Types of Chemical. Types of Reactions. Chapter 8 Chemical Reactions. Reactions. Synthesis Reactions. Synthesis Reactions. Synthesis Reactions

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1 Chapter 8 Chemical Reactions Types of Chemical Reactions Types of Reactions There are six types of chemical reactions that you will learn about in this lesson: 1. Synthesis reactions 2. Decomposition reactions 3. Single displacement reactions 4. Double displacement reactions 5. Combustion reactions 6. Acid/Base reactions At the end of the lesson, you should be able to identify the type of reaction and predict the product(s) Synthesis reactions occur when two substances (generally elements) ) combine and form a compound.. (Sometimes these are called combination or addition reactions.) reactant + reactant 1 product Or, basically: A + B AB Example: Example: 2H 2 + O 2 2H 2 O C + O 2 CO 2 Synthesis reactions occur when two substances (generally elements) ) combine and form a compound. Sodium metal reacts with chlorine gas to form sodium chloride: Na + Cl 2 NaCl 2Na + Cl 2 2NaCl Another example of a synthesis reaction Chlorine gas reacts with oxygen to form dichlorine pentoxide: Cl 2 + O 2 Cl 2 O 5 2Cl 2 + 5O 2 2Cl 2 O 5 Decomposition Reactions Decomposition reactions occur when a compound breaks up into the elements or to a few simpler compounds 1 Reactant Product + Product In general: AB A + B Examples: 2 H 2 O 2H 2 + O 2 2 HgO 2Hg + O 2 1

2 Decomposition Reactions Decomposition: a compound breaks up A practical example of decomposition: an automobile airbag Sodium nitride breaks down to sodium metal and nitrogen gas: occur when one element replaces another in a compound. A + XY AY Y + X Na 3 N Na + N 2 2Na 3 N 6Na + N 2 There are generally two types of single replacement reactions Keep in mind Na F Cationic: A metal can replace a metal A + BC AC C + B (A & B are metals) Anionic: A nonmetal can replace a nonmetal D + EFE ED + F (D & F are nonmetals) cationic metal anionic nonmetal Zinc reacts with Hydrochloric Acid to form Zinc chloride and hydrogen gas Zn (s) + HCl (aq) ZnCl 2(s) + H 2(g) The Balanced Equation Zn (s) + 2 HCl (aq) ZnCl 2(s) + H 2(g) Metal Replaces Metal An Investigation; The Aluminum Soda Can Are they all made of the same amount of Aluminum Do they have the same wall thickness Would you expect Coca Cola cans to be different than Dr. Pepper Let s s try to Rip one of each can An Investigation; The Aluminum Soda Can Aluminum metal reacts with aqueous copper (II) chloride Al (s) + CuCl 2(aq) 2(aq) --- Is it Balanced 2Al (s) + 3CuCl ---> > AlCl 3(aq) + Cu CuCl 2(aq) --- Cu (s) ---> 2AlCl 3(aq) + 3Cu AlCl 3(aq) (Skeleton) Cu (s) 2

3 Let s Revisit the Soda Can Reaction. Could We have predicted the Products How Do We Know if one Metal Replaces Another Al(s) (s) + CuCl2(aq) Æ Which is more reactive, Al of Cu Al(s) (s) + CuCl2(aq) Æ AlCl3(aq) + Cu(s) (s) Predicting Single Replacement of Metals What About Nonmetal Replacing Nonmetal Iron reacts with aqueous copper (II) chloride Fe(s) (s) + CuCl2(aq) Æ Is Iron More Active than Copper on the Activity Chart Fe(s) (s) + CuCl2(aq) Æ FeCl2(aq) + Cu(s) (s) Fluorine reacts with Hydrochloric Acid to form Chlorine and Hydrogen fluoride F2(g) + HCl(aq) (aq) Æ HF(aq) (aq) + Cl2(g) The Balanced Equation F2(g) + 2 HCl(aq) (aq) Æ 2 HF(s) (s) + Cl2(g) Predicting Single Replacement of Nonmetals How Do We Know if one Nonmetal Replaces Another More Active Cl2 + HBr Æ I2 + HCl Æ F2 + HI Æ Less Active 3

4 Double Replacement Reactions Double Replacement Reactions occur when a metal replaces a metal in a compound and a nonmetal replaces a nonmetal in a compound AB + CD AD + CB Double Replacement Reactions Think about it like foil inging in algebra, first and last ions go together + inside ions go together Example: AgNO 3(aq) + NaCl (aq) AgCl (s) + NaNO 3(aq) Another example: K 2 SO 4(aq) + Ba(NO 3 ) 2(aq) 2 KNO KNO 3(aq) BaSO 4(s) (aq) + BaSO Combustion Reactions Combustion Reactions occur when a substance combines with oxygen releasing a large amount of energy in the form of light and heat,, it is a combustion reaction. i.e Combustion of Propane, C 3 H 8 C 3 H O 2 3 CO H 2 O + heat In addition to light and heat, CO 2 and H 2 O are always released during Complete Combustion Combustion Reactions Combustion Reactions; substance combines with oxygen releasing a large amount of energy in the form of light and heat,, as well as CO 2 and H 2 O. Let s s try to balance a few Combustion Reactions 1. CH O 2 ---> > CO H 2 O 2. 2 C 2 H O 2 ---> > 4 CO H 2 O 3. C 6 H 12 O O 2 ---> > 6 CO H 2 O 4. C 2 H 6 O + 3 O 2 ---> > 2 CO H 2 O Acid/Base Reactions According to Bronsted Lowery: An acid is any compound which can donate a proton. A base is any compound which can accept a proton. In an acid-base reaction,, an acid and a base will react to form a salt and water. During the reaction, a proton is donated by the acid to the base to yield water. The remaining ions form a salt. HCl + NaOH NaCl + H 2 O Acid/Base Reactions More examples: H 2 SO 4 + H 2 O HSO - 4 HF + NaOH HCN + CH 3 COO - NaF + H 3 O + + HOH CN - + CH 3 COOH 4

5 Let s s Summarize 1. Synthesis reactions: two substances combine to form a compound. i.e. 2H 2 + O 2 2H 2 O 2. Decomposition reactions occur when a compound breaks up. i.e. 2 H 2 O 2H 2 + O 2 3. Single Replacement reactions occur when one element replaces another in a compound. i.e. Zn (s) + 2 HCl (g) ZnCl 2(s) + H 2(g) Let s s Summarize 4. Double Displacement reactions: when a metal replaces a metal in a compound and a nonmetal replaces a nonmetal in a compound i.e. AgNO 3 (aq) + NaCl Cl(s) AgCl(s (s)) + NaNO 3 (aq) 5. Combustion reactions when a substance combines with oxygen releasing a large amount of energy in the form of light and heat,, as well as CO 2 and H 2 O. i.e. C 3 H O 2 3 CO H 2 O + heat 6. Acid/Base Reactions:: : Acids donate a proton (H+) to a base, producing a salt and water. i.e. HCl + NaOH NaCl + H 2 O 5

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