5 types of chemical reactions

types of chemical reactions

1. 5 Types of Chemical Reaction

2. 1. Combination Reaction 2. Decomposition Reaction 3. Single Replacement Reaction 4. Double Re placement Reaction 5. Combustion Reaction

3. Combination Reaction Synthesis Reaction Combination reaction is the direct union or combination of two substances to form a single compound. A + B AB General Formula:

4. Xander Agnes

5. A combination reaction may also involves an element and a compound, or two simple compounds: 2 SO 2 + O 2 SO 3 MgO + H 2 O Mg(OH) 2 Examples:

6. Examples: 2 Ni O + O 2 2 Ni 1. Nickel reacts with oxygen to form Nickel Oxide 2. Silver reacts with chlorine to form Silver Chloride. 2 Ag + Cl 2 2 Ag Cl 3. Oxygen gas reacts to magnesium form magnesium oxide O 2 + 2 Mg 2 Mg O

7. Try This: H 2(g) + Cl 2(g) 2. Fe 2(s) + S (s) 2 HCl ( aq ) FeS (s)

8. Decomposition Reaction Analysis Reaction Decomposition reaction is a single substance broken into two or more different substances . B AB A + General Formula:

9. Xander Agnes

10. Various Types of decomposition Reactions: Thermal Decomposition Reaction - decomposition reaction caused by a rise in temperature. 2 HgO (S) 2 Hg (g) + O 2(g) CaCO 3(s ) CaO (s) + CO 2(g) Examples:

11. 2. Electrolytic Decomposition Reaction - decomposition reaction caused by electricity. Ionic compounds can be decomposed in this manner, either in molten state or in solution. 2 NaCl (l) 2 Na (l) + Cl 2(g) PbBr 2( aq ) Pb (s) + Br 2( aq ) Examples: electrolysis electrolysis

12. 3. PhotoChemical decomposition Reaction - decomposition reaction caused by light. 2 AgCl 2(s) Ag (s ) + Cl 2(g ) 2 AgBr (s) 2 Ag (s) + Br 2(g) Examples: light light

13. 4. Catalysts cannot cause chemicals to decompose, they can speed up the rate of chemical decomposition. Example: 2 H 2 O 2(l ) 2 H 2 O (l) + O 2(g ) m anganese dioxide catalyst

14. 2 Au 2 O 3 2 KClO 3 Try This: 4 Au + 3 O 2 2 KCl + 3 O 2

15. replacement - An atom or a group of atom that replaces part of a compound. Types of Replacement Reaction: Single Replacement Double Replacement

16. Single Replacement Reaction Substitution Reaction In this type of chemical reaction, an element and a compound react and form a different element and a different compound. A more reactive element replaces a less active element in its compound. Two possibilities of replacement in the Substitution Reaction: Cation Replacement Anion Replacement

17. Activity Series of the Elements Metals Non-Metals Li (most active) F Activity Series of the Element Metals Non-metals Li K Ba Ca Na Mg Al Mn Zn Cr Fe Ni Sn Pb H Cu Bi Sb Hg Ag Pt Au F Cl Br O I S ( most active) (least active)

18. Fe (s) + CuSO 4( aq ) FeSO 4( aq ) + Cu (s) * Iron is more reactive than Copper Zn (s) + 2 HCl ( aq ) ZnCl 2( aq ) + H 2(g) * Zinc is more reactive than Hydrogen Examples:

19. Cations REplacement Examples: General Formula: A + BC B + AC Cu + 2 AgNO 3  → 2 Ag + Cu(NO 3 ) 2 Fe + Cu(NO 3 ) 2  → Fe(NO 3 ) 2  + Cu

20. Ag + Cu(NO 3 ) 2  → No reaction Au + HCl → No reaction   Note: if the reactant in elemental form is not the  more reactive metal , then no reaction will occur. Examples:

21. Activity Series of the Elements Metals Non-Metals Li (most active) F Activity Series of the Element Metals Non-metals Li K Ba Ca Na Mg Al Mn Zn Cr Fe Ni Sn Pb H Cu Bi Sb Hg Ag Pt Au F Cl Br O I S ( most active) (least active)

22. Try This: Zn + 2 HCl Fe 2 O 3(s) + 2 Al (s) ZnCl 2  + H 2 Fe 2(l) + Al 2 O 3(s)

23. Anions Replacement Cl 2  + 2 Na Br → 2 NaCl + Br 2 Br 2  + 2 KI → 2 KBr + I 2 Examples: General Formula: A + BC C + AB

24. I 2  + 2 KBr → No reaction   Note: Less reactive halogen cannot replace the more reactive halogen. no reaction will occur. Example:

25. Activity Series of the Elements Metals Non-Metals Li (most active) F Activity Series of the Element Metals Non-metals Li K Ba Ca Na Mg Al Mn Zn Cr Fe Ni Sn Pb H Cu Bi Sb Hg Ag Pt Au F Cl Br O I S ( most active) (least active)

26. Ionic Reaction when the negative ions in the two compounds switch places forming two new compounds. Double Replacement Reaction General Formula: AB+CD AD+CB

27. Several types of double replacement reactions are frequently encountered: 1. A reaction between a base such as NaOH , KOH or Ca (OH) 2 in aqueous solution and an acid such as HCl , H 2 SO 4 or CH 3 COOH. Reactions of this type are called Neutralization and the products are always water molecules and salt. Example: HCl ( aq ) + NaOH ( aq ) NaCl ( aq ) + H 2 O ( aq )

28. 2. A reaction between solutions of two soluble salts, a soluble salt and an acid, or a soluble salt and an alkali which, by exchanging cations and anions, can produce one insoluble compound or gas. Example: NaCl ( aq ) + AgNO 3( aq ) NaNO 3( aq ) + AgCl (s)

29. Sodium Chloride reacts with Potassium Bromide to form Sodium Bromide and Potassium Chloride. NaCl + KBr NaBr + KCl 2. Iron Sulfide reacts with Hydrochloric Acid to produce Iron Chloride and Hydrogen Sulfide. FeS + 2 HCl FeCl 2  + H 2 S Examples:

30. 1. Silver Nitrate reacts with Potassium Chloride to produce Silver Chloride and Potassium Nitrate. AgNO 3  + KCl    AgCl + KNO 3 2. Silver Nitrate reacts with Hydrochloric acid to form Hydrogen Nitrate and Silver Nitrate. AgNO3 + H Cl → HNO 3 +  AgNO3 Try This:

31. Combustion Reaction a chemical reaction in which a substance combines with oxygen and releases energy. Always produce Carbon Dioxide and Water General Formula: C x H y + O 2 CO 2 + H 2 O

32. Methane reacts with Oxygen gas to produce Carbon Dioxide and Water. CH 4   + 2 O 2   CO 2   + 2 H 2 O 2. Ethane reacts with Oxygen gas to form Carbon Dioxide and Water. 2 C 2 H 6   + 7 O 2   4 CO 2   + 6 H 2 O 3. Glucose (Sugar) reacts with Oxygen gas forming Carbon Dioxide and Water. C 6 H 12 O 6   + 6 O 2   6 CO 2  + 6 H 2 O Examples:

33. Exercises Identify the Types of Chemical Reaction of the following Chemical Equations: 3. N 2(g) + 3 H 3(g) 2 NH 3(g) 1. 2. 2 AgBr (s ) 2 Ag (s) + Br 2(g) Cu (s) + 2 AgNO 3(s)  → 2 Ag (s) + Cu(NO 3 ) 2(s) 4. BaCl 2(s) + MgSO 4(s) BaSO 4(s) + MgCl 2(s) 5. C 3 H 8(g )  + 12 O 2(g)  → 10 CO 2(g)  + 4 H 2 O (g)

34. Answers : 1. Single Replacement or Substitution Reaction 2. Decomposition Reaction or Analysis Reaction 3. Combination Reaction or Synthesis Reaction 4. Double Replacement 5. Combustion Reaction

35. Prepared by: Danica Z. Gutierrez.

36. 1. Silver Nitrate reacts with Copper metal to produce Copper (II) Nitrate and Silver. 2 AgNO 3  + Cu   Cu(NO3) 2  + 2 Ag 2. Magnesium metal reacts with Hydrochloric acid to form Magnesium Chloride and Hydrogen gas. Mg ( s )  + 2 HCl ( aq)  → MgCl 2(aq)  + H 2(g) Try This:

37. Examples: 1. Zinc combines with Hydrochloric Acid producing Zinc Chloride and Hydrogen gas. 2. Sodium Iodide reacts with Bromine gas to form Sodium Bromide and Iodine gas. 2 NaI + Br 2   → 2 NaBr + I 2 3. Aluminum reacts with Hydrochloric Acid to produce Aluminum Chloride and Hydrogen gas. 2 Al + 6 HCl → 2 AlCl 3 + 3 H 2 Zn + 2 HCl → ZnCl 2  + H 2