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Predicting Reactions

Predicting Reactions. Today, we will focus on Single-Displacement and Double-displacement reactions, because predicting the reaction is based on very specific rules. In the case of the other types of reactions, you can assume that reaction will occur under the conditions present.

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Predicting Reactions

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  1. Predicting Reactions Today, we will focus on Single-Displacement and Double-displacement reactions, because predicting the reaction is based on very specific rules. In the case of the other types of reactions, you can assume that reaction will occur under the conditions present. How do you know if a reaction will occur? Chapter 8.2 & 8.3

  2. Single- Displacement Reactions • How do you know if a reaction will occur? • For SD reactions involving a cation change, use the Activity Series of Metals(found on the back of your periodic table) • Magnesium is more reactive than iron, but less reactive than calcium • For SD involving anions, it is limited to halogens. As you move down the P.T. halogen reactivity decreases. • Bromine is more reactive than Iodine, but less reactive than flourine. ** the reactivity of elements, allows you to predict if a reaction will occur.**

  3. Single- Displacement Reactions Example:Will aqueous lithium nitrate reacts with magnesium? LiNO3 + Mg(s) ? 1. Look at the activity series of metals. 2. Which is more reactive, Lithium or magnesium? - In order for this reaction to happen, the free element must be more reactive than the bonded element. 3. According to the table, magnesium is less reactive than lithium. 4. This reaction will not happen

  4. Single- Displacement Reactions Example:Will aqueous silver nitrate react with magnesium? AgNO3(aq) + Mg(s) ? 1. Look at the activity series of metals. 2. Which is more reactive, silver or magnesium? - In order for this reaction to happen, the free element must be more reactive than the bonded element. 3. According to the table, magnesium is more reactive than silver. 4. This reaction will happen 2AgNO3(aq) + Mg(s) Mg(NO3)2(aq) + 2Ag(s)

  5. Double-Displacement Reactions • In order for a DD reaction to occur: • Both reactants need to be ionic compounds • One of the products must be insoluble: • A precipitate will form • A gas will form (indicated by the presence of bubbles) • water will be a product Pb(NO3)2(aq)+ 2KI (aq)PbI2(s) +2KNO3(aq) **Once you know if a product is insoluble, you can begin to predict whether or not a DD reaction will occur. **

  6. Solubility Rules(a version of these can be found on the back of your periodic table) 1 2 3 4 5

  7. Double-Displacement Reactions • Will a reaction occur between aqueous solutions of calcium nitrate and sodium hydroxide? Ca(NO3)2(aq) + NaOH(aq) ? • Look at ions in solutions: • Ca2+(aq) + 2NO32-(aq) + Na1+(aq) + OH1-(aq) 2. What are the new products that could form? Ca(OH)2 & NaNO3 3. Are either of these two products insoluble, water, or a gas? If the answer is yes, then reaction WILL occur

  8. Double-Displacement Reactions According to the Solubility rules (#1 & #5): Ca(OH)2is insoluble which means it will be a precipitate NaNO3is soluble, which means it will stay in solution. The reaction will occur: Ca(NO3)2(aq) + 2NaOH(aq) Ca(OH)2(s) + 2NaNO3(aq)

  9. Double-Displacement Reactions Example 2: will aqueous sodium chloride react with aqueous potassium nitrate? NaCl(aq) + KNO3(aq) ? Look at possible products Is either product insoluble, water, or a gas? Decide if the reaction will occur KCl & NaNO3 According to solubility table, both are Soluble Since both products will stay in solution, nothing will change NaCl(aq) + KNO3(aq) N.R.

  10. Practice problems Look at the following reactions. Predict whether or not they will occur. Then write the products, if necessary. Make sure the equation is balanced! (assume all ionic compounds are in solution) Zn + LiCl  ? Ca(NO3)2 + K2SO4  ? H3PO4 + Mg  ? NaCl + Pb(ClO3)2 ? NH4NO3 + FeI2 ? Zn + LiCl  no reactionLithium is more reactive than zinc, so zinc will not be able to move it. Ca(NO3)2 + K2SO4  CaSO4(s) + 2KNO3(aq) 2H3PO4 + 3Mg  Mg3(PO4)2 + 3H2(g) 2NaCl + Pb(ClO3)2 PbCl2(s) + 2NaClO3(aq) No reaction will occur. Both possible products will remain in solution

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