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Chemical Reactions: Synthesis, Decomposition, Displacement, and Combustion, Slides of Chemistry

An overview of different types of chemical reactions, including synthesis, decomposition, single displacement, double displacement, and combustion. It explains the definition of each reaction type, provides examples, and discusses how to identify the type of reaction based on the reactants. The document also includes illustrations to help clarify the concepts.

What you will learn

  • What is a decomposition reaction?
  • What is a synthesis reaction?
  • What is a single displacement reaction?
  • What is a combustion reaction?
  • What is a double displacement reaction?

Typology: Slides

2021/2022

Uploaded on 09/27/2022

ekanga
ekanga 🇺🇸

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TYPES OF
CHEMICAL REACTIONS
To react or not to react? THAT is
the question!
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TYPES OF

CHEMICAL REACTIONS

To react or not to react? THAT is

the question!

 Chemical changes are a result of chemical reactions.

 All chemical reactions involve a change in substances and a change in energy.

 Neither matter or energy is created or destroyed in a chemical reaction---only changed.

Chemical Reactions

#1 Synthesis Reactions

 Synthesis = combine = put together

 Two or more simple substances combine to form a more complex substance.

 The reaction through the equation:

reactant + reactant -------> product A + B -------> AB

 Ca + O 2 CaO

 SO 3 + H 2 O  H 2 SO 4

 For example, simple hydrogen gas combined with simple oxygen gas can produce a more complex substance— water!

 The chemical equation for this synthesis reaction is:

2H 2 + O 2  2H 2 O

#1 Synthesis Reactions

 metal + oxygen  metal oxide

4Fe(s) + 3O2(g)  2Fe 2 O3(s)

 nonmetal + oxygen  nonmetal oxide

S(s) + O2(g)  SO2(g)

 metal oxide + water  metallic hydroxide

MgO(s) + H 2 O(l)  2Mg(OH)2(s)

#1 Synthesis Reactions

 nonmetallic oxide + water  acid

SO3(g) + H 2 O(l)  H 2 SO4(aq)

 metal + nonmetal  salt

2Na(s) + Cl2(g)  2NaCl(s)

#1 Synthesis Reactions

 In a decomposition reaction a more complex substance breaks down into its more simple parts.

 One reactant yields 2 or more products. Basically, synthesis and decomposition reactions are opposites. reactant -------> product + product AB -------> A + B

#2 Decomposition Reactions

 For example, water can be broken down into hydrogen gas and oxygen gas.

 The chemical equation for this decomposition reaction looks like:

2H 2 O  2H 2 + O 2

#2 Decomposition Reactions

 The explosion of a dynamite is an example of a decomposition reaction.

  • When suitably activated, a highly exothermic reaction occurs in which large amounts of gaseous products form.

 Nitroglycerin, which can be activated merely by shaking, decomposes as follows: 4C 3 H 5 (NO 3 )3(l)  6N2 (g) + 12CO2(g) + 10H 20 (g) + O2(g)

#2 Decomposition Reactions

 The egg (the reactant), which contained the turtle at one time, now has opened and the turtle (product) and egg shell (product) are now two separate substances.

#2 Decomposition Reactions

 Some oxides, when heated, decompose.

2HgO(s)  2Hg(l) + O2(g)

 Some acids, when heated, decompose into nonmetallic oxides and water. H 2 SO4(s)  H 2 O(l) + SO3(g)

#2 Decomposition Reactions

#3 Single Displacement

 In a single displacement reaction a single uncombined element replaces another in a compound.

  • Reactants must be an element and a compound.
  • Products will be a different element and a different compound.

 Two reactants yield two products. reactant + reactant ---------> product + product AB + C -------> AC + B

  • Na + KCl  K + NaCl
  • F 2 + LiCl  LiF + Cl 2

#3 Single Replacement

 Metals replace metals (and hydrogen)

  • K + AlN 
  • Zn + HCl 

 Think of water as HOH

 Metals replace one of the H’s, combine with hydroxide.

  • Na + HOH 

 Notice, the guy in the orange shirt steals the date of the other guy.  So, a part of one of the reactants trades places and is in a different place among the products.

#3 Single Displacement