Name/……………… Date/…………….. TYPES OF CHEMICAL REACTIONS LAB ● COMPLETECOMPLETE THE REACTION TABLE ON THE LAST PAGE OF THE HANDOUT. ● Write the balanced equations for each of these reactions in the Reaction Table. Remember to write the State symbol [(g),(l),(s), or (aq)] after each reactant or product for all of the chemical equations in your Reaction Table. Many of the changes you observe in the world around you are caused by chemical reactions. Examples include changing colors of leaves, cooking food and getting clean. Knowing some chemistry can help you make day to day decisions that affect your life. Can I mix these household chemicals? What are safe mosquito repellents? Will my bottled water expire? The evidence that reactions are occurring may be (1) a gas is produced (2) a precipitate (a solid produced when two solutions are mixed) is formed, (3) a color change is observed, (4) a temperature change is noted, or (5) a flame is produced. I. Purpose: To view the actual chemical reactions, write the correct balanced chemical equation, and type of chemical reaction. II. Materials: Burner, test tube, metal tongs (only…no rubber ends), microspatula, evaporating dish, wood splints Chemicals: magnesium (ribbon), copper (II) carbonate , hydrochloric acid, lead (II) nitrate , sodium chloride, potassium iodide, sodium bicarbonate, Potassium iodide Calcium carbonate, Copper (II) Carbonate and Lime water(calcium oxide+water). Safety goggles, test tube holder. III. Procedure PART A - SYNTHESIS REACTIONS https://chem.libretexts.org/Bookshelves/Ancillary_Materials/Demos%2C_Techniques%2C_a nd_Experiments/Lecture_Demonstrations/Burning_Magnesium 1. Magnesium and oxygen A. Procedure Obtain a piece of magnesium ribbon. In order not to damage the bench top, perform the next step of the experiment over your evaporating dish (an evaporating dish looks like a small, white ceramic bowl and is located in your locker drawer). Holding one end of the magnesium ribbon with your tongs (tongs are located in the common locker), ignite the other end in the burner flame. Look for just a moment at the burning magnesium; do not stare at the magnesium while it is burning because of the intensity of the light Dispose of the ash from this part of the experiment in the trashcan. Name/……………… Date/…………….. PART B -SINGLE REPLACEMENT REACTIONS 2. hydrochloric acid + METAL https://www.youtube.com/watch?v=SeKsLi_6WkY Place 3mL of 6M hydrochloric acid (HCl) into a medium test tube. Add a small piece of magnesium or zinc metal (labelled "magnesium turnings") to the test tube. If a gas is produced, hold your thumb over the mouth of the test tube for about one minute, light a wooden splint with a Bunsen burner, then remove your thumb and hold the burning splint to the mouth of the test tube. You will hear a sound when the H2 gas that was produced. . PART C – DOUBLE REPLACEMENT REACTIONS PRECIPITATION REACTIONS 3. lead (II) nitrate + sodium chloride https://www.youtube.com/watch?v=s64_8dO0EXc Place about 2 mL of lead (II) nitrate solution into a clean, medium test tube, and place about 2 mL of sodium chloride solution into a second clean, medium test tube. Add about 2 mL of potassium iodide solution to both of the test tubes. Record any evidence of chemical change in your Data Table. write the balanced equations in the Reaction Table. 4. lead (II) nitrate + potassium iodide https://www.youtube.com/watch?v=73dw6w0zNXA Place about 2 mL of lead (II) nitrate solution into a clean, medium test tube, and about 2 mL of potassium iodide solution. Record any evidence of chemical change in your Data Table. Write the balanced equations in the Reaction Table 5. sodium bicarbonate (NaHCO3) + Hydrochloric acid HCl solution https://www.youtube.com/watch?v=xRfPvDEs2gM Place about 3.0 mL of sodium bicarbonate (NaHCO3) solution in the bottom of a large test tube. Add a few drops of 6M HCl solution. Record any evidence of chemical change in the Observation Data 6. Sodium sulphite NaSO3 + Hydrochloric acid HCl solution https://www.youtube.com/watch?v=BlpjKceHF3g Sodium sulfite reacted with hydrochloric acid to form sodium chloride, sulfur dioxide (stinky gas usually released from volcanoes), and water. PART D –DECOMPOSITION 7. Heating calcium carbonate CaCO3 Calcium carbonate is strongly heated until it undergoes thermal decomposition to form calcium oxide and carbon dioxide. The calcium oxide (unslaked lime) is dissolved in water to form calcium hydroxide (limewater). Bubbling carbon dioxide through this forms a milky suspension of calcium carbonate. https://www.youtube.com/watch?v=RLL5rT_DeKc Name/……………… Date/…………….. 8. Heating Copper (II) Carbonate CuCO3 https://www.youtube.com/watch?v=D9amrlph-rA Copper (II) carbonate decomposes when heated to give copper oxide and gaseous carbon dioxide. Green colored copper carbonate gives black colored copper oxide. DATA TABLE Reactants 1. Magnesium and oxygen 2. HCl + METAL 3. Pb(NO3)2 + NaCl 4. Pb(NO3)2 + KI 5. NaHCO3+ HCl 6. NaSO3 + HCl 7. Heating CaCO3 8. Heating CuCO3 Balanced Equation Evidence of reaction Name/……………… Date/…………….. HW I. ANSWER THE FOLLOWING QUESTIONS Copper (II) and magnesium burn to form new compounds. Both react with oxygen to form oxides of each metal. Write a balanced chemical equation for each reaction below. What type of chemical reactions occurred with the copper and magnesium? II. In both the mercury (II) oxide and copper (II) carbonate HEATING reactions, a gas was produced. If oxygen was produced the flame would have gotten brighter and burned more, if hydrogen was produced a “pop” and short blue flame will be produced, but if carbon dioxide was produced it would extinguish the flame. A. What gas was produced in the mercury (II) oxide reaction? B. What gas was produced in the copper (II) carbonate reaction? C. write out a balanced equation for each reaction IN A and B. D. What type of reactions occurred with the mercury (II) carbonate and copper (II) carbonate? ● Conclusion: How does a person know if a chemical reaction has occurred?
