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Types of Chemical Reactions

Types of Chemical Reactions. Chemical Reactions. A chemical reaction has occurred when the starting substances ( reactants ) recombine to form ending substances ( products ). The reactants will, most often, have different chemical and physical properties than the products.

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Types of Chemical Reactions

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  1. Types of Chemical Reactions

  2. Chemical Reactions • A chemical reaction has occurred when the starting substances (reactants) recombine to form ending substances (products). • The reactants will, most often, have different chemical and physical properties than the products. • Evidence of a chemical reaction can include (but is not limited to): bubbles, flames, change of color, change of state, precipitate.

  3. Basic Types of Chemical Reactions • Synthesis (or combination) • Decomposition • Single Replacement • Double Replacement • Combustion

  4. Synthesis (Combination) • Just like the name implies, a new substance is formed from two or more reactants. • The typical chemical equation will appear in the form of A + B → AB • A and B can be single elements or molecules. • Example: 2H2 + O2 → 2H2O

  5. Decomposition • Again, as the name implies, this type of reaction involves breaking reactants down into simpler substances. • In many ways, it is the opposite of a synthesis reaction. • The typical chemical equation will appear in the form of AB → A + B • Example: 2KClO3 → 2KCl + 3O2

  6. Single Replacement • In this type of reaction a single, reactive metal will replace a less reactive metal already bonded in an ionic compound. • The typical chemical will appear as A + BC → B + AC • Example: Cu + 2AgNO3 → 2Ag + Cu(NO3)2 • You will need to use the activity series to determine whether this type of reaction will take place.

  7. Activity Series • The only time a single replacement will take place is when the free metal is more reactive than the metal cation bonded in the ionic compound. • This reactivity is based on ionization energy. A metal with a lower ionization energy is more reactive than one with a higher ionization energy. • You will need to use the activity series to determine which metals are more reactive than others.

  8. Activity Series A metal high on the table is more reactive and can replace a metal lower on the table. A metal lower on the table CANNOT replace a metal higher on the table.

  9. Double Replacement Reactions • In this type of reaction, already bonded metal cations basically switch places with one another and bond with the already bonded nonmetal anions. • These reactions usually take place in aqueous solution. • The typical chemical equation will appear as AB + CD → AD + CB • Example: CaF2 + 2NaNO3 → Ca(NO3)2 + 2NaF

  10. Double Replacement Reactions • Usually produce bubbles, a precipitate, or a molecular compound such as water. • In order to occur, one of the following is usually true. • One of the products is only slightly soluble and precipitates. • One of the products is a gas. • One product is a molecular compound such as water.

  11. Predicting Precipitates • When a precipitate is formed, the precipitate can be predicted by using rules of solubility or a solubility table. • Remember, an insoluble substance will not dissolve in water and will therefore precipitate. • In a chemical reaction, a down arrow (↓) is usually written after the formula for the precipitate in order to indicate the precipitate.

  12. Solubility Rules

  13. Acid – Base Double Replacement • An acid, for now, is defined as a substance that produces a hydrogen ion in solution. We will recognize an acid as an ionic compound that starts with H. • Example: HCl, H2SO4 • A base, for now, is defined as a substance that produces a hydroxide ion in solution. We will recognize a base as an ionic compound that ends with –OH. • Example: NaOH, Ca(OH)2

  14. Acid – Base D.R. Reaction • When an acid and a base react, in a double replacement reaction, the products formed will be an ionic compound (salt) and water. • Example: 2NaOH + H2SO4 → Na2SO4 + 2H2O base Ionic salt water acid

  15. Combustion Reaction • In a combustion reaction, a hydrocarbon burns in oxygen. The products formed are always carbon dioxide and water. • The typical format for this reaction is CxHy + O2→ CO2 + H2O • Example: CH4 + 2O2 → CO2 + 2H2O

  16. Try These Worksheets! • http://misterguch.brinkster.net/6typesofreaction.pdf • http://www.everettcc.edu/uploadedFiles/Student_Resources_and_Services/TRIO/Types_of_reactions_worksheet.pdf • http://www.sciencegeek.net/Chemistry/chempdfs/EquationsWorksheet4.pdf • http://www.sciencegeek.net/Chemistry/chempdfs/EquationsWorksheet2.pdf • http://www.sciencegeek.net/Chemistry/chempdfs/EquationsWorksheet3.pdf • http://misterguch.brinkster.net/equationworksheets.html • From this link, choose reaction products worksheet, six types of reactions, or double displacement reactions

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