Classifying chemical reactions


Published on

  • Be the first to comment

  • Be the first to like this

No Downloads
Total views
On SlideShare
From Embeds
Number of Embeds
Embeds 0
No embeds

No notes for slide

Classifying chemical reactions

  1. 1. Classifying Chemical Reactions
  2. 2. Synthesis Reactions• A chemical reaction in which 2 or more substances ( A and B) react to produce a single product (AB)• A+B AB
  3. 3. • When 2 elements react it is always synthesis• 2 compounds can combine to form one compound – CaO (s) + H2O (l) Ca(OH)2• A compound and an element can combine – 2SO2 (g) + O2 (g) 2SO3 (g)
  4. 4. Combustion Reactions• Oxygen combines with a substance and releases energy in the form of heat and light
  5. 5. • Combustion reactions are common• Combustion reactions can be synthesis reactions, but not all are• Coal is burned to produce energy and comprised of carbon. Below is the equation for this combustion reaction: – C (s) + O2 (g) CO2 (g) – CH4 (g) + 2O2 (g) CO2 (g) + 2H2O (g)
  6. 6. Write the chemical Equations for these reactions then classify1. The solids aluminum and sulfur react to produce aluminum sulfide2. Water and dinitrogen pentoxide gas react to produce aqueous hydrogen nitrate3. The gases nitrogen dioxide and oxygen react to produce dinitrogen pentoxide gas
  7. 7. Decompisition Reactions• A single compound breaks down into 2 or more elements or new compounds• AB A+B
  8. 8. • Require an energy source – Heat, light or electricity• A real life example is an air bag activating• Sodium Azide decomposes producing nitrogen gas to inflate the bag• 2NaN3 (s) 2Na (s) + 3N2 (g)
  9. 9. Write the Chemical Equations for the following• Aluminum oxide (s) decomposes when electricity passes through it• Nickel (II) hydroxide (s) decomposes to produce nickel (II) oxide (s) and water
  10. 10. Single Replacement Reactions• A reaction in which the atoms of one element replace the atoms of another element• They “swap spots”
  11. 11. • Metal replaces hydrogen or another metal – One metal replaces another metal in a compound dissolved in water – Copper is placed in aqueous silver nitrate. – Crystals made of silver accumulate on the copper bar – Cu (s) + 2AgNO3 (aq) 2Ag (s) + Cu(NO3)2 (aq)
  12. 12. • A metal will not always replace another metal in a compound dissolved in water because metals differ in their reactivities• Reactivity is the ability to react with another substance
  13. 13. • A metal can replace any metal below it that is in a compound• Example:Silver wire in a copper(II) nirate solution willnot produce a reaction• We use NR if there is no reaction• Ag(s) + Cu(NO3)2 (aq) NR
  14. 14. • Nonmetal replaces nonmetal – Frequently involves halogens – A more reactive halogen replaces a less reactive halogen that is part of a compound dissolved in water (aqueous) – Fluorine replaces bromine in water containing dissolved sodium bromide • F2 (g) + 2NaBr (aq) 2NaF(aq) + Br2(l) – Bromine DOES NOT replace fluorine in water containing dissolved sodium fluoride • Br2 (g) + 2NaF (aq) NR
  15. 15. Predicting the Products1. Determine if the reaction will occur2. Determine the products of the reaction3. Write a skeleton equation4. Balance
  16. 16. Fe(s) + CuSO4(aq) ?1. Iron is placed in copper sulfate.2. Iron is above copper in the activity series3. Iron will replace copper Fe(s) + CuSO4(aq) FeSO4 (aq) + Cu (s)
  17. 17. Br2 (l) + MgCl2 (aq) NR1. Bromide is placed in magnesium chloride2. Chlorine is more reactive than Bromide3. A reaction will not occur
  18. 18. Mg(s) + AlCl3 (aq)• Magnesium is placed in Aluminum Chloride• Magnesium is more reactive than aluminum• See if you can figure out the answer – Remember to CRISS CROSS for ionics!
  19. 19. Double Replacement Reactions