not they are balanced.

Tell students that, in addition to the wax and methane, some other common hydrocarbons are propane (the fuel in outdoor gas grills), and butane (the fuel in disposable lighters). Have students count the number of carbon, hydrogen, and oxygen atoms in the reactants and products of each equation to see if the equation is balanced. They should record the number of each type of atom in the chart on their activity sheet.

Lighting an outdoor gas grill—Combustion of propane

C 3 H 8 + 5O 2 → 3CO 2 + 4H 2 0

Using a disposable lighter—Combustion of butane

2C 4 H 10 + 13O 2 → 8CO 2 + 10H 2 O

After students have counted each type of atom, review their answers to make sure they know how to interpret subscripts and coefficients

What is the 5-E format?

The 5-E instructional model is an approach to teaching and learning that focuses on active engagement, inquiry-based learning, and collaboration.

Simulations for Lesson 6.1

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• Lesson 6.1 Lesson Plan  PDF  |  DOCX  |  Google Doc

Resources for the entire Chapter 6

• Chapter 6 Student Reading  PDF  |  DOCX  |  Google Doc
• Chapter 6 Test Bank  PDF  |  DOCX  |  Google Doc

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• Lesson 6.1 Online Assignments  Google Form

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This lesson is part of:  Chapter 6: Chemical Change

Lesson 5.9: Temperature Changes in Dissolving

Lesson 6.2: Controlling the Amount of Products in a Chemical Reaction

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Historical overview

• The conservation of matter
• Energy considerations
• Kinetic considerations
• Gas-forming reactions
• Precipitation reactions
• Oxidation-reduction reactions
• The Arrhenius theory
• The Brønsted-Lowry theory
• The Lewis theory
• Decomposition reactions
• Substitution, elimination, and addition reactions
• Polymerization reactions
• Solvolysis and hydrolysis
• Chain reactions
• Photolysis reactions

What are the basics of chemical reactions?

What happens to chemical bonds when a chemical reaction takes place, how are chemical reactions classified.

• What are acids and bases?
• How are acids and bases measured?

chemical reaction

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• Royal Society of Chemistry - Introducing “chemical reactions”
• Chemistry LibreTexts - Chemical Reactions
• Khan Academy - Chemical reactions
• University of Hawaii pressbooks - Chemical Reactions
• CoolKidFacts.com - Chemical Reactions
• Florida State University - Department of Chemistry and Biochemistry - Chemical Reactions
• BCcampus Open Publishing - Enthalpy and Chemical Reactions
• chemical reaction - Student Encyclopedia (Ages 11 and up)
• Table Of Contents

• A chemical reaction is a process in which one or more substances, also called reactants, are converted to one or more different substances, known as products. Substances are either chemical elements or compounds .
• A chemical reaction rearranges the constituent atoms of the reactants to create different substances as products. The properties of the products are different from those of the reactants.
• Chemical reactions differ from physical changes, which include changes of state, such as ice melting to water and water evaporating to vapor. If a physical change occurs, the physical properties of a substance will change, but its chemical identity will remain the same.

According to the modern view of chemical reactions, bonds between atoms in the reactants must be broken, and the atoms or pieces of molecules are reassembled into products by forming new bonds. Energy is absorbed to break bonds, and energy is evolved as bonds are made. In some reactions the energy required to break bonds is larger than the energy evolved in making new bonds, and the net result is the absorption of energy. Hence, different types of bonds may be formed in a reaction. A Lewis acid-base reaction , for example, involves the formation of a covalent bond between a Lewis base, a species that supplies an electron pair, and a Lewis acid, a species that can accept an electron pair. Ammonia is an example of a Lewis base. A pair of electrons located on a nitrogen atom may be used to form a chemical bond to a Lewis acid.

Chemists classify chemical reactions in a number of ways: by type of product, by types of reactants, by reaction outcome, and by reaction mechanism. Often a given reaction can be placed in two or even three categories, including gas -forming and precipitation reactions. Many reactions produce a gas such as carbon dioxide , hydrogen sulfide , ammonia , or sulfur dioxide . Cake batter rising is caused by a gas-forming reaction between an acid and baking soda (sodium hydrogen carbonate). Classification by types of reactants include acid-base reactions and oxidation-reduction reactions , which involve the transfer of one or more electrons from a reducing agent to an oxidizing agent. Examples of classification by reaction outcome include decomposition, polymerization , substitution , and elimination and addition reactions. Chain reactions and photolysis reactions are examples of classification by reaction mechanism, which provides details on how atoms are shuffled and reassembled in the formation of products.

chemical reaction , a process in which one or more substances, the reactants , are converted to one or more different substances, the products. Substances are either chemical elements or compounds . A chemical reaction rearranges the constituent atoms of the reactants to create different substances as products.

Chemical reactions are an integral part of technology, of culture , and indeed of life itself. Burning fuels, smelting iron , making glass and pottery , brewing beer , and making wine and cheese are among many examples of activities incorporating chemical reactions that have been known and used for thousands of years. Chemical reactions abound in the geology of Earth , in the atmosphere and oceans , and in a vast array of complicated processes that occur in all living systems.

Chemical reactions must be distinguished from physical changes. Physical changes include changes of state, such as ice melting to water and water evaporating to vapour. If a physical change occurs, the physical properties of a substance will change, but its chemical identity will remain the same. No matter what its physical state, water (H 2 O) is the same compound , with each molecule composed of two atoms of hydrogen and one atom of oxygen . However, if water, as ice, liquid, or vapour, encounters sodium metal (Na), the atoms will be redistributed to give the new substances molecular hydrogen (H 2 ) and sodium hydroxide (NaOH). By this, we know that a chemical change or reaction has occurred.

The concept of a chemical reaction dates back about 250 years. It had its origins in early experiments that classified substances as elements and compounds and in theories that explained these processes. Development of the concept of a chemical reaction had a primary role in defining the science of chemistry as it is known today.

The first substantive studies in this area were on gases . The identification of oxygen in the 18th century by Swedish chemist Carl Wilhelm Scheele and English clergyman Joseph Priestley had particular significance. The influence of French chemist Antoine-Laurent Lavoisier was especially notable, in that his insights confirmed the importance of quantitative measurements of chemical processes. In his book Traité élémentaire de chimie (1789; Elementary Treatise on Chemistry ), Lavoisier identified 33 “elements”—substances not broken down into simpler entities. Among his many discoveries, Lavoisier accurately measured the weight gained when elements were oxidized, and he ascribed the result to the combining of the element with oxygen . The concept of chemical reactions involving the combination of elements clearly emerged from his writing, and his approach led others to pursue experimental chemistry as a quantitative science.

The other occurrence of historical significance concerning chemical reactions was the development of atomic theory . For this, much credit goes to English chemist John Dalton , who postulated his atomic theory early in the 19th century. Dalton maintained that matter is composed of small, indivisible particles, that the particles, or atoms , of each element were unique, and that chemical reactions were involved in rearranging atoms to form new substances. This view of chemical reactions accurately defines the current subject. Dalton’s theory provided a basis for understanding the results of earlier experimentalists, including the law of conservation of matter (matter is neither created nor destroyed) and the law of constant composition (all samples of a substance have identical elemental compositions).

Thus, experiment and theory, the two cornerstones of chemical science in the modern world, together defined the concept of chemical reactions. Today experimental chemistry provides innumerable examples, and theoretical chemistry allows an understanding of their meaning.

Basic concepts of chemical reactions

When making a new substance from other substances, chemists say either that they carry out a synthesis or that they synthesize the new material. Reactants are converted to products, and the process is symbolized by a chemical equation . For example, iron (Fe) and sulfur (S) combine to form iron sulfide (FeS). Fe(s) + S(s) → FeS(s) The plus sign indicates that iron reacts with sulfur. The arrow signifies that the reaction “forms” or “yields” iron sulfide, the product. The state of matter of reactants and products is designated with the symbols (s) for solids , (l) for liquids , and (g) for gases .

• Chemical Reactions and Equations
• Types Of Chemical Reactions

Types of Chemical Reactions

Table of Contents

Recommended videos, different types of chemical reactions, example problem, frequently asked questions – faqs.

Different Types of Chemical Reactions – Combination, Decomposition, Combustion, Neutralization & Displacement Reactions

Also, check ⇒  Chemistry Concept Questions and Answers

Chemical Reactions and Equations – Types of Chemical Reactions

Types Of Organic Reactions

The 5 primary types of chemical reactions are:

• Combination reaction
• Decomposition reaction
• Displacement reaction
• Double Displacement reaction
• Precipitation Reaction

1. Combination Reaction

• A reaction in which two or more reactants combine to form a single product is known as a combination reaction.
• It takes the form of X + Y → XY
• Combination reaction is also known as a synthesis reaction.
• Example of combination reaction: 2Na + Cl 2  → 2NaCl

Related Video

Combination reactions.

2. Decomposition Reaction

• A reaction in which a single compound breaks into two or more simpler compounds is known as a decomposition reaction.
• It takes the form of XY → X + Y
• A decomposition reaction is just the opposite of a combination reaction.
• Example of a decomposition reaction: CaCO 3  → CaO + CO 2
• The reaction in which a compound decomposes due to heating is known as a thermal decomposition reaction.

3. Displacement Reaction

• A chemical reaction in which a more reactive element displaces a less reactive element from its aqueous salt solution.
• It takes the form X + YZ → XZ + Y
• It is also called a substitution reaction
• Example of displacement reaction: Zn + CuSO 4  → ZnSO 4 + Cu

4. Double Displacement Reaction

• A chemical reaction in which ions get exchanged between two reactants which form a new compound is called a double displacement reaction.
• It takes the form of XY + ZA → XZ + YA
• It is also called a metathesis reaction
• Example of double displacement reaction:

\(\begin{array}{l}~~~~~~~~~~~\end{array} \) BaCl 2 + Na 2 SO 4  → BaSO 4 + 2NaCl

5. Precipitation Reaction

• A chemical reaction that involves the formation of an insoluble product (precipitate; solid) is called Precipitation reaction.
• The reactants are soluble, but the product formed would be insoluble and separates out as a solid.
• The chemical equation by which a chemical change is described is adequate for reaction in solutions, but for reactions of ionic compounds in aqueous solution (water), the typical molecular equation has different representations.
• A molecular equation may indicate formulas of reactants and products that are not present and eliminate completely the formulas of the ions that are the real reactants and products.
• If the substance in the molecular equation that is actually present as dissociated ions are written in the form of their ions, the result is an ionic equation.

A precipitation reaction occurs when a solution, originally containing dissolved species, produces a solid, which generally is denser and falls to the bottom of the reaction vessel.

The most common precipitation reactions occurring in aqueous solution involve the formation of an insoluble ionic compound when two solutions containing soluble compounds are mixed. Consider what happens when an aqueous solution of NaCl is added to an aqueous solution of AgNO 3 . The first solution contains hydrated Na + and Cl − ions and the second solution, Ag + , and NO 3 − ions.

NaCl(s) → Na + (aq) + Cl − (aq)

AgNO 3 (s) → Ag + (aq) + NO 3 − (aq)

When mixed, a double displacement reaction takes place, forming the soluble compound NaNO 3 and the insoluble compound AgCl. In the reaction vessel, the Ag + and Cl − ions combine, and a white solid precipitated from the solution. As the solid precipitates, the Na + and NO 3 − ions remain in solution.

The overall double displacement reaction is represented by the following balanced equation:

NaCl(aq) + AgNO 3 (aq) → AgCl(s) + NaNO 3 (aq)

• When aqueous solutions of Pb(NO 3 ) 2 and KI are mixed, does a precipitate form?
• Write a balanced equation for the precipitation reaction that occurs when aqueous solutions of copper(II) iodide and potassium hydroxide are combined.

You are asked to predict whether a precipitate will form during a chemical reaction and to write a balanced equation for a precipitation reaction.

You are given the identity of two reactants.

1. Yes, a solid precipitate, PbI 2 , forms when these solutions are mixed:

Pb(NO 3 ) 2 (aq) + KI(aq)  → PbI 2 (s) + 2KNO 3 (aq)

2. The two products of the reaction are insoluble copper (II) hydroxide and soluble potassium  iodide.

How do you identify a chemical reaction?

A chemical reaction is typically followed by physical signs that are readily detected, such as heat and light emission, precipitate formation, gas evolution, or a change of appearance.

How do you identify physical and chemical changes?

The shape or form of the matter varies through a physical transition, but the sort of matter in the material does not. In a chemical shift, however, the type of matter shifts and at least one new material with new properties is created. There is no straight cut of the gap between physical and chemical transition.

Why do we write a chemical equation?

The purpose of writing a balanced chemical equation is to explain the occurring reactants (starting material) and products (end results). The ratios in which they answer so that you can measure the amount of reactants you need and the amount of goods you can make.

What is chemical reaction and equation?

A chemical equation is the symbolic representation in the form of symbols and formulas of a chemical reaction in which the reactant entities on the left-hand side and the product entities on the right-hand side are given.

What is the skeleton equation?

A skeleton equation is when each product that takes part in the reaction is written with the chemical formulas describing the chemical reaction. Examples: The term equation: oxygen + methane. Dioxide with carbon + Vapour.

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Resource Type: Virtual Labs

The Virtual Lab is an online simulation of a chemistry lab. It is designed to help students link chemical computations with authentic laboratory chemistry. The lab allows students to select from hundreds of standard reagents (aqueous) and manipulate them in a manner resembling a real lab. More information and offline downloads . Please scroll below to find our collection of pre-written problems, they have been organized by concept and ranked by difficulty.

Stoichiometry

The mole, molarity, and density, glucose dilution problem.

In this activity, students use the virtual lab to create a 0.025M glucose solution from a standard 1M glucose solution. First, they calculate the correct volumes of 1M glucose solution and water to mix together…

Acid Dilution Problem

In this activity, students use the virtual lab to create 500mL of 3M HCl solution from a concentrated stock solution of 11.6M HCl. They must first calculate the correct volumes of 11.6M HCl solution and water to…

Cola and Sucrose Concentration Problem

In this activity, students use the virtual lab to prepare a sucrose solution for a soda recipe. They next calculate the concentration of their solution in terms of molarity, percent mass and density. Finally, they…

Making Stock Solutions from Solids

In this activity, students use the virtual lab to create stock solutions starting from solid salts. Students must first calculate the correct amount of solid to make the solution. Next, they prepare the solution…

Identifying the Unknown Metal (Metals Density Problem)

In this activity, students use the virtual lab to identify an unknown metal by measuring its density and comparing their measurements to the densities of known metals.

Identifying an Unknown Liquid from its Density

In this activity students use the virtual lab to design an experiment to determine the identity of mislabeled bottles using the densities of the solutions inside.

Alcohol Density Problem

Determine the concentration of an alcohol solution from its density.

Reaction Stoichiometry and Limiting Reagents

Gravimetric determination of arsenic.

Set in the context of ground water contamination in Bangladesh, this stoichiometry and analytical chemistry activity examines the issues around identifying wells contaminated with arsenic. (Part of a larger online…

Determining Stoichiometric Coefficients

In this activity, students use the virtual lab to determine how 4 unknown substances react with each other including their stoichiometric coefficients.

Stoichiometry and Solution Preparation Problem

In this limiting reagents problem, students mix together solutions in different ratios in an attempt to produce a final solution that contains only 1 product.

Textbook Style Limiting Reagents Problems

Textbook-style practice limiting reagent exercises with that can be used as a way to "predict and check" your answers using the virtual lab.

Textbook Style Limiting Reagents Problem II

In this activity, students practice with experiments involving limiting reagents and the test their knowledge to determine the concentration of an unknown solution.

Predicting DNA Concentration

In this limiting reagents problem, students are given specific concentrations of DNA solutions and are asked to predict what products and reactants will remain after a specific volumes are mixed and reaction has…

Unknown Concentration of DNA Solution Problem

In this advanced limiting reagent problem, students use the virtual lab to determine the concentration of a solution of DNA by reacting it with known amounts of a fluorescent dye which binds to the DNA.

Thermochemistry

Energy and enthalpy, camping problem i.

In this part of the MRE scenario, students measure the enthalpy of a reaction.

Camping Problem II

In this part of the MRE scenario, students determine change in the enthalpy of a reaction as the concentration of reactants are varied.

ATP Reaction (Thermochemistry and Bonding)

Determine the enthalpy of the ATP reaction.

Determining the Heat of Reaction in Aqueous Solution

In this activity, students perform an experiment to determine the heat of a reaction.

Coffee Problem

Use the virtual lab to determine how much milk to add to hot coffee to reach the desired temperature

Measuring the heat capacity of an engine coolant.

As an analytical chemist at a company developing new engine coolants your task is to determine the heat capacity of a newly developed product and then to determine if its heat capacity is greater of less than that…

Measuring the heat capacity of an engine coolant II (Advanced version)

Measure and compare the heat capacity of an unknown liquid with an unknown density.

Camping Problem III

In this part of the MRE scenario, students create solutions that when mixed, increase to a certain temperature.

Heats of Reaction - Hess' Law

This activity provides a demonstration of Hess' Law using three reactions: the solubility NaOH in water, the solubility NaOH in HCl and the reaction of a solution of HCl and a solution of NaOH.

Equilibrium

Lechatlier's principle, cobalt chloride and lechatlier’s principle.

In this activity, students safely explore the equilibrium reaction of the cobalt chloride reaction.

Equilibrium Calculations

Dna binding problem.

In this activity, students explore equilibrium constants in biochemical systems by measuring the binding constant of a DNA-Dye reaction.

Acid-Base Chemistry

Strong acids and bases, strong acid and base problems.

Textbook-style strong acid and base problems that can be checked using the Virtual Lab.

Determination of the pH Scale by the Method of Successive Dilutions

This activity was created as an accompaniment to an in-class demonstration of the method of successive dilutions using HCl, NaOH, a pH meter, and universal indicator solution. After the demonstration, students…

Weak Acids and Bases

Weak acid and base problems.

Textbook-style weak acid and base problems that can be checked using the Virtual Lab.

Determining the pKa and Concentration Ratio of a Protein in Solution

Use the virtual lab to determine the pKa of a protein then create a buffer solution with a specific concentration ratio of the protein in its protonated/ unprotonated form.

Unknown Acid and Base Problem

In this exercise, students graph the titration curve of an unknown acid and base to determine their pKa’s and concentrations.

Buffer Solutions

Creating a buffer solution.

An exercise to design a buffer solution with specific properties.

DNA - Dye Binding: Equilibrium and Buffer Solutions

Students examine equilibrium and buffer solutions in a biological setting.

Acid/Base Titrations

Standardization of naoh with a khp solution: acid base titration.

Use the Virtual Laboratory to standardize an unknown NaOH solution (approximately 0.2M) to four significant figures via titration with 25.00 mL of a KHP standard solution.

Solubility Product

Determining the solubility product.

Determine the solubility product constatnt (Ksp) for various solids.

Temperature and the Solubility of Salts

Examine the solubilities of salts based on temperature.

Determining the solubility of copper chloride at different temperatures

GIven the solubility of CuCl at 2 different temperatures, predict its solubility at a third temperature. Then test your prediction by creating the solution in the virtual lab

Oxidation/Reduction and Electrochemistry

Standard reduction potentials, exploring oxidation-reduction reactions.

Design an experiment to order Cu, Mg, Zn and Pb from strongest to weakest reducing agent.

Analytical Chemistry/Lab Techniques

Gravimetric analysis, unknown silver chloride.

Determine the concentration of Silver ion in a Silver Nitrate solution using gravimetric analysis

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Examples of Chemical Reactions in Everyday Life

ThoughtCo / Emily Roberts

• Chemistry In Everyday Life
• Chemical Laws
• Periodic Table
• Projects & Experiments
• Scientific Method
• Biochemistry
• Physical Chemistry
• Medical Chemistry
• Famous Chemists
• Activities for Kids
• Abbreviations & Acronyms
• Weather & Climate
• Ph.D., Biomedical Sciences, University of Tennessee at Knoxville
• B.A., Physics and Mathematics, Hastings College

Chemistry happens in the world around you, not just in a lab. Matter interacts to form new products through a process called a chemical reaction or chemical change. Every time you cook or clean, it's chemistry in action. Your body lives and grows thanks to chemical reactions. There are reactions when you take medications, light a match, and draw a breath. 

These examples of chemical reactions from everyday life are a small sampling of the hundreds of thousands of reactions you experience as you go about your day.

Key Takeaways: Chemical Reactions in Everyday Life

• Chemical reactions are common in daily life, but you may not recognize them.
• Look for signs of a reaction. Chemical reactions often involve color changes, temperature changes, gas production, or precipitant formation.
• Simple examples of everyday reactions include digestion, combustion, and cooking.

What Is a Chemical Reaction?

A chemical change , often called a chemical reaction , occurs when substances transform into new and distinct substances. Essentially, it involves the rearrangement of atoms. Generally, chemical changes can be identified by temperature changes, light emission, bubble formation, precipitate formation, color changes, and odor release. These effects signify a change in composition, but they may not always be immediately apparent.

Usually, chemical changes are permanent, so they cannot be undone. Conversely, physical changes do not create new substances and can be reversed. Understanding these distinctions is fundamental to the study of chemistry .

Photosynthesis

Frank Krahmer / Getty Images

Plants apply a  chemical reaction  called photosynthesis to convert  carbon dioxide  and water into food (glucose) and oxygen. It's one of the most  common everyday chemical reactions  and also one of the most important because this is how plants produce food for themselves (and animals) and convert carbon dioxide into oxygen. The equation for the reaction is:

6 CO 2  + 6 H 2 O + light → C​ 6 H 12 O 6  + 6 O 2

Aerobic Cellular Respiration

Kateryna Kon/Science Photo Library / Getty Images

Aerobic cellular respiration  is the opposite process of photosynthesis in that energy molecules are combined with the oxygen we breathe to release ​the energy needed by our cells plus carbon dioxide and water. Energy used by cells is chemical energy in the form of ATP, or adenosine triphosphate .

Here is the overall equation for aerobic cellular respiration:

C 6 H 12 O 6  + 6O 2  → 6CO 2  + 6H 2 O + energy (36 ATPs)

Anaerobic Respiration

Tastyart Ltd Rob White / Getty Images

Anaerobic respiration is a  set of chemical reactions  that allows cells to gain energy from complex molecules without oxygen. Your muscle cells perform anaerobic respiration whenever you exhaust the oxygen being delivered to them, such as during intense or prolonged exercise. Anaerobic respiration by yeast and bacteria is harnessed for fermentation to produce ethanol, carbon dioxide, and other chemicals that make cheese, wine, beer, yogurt, bread, and many other common products.

The  overall chemical equation for one form of anaerobic respiration is:

C 6 H 12 O 6  → 2C 2 H 5 OH + 2CO 2  + energy

Every time you strike a match, burn a candle, build a fire, or light a grill, you see the combustion reaction. Combustion combines energetic molecules with oxygen to produce carbon dioxide and water.

For example, the equation for  the combustion reaction  of propane, found in gas grills and some fireplaces, is:

C 3 H 8  + 5O 2  → 4H 2 O + 3CO 2  + energy 

Alex Dowden/EyeEm / Getty Images

Over time, iron develops a red, flaky coating called rust. This is an  example of an oxidation reaction . Other everyday examples include the formation of verdigris on copper and the tarnishing of silver.

Here is the  chemical equation  for the rusting of iron:

Fe + O 2  + H 2 O → Fe 2 O 3 . XH 2 O

If you combine vinegar and  baking soda for a chemical volcano  or milk  with baking powder  in a recipe, you experience a  double displacement , or metathesis reaction (plus some others.) The ingredients recombine to produce  carbon dioxide gas  and water. The carbon dioxide forms bubbles in the volcano and  helps baked goods rise .

These reactions seem simple in practice but often consist of multiple steps. Here is the  overall chemical equation  for the reaction between baking soda and vinegar:

HC 2 H 3 O 2 (aq) + NaHCO 3 (aq)  → NaC 2 H 3 O 2 (aq) + H 2 O(l) + CO 2 (g)

Electrochemistry

Batteries use electrochemical or redox reactions to convert  chemical energy  into electrical energy. Spontaneous redox reactions occur  in galvanic cells , while  nonspontaneous chemical reactions  take  place in electrolytic cells .

Peter Dazeley/Photographer's Choice / Getty Images

Thousands of chemical reactions  take place during digestion. As soon as you put food in your mouth, an enzyme in your saliva called amylase starts to break down sugars and other carbohydrates into simpler forms your body can absorb.  Hydrochloric acid  in your stomach reacts with food to further break it down, while enzymes cleave proteins and fats so they can be absorbed into your bloodstream through the walls of the intestines.

Acid-Base Reactions

Lumina Imaging / Getty Images

Whenever you combine an acid (e.g., vinegar, lemon juice,  sulfuric acid , or muriatic acid ) with a base (e.g.,  baking soda , soap, ammonia, or acetone), you are performing an acid-base reaction. These reactions neutralize the acid and base to yield salt and water.

Sodium chloride isn't the only salt that can be formed. For example, here is the  chemical equation for an acid-base reaction  that produces potassium chloride, a common table salt substitute:

HCl + KOH → KCl + H 2 O

Soap and Detergent Reactions

JGI/Jamie Grill / Getty Images

Soaps and detergents clean by way of chemical reactions . Soap emulsifies grime, which means oily stains bind to the soap so they can be lifted away with water. Detergents act as surfactants, lowering the surface tension of water so it can interact with oils, isolate them, and rinse them away.

Cooking uses heat to cause chemical changes in food. For example, when you hard boil an egg, the hydrogen sulfide produced by heating the egg white can react with iron from the egg yolk to form a grayish-green ring around the yolk . When you brown meat or baked goods, the Maillard reaction between amino acids and sugars produces a brown color and a desirable flavor.

More Examples of Chemistry in Everyday Life

Chemical reactions are everywhere, and in a way, chemistry really makes up everything. From the emotions you feel to peculiar questions such as, "Can bottled water go bad?" Here are some examples of chemistry in everyday life.

• Does the Taurine in Red Bull Really Come From Bull Semen?
• The Tin Man's Toxic Metal Makeup
• Words Made Using Periodic Table Element Symbols
• Chemistry Element Jokes and Puns
• Do You Know If Milk Is an Acid or a Base?
• How to Substitute for Baking Powder and Baking Soda
• What Glows Under Black Light?
• Examples of Organic Chemistry in Everyday Life
• Why Is Chemistry Important in Everyday Life?
• Chemistry in Daily Life
• Is It Ever Safe to Drink Bleach?
• What Is Mylar?
• Canned Air Isn't Air (Chemical Composition)
• How Glow Stick Colors Work
• Examples of Endothermic Reactions
• What Is an Element in Chemistry? Definition and Examples