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Chapter 9: Problem 76

List each of the four types of chemical reactions and give an example for each type.

Short Answer

Expert verified
The four types of chemical reactions are synthesis, decomposition, single displacement, and double displacement. 1. Synthesis Reaction: Two or more substances combine to form a single, more complex substance. Example: \(2H_2(g) + O_2(g) \to 2H_2O(l)\) 2. Decomposition Reaction: A single complex substance breaks down into smaller, simpler substances. Example: \(2H_2O(l) \to 2H_2(g) + O_2(g)\) 3. Single Displacement Reaction: An element in a compound is displaced or replaced by another element. Example: \(Zn(s) + 2HCl(aq) \to ZnCl_2(aq) + H_2(g)\) 4. Double Displacement Reaction: The ions in two compounds exchange places, forming two new compounds. Example: \(AgNO_3(aq) + NaCl(aq) \to AgCl(s) + NaNO_3(aq)\)

Step by step solution

01

Synthesis Reaction

: A synthesis reaction occurs when two or more substances combine to form a single, more complex substance. The general pattern of a synthesis reaction can be represented as: A + B -> AB Example: \(2H_2(g) + O_2(g) \to 2H_2O(l)\) In this example, two molecules of hydrogen gas (H2) react with one molecule of oxygen gas (O2) to form two molecules of water (H2O).
02

Decomposition Reaction

: A decomposition reaction is the reverse of a synthesis reaction. In this type of reaction, a single complex substance breaks down into smaller, simpler substances. The general pattern for a decomposition reaction is: AB -> A + B Example: \(2H_2O(l) \to 2H_2(g) + O_2(g)\) Here, two molecules of water (H2O) decompose into two molecules of hydrogen gas (H2) and one molecule of oxygen gas (O2).
03

Single Displacement Reaction

: A single displacement reaction takes place when an element in a compound is displaced or replaced by another element. The general pattern for a single displacement reaction can be represented as: A + BC -> AC + B Example: \(Zn(s) + 2HCl(aq) \to ZnCl_2(aq) + H_2(g)\) In this example, zinc (Zn) displaces hydrogen (H) in hydrochloric acid (HCl), forming zinc chloride (ZnCl2) and hydrogen gas (H2).
04

Double Displacement Reaction

: A double displacement reaction occurs when the ions in two compounds exchange places, forming two new compounds. The general pattern for a double displacement reaction is: AB + CD -> AD + CB Example: \(AgNO_3(aq) + NaCl(aq) \to AgCl(s) + NaNO_3(aq)\) In this example, silver nitrate (AgNO3) and sodium chloride (NaCl) react to form silver chloride (AgCl), which precipitates as a solid, and sodium nitrate (NaNO3) dissolved in the solution.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Synthesis Reaction
Imagine combining two pieces from a jigsaw puzzle to create a complete picture. This is akin to a synthesis reaction, where two or more reactants join forces to create a single more complex product. It's like addition in chemistry, where you combine simple substances to form one complex substance.

For instance, when hydrogen and oxygen gases, the reactants, come together, they form water, the product. The reaction looks like this: \(2H_2(g) + O_2(g) \to 2H_2O(l)\). Synthesis reactions are foundational in chemical manufacturing, creating compounds ranging from table salt to the chemicals in medicines.
Decomposition Reaction
Now, imagine taking a whole cake and slicing it into pieces. In chemistry, this is a decomposition reaction, where a complex molecule breaks apart into simpler substances. Think of it as the opposite of a synthesis reaction; it's a form of chemical subtraction.

Water, when decomposed by an electric current, splits into hydrogen and oxygen gases, showcasing this process: \(2H_2O(l) \to 2H_2(g) + O_2(g)\). Decomposition reactions are critical in processes like recycling materials and understanding the breakdown of organic matter in nature.
Single Displacement Reaction
Consider a dance where one person steps away, allowing another to take their place. This scenario resembles a single displacement reaction in chemistry, where an element from a compound is replaced by a more reactive element. Here, elements essentially swap dance partners.

An example of this would be zinc trading places with hydrogen in a hydrochloric acid solution to form zinc chloride and release hydrogen gas: \(Zn(s) + 2HCl(aq) \to ZnCl_2(aq) + H_2(g)\). Such reactions are fundamental for extracting metals from their ores and in batteries where metals displace ions to generate electricity.
Double Displacement Reaction
Picture two pairs of dancers switching partners. This dance of atoms is what we call a double displacement reaction, where parts of two compounds exchange places with each other, forming two entirely different compounds. It's a chemical partner swap!

For instance, when silver nitrate reacts with sodium chloride, the silver pairs up with the chloride, and the sodium joins the nitrate, resulting in the formation of silver chloride and sodium nitrate: \(AgNO_3(aq) + NaCl(aq) \to AgCl(s) + NaNO_3(aq)\). This type of reaction is prominent in the processes of neutralization between acids and bases and in precipitation reactions that occur in various analytical and synthetic chemistry techniques.

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Most popular questions from this chapter

A reaction occurs when hydrosulfuric acid \(\left(\mathrm{H}_{2} \mathrm{S}\right)\) is mixed with an aqueous solution of iron(III) bromide. The reaction produces solid iron(III) sulfide and aqueous hydrogen bromide. Write the chemical and net ionic equations for the reaction.

Challenge A piece of zinc metal is added to a solution of hydroge sulfate. This reaction produces a gas and a solution of zinc sulfate.

Write complete ionic and net ionic equations for the reaction between sulfuric acid \(\left(\mathrm{H}_{2} \mathrm{SO}_{4}\right)\) and calcium carbonate \(\left(\mathrm{CaCO}_{3}\right)\). $$\mathrm{H}_{2} \mathrm{SO}_{4}(\mathrm{aq})+\mathrm{CaCO}_{3}(\mathrm{s}) \rightarrow \mathrm{H}_{2} \mathrm{O}(\mathrm{l})+\mathrm{CO}_{2}(\mathrm{g})+\mathrm{CaSO}_{4}(\mathrm{aq})$$

Aqueous solutions of ammonium phosphate and sodium sulfate are mixed. No precipitate forms and no gas is produced.

Identify the reactants in the following reaction: When potassium is dropped into aqueous zinc nitrate, zinc and aqueous potassium nitrate form.
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