synthesis (combination) reaction definition

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What Is a Synthesis Reaction? Definition and Examples

A synthesis reaction is one of the four main types of chemical reactions , along with decomposition, single replacement , and double replacement reactions. Here is the synthesis reaction definition, examples of the reaction using elements and compounds, a look at how many reactants are involved, and how to recognize a synthesis reaction.

Synthesis Reaction Definition

A synthesis reaction is a chemical reaction that combines two or more simple elements or compounds to form a more complex product . A + B → AB This type of reaction is also called a direct combination reaction or simply a combination reaction. It’s the type of reaction that forms compounds from their elements. Synthesis reactions also make large molecules from smaller ones. A synthesis reaction is the opposite of a decomposition reaction , which breaks complex molecules into simpler ones.

Synthesis Reaction Examples

There are many examples of synthesis reactions. Some involve elements. In others, an element reacts with a compound. In still other cases, compounds react with other compounds to form larger molecules.

Synthesis Reactions Between Elements

• Iron and sulfur react to form iron sulfide. 8 Fe + S 8  → 8 FeS
• Potassium and chlorine react to form potassium chloride. 2K (s)  + Cl 2(g)  → 2KCl (s)
• Iron and oxygen react to form rust. 4 Fe (s) + 3 O 2  (g) → 2 Fe 2 O 3  (s)
• Hydrogen reacts with oxygen to form water. 2 H 2 (g) + O 2 (g) → 2 H 2 O(g)

Synthesis Reactions Between an Element and a Compound

• Carbon monoxide reacts with oxygen to form carbon dioxide. 2 CO(g) + O 2 (g) → 2CO 2 (g)
• Nitric oxide reacts with oxygen to form nitrogen dioxide. 2NO + O 2  → 2NO 2
• CH 2 CH 2 (g) + Br 2 (ℓ) → CH 2 BrCH 2 Br

Synthesis Reactions Between Compounds

• Sulfur oxide reacts with water to form sulfuric acid. SO 3  (g) + H 2 O (l) → H 2 SO 4  (aq)
• Calcium oxide reacts with water to form calcium hydroxide. 2CaO (s) + 2H 2 O (l) → 2Ca(OH) 2 (aq)
• Iron oxide and sulfur oxide react to form iron sulfate. Fe 2 O 3  + 3SO 3  → Fe 2 (SO 4 ) 3

How Many Reactants Are There?

Usually, there are two reactants in a synthesis reaction. They could be two elements, an element and a compound, or two compounds. However, sometimes more reactants combine to form a product. Here are examples of synthesis reactions involving three reactants:

• Sodium carbonate reacts with water and carbon dioxide to form sodium bicarbonate. Na 2 CO 3  + H 2 O + CO 2 → 2NaHCO 3
• Nitrogen reacts with water and oxygen to form ammonium nitrate. 2N 2 (g) + 4H 2 O(g) + O 2 (g) → 2NH 4 NO 3 (s)

How to Recognize a Synthesis Reaction

The easiest way to recognize a synthesis reaction is to look for a reaction where multiple reactants produce a single product. However, sometimes a synthesis reaction equation includes multiple products and reactants. A good example is the overall reaction for photosynthesis, in which carbon dioxide and water combine to form glucose and oxygen. CO 2  + H 2 O → C 6 H 12 O 6  + O 2 But, even in this case, two simpler molecules react to form a more complex one. So, this is the key in synthesis reaction identification.

Some synthesis reactions form predictable products. If you recognize them, it’s easy to recognize the reaction type:

• Reacting two elements forms a binary compound. For example, hydrogen and oxygen react to form water.
• When two nonmetals react, more than one product is possible. For example, sulfur and oxygen react to form sulfur dioxide or sulfur trioxide.
• Alkali metals react with nonmetals to form ionic compounds. For example, sodium and chlorine form sodium chloride.
• Transition metals react with nonmetals to form more than one possible product. To predict the product, you need to know the oxidation state (charge) or the metallic cation.
• Nonmetal oxides react with water to form acids. For example sulfur dioxide reacts with water to make sulfurous acid.
• Metallic oxides react with water to form bases.
• Nonmetal oxides react with one another to form salts.

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Synthesis Reactions — Definition & Examples - Expii

Combination Reaction Definition

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A combination reaction is a reaction where two reactants are combined into one product . A combination reaction is also known as a synthesis reaction . The reaction has the following general form:

X + Y → XY

Combination Reaction Examples

Recognize a combination reaction by examining the number of reactants and products. In this reaction, two reactants become a single product. Combination reaction may occur between two elements, two compounds, or between a compound and an element.

The burning of carbon in the presence of oxygen to produce carbon dioxide is a combination reaction:

C + O 2 → CO 2

Magnesium oxide combines with carbon dioxide to form magnesium carbonate in a combination reaction:

MgO + CO 2 → MgCO 3

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Synthesis Reactions

Synthesis reactions, also known as combination reactions, are chemical reactions in which two or more reactants combine to form a single product. This type of reaction is represented by the general equation: A + B → AB

Formation of a new substance: Synthesis reactions result in creating a new compound or molecule from simpler reactants.

Energy absorption: These reactions often require an input of energy, typically in the form of heat or light, to initiate the reaction.

Common examples of synthesis reactions include the formation of water (2H 2 + O 2 → 2H 2 O), the synthesis of ammonia (3H₂ + N₂ → 2NH₃), and photosynthesis (6CO 2 + 6H 2 O → C 6 H 12 O 6 + 6O 2 + 6H 2 ).

Whats the Difference between synthesis and combination reaction?

Direct combination reaction : the reaction in which two or more substances combine to form a single substance is called direct combination reaction. synthesis reaction: the reaction in which two or more elements combine to form a compound is called direct combination reaction. → → combination reaction is also known as synthesis reaction because in these reactions, two or more substances chemically combine to form a new compound..

How do synthesis reactions differ from Combination reactions?

State why a direct combination reaction is called a synthesis reaction.

Are combination and synthesis reactions the same thing?

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Chapter 4: Chemical Quantities and Aqueous Reactions

Back to chapter, synthesis and decomposition reactions, previous video 4.12: acids, bases and neutralization reactions.

Generally, in a chemical reaction, molecules interact by breaking one set of bonds and forming a new set of bonds. 

A redox, or oxidation–reduction, reaction is a type of chemical reaction involving the partial or complete transfer of electrons. In such reactions, one reactant is oxidized and the other is reduced, with an observable change in their oxidation states. 

The oxidized element, which has lost electrons, undergoes an increase in oxidation state. The reduced element, which has gained electrons, undergoes a decrease in oxidation state.

Among the most common redox reactions are synthesis and decomposition reactions. The synthesis of proteins from different amino acids and the digestion of proteins into amino acids are important examples.

Synthesis, or combination, reactions involve the formation of bonds between reactants to create a single product. The reactants may include only elements, elements and compounds, or only compounds. 

Examples are the combination of elemental hydrogen and oxygen to create water, the addition of carbon monoxide to elemental oxygen to form carbon dioxide, and the combination of calcium oxide and water to form calcium hydroxide.

Notice that in all cases, multiple simpler reactants combined into a single complex product.

A decomposition reaction is the opposite of a synthesis reaction. In decomposition reactions, a single complex reactant breaks down into simpler products like elements, elements and compounds, or just compounds. 

Decomposition reactions require an input of some form of energy. For example, under the influence of an electric field, water breaks down to give hydrogen and oxygen.

In the presence of sunlight, hydrogen peroxide decomposes into oxygen and water. Similarly, calcium hydroxide, upon being heated, decomposes into calcium oxide and water.

Synthesis and decomposition are two types of redox reactions. Synthesis means to make something, whereas decomposition means to break something. The reactions are accompanied by chemical and energy changes. 

Synthesis Reactions

Synthesis reactions are also called combination reactions. It is a reaction in which two or more substances combine to form a complex substance. Synthesis reactions are generally represented as: A + B → AB or A + B → C. The formation of nitrogen dioxide is a synthesis reaction: 2 NO ( g ) + O 2 ( g ) → 2 NO 2 ( g ).

In synthesis reactions, the reactants could be all elements (1), or a combination of an element and a compound (2), or all compounds (3).

1) C ( s ) + O 2 ( g ) → CO 2 ( g )     2) 2 CO ( g ) + O 2 ( g ) → 2 CO 2 ( g )  3) 2 CaO ( s ) + 2 H 2 O ( l ) → 2 Ca(OH) 2 ( s )

A combination reaction between a metal and a nonmetal always produces an ionic solid. For example, the formation of sodium chloride or table salt from sodium and chlorine is a combination reaction: 2 Na (s) + Cl 2 ( g ) → 2 NaCl ( s ).

A synthesis reaction is generally accompanied by the release of energy. In the above example of sodium chloride, 787 kJ of heat energy is released. 

Decomposition Reactions

Oxygen was first discovered by the scientist Joseph Priestley, in 1774, by heating mercury oxide with a burning glass. The reaction was a result of decomposition. Priestley had broken down mercury(II) oxide with heat into its elements.  The reaction is represented as: 2 HgO ( s ) → 2 Hg ( l ) + O 2 ( g )

Decomposition reactions involve breaking down a more complex substance into two or more smaller substances. This reaction is often represented as: AB → A + B or C → A + B. Decomposition reactions occur everywhere. For instance, the digestion of proteins, fats, and carbohydrates in our food is an important decomposition reaction. Another example is the decomposition of sodium azide into nitrogen gas. 

The reaction is represented as: 2 NaN 3 ( s ) → 2 Na ( s ) + 3 N 2 ( g )

In the above reaction, although the coefficient 2 indicates two molecules of sodium azide being decomposed, there is only one reactant. It is, therefore, a decomposition reaction. Similar to the synthesis reaction, in a decomposition reaction, the products formed could be all elements (1), or a combination of elements and compounds (2), or all compounds (3).

1)    2 Al 2 O 3 ( s ) → 4 Al ( s ) + 3 O 2 ( g ) 2)    2 KClO 3 ( s ) → 2 KCl ( s ) + 3 O 2 ( g ) 3)    NH 4 Cl ( s ) → NH 3 ( g ) + HCl ( g )

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Combination Reaction

Combination Reaction is a type of chemical reaction that occurs when two or more substances combine to form a new substance without any separate byproducts, due to that, it is also called an Addition Reaction or Synthesis Reaction. Combination Reaction involves the synthesis of a single compound from its constituent elements or other compounds.

This article covers the concepts related to combination reaction, like the formula of combination reaction, types of combination reaction, synthesis, cause, examples and real-life examples of combination reaction.

Table of Content

What is a Combination Reaction?

Cause of combination reaction, example of combination reactions, properties of combination reaction, types of combination reactions, real-life examples of combination reaction.

A process in which two or more chemicals combine to create a single new substance is known as a combination reaction. Synthesis reactions are another name for combination reactions.

Generally, in any combination reaction reactants A and B, combine to form the product, which is AB. There is no restriction on the quantity of reactants that can participate in combination reactions. Moreover, a combination reaction forms a new bond between the reactant molecules, which releases heat and makes the reaction generally exothermic.

Definition of Combination Reaction

A process in which two or more chemicals combine to create a single new substance is known as a combination reaction.

Chemical Equation for Combination Reaction

General chemical equation for combination or addition reaction is give by:

Read More about Types of Chemical Reaction .

In a chemical reaction , components or compounds come together to generate a result. In order to achieve stability, every element or compound participates in a chemical combination. According to Lewis theory, an atom becomes stable when it assumes the configuration of a noble gas .

As a result, atoms share electrons during a chemical reaction and establish a stable electronic configuration. Chemical combination is therefore caused by an atom’s tendency to acquire stability through the formation of a noble gas configuration.

Some of common examples of Combination Reactions are:

• Formation of Sodium Cholride

Formation of Magnesium Oxide

Formation of barium fluoride, formation of ammonia.

• Formation of Other Substances

Formation of Sodium Chloride

Solid sodium metal reacts with chlorine gas to form sodium chloride.

2Na(s)+Cl 2 (g)→2NaCl(s)

When magnesium is lit, it reacts rapidly, combining with oxygen in the air to form a fine powder known as magnesium oxide.

2Mg(s)+O 2 (g)→2MgO(s)

Formed by the combination of barium metal and fluorine gas is a highly exothermic reaction.

Ba(s) + F 2 (g) → BaF 2 (s)

Hydrogen and nitrogen gas combines to form ammonia.

3H 2 + N 2 → 2NH 3

Formation of Some Other Substances

Some other subtance that are formed with the help of combination reaction are listed as follows:

• When sulfur dioxide gas reacts with oxygen gas, sulfur trioxide is produced.

2SO₂(g) + O₂(g) → 2SO₃(g)

• Iron reacts with oxygen to form iron(III) oxide, commonly known as rust.

4Fe(s) + 3O₂(g) → 2Fe₂O₃(s)

• The reaction between calcium oxide and water produces calcium hydroxide.

CaO(s) + H₂O(l) → Ca(OH)₂(aq)

Some properties of combination or addition reaction are:

• Reactants can participate in a chemical reaction in combination reactions in an infinite number.
• An ionic solid is always the final result of a combination reaction involving a metal and a non-metal.
• Elements or compounds combine together to attain stability.

There are 3 ways in which a combination reaction can take place.

Combination of Two or More Elements

Combination of two or more compounds, combination of a compound with an element.

This type of combination reaction takes place when two or more elements combine together and form a single compound.

• Hydrogen and oxygen combine to form water.

H 2 (g) + O 2 (g) → 2H 2 O(l)

• Carbon and oxygen combine to form Carbon Dioxide gas.

C(g) + O 2 (g) → CO 2 (g)

This type of combination reaction takes place when two or more compounds combine together and form a single compound.

Example: The formation of calcium hydroxide (slaked lime) by the reaction of calcium oxide (quick lime) and water.

CaO(s) + H 2 O(l) → Ca(OH) 2 (s)

This type of combination reaction takes place when compound react with an element to form a single compound.

Example: Formation of Carbon Dioxide gas from the compound carbon monoxide and the element oxygen

2CO(g) + O 2 (g) → 2CO 2 (g)

• Redox Reaction
• Decomposition Reaction
• Neutralization Reaction

Some real life examples of combination reaction are listed as follows:

• When it rains, pollutants in our environment, such as sulfur oxide, interact with the rainwater to generate sulfuric acid. As a result, some acidic materials are present in the rainwater.
• During dental treatment, a white powder known as calcium hydroxide can be used to fill a root canal. A combined reaction between calcium oxide and water produces calcium hydroxide. Applications for calcium hydroxide include food processing, paper manufacturing, and sewage treatment.
• Burning coal is a combustion reaction, and carbon dioxide is the byproduct of all combustion reactions.

Steps to Determine a Combination Reaction

To determine any reaction is a combination reaction or not, we can use the following steps:

Step 1: Identify if there is a single product in the reaction. Step 2: Look for multiple reactants involved in the reaction. Step 3: Double-check to ensure nothing is overlooked by carefully reviewing each potential answer twice.

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• Balancing Chemical Reaction
• Rate of Reaction

Sample Question on Combination Reaction

Question 1: Because potassium is an extremely reactive alkali metal, it needs to be kept submerged in oil to keep from interacting with the air. Write the balanced chemical equation for the potassium-oxygen combination process.

The chemical equation according to the question: K(s)+O 2 (g)→K 2 O(s) Balanced chemical equation will be: 4K(s)+O 2 (g)→2K 2 O(s)

Question 2: Write combination reaction for the formation of aluminum oxide (Al 2 O 3 ).

Chemical balance equation for formation of aluminum oxide (Al 2 O 3 ) is given as follows: 4Al + 3O 2 → 2Al 2 O 3

Question 3: When Ag is exposed to air it gets a black coating of?

A black layer of silver sulfide is created when silver is exposed to air and reacts with the hydrogen sulfide gas in the atmosphere. In every solvent, silver sulfide remains insoluble.

Combination Reaction: Practice Questions

Q1: What white powder forms on burning magnesium in air?

Q2: What does the combination of nitrogen and hydrogen gas formed?

Q3: Write balanced combination reaction for photosynthesis.

Q4: Explain the formation of ferrous sulphide with balanced chemical reaction.

Q5: Write chemical reaction for formation of slaked lime.

Combination Reaction: FAQs

1. what is combination or addition reaction.

Combination or addition reaction involves two or more substances combining to form a new compound.

2. What are the 4 Types of Chemical Reactions?

The four types of chemical reactions are synthesis, decomposition, single replacement, and double replacement.

3. What are some Other name for Combination Reaction?

Combination reaction is also called synthesis or composition reaction.

4. Is Combination Reaction Exothermic or Endothermic?

The exothermic or endothermic nature of a combination reaction depends on the specific reaction.

5. What is the General Formula for Combination Reaction?

There is no single general formula for combination reactions as they vary based on the specific substances involved, but for two subtance combining together we can write the general formula as: A + B → AB

6. What are Some Examples of Combination Reaction?

Examples of combination reactions include the formation of water (2H₂ + O₂ → 2H₂O) and the synthesis of ammonia (N₂ + 3H₂ → 2NH₃).

7. Is Photosynthesis is Combination Reaction?

No, Photosynthesis is neither combination nor decomposition reaction as there are two product and two reactant as well. 6CO 2  + 6H 2 O → C 6 H 12 O 6  + 6O 2

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• Synthesis Reaction

For millennia, all the way back to Ancient Egypt, alchemists have been attempting to synthesize gold from more common metals like lead. While their attempts always failed, the scientists of today have been able to do the impossible: make gold (though in a very, very  expensive way).

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What is a synthesis reaction?

What is the basic structure for a synthesis reactions?

True or False: A synthesis can form an element or compound

True or False: Synthesis reactions only have 2 reactants

True or False: Synthesis reactions only make one (unique) product

Which of the following is NOT a synthesis reaction?

Which of the following is NOT possible for synthesis reaction?

What are the differences between a synthesis reaction and the synthesis performed in organic chemistry?

What is a single replacement reaction?

What is the difference between single-replacement reactions and synthesis reactions?

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In 1980, Glenn Seaborg was able to "steal" protons and neutrons from bismuth, which did produce several thousand atoms of gold. However, this method was much too expensive for gold to be made this way.

While he was able to make gold, he didn't "synthesize" it in the traditional sense. In this article, we will be learning all about the synthesis reaction . After reading this article, you'll see why the alchemists dream of synthesizing gold was always destined to fail.

• This article cover the topic synthesis reactions.
• First, we will define what a synthesis reaction is .
• Next, we will look at the basic chemical equation for a synthesis reaction.
• Then, we will look at some different examples of these reactions.
• After that, we will summarize the characteristics of the synthesis reaction.
• Lastly, we will compare and contrast these reactions with another type of reaction called single replacement.

Synthesis reaction definition

• A synthesis reaction (also called a combination reaction) is a reaction where two or more elements or compounds combine to form a new compound.

A key characteristic about synthesis reactions is that they only make one unique product. However, there can be multiple of that product produced.

As discussed in the intro, it is impossible to (traditionally) synthesis gold. Why? Because it is an element. When elements react, they will always form compounds.

There are ways for elements to combine to form other elements, but these methods are different from your typical reaction. For example, the sun fuses hydrogen nuclei into helium atoms by essentially smashing the nuclei together at very high temperatures.

Synthesis reaction chemical equation

All synthesis reactions follow this basic formula:

$$A + B \rightarrow AB$$

The basic structure is two (or more) elements and compounds combining to create one product.

Let's look at some examples, shall we?

Synthesis reaction examples

Let's have a look at some synthesis reaction examples to fully understand what synthesis reactions are and how they are represented.

First up, let's look at the synthesis of salt:

$$2Na_{(s)} + Cl_{2\,(g)} \rightarrow 2NaCl_{(s)}$$

As you can see, we have two elements (chlorine is naturally diatomic) forming one. Even though chlorine is a gas, it still forms a solid product. Synthesis reactions (and all reactions for that matter) don't always form a product of the same state as the reactants, so keep your eyes on the states listed in the equation.

Now let's look at a more complex example:

Here we have two compounds forming a product instead of elements. As long as one product is formed, it is a synthesis reaction, whether it is formed from elements or compounds.

$$CaO_{(s)} + H_2O_{(l)} \xrightarrow {heat} Ca(OH)_{2\,(aq)}$$

As a side not, the (aq) on Ca(OH) 2 means "aqueous". This means that the compound is dissolved in water. Usually, but not always, reactions that contain water will produce aqueous products.

Also, "heat" is written above the arrow to show heat is required for the reaction to proceed.

Let's look at one last example:

$$2N_{2\,(g)} + 4H_2O_{(l)} + O_{2\,(g)} \rightarrow 2NH_4NO_{3\,(s)}$$

The above reaction has 3 reactants instead of 2. While two-reactant synthesis reactions are more common, it's important to keep in mind that these reactions can have more than 2 reactants.

Characteristics of a synthesis reaction

Synthesis reactions are pretty easy to spot when you know what to look for. As a summary, here are the characteristics of a synthesis reaction:

• Have 2 or more reactants.
• Reactants can be elements and/or compounds.
• Reactants combine to form one compound.
• The compound formed is more complex than the reactant.

Synthesis reactions in Organic Chemistry

When you read up on synthesis reactions, you might encounter a different type used in Organic Chemistry .

In organic chemistry , a synthesis reaction involves taking one simple compound and transforming through a series of steps to get a much more complex compound. While they are similar, they have some key differences, such as the fact that Organic Synthesis reactions are multiple steps a nd that they can produce side products.

Synthesis reaction vs single replacement

Synthesis reactions can often be confused with another reaction called single replacement.

In a single-replacement reaction , an element will displace another element present in a compound, "swapping" with it.

A general single-replacement reaction looks like this:

$$A + BC \rightarrow AB + C$$

The lone element essentially "kicks out" the like element (i.e. metals swap with metals, non-metals swap with non-metals).

Below is an example:

Here the zinc is swapping with the copper (both are Transition Metals ).

Single replacement reactions are similar to synthesis reactions, since they involve 2 reactants coming together to form a new product. The key difference is that two products are formed instead of one. Also, this process involves swapping with synthesis involves only combining .

Synthesis Reaction - Key takeaways

Synthesis reactions are separate from single replacement reaction

Flashcards in Synthesis Reaction 10

A synthesis  reaction (also called a combination reaction)  is a reaction where two or more elements or compounds combine to form a new compound.

$$Al + FeCl_2 \rightarrow AlCl_3 + Fe$$

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Frequently Asked Questions about Synthesis Reaction

What is the meaning of synthesis reaction?

A synthesis reaction is a chemical reaction in which two or more reactants combine to produce a single product:

A + B → AB

What is an example of a synthesis reaction?

An example of a synthesis reaction is the production of salt (NaCl) from sodium (Na) and chlorine (Cl):

2 Na (s) + Cl 2 (g) → 2NaCl (s)

How do you solve synthesis chemical equations?

A synthesis chemical equation always follows the same reaction structure, and thus always has the following general equation:

Sometimes AB can be represented as C (A + B → C), but it's the same concept: a synthesis chemical equation.

What are the characteristics of a synthesis reaction?

The characteristics of a synthesis reaction are:

Are synthesis reactions the same as a single replacements?

No, synthesis reactions and single replacement reactions are different types of reactions. Synthesis reactions consist of two or more reactants combining to produce a new product (A + B → C).

In the case of a single replacement, one of the reactants displaces an element in the other reactant, producing two products: the new compound with the replacement, and the element that was "kicked out" of the original reactant (A + BC → AB + C).

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