The document discusses balancing chemical equations and types of chemical reactions. It defines six types of chemical reactions: synthesis, decomposition, single replacement, double replacement, acid-base, and combustion reactions. It provides examples of each type of reaction and their balanced chemical equations. Worksheets are included for the reader to balance additional example reactions and identify the reaction type.

1. Balancing Chemical Equations

6. Give the number of atoms present for each of the following compounds. 1 2 6 2 1 4 2 2 8 Fe=_____ S=_____ O=______ Fe 2 (SO 4 ) 2 H=_____ S=_____ O=______ H 2 SO 4 Pb=_____ N=_____ O=______ Pb(NO 3 ) 2 Number of Atoms Compound

8. 1. ______ Na + ______ O 2 ______ Na 2 O 2. ______ H 2 + ______ O 2 _________H 2 O 3. _____ Na 2 SO 4 + _____ CaCl 2 _____CaSO 4 + ____ NaCl O= O= Na= Na= O= O= H= H= Ca= Ca= O= O= Cl= Cl= S= S= Na= Na=

9. 4. ______ Al 2 O 3 ______Al + ______O 2 5. ______ N 2 + ______ H 2 _________H 2 N 6. _____ Fe + _____ H 2 O _____Fe 3 O 4 + ____ H 2 O= O= Al= Al= H= H= N= N= O= H= Fe= O= H= Fe=

10. 7. ______ P 2 + ______ O 2 _________P 4 O 10 8. ______ C 2 H 6 + ______ O 2 ______ CO + _______H 2 O 9. _____SiCl 4 ______Si + ______Cl 2 10. ______ C + ______ H 2 _________CH 4 O= O= P= P= H= H= O= O= C= C= Cl= Cl= Si= Si= H= H= C= C=

11. 2. ______ H 3 PO 4 + ______ KOH  ______K 3 PO 4 + ______ H 2 O 3. ______K + ______ B 2 O 3  ______K 2 O + ______B 4. ______HCl + ______NaOH  ______NaCl + ______H 2 O K= K= O= O= P= P= H= H= O= O= B= B= K= K= O= O= Na= Na= Cl= Cl= H= H=

12. 5. ______Na + ______NaNO 3  ______Na 2 O + ______N 2 6. ______ C + ______S 8  ______CS 2 7. ______Na + ______O 2  ______Na 2 O 2 8. ______N 2 + ______O 2  ______N 2 O 2 O= O= N= N= Na= Na= S= S= C= C= O= O= Na= Na= O= O= N= N=

13. 9. _____ H 3 PO 4 + _____Mg(OH) 2  _____Mg 3 (PO 4 ) 2 + _____H 2 O 10. ______NaOH + ______H 2 CO 3  ______Na 2 CO 3 + ______H 2 O 11. SKIP Mg= Mg= O= O= P= P= H= H= C= C= H= H= O= O= Na= Na= Br= Br= H= H= O= O= K= K=

14. 12. ______H 2 + ______O 2  ______H 2 O 2 13. ______Na + ______O 2  ______Na 2 O 14. ______Al(OH) 3 + ______H 2 CO 3  ______Al(CO 3 ) 3 + ______H 2 O 15. ______Al + ______S 8  ______Al 2 S 3 O= O= H= H= O= O= Na= Na= C= C= H= H= O= O= Al= Al= S= S= Al= Al=

15. 16. ______Cs + ______N 2  ______Cs 3 N 17. ______Mg + ______Cl 2  ______Mg Cl 2 18. ______Rb + ______RbNO 3  ______Rb 2 O + ______N 2 19. ______ C 6 H 6 + ______O 2  ______CO 2 + H 2 O N= N= Cs= Cs= Cl= Cl= Mg= Mg= O= O= N= N= Rb= Rb= O= O= H= H= C= C=

16. 20. ______N 2 + ______H 2  ______NH 3 21. ______ C 10 H 22 + ______O 2  ______CO 2 + H 2 O 22.______Al(OH) 3 + ______H 2 Br  ______AlBr 3 + ______H 2 O 23.____CH 3 +____CH 2 +____CH 2 +____CH 3 +____O 2  ____CO 2 + ____H 2 O H= H= N= N= O= O= H= H= C= C= C= C= H= H= O= O= Al= Al= O= O= H= H= C= C=

17. 24. ____C + ____O 2  ____CO 2 25. ____C 3 H 8 + ____O 2  ____CO 2 + ____H 2 O 26. ______ Li + ______AlCl 3  ______LiCl + ______Al 27. ____C 2 H 6 + ____O 2  ____CO 2 + ____H 2 O O= O= C= C= O= O= H= H= C= C= Cl= Cl= Al= Al= Li= Li= O= O= H= H= C= C=

18. 28. ____NH 4 OH + ____ H 3 PO 4  ____(NH 4 ) 3 PO 4 + ____H 2 O 29. ______ Rb + ______P  ______Rb 3 P 30. ______ CH 4 + ______O 2  ______ CO 2 + ______H 2 O P= P= O= O= H= H= N= N= P= P= Rb= Rb= O= O= H= H= C= C=

19. 31.______Al(OH) 3 + ______H 2 SO 4  ______ Al(S) 4 ) 3 + ______H 2 O 32. ______Na + ______Cl 2  ______NaCl 33. ______ Rb + ______S 8  ______Rb 2 S 34. _____ H 3 PO 4 + _____Ca(OH) 2  _____MCa 3 (PO 4 ) 2 + _____H 2 O S= S= H= H= O= O= Al= Al= Cl= Cl= Na= Na= S= S= Rb= Rb= Ca= Ca= O= O= P= P= H= H=

20. 35 . ______NH 3 + ______HCl  ______NH 4 Cl 36. ____Li + ____H 2 O  ____LiOH + ____H 2 37.____ Ca 3 (PO 4 ) 2 + ____SiO 2 + ____C  _____CaSiO 3 +_____CO+_____P Cl= Cl= H= H= N= N= O= O= H= H= C= C= C= C= Si= Si= O= O= P= P= Ca= Ca=

21. 38. ______ NH 3 + ______O 2  ______N 2 + ______H 2 O 39. ______FeS 2 + ______O 2  ______Fe 2 O 3 + ______SO 2 40. ______C + ______SO 2  _______CS 2 + ______CO O= O= H= H= N= N= O= O= S= S= Fe= Fe= O= O= S= S= C= C=

22. 6 Types of Chemical Reactions

23. 1) SYNTHESIS REACTION In a synthesis reaction two or more simple substances combine to form a more complex substance. Two or more reactants yielding one product is another way to identify a synthesis reaction. For example, simple hydrogen gas combined with simple oxygen gas can produce a more complex substance-----water! The chemical equation for this synthesis reaction looks like: reactant + reactant -------> product A + B  AB 8 Fe + S 8  8 FeS To visualize a synthesis reaction look at the following cartoon:

24. 2) DECOMPOSITION REACTION 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. For example, water can be broken down into hydrogen gas and oxygen gas. The chemical equation for this decomposition reaction looks like: reactant -------> product + product To visualize a decomposition reaction look at the following cartoon: 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. AB  A + B 2 H 2 O  2 H 2 + O 2

25. 3) SINGLE REPLACEMENT (DISPLACEMENT) REACTION In a single replacement reaction a single uncombined element replaces another in a compound. Two reactants yield two products. For example when zinc combines with hydrochloric acid, the zinc replaces hydrogen. The chemical equation for this single replacement reaction looks like: reactant + reactant ---------> product + product To visualize a single replacement reaction look at the following cartoon: 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. A + BC  AC + B Mg + 2 H 2 O  Mg(OH) 2 + H 2

26. 4) DOUBLE REPLACEMENT (DISPLACEMENT) REACTION In a double replacement reaction parts of two compounds switch places to form two new compounds. Two reactants yield two products. For example when silver nitrate combines with sodium chloride, two new compounds--silver chloride and sodium nitrate are formed because the sodium and silver switched places. The chemical equation for this double replacement reaction looks like: reactant + reactant ---------> product + product To visualize a double replacement reaction look at the following cartoon: AB + CD ---> AD + CB Pb(NO 3 ) 2 + 2 KI ---> PbI 2 + 2 KNO 3

28. Six Types of Chemical Reaction Worksheet Balance the following reactions and indicate which of the six types of chemical reaction are being represented:

29. 1) ____ NaBr + ____ Ca(OH) 2  ___ CaBr 2 + ____ NaOH Type of reaction: _____________________________ 2) ____ NH 3 + ____ H 2 SO 4  ____ (NH 4 ) 2 SO 4 Type of reaction: _____________________________ H= H= O= O= Ca= Ca= Br= Br= Na= Na= O= O= S= S= H= H= N= N=

30. 3) ____ C 5 H 9 O + ____ O 2  ____ CO 2 + ____ H 2 O Type of reaction: _____________________________ 4) ____ Pb + ____ H 3 PO 4  ____ H 2 + ____ Pb 3 (PO 4 ) 2 Type of reaction: _____________________________ O= O= H= H= C= C= O= O= P= P= H= H= Pb= Pb=

31. 5) ____ Li 3 N + ____ NH 4 NO 3  ___ LiNO 3 + ___ (NH 4 ) 3 N Type of reaction: _____________________________ 6) ____ HBr + ___ Al(OH) 3  ___ H­ 2 O + ___ AlBr 3 Type of reaction: _____________________________ O= O= H= H= N= N= Li= Li= O= O= Al= Al= Br= Br= H= H=