CHEMICAL REACTIONS PART II Arbuiso Chem This is work that you are supposed to DO, and most of the time, HAND IN for a grade. MAKE SURE YOU PUT YOUR NAME ON TOP OF EACH ONE.
Table F Handout name ________________ List only the precipitates. If both products are aqueous there is NO EVIDENCE that a chemical reaction has taken place, mark those boxes with an “X” for no reaction. The two boxes filled in are your examples. Solutions Lead (II) calcium potassium silver ammonium you mix nitrate chloride hydroxide nitrate chloride 1 2 3 4 PbCl 2(S) sodium chloride Lead II chloride 5 6 7 8 9 sodium sulfate 10 11 12 14 15 sodium hydroxide 16 17 18 19 20 lithium bromide 21 22 23 24 25 potassium phosphate 26 27 28 29 ammonium X carbonate
Balancing Chemical Equations #1 name: _____________________ Type of Balance perfectly, name the type of reaction (Synth, Decomp, SR, DR, or Comb.) Reaction Many of the dashes will be “ones” and we don’t write ones in chem, we are Number 1! __H 2(G) + __O 2(G) → __H 2 O (G) __Sr(OH) 2(AQ) + __Li 2 CrO 4(AQ) → __SrCrO 4(S) + __LiOH (AQ) __ZnBr 2(AQ) + __Al (S) → __AlBr 3(AQ) + __Zn (S) __C (S) + __S 8(S) → __CS 2(S) __K (S) + __Ni(C 2 H 3 O 2 ) 3(AQ) → __KC 2 H 3 O 2(AQ) + __Ni (S) __N 2(G) + __O 2(G) → __N 2 O 5(G) __P (S) + __Cl 2(G) → __PCl 5(S) __Pb(NO 3 ) 2(AQ) + __LiCl (AQ) → __PbCl 2(S) + __LiNO 3(AQ) __Al (S) + __S 8(S) → __Al 2 S 3(S) __H 2 O (L) → __H 2(G) + __O 2(G) __Mg (S) + __Cl 2(G) → __MgCl 2(S) __C 15 H 32(S) + __O 2(G) → __CO 2(G) + __H 2 O (G) __C 6 H 6(G) + __O 2(G) → __CO 2(G) + __H 2 O (G) __N 2(G) + __H 2(G) → __NH 3(G)
Balancing Chemical Equations #2 name: _____________________ Type of Balance perfectly, name the type of reaction (Synth, Decomp, SR, DR, or Comb.) Reaction Many of the dashes will be “ones” and we don’t write ones in chem, we are Number 1! __Li (S) + __TiCl 3(AQ) → __LiCl (AQ) + __Ti (S) __C 2 H 6(G) + __O 2(G) → __CO 2(G) + __H 2 O (G) __Rb (S) + __P (S) → __Rb 3 P (S) __CH 4(G) + __O 2(G) → __CO 2(G) + __H 2 O (G) __Na (S) + __I 2(S) → __NaI (S) __Rb (S) + __S 8(S) → __Rb 2 S (S) __Al(HCO 3 ) 3(AQ) + __CaCrO 4(AQ) → __Al 2 (CrO 4 ) 3(S) + __Ca(HCO 3 ) 2(AQ) __Li (S) + __SnCl 4(AQ) → __LiCl (AQ) + __Sn (S) __NH 3(G) → __N 2(G) + __H 2(G) __Cs (S) + __N 2(G) → __Cs 3 N (S) __CaCO 3(S) → __CaO (S) + __CO 2(G) __C 10 H 22(S) + __O 2(G) → __CO 2(G) + __H 2 O (G) __Mn (S) + __ZnSO 4AQ) → __Mn 2 (SO 4 ) 7(AQ) + __Zn (S) __C 3 H 8(G) + __O 2(G) → __CO 2(G) + __H 2 O (G)
Precipitate Lab: Making Ionic Compounds Name_____________________________ (40 minutes) Objectives: In this laboratory activity, you will do 9 double replacement reactions, observe any precipitates that form, and then use table F to balance and provide phase symbols to these 9 reactions. All of these react, although “E” will be very, very faint. Always trust table F. Directions: Lay the sheet with the boxes on a flat table surface. Place a plastic sheet over it. In each of the squares: put 2 drops of both of the aqueous solutions in each square. NEVER EVER MIX CHEMICALS, or TOUCH DROPPER TO THE SHEET!! Observe carefully on the white sheet, and on the black table top, for precipitates. Once you have finished trash the plastic sheets. Clean your lab area up. Six Lab Questions 1. Explain the “KB square dance” reference that explains how a double replacement reaction happen. (Love = precipitate = DR) 2. Describe what happens when sodium chloride is put into water. Try to include “The solution contains loose…” Would this solution conduct electricity? Include the chemical symbols (look on table I for a hint for this). 3. Describe what happens when table sugar (C 12 H 22 O 11 ) dissolves into water. Try to include “The solution contains loose…, but does not contain any…” How is this different than ionic compounds like NaCl that dissolve in water? Would this solution conduct electricity? 4. Describe what happens when you put calcium sulfate into water. Why would it NOT dissolve? Would this conduct electricity? How is this different than when NaCl solid goes into water? 5. Write a balanced chemical equation with phases for the double replacement reaction between ammonium phosphate and niobium (V) nitrate solutions. 6. Write a balanced chemical equation with phases for the double replacement reaction between the two aqueous solutions of lead (II) acetate and sodium bromide. This lab Includes points report Cover Title, optional drawing, single sentence explaining what you did today. 1 1 9 balanced chemical reactions WITH PHASE SYMBOLS 9 2 6 lab questions - above (do them on loose leaf paper) 6 Name the 6 main indicators of chemical reactions Explain what this means: AQ + AQ → diff AQ + Solid Explain what this means: AQ + AQ → diff AQ + diff AQ Then tell how and why we use Table F. Conclusion 9 Define electrolytic solution + give 3 examples of electrolyte solutions. Using table F, Name 3 ionic compounds that do not dissolve in water. If an ionic compound FORMS during a Double Replacement Reaction it precipitates. What would happen if we put that same insoluble ionic compound into water? 25 THIS LAB REPORT IS DUE _____________
BALANCED EQUATIONS REACTI0N PHASE SYMBOLS ARE MANDATORY BOX A B C D E F G H I
Copper (II) sulfate Magnesium nitrate Cobalt (II) nitrate A B C sodium carbonate D E F sodium phosphate G H I sodium hydroxide
Type of Skeletons, finish them, balance whenever possible, use phase symbols Reaction exam- SR ple Mg (S) + H 2 SO 2(AQ) → MgSO 4(AQ) + H 2(G) (balanced as is) 1 C 3 H 8(G) + O 2(G) → 2 (NH 4 ) 2 S (AQ) + Al(NO 3 ) 3(AQ) → 3 Ba 3 P 2(S) → 4 Al + O 2(G) → Al 2 O 3(S) 5 Na 2 SO 4(AQ) + SrCl 2(AQ) → 6 Fe (S) + CuCl 2(AQ) → FeCl 3(AQ) + Cu (S) 7 C 8 H 18 + O 2(G) → 8 Co (S) + S (S) → Co 2 S 3(S) 9 KNO 3(S) → KNO 2(S) + O 2(G) 10 Cl 2(G) + LiBr (AQ) → 11 Al(NO 3 ) 3(AQ) + (NH 4 ) 2 SO 4(AQ) → 12 Pb(NO 3 ) 2(AQ) + LiF (AQ) → 14 BeF 2(S) → Be (S) + F 2(G)
Reactions HW #1 - Synthesis and Decomposition Name: ___________________________________ Write out the word equations or balanced chemical equations for these 7 reactions, including phases, then indicate if they are Synthesis or Decomposition reactions in the last column. Is this reaction synthesis or If there are symbols, write the word equation, if there are words, # decomposition? write the balanced chemical equation with phase symbols. S or D 2Mg + O 2 → 2MgO 1 Fe 2 S 3 → 2Fe + 3S 2 MgO + CO 2 → MgCO 3 3 copper I sulfide powder breaks down into copper and sulfur 4 beryllium combines with oxygen to form beryllium oxide 5 calcium reacts with nitrogen to form calcium nitride 6 Potassium chlorate breaks down to potassium chloride & oxygen 7 N 2(G) + O 2(G) → 2NO (G) 8
Reactions HW #2 - Single Replacement Reactions Name: ____________________________________ Write balanced chemical reactions for each of these, with phase symbols. If there is no reaction, write the symbols for the reactants, an arrow and an “X”. A solution means it is AQUEOUS. Zinc reacts with 1 hydrochloric acid solution Iron (II) nitrate solution 2 plus silver metal Fluorine gas mixed with 3 sodium bromide solution Gold (III) chloride solution 4 with magnesium metal Copper (II) sulfate solution 5 with silver metal Bromine liquid into 6 ammonium iodide solution Ammonium fluoride 7 solution and chlorine gas Lithium hydroxide solution 8 with titanium metal Barium hydrogen 9 carbonate solution and lithium metal Potassium sulfate solution 10 with lead metal Aluminum metal into 11 nickel (II) chlorate solution
Reactions HW #3 - Double Replacement Reactions Name: __________________________________ Write balanced equations with PHASES, which are mandatory. Use the Solubility Guidelines Table (table F). One of these is not a reaction, will you find it? If it is a “no reaction”, you will still balance the equation and indicate both products as AQ. Do not just write NO REACTION, that is not enough. Sodium carbonate + zinc chlorate solutions react Copper (II) sulfate + calcium chloride solutions react Potassium hydroxide + lead (IV) nitrate solutions react Silver hydrogen carbonate + Iron (II) bromide solutions react Barium hydroxide + lithium sulfate solutions react Ammonium phosphate + tin (II) acetate solutions react Calcium chromate + sodium sulfide solutions react Strontium acetate + lithium carbonate solutions react Ammonium phosphate + rubidium nitrate solutions react
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