Name: 1. Law of Conservation of Mass atoms going into the reaction (reactants) must equal atoms coming out of the reaction (products)

Transcription

1 Unit 8: Balancing and Identifying Chemical Reactions Packet Name: 1. Law of Conservation of Mass atoms going into the reaction (reactants) must equal atoms coming out of the reaction (products) C O 2 CO 2 Reactants (left) Products (right) Q: How many carbon on the left? Q:How many carbon on the right? A: 1 atom of carbon A: 1 atom of carbon Q: How many oxygen on the left? Q:How many oxygen on the right? A: 2 atoms of oxygen A: 2 atoms of oxygen This chemical equation is balanced! 2. To balance a chemical equation only add or change coefficients! Thou shalt NOT change subscripts when balancing chemical equations! Again: Do Not Change Subscripts!!!! You can only change Coefficients!! 1

2 Balancing Act Notes + Practice Name Atoms are not or during a chemical reaction. Scientists know that there must be the number of atoms on each of the. To balance the chemical equation, you must add in front of the chemical formulas in the equation. You cannot or subscripts! 1) Determine number of atoms for each element. 2) Pick an element that is not equal on both sides of the equation. 3) Add a coefficient in front of the formula with that element and adjust your counts. 4) Continue adding coefficients to get the same number of atoms of each element on each side. Mg + O 2 MgO Mg = Mg = O = O = 2

3 Step-by-Step Example Problem: Step 1: Determine number of atoms for each element. Mg + O 2 MgO Balancing Act Teacher Notes Mg = 1 O = 2 Mg = 1 O = 1 Step 2: Pick an element that is not equal on both sides of the equation. Mg + O 2 MgO Mg = 1 O = 2 Mg = 1 O = 1 Since the O atoms are not equal, we ll target those first! Step 3: Add a coefficient in front of the formula with that element and adjust your counts. Mg + O 2 2 MgO Mg = 1 O = 2 Mg = 1 2 O = 1 2 Adding a 2 in front of MgO will change the number of atoms on the product side of the equation. Step 4: Continue adding coefficients to get the same number of atoms of each element on each side. 2 Mg + O 2 2 MgO Mg = 1 2 O = 2 Mg = 1 2 O = 1 2 Now we need to increase the number of Mg atoms we have on the reactant side. Adding a 2 in front of Mg will give us 2 atoms of Mg and balance the equation. 3

4 Balancing Equations Practice Name Part A: Identify the following parts of each chemical formula by circling the subscripts and drawing a square around the coefficients. H 2 2 HCl 4 O 2 CH 4 3 CO 3 2 NaOH Part B: List the symbols for the atoms in each formula and give the number of each. C 2 H 6 2MgO 4P 4 O 10 NH 3 3 Al(OH) 3 2 H 2 O 2 Try these: Ca + O 2 CaO Ca = Ca = O = O = N 2 + H 2 NH 3 N = N = H = H = Cu 2 O + C Cu + CO 2 Cu = Cu = O = O = C = C = H 2 O 2 H 2 O + O 2 H = H = O = O = 4

5 Name Class Date Balancing Chemical Equations Worksheet For the following: 1. Draw a circle around each subscript. 2. Draw a square around each coefficient. H2O 5Cl2 2Mg 3H2O2 For the following 1. List the chemical symbols of each element. 2. Give the number of atoms of each element. HCl CO2 Na2SO4 Balance the following chemical equations. 1. Cu2O + C g Cu + CO2 2. H2O2 g H2O + O2 3. Al + Fe3N2 g AlN + Fe 4. Ag2S g Ag + S8 5

6 5. ZnS + AlP g Zn3P2 + Al2S3 6. Fe(OH)3 g Fe2O3 + H2O Given the two chemical equations, circle the one that is balanced. 7. a. 2Na + Cl2 g 2NaCl b. 2Na + 2Cl2 g 2NaCl 8. a. C3H8 + 5O2 g 3CO2 + 4H2O b. 2C3H8 + 5O2 g 3CO2 + 8H2O 9. a. 2NH3 + 5O2 g 2NO + 3H2O b. 4NH3 + 5O2 g 4NO + 6H2O 10. a. Y(NO3)2 + GaPO4 g YPO4 + Ga(NO3)2 b. 2Y(NO3)2 + 2GaPO4 g 2YPO4 + Ga(NO3)2 6

7 ` Balancing Act Practice Name Balance each equation. Be sure to show your lists! Remember you cannot add subscripts or place coefficients in the middle of a chemical formula. 1. Na + MgF 2 NaF + Mg 2. Mg + HCl MgCl 2 + H 2 3. Cl 2 + KI KCl + I 2 4. NaCl Na + Cl 2 5. Na + O 2 Na 2 O 6. Na + HCl H 2 + NaCl 7. K + Cl 2 KCl Challenge: This one is tough! C 2 H 6 + O 2 CO 2 + H 2 O 7

8 Balancing Chemical Equations Balance the equations below: 1) N2 + H2 NH3 2) KClO3 KCl + O2 3) NaCl + F2 NaF + Cl2 4) H2 + O2 H2O 5) Pb(OH)2 + HCl H2O + PbCl2 6) AlBr3 + K2SO4 KBr + Al2(SO4)3 7) CH4 + O2 CO2 + H2O 8) C3H8 + O2 CO2 + H2O 9) C8H18 + O2 CO2 + H2O 10) FeCl3 + NaOH Fe(OH)3 + NaCl 8

9 11) P + O2 P2O5 12) Na + H2O NaOH + H2 13) Ag2O Ag + O2 14) S8 + O2 SO3 15) CO2 + H2O C6H12O6 + O2 16) K + MgBr2 KBr + Mg 17) HCl + CaCO3 CaCl2 + H2O + CO2 18) HNO3 + NaHCO3 NaNO3 + H2O + CO2 19) H2O + O2 H2O2 20) NaBr + CaF2 NaF + CaBr2 21) H2SO4 + NaNO2 HNO2 + Na2SO4 9

10 Chemical Reaction Types All chemical reactions can be placed into one of six categories. Here they are, in no particular order: 1) Combustion: A combustion reaction is when oxygen combines with another compound to form water and carbon dioxide. These reactions are exothermic, meaning they produce heat. An example of this kind of reaction is the burning of napthalene: C 10 H O 2 ---> 10 CO H 2 O 2) Synthesis: A synthesis reaction is when two or more simple compounds combine to form a more complicated one. These reactions come in the general form of: A + B ---> AB One example of a synthesis reaction is the combination of iron and sulfur to form iron (II) sulfide: 8 Fe + S8 ---> 8 FeS 3) Decomposition: A decomposition reaction is the opposite of a synthesis reaction - a complex molecule breaks down to make simpler ones. These reactions come in the general form: AB ---> A + B One example of a decomposition reaction is the electrolysis of water to make oxygen and hydrogen gas: 2 H2O ---> 2 H2 + O2 4) Single displacement: This is when one element trades places with another element in a compound. These reactions come in the general form of: A + BC ---> AC + B One example of a single displacement reaction is when magnesium replaces hydrogen in water to make magnesium hydroxide and hydrogen gas: Mg + 2 H2O ---> Mg(OH)2 + H2 10

11 5) Double displacement: This is when the anions and cations of two different molecules switch places, forming two entirely different compounds. These reactions are in the general form: AB + CD ---> AD + CB One example of a double displacement reaction is the reaction of lead (II) nitrate with potassium iodide to form lead (II) iodide and potassium nitrate: Pb(NO3)2 + 2 KI ---> PbI2 + 2 KNO3 11

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14 Types of Reactions Chemical reactions can be categorized into a variety of types. Five common types that we will study are synthesis, decomposition, combustion, single replacement and double replacement. Be familiar enough with the description of each type so that you are able to classify a reaction if given a chemical equation or verbal description. Synthesis: Synthesis reactions involve the formation of more complex compounds (many atoms) from simpler compounds and/or elements. The most common synthesis reaction involves the formation of a compound from its elements. Examples: 2 H 2(g) + O 2(g) 2 H 2 O (g) 3 H 2(g) + N 2(g) 2 NH 3(g) General: A + B AB Synthesis reactions are also referred to as combination, formation, and addition reactions. Decomposition: Decomposition reactions involve the breaking down of more complex compounds (larger, more atoms) into simpler compounds and/or elements. These reactions can often be thought of as being the opposite of synthesis reactions. Decomposition reactions often require heating in order to occur. Examples: 2 H 2 O (l) 2 H 2(g) + O 2(g) 2 KClO 3(s) 2 KCl (s) + 3 O 2(g) General: AB A + B Combustion: Combustion reactions involve the reaction of a substance with oxygen gas (O 2 ). It is often referred to as burning. The products of the reaction are oxides of the elements in the reactants. Hydrocarbon combustion leads to the formation of carbon dioxide gas and water vapor. Examples: 2 Mg (s) + O 2(g) 2 MgO (s) CH 4(g) + 2 O 2(g) CO 2(g) + 2 H 2 O (g) General: AB + O 2(g) A x O y + B w O z Some combustion reactions are also synthesis reactions. For instance, the combustion of magnesium leads to the formation of magnesium oxides 1. Synthesis: EX: YOUTUBE EXAMPLES: 14

15 Yours: 2. Decomposition: EX: Yours: 3. Single Replacement: EX: Yours: 4. Double Replacement: EX: Yours: 5. Combustion: EX: Yours: 15

16 Synthesis Worksheet #2: Synthesis Reactions 1. calcium + oxygen calcium oxide Ca + O 2 2. copper + sulfur copper(ii) sulfide Cu + S 8 4. hydrogen + nitrogen ammonia H 2 + N 2 5. hydrogen + chlorine hydrogen chloride H 2 + Cl 2 6. silver + sulfur silver sulfide Ag + S 8 7. chromium + oxygen chromium(iii) oxide Cr + 3O 2 8. aluminum + bromine aluminum bromide Al + Br 2 9. sodium + iodine sodium iodide Na + I hydrogen + oxygen water H 2 + O 2 16

17 In synthesis reactions, two or more reactants come together to form one compound. A + B AB Complete the following word equations, and write and balance the formula equation. 1. calcium + oxygen 2. copper + sulfur copper(ii) sulfide 3. calcium oxide + water calcium hydroxide 4. hydrogen + nitrogen 5. hydrogen + chlorine 6. silver + sulfur 7. chromium + oxygen 8. aluminum + bromine 9. sodium + iodine 10. hydrogen + oxygen 11. aluminum + oxygen 17

18 CHEMISTRY DECOMPOSITION REACTION WORKSHEET REACTION CATEGORY REACTION DESCRIPTION REACTION FORMAT DECOMPOSITION During decomposition, one compound splits apart into two or more substances. These substances can be elements or simpler compounds. AB > A + B 1. Binary compounds breakdown into their elements. 2. Carbonates break down into an oxide and carbon dioxide REACTION GUIDELINES 3. Chlorates break down to a binary salt and oxygen. 4. Bases break down to the oxide of the metal and water. 5. Acids break down to the oxide of the nonmetal plus water. REACTION GUIDELINE EXAMPLES 1. 2 NaCl ----> 2 Na + Cl2 2. Na2CO3 ----> Na2O + CO2 3. Ba(ClO3)2 ----> BaCl2 + O2 4. Ca(OH)2 ----> CaO + H2O 5. 2 H3PO4 ----> P2O5 + 3 H2O Decomposition Reaction Practice 1) Ni(ClO3)2 ---> 6) Cs2CO3 ---> 2) Ag2O ---> 7) Al(OH)3 ---> 3) HNO2 ---> 8) H2SO4 ---> 4) Fe(OH)3 ---> 9) RbClO3 ---> 5) ZnCO3 ---> 10) RaCl2 ---> 18

19 Synthesis and Decomposition Reactions Synthesis reactions are chemical reactions in which two or more substances react to form a new product. The general form of a synthesis reaction is written as: A + B à AB Decomposition reactions are chemical reactions in which a reactant breaks down into two or more products. The general form of a decomposition reaction is written as: AB à A + B Balance the following reactions and identify whether the reaction is a synthesis or decomposition reaction. Balance the Reactions: Synthesis or Decomposition? 1. Ca + O 2 à CaO 2. H 2 + N 2 à NH 3 3. H 2 O 2 à H 2 O + O 2 4. H 2 + O 2 à H 2 O 5. CaCO 3 à CaO + CO 2 6. H 2 + Cl 2 à HCl 7. Al + Br 2 à AlBr 3 8. Zn(OH) 2 à ZnO + H 2 O 9. HgO à Hg + O Cr + O 2 à Cr 2 O Na + I 2 à NaI 12. Ag 2 O à Ag + O 2 19

20 Balancing Equations Balance the reactions: Synthesis or Decomposition? 1. Cu + S 8 à CuS 2. NaClO 3 à NaCl + O 2 3. MgCO 3 à MgO + CO 2 4. Al 2 O 3 à Al + O 2 5. Ag + S 8 à Ag 2 S 6. P + O 2 à P 2 O 5 7. S 8 + O 2 à SO 3 8. H 2 O à H 2 + O 2 9. CO + O 2 à CO H 2 SO 4 à H 2 + SO KClO 3 à KCl + O AlCl 3 à Al + Cl Cu + O 2 à CuO 20

21 14. Fe + O 2 à Fe 2 O 3 Double Replacement Reaction CHEMISTRY REPLACEMENT REACTION WORKSHEET DISCRIPTION During double replacement, the cations and anions of two different compounds switch places. AB + CD -----> AD + CB REACTION GUIDELINE 1. It is important that the formulas of the products be written correctly. If they are correct, balancing the equation is a simple task; if not, the equation will probably never balance. 2. In these reactions, there is never a change in oxidation state (in other words, the charges stay the same). EXAMPLES AgNO3 + NaCl ---> AgCl + NaNO3 Silver nitrate + sodium chloride silver chloride + sodium nitrate Pb(NO3)2 + CuSO4 ---> PbSO4 + Cu(NO3)2 Lead (II) nitrate + copper (II) sulfate lead (II) sulfate + copper (II) nitrate DOUBLE REPLACEMENT PRACTICE REACTIONS For each reaction predict the products and balance the equation. State the reaction in chemical formulas and in symbols. For example: AgNO 3 + NaCl ---> Silver nitrate + sodium chloride silver chloride + sodium nitrate AgNO 3 + NaCl ---> AgCl + NaNO 3 1) Ca(OH) 2 + H 3 PO 4 ---> 2) K 2 CO 3 + BaCl 2 ---> 3) Cd 3 (PO4) 2 + (NH 4 ) 2 S ---> 4) Co(OH) 3 + HNO 3 ---> 21

22 5) AgNO3 + KCl ---> 6) Na 2 CO3 + H 2 SO 4 ---> 7) Al(OH) 3 + HC 2 H 3 O 2 ---> 8) Al 2 (SO 4 ) 3 + Ca 3 (PO 4 ) 2 ---> 9) Cr 2 (SO 3 ) 3 + H 2 SO 4 ---> 10) AgC 2 H 3 O 2 + K 2 CrO 4 ---> 11) FeBr 2 + K 2 CO 3 ---> Single Replacement Reaction Chart 22

23 Activity Series Chart Metals Non-Metals Most Active Least Active Name Symbol Name Symbol Lithium Li Fluorine F Potassium K Chlorine Cl Barium Ba Bromine Br Strontium Sr Iodine I Calcium Ca Sodium Na Magnesium Mg Aluminum Al Manganese Mn Zinc Zn Iron Fe Cadmium Cd Cobalt Co Nickel Ni Tin Sn Lead Pb Hydrogen H Copper Cu Silver Ag Mercury Hg Gold Au *** Elements CANNOT replace anything ABOVE them. The reaction DOES NOT OCCUR in this situation. *** 23

24 Name: Single Replacement Reactions Worksheet A. Predict the products and balance the following single replacement reactions. If no reaction occurs write N.R. For transition metals use the following charges: Iron: Fe 3+ Mercury: Hg 2+ Lead: Pb 4+ Copper: Cu 1+ Gold: Au +3 1) Fe + CuCl 2 2) Hg + Sn(SO 4 ) 2 3) Ba + Ni 3 (PO 4 ) 2 4) Pb + Au(NO 3 ) 3 5) Li + HOH 6) K + AgCl 7) Ca + NaOH 8) Cu + Fe(OH) 3 9) Fe + Cu(OH) 2 24

25 Single Replacement Practice Name 1. Ag + K(NO3) à 2. Zn + 2 Ag(NO3) à 3. Al + H2(SO4) à 4. Cl2 + KI à 5. Li + H2O à 6. Cu + Fe(SO4) à 7. Na + H2O à 8. Cu + H2O à 9. Cl2 + NaI à 10. Al + CuCl2 à 11. Br2 + CaI2 à 12. Al + HCl à 13. Cl2 + MgI2 à 14. Fe + Cu(SO4) à 25

26 15. Cl + Cu(SO4) à Types of Reactions Worksheet Balance the following equations and indicate the type of reaction taking place: 1) NaBr + H3PO4 à Na3PO4 + HBr Type of reaction: 2) Ca(OH)2 + Al2(SO4)3 à CaSO4 + Al(OH)3 Type of reaction: 3) Mg + Fe2O3 à Fe + MgO Type of reaction: 4) C2H4 + O2 à CO2 + H2O Type of reaction: 5) PbSO4 à PbSO3 + O2 Type of reaction: 6) NH3 + I2 à N2I6 + H2 Type of reaction: 7) H2O + SO3 à H2SO4 Type of reaction: 26

27 8) H2SO4 + NH4OH à H2O + (NH4)2SO4 Type of reaction: Reaction Types + Balancing Equations Practice Problems: Balance Equations (add or coefficients only) 1. C O 2 CO 2 Type of reaction is 2. NaCl F 2 NaF Cl 2 Type of reaction is 3. H 2 F 2 HF Type of reaction is 4. C 6 H 12 O 6 C H 2 O Type of reaction is 5. AgNO 3 NaCl AgCl NaNO 3 Type of reaction is 27

28 Types of Reactions Worksheet Indicate the type of reaction taking place: 1) NaBr + H 3 PO 4 Na 3 PO 4 + HBr Reaction type: 2) Ca(OH) 2 + Al 2 (SO 4 ) 3 CaSO 4 + Al(OH) 3 Reaction type: 3) Mg + Fe 2 O 3 Fe + MgO Reaction type: 4) C 2 H 4 + O 2 CO 2 + H 2 O Reaction type: 5) PbSO 4 PbSO 3 + O 2 Reaction type: 6) NH 3 + I 2 N 2 I 6 + H 2 Reaction type: 7) H 2 O + SO 3 H 2 SO 4 Reaction type: 8) O 2 + C 3 H 8 H 2 O + CO 2 Reaction type: 28

29 9) NaOH + KNO 3 --> NaNO 3 + KOH Reaction type: 10) CH 4 + O 2 --> CO 2 + H 2 O Reaction type: 11) Fe + NaBr --> FeBr 3 + Na Reaction type: 12) CaSO 4 + Mg(OH) 2 --> Ca(OH) 2 + MgSO 4 Reaction type: 13) Na 2 CO 3 --> Na 2 O + CO 2 Reaction type: 14) Pb + O 2 --> PbO 2 Reaction type: 29

30 Identify each chemical reaction as a synthesis (combination), decomposition, singlereplacement, double-replacement, or combustion reaction. 1. 2SO 2 + O 2 2SO 3 2. Al 2 (SO 4 ) 3 + 3Ca(OH) 2 2Al(OH) 3 + 3CaSO C 2 H 2 + 5O 2 4CO 2 + 2H 2 O 4. Mg + 2AgNO 3 Mg(NO 3 ) 2 + 2Ag 5. 3Ba(NO 3 ) 2 + 2H 3 PO 4 Ba 3 (PO 4 ) 2 + 6HNO 3 6. Mg(ClO 3 ) 2 MgCl 2 + 3O Be + O 2 2BeO 8. 2Al + 3CuSO 4 Al 2 (SO 4 ) 3 + 3Cu 9. 2PbO 2 2PbO + O C 2 H 6 + 7O 2 4CO 2 + 6H 2 O Complete the chemical equations for the following SYNTHESIS (COMBINATION) reactions. 11. Mg + O Ca + S 13. Na + O Na + Cl Al + O 2 Use the activity series of metals to complete the following SINGLE-REPLACEMENT reactions. Write NR if there is no reaction. 16. Zn(s) + AgNO Au(s) + KNO Al(s) + H 2 SO Cu(s) + H 2 O 20. Al(s) + CuSO 4 Write the chemical equation for the complete COMBUSTION of the following compounds. 21. octane (C 8 H 18 ) C 8 H glucose (C 6 H 12 O 6 ) C 6 H 12 O

31 Complete the chemical equations for the following DOUBLE-REPLACEMENT reactions. 23. Ag 2 SO 4 + AlCl CdBr 2 + Na 2 S 25. Pb(NO 3 ) 2 + NaI 26. NaOH + Fe(NO 3 ) NaNO 3 + BaCl 2 Write the type of reaction on the line. Then, predict the products of each reaction to complete the chemical equation. Write the correct formulas of the products after the arrow. Write NR if there is no reaction. 28. Ag 2 O 29. C 4 H 8 + O Al + N Zn + CuSO Pb(NO 3 ) 2 + K 2 CrO Li + O Al 2 (SO 4 ) 3 + Ba(OH) Cu + CaCO C 3 H 6 + O Na 3 PO 4 + Pb(NO 3 ) 2 Write the chemical equation for the following reactions. Remember the diatomics. Use appropriate state symbols. 38. Solid silver carbonate decomposes into solid silver oxide and gaseous carbon dioxide when heated. 39. Adding chlorine gas to a solution of potassium iodide gives solid iodine and a solution of potassium chloride. 40. Iodine crystals react with chlorine gas to form solid iodine trichloride. 31

32 WebQuest!! -Get into your pre-assigned groups for this project. -Go to the link listed above. -First: read the introduction -Second: read the task -Third: read the process etc. -Your lesson should be at least 20 minutes, but no more than 30 minutes! 32

33 Formula Writing Refresher Write chemical formulas for the compounds in each box. The names are found by finding the intersection between the cations and anions. Example: The first box is the intersection between the zinc cation and the chloride anion, so you should write ZnCl 2, as shown. Cations Anions zinc iron (II) iron (III) gallium silver lead (IV) chloride ZnCl 2 acetate nitrate oxide nitride sulfate Write the formulas for the following compounds: 1) copper (II) chloride 2) lithium acetate 3) vanadium (III) selenide 4) manganese (IV) nitride 5) beryllium oxide 6) sodium sulfate 7) aluminum arsenide 8) potassium permanganate 9) chromium (VI) cyanide 10) tin (II) sulfite 11) vanadium (V) fluoride 12) ammonium nitrate 33

34 Writing Word Equations 1. You will combine formula writing, reaction type, and balancing equation to create an appropriate chemical reaction from each of the word equations provided. Diatomic Molecules- molecules that naturally occur in pairs, and they are: H 2, N 2, O 2, F 2, Cl 2, Br 2, I 2 EX: When sodium reacts with iron (II) chloride, iron and sodium chloride are formed. 1. Break the sentence down: When sodium reacts with iron (II) chloride, iron and sodium chloride are formed 2. Write out the reactant and product formulas. Reactants, reacts: Sodium (Na), Iron (II) Chloride (FeCl 2 ) Products, formed: Iron (Fe), Sodium Chloride (NaCl) 3. Put it all together: Na + FeCl 2 à Fe + NaCl 4. Make sure everything is balanced!! Na + FeCl 2 à Fe + NaCl Na: 1 Na: 1 Fe: 1 Fe: 1 Cl: 2 Cl: 1 SO our final reaction: 2 Na + FeCl 2 à Fe + 2 NaCl 34

35 Writing the Complete Equation Homework Write the complete chemical equation for each of the following chemical reactions: 1) When iron solid is placed in liquid lithium sulfate and electricity is added to it, iron (II) sulfate crystals and solid lithium metal are formed. 2) When the ethanol (C 2 H 6 O) in some gasoline burns with oxygen gas in an automobile engine, it forms carbon dioxide gas and water vapor. 3) When the pressure on an aqueous solution of carbonic acid is decreased to 0.1 atmospheres, it decomposes to form carbon dioxide gas and water. 4) When iodine gas reacts with methane gas at very high temperatures, CH 3 I gas and hydrogen iodide gas are formed. 5) When dinitrogen hexaiodide crystals are hit with a hammer, they spontaneously and explosively decompose to form nitrogen gas and iodine powder. 6) When hydrochloric acid gas reacts with gaseous ammonia, water vapor and solid ammonium chloride are formed. 35

36 Word Equations Write the word equations below as chemical equations and balance: 1) Zinc and lead (II) nitrate react to form zinc nitrate and lead. 2) Aluminum bromide and chlorine gas react to form aluminum chloride and bromine gas. 3) Sodium phosphate and calcium chloride react to form calcium phosphate and sodium chloride. 4) Potassium metal and chlorine gas combine to form potassium chloride. 5) Aluminum and hydrochloric acid react to form aluminum chloride and hydrogen gas. 6) Calcium hydroxide and phosphoric acid react to form calcium phosphate and water. 7) Copper and sulfuric acid react to form copper (II) sulfate and water and sulfur dioxide. 8) Hydrogen gas and nitrogen monoxide react to form water and nitrogen gas. 36

37 Word Equations Problems Write out the following chemical equations, be sure to balance the equations. 1. Zinc and lead (II) nitrate react to form zinc nitrate and lead. 2. Aluminum bromide and chlorine gas react to form aluminum chloride and bromine gas. 3. Sodium phosphate and calcium chloride react to form calcium phosphate and sodium chloride. 4. Potassium metal and chlorine gas combine to form potassium chloride. 37

38 5. Aluminum and hydrochloric acid react to form aluminum chloride and hydrogen gas. 6. Calcium hydroxide and phosphoric acid (HPO 4 ) react to form calcium phosphate and water. 7. Copper and sulfuric acid (H 2 SO 4 ) react to form copper (II) sulfate and water and sulfur dioxide. 8. Hydrogen gas and nitrogen monoxide react to form water and nitrogen gas. 38

39 Activity Series Chart Metals Non-Metals Most Active Least Active Name Symbol Name Symbol Lithium Li Fluorine F Potassium K Chlorine Cl Barium Ba Bromine Br Strontium Sr Iodine I Calcium Ca Sodium Na Magnesium Mg Aluminum Al Manganese Mn Zinc Zn Iron Fe Cadmium Cd Cobalt Co Nickel Ni Tin Sn Lead Pb Hydrogen H Copper Cu Silver Ag Mercury Hg Gold Au *** Elements CANNOT replace anything ABOVE them. The reaction DOES NOT OCCUR in this situation. *** 39