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Single Replacement Reactions

Single Replacement Reactions. +. . +. General Equation. A + BX  AX + B. Helpful Hints. Metals replace metals and hydrogen Halogens replace halogens If an element can take more than one charge, use the +2 charge Metals + H 2 O metal OH + H 2.

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Single Replacement Reactions

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  1. Single Replacement Reactions +  +

  2. General Equation A + BX  AX + B

  3. Helpful Hints • Metals replace metals and hydrogen • Halogens replace halogens • If an element can take more than one charge, use the +2 charge • Metals + H2O metalOH + H2

  4. Steps to Predicting a single replacement reaction • Look at the reactants given and determine if the single element is a metal or a halogen • Look at the compound given in the reactants, and find the same type of element (metal or halogen) identified in step 1 • Find both elements on the reactivity series

  5. If the element identified in step 1 is higher on the reactivity series than the element in step 2, then they will switch places to form new products • Look at the products formed • If the single element is a diatomic molecule, it needs a subscript of 2 • If your compound is not neutral; look at the charges and add subscripts to make it neutral

  6. Example 1: Ag + Zn(NO3)2 • Zn + AgNO3 ______________ Step 1: Zn is the single element, and it is a metal Step 2: Ag is the metal in the compound Step 3: Look at the activity series for metals (next slide) Step 4: Zn is higher on the list (more reactive) so it will switch places with Ag (new products = Ag + ZnNO3 Step 5: Ag is not a diatomic molecule so it doesn’t need a subscript; ZnNO3 is not a neutral compound so we need to look at the charges and make it neutral; Zn2+ NO31- Zn(NO3)2

  7. Activity Series Metals Li Rb K Cs Ba Sr Ca Na Mg Al Ti Mn Zn Cr Fe Cd Co Ni Sn Pb H Sb Bi Cu Hg Ag Pt Au Most reactive Least reactive

  8. Example 2: KCl + I2 • Cl2+ KI __________ Step 1: Cl is the single element, and it is a halogen Step 2: I is the halogen in the compound Step 3: Look at the activity series for non-metals (next slide) Step 4: Cl is higher on the list (more reactive) so it will switch places with I (new products = KCl + I Step 5: I is a diatomic molecule so it needs a subscript of 2; KClis a neutral compound because the charges are equal and opposite

  9. Activity Series Non-metals F2 Cl2 Br2 I2 Most reactive Least reactive

  10. Example 3: NR • Ag + KNO 3 ______________ Step 1: Ag is the single element, and it is a metal Step 2: K is the metal in the compound Step 3: Look at the activity series for metals (next slide) Step 4: K is higher on the list (more reactive) so Ag will not switch places with K Step 5: There will be NO REACTION (NR)

  11. Activity Series Metals Li Rb K Cs Ba Sr Ca Na Mg Al Ti Mn Zn Cr Fe Cd Co Ni Sn Pb H Sb Bi Cu Hg Ag Pt Au Most reactive Least reactive

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