Compounds & Reactions Week 1. Writing Formulas & Balancing Equations. Write the chemical formula for each molecular (covalent) compound.
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1 Compounds & Reactions Week 1 Name Writing Formulas & Balancing Equations Write the chemical formula for each ionic compound. 1. Lithium fluoride 2. Copper (II) chloride 3. Manganese (II) oxide 4. Potassium permanganate 5. Silver acetate 6. Calcium hydride 7. Ammonium Sulfate 8. Zinc hydroxide Write the chemical formula for each molecular (covalent) compound. 9. Carbon dioxide 10. Ammonia 11. Hydrogen sulfide 12. Carbon disulfide 13. Sulfur trioxide 14. Oxygen gas 15. Nitrogen monoxide 16. Boron trichloride Write the chemical formula for each acid. 17. Acetic acid 18. Sulfuric acid 19. Hydrochloric acid 20. Nitric acid Balance each reaction with coefficients. 21. H2S (g) + Cd(NO3)2 (aq) CdS (s) + HNO3 (aq) 22. Na2O + H2O (l) NaOH (aq) 23. C3H7OH (l) + O2 (g) CO2 (g) + H2O (g) 24. H2O2 (aq) H2O (l) + O2 (g) 25. Al (s) + AgNO3 (aq) Al(NO3)3 (aq) + Ag
2 Compounds & Reactions Week 2 Name Solubility Rules & Writing Equations Name Formula Soluble? State Particles found in solution (if aqueous) Sodium Acetate NaC2H3O2 Yes (aq) Na + and C2H3O2 - Acetic Acid HC2H3O2 Yes (aq) HC2H3O2 Sodium hydroxide Hydrofluoric acid Tin (III) chloride Iron (III) oxide Potassium iodide Nitric acid Sulfurous acid Sodium carbonate Write a balanced equation for each set of reactants by predicting the products then balancing. Include the states (s), (l), (g), or (aq) with each chemical formula. Use the sentences for clues and remember your solubility rules. If there is no mention of water or solutions, you cannot have anything (aq). 1. A strip of magnesium is added to a solution of silver nitrate. 2. Solutions of manganese (II) sulfate and ammonium sulfide are mixed. 3. Calcium metal is heated strongly in nitrogen gas. 4. Solid magnesium carbonate is heated.
3 Compounds & Reactions Week 3 Name Part 1 Write the chemical formula. 1. Hydrogen gas 2. Atomic hydrogen 3. Copper(II) oxide 4. Lead (III) acetate 5. Strontium nitrate Part 2 Write a balanced equation. 6. A strip of lead metal is added to a solution of silver nitrate. 7. Propanol is burned in oxygen. 8. A strip of aluminum foil is placed in liquid bromine. 9. Solutions of cobalt(ii) nitrate and sodium hydroxide are mixed. 10. Solid magnesium carbonate is heated.
4 Part 3 Write the net ionic equation in the box. All other work should be outside the box. Answer the questions following each reaction. 11. A piece of aluminum metal is added to a solution of silver nitrate. ii. What type of reaction is this? 12. An excess of sodium hydroxide solution is added to a solution of magnesium nitrate. ii. What compound is the precipitate? 13. The hydrocarbon hexane is burned in excess oxygen. ii. What type of reaction is this?
5 Compounds & Reactions Week 4 Name Part 1 Write the chemical formula. 1. Ethanol 2. Manganese(II) sulfide 3. Nitric acid 4. Chlorine gas 5. Sodium bromide Part 2 Write a balanced equation. 6. A small piece of sodium is added to a beaker of distilled water. 7. Solid magnesium carbonate is heated. 8. A solution of sodium hydroxide is added to a solution of lead (II) nitrate. 9. Magnesium metal is burned in nitrogen gas 10. A strip of zinc is added to a solution of 6.0 molar hydrochloric acid.
6 Part 3 Write the net ionic equation in the box. All other work should be outside the box. Answer the questions following each reaction. 11. Excess nitric acid is added to solid calcium carbonate. ii. Which chemical could be described as an intermediate? Explain your reasoning. 12. Dilute hydrochloric acid is added to a solution of potassium carbonate. ii. What are the spectator ion(s) in this reaction? 13. Chlorine gas is bubbled into a solution of sodium bromide ii. Which element is oxidized?
7 Compounds & Reactions Week 5 Name Part 1 Write the chemical formula. 1. potassium bicarbonate 2. nickel (III) acetate 3. tin (II) hydroxide 4. oxalic acid 5. sodium sulfite Part 2 Write a balanced equation. 6. Solid potassium chlorate is heated in the presence of manganese dioxide as a catalyst. 7. A solution of silver acetate is added to a solution of sodium phosphate. 8. Solid zinc strips are added to a solution of copper(ii) sulfate. 9. Octane is burned completely in air. 10. Powdered magnesium oxide is added to a container of carbon dioxide gas.
8 Part 3 Write the net ionic equation in the box. All other work should be outside the box. Answer the questions following each reaction. 11. Liquid bromine is added to a solution of potassium iodide. ii. Which element is being reduced? 12. Solid potassium oxide is added to water.. ii. What color would the reaction mixture be if you added phenolphthalein?? 13. Solutions of silver nitrate and sodium chromate are mixed. ii. If 1.0 L of 2 M silver nitrate is added to 1.0 L of 1 M sodium chromate, how many moles of precipitate will be formed?
9 Compounds & Reactions Week 6 Name Part 1 Write the chemical formula. 1. sodium nitrate 2. sulfur trioxide 3. lead (IV) chlorate 4. potassium peroxide 5. sulfurous acid Part 2 Write a balanced equation. 6. Dilute hydrochloric acid is added to a solution of potassium carbonate 7. Dilute sulfuric acid is added to a solution of barium chloride. 8. Solutions of zinc sulfate and sodium phosphate are mixed. 9. Concentrated hydrochloric acid is added to solid manganese(ii) sulfide. 10. Solid barium oxide is added to distilled water.
10 Part 3 Write the net ionic equation in the box. All other work should be outside the box. Answer the questions following each reaction. 11. Carbon dioxide gas is bubbled through water. ii. Describe the ph of the resulting solution. 12. Solid strontium carbonate is heated. ii. If 2 moles of solid are heated, how many moles of solid are produced? 13. Solutions of zinc sulfate and sodium phosphate are mixed. ii. Name the spectator ions in this reaction.
11 Compounds & Reactions Week 7 Name Part 1 Write the chemical formula. 1. aluminum hydroxide 2. diphosphorus pentoxide 3. nitrous acid 4. sodium nitrite 5. pentane Part 2 Write a balanced equation. 6. A solution of hydrogen peroxide is heated. 7. Solutions of silver nitrate and sodium chromate are mixed. 8. Calcium metal is heated strongly in nitrogen gas. 9. Solid potassium oxide is added to water. 10. Dilute sulfuric acid is added to a solution of barium chloride.
12 Part 3 Write the net ionic equation in the box. All other work should be outside the box. Answer the questions following each reaction. 11. Propanol is burned completely in air. ii. If 5 moles of propanol are burned, how many moles of oxygen are required? 12. Lead foil is immersed in silver nitrate solution ii. Which species is gaining electrons? 13. Gaseous hydrogen sulfide is bubbled through a solution of nickel(ii) nitrate. ii. Name the spectator ion(s) in this reaction,
13 Compounds & Reactions Week 8 Name Part 1 Write the chemical formula. 1. sodium nitrite 2. calcium acetate 3. ammonium phosphate 4. barium cyanide 5. pentanol Part 2 Write a balanced equation. 6. Solid calcium oxide is heated in the presence of carbon dioxide gas. 7. Calcium metal is heated strongly in nitrogen gas. 8. A piece of aluminum metal is added to a solution of silver nitrate. 9. Dilute hydrochloric acid is added to a solution of potassium carbonate. 10. Solid ammonium carbonate is heated.
14 Part 3 Write the net ionic equation in the box. All other work should be outside the box. Answer the questions following each reaction. 11. Excess chlorine gas is passed over hot iron filings. ii. What is the type of reaction for the reverse process of the above reaction? 12. Solid potassium oxide is added to water. ii. Name another compound that would result in a similar reaction with water. 13. A small piece of sodium metal is added to distilled water. ii.all group I metals are very reactive. Name a group I metal that is more reactive than sodium.
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