1 / 11

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.

sara-craig
Télécharger la présentation

Single Replacement Reactions

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  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

More Related