1. Predicting Products of Reactions Test Practice

2. Synthesis and Decomposition Objectives: Given the reactants, predict the products for synthesis and decomposition reactions.

3. Diatomic Molecules Certain elements exist as diatomic molecules. They are Iodine, Bromine, Chlorine, Fluorine, Oxygen, Nitrogen, Hydrogen. Anytime these elements are by themselves in a reaction they will be a molecule of two of the atoms: I 2, Br 2, Cl 2, F 2, O 2, N 2, H 2 I Bring Clay For Our New Home

4. Synthesis General Equation: A + B → AB Given the reactants, write the ions they will form. Swap and drop to find the compound. Example: –Magnesium + oxygen –Mg + O 2 → ? –Mg 2 + O 2 - –MgO –ANSWER: Mg + O 2 → MgO –Then Bal;ance

5. Decomposition AB → A + B Write the elements from the compound separately. Remember diatomic molecules. Example: H 2 O 2 → ? H, O – both diatomics H 2, O 2 ANSWER: H 2 O 2 → H 2 + O 2

6. Single and Double Displacement Objective Given reactants, predict the products for single and double displacement reactions.

7. Single Displacement General Equation: AB + X → AX + B If “X” is a metal, it will replace the metal in the compound. If “X” is a nonmetal, it will replace the nonmetal in the compound. Write ions and swap and drop to find “AX”. When writing “B”, remember diatomic molecules.

8. Example: Aluminum and copper (I) chloride Al + CuCl Al is a metal so it will replace the metal in the compound (Cu) Al 3+ and Cl 1- AlCl 3 Al + CuCl → AlCl 3 + Cu

9. Double Displacement General Equation: AX + BY → AY + BX Each compound (“AX” and “BY”) has a cation and an anion. Switch partners. Be sure you don’t put a cation with a cation or an anion with an anion. Write ions and swap and drop to find the formulas.

10. Example : Iron (III) chloride and sodium hydroxide FeCl 3 + NaOH –FeCl3: Cation: Fe 3+, Anion: Cl 1- –NaOH: Cation: Na 1+, Anion OH 1- Switch: Fe(OH) 3 and NaCl FeCl 3 + NaOH → Fe(OH) 3 + NaCl

11. Practice Predicting Products of Reactions Synthesis hydrogen burned in oxygen hydrogen gas + nitrogen gas sulfur burned (complete combustion)sulfur burned (complete combustion) calcium oxide added to water

12. Decomposition barium hydroxide (heated) sodium carbonate (heated) lithium chlorate (heated) electrolysis of aluminum oxide sulfuric acid heated gently

13. Replacement iron filings added to copper(II) sulfate in solutioniron filings added to copper(II) sulfate in solution aluminum in hydrochloric acid potassium metal added to cold water zinc metal added to mercury(II) nitrate silver metal added to copper(II) sulfate chlorine gas bubbled through a solution of calcium bromidechlorine gas bubbled through a solution of calcium bromide

14. Ionic potassium iodide added to lead(II) nitratepotassium iodide added to lead(II) nitrate sodium sulfite combined with acetic acidsodium sulfite combined with acetic acid sodium chloride added to sulfuric acid barium nitrate added to sodium oxalatebarium nitrate added to sodium oxalate sodium bicarbonate added to hydrochloric acidsodium bicarbonate added to hydrochloric acid