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There are five types of chemical reactions you need to know: 1.Synthesis reactions 2.Decomposition reactions 3.Single displacement reactions 4.Double.

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Presentation on theme: "There are five types of chemical reactions you need to know: 1.Synthesis reactions 2.Decomposition reactions 3.Single displacement reactions 4.Double."— Presentation transcript:

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2 There are five types of chemical reactions you need to know: 1.Synthesis reactions 2.Decomposition reactions 3.Single displacement reactions 4.Double displacement reactions 5.Combustion reactions

3 By the end of this lesson you should be able to: Classify the type of reaction Predict the product(s) of the reaction Balance the final equation including state symbols

4 Some steps for doing reactions 1. Identify the type of reaction 2. Predict the product(s) using the type of reaction as a model 3. Balance it  Don’t forget about the diatomic elements!  (Br I N Cl H O F) For example, Oxygen is O 2 which is a compound

5 Synthesis reactions occur when two substances (generally elements) combine and form a compound. (Sometimes these are called combination or addition reactions.) reactant + reactant  1 product Basically: A + B  AB Example: 2H 2 + O 2  2H 2 O Example: C + O 2  CO 2

6 Here is another example of a synthesis reaction

7 Predict the products. Write and balance the following synthesis reaction equations. Sodium metal reacts with chlorine gas Na (s) + Cl 2(g)  Mg (s) + F 2(g)  Al (s) + F 2(g)  Aluminum metal reacts with fluorine gas Solid Magnesium reacts with fluorine gas NaCl (s) 2 2 MgF 2(s) AlF 3(s) 2 2 3

8 Decomposition reactions occur when a compound breaks up into the elements or in a few to simpler compounds 1 Reactant  Product + Product In general: AB  A + B Example: 2 H 2 O  2H 2 + O 2

9 Another view of a decomposition reaction:

10 Carbonates and chlorates are special case decomposition reactions that do not go to the elements. Carbonates (CO 3 2- ) decompose to carbon dioxide and a metal oxide Example: CaCO 3  CO 2 + CaO Chlorates (ClO 3 - ) decompose to oxygen gas and a metal chloride Example: 2 Al(ClO 3 ) 3  2 AlCl 3 + 9 O 2 There are other special cases, but we will not explore those in this year

11 Predict the products. Then, write and balance the following decomposition reaction equations: Solid Lead (IV) oxide decomposes PbO 2(s)  Aluminum nitride decomposes AlN (s) 

12 Identify the type of reaction for each of the following synthesis or decomposition reactions, and write the balanced equation: N 2(g) + O 2(g)  BaCO 3(s)  Co (s) + S (s)  NH 3(g) + H 2 CO 3(aq)  NI 3(s)  (make Co be +3) Nitrogen monoxide

13 Single Replacement Reactions occur when one element replaces another in a compound. A metal can replace a metal (+) OR a nonmetal can replace a nonmetal (-). element + compound  element + compound A + BC  AC + B (if A is a metal) OR A + BC  BA + C (if A is a nonmetal) (remember the cation always goes first!) When H 2 0 splits into ions, it splits into H + and OH -

14 Another view:

15  To determine if a single replacement reaction will take place we must look at the reactivity of the elements involved.  Elements higher on the table will replace elements lower on the table.  Elements lower will NOT replace elements higher.

16 Write and balance the following single replacement reaction equation: Zinc metal reacts with aqueous hydrochloric acid Zn(s) + HCl(aq)  Note: Zinc replaces the hydrogen ion in the reaction 2 ZnCl 2 + H 2(g)

17 Sodium chloride solid reacts with fluorine gas NaCl (s) + F 2(g)  Note that fluorine replaces chlorine in the compound NaF (s) + Cl 2(g) 2 2 Aluminum metal reacts with aqueous copper (II) nitrate Al (s) + Cu(NO 3 ) 2 (aq)  Al(NO 3 ) 3(aq) + Cu (s) 2 32 3

18 Double Replacement Reactions occur when a metal replaces a metal in a compound and a nonmetal replaces a nonmetal in a compound Compound + compound  compound+ compound AB + CD  AD + CB

19 Think about it like “foil”ing in algebra, first and last ions go together + inside ions go together Example: AgNO 3(aq) + NaCl (s)  AgCl (s) + NaNO 3(aq) Another example: K 2 SO 4(aq) + Ba(NO 3 ) 2(aq)  2 KNO 3(aq) + BaSO 4(s)

20  To determine if products are soluble in water (aq) or insoluble (form a solid precipitate) we use a solubility table.

21 Predict the products. Balance the equation 1. HCl (aq) + AgNO 3(aq)  2. CaCl 2(aq) + Na 3 PO 4(aq)  3. Pb(NO 3 ) 2(aq) + BaCl 2(aq)  4. FeCl 3(aq) + NaOH (aq)  5. H 2 SO 4(aq) + NaOH (aq)  6. KOH (aq) + CuSO 4(aq) 

22 Combustion reactions occur when a hydrocarbon reacts with oxygen gas. This is also called burning!!! In order to burn something you need the 3 things in the “fire triangle”: 1.A Fuel (hydrocarbon) 2.Oxygen 3.Something to ignite the reaction (spark)

23 In general: C x H y + O 2  CO 2 + H 2 O Products in combustion are ALWAYS carbon dioxide and water. (although incomplete burning does cause some by- products like carbon monoxide) Combustion is used to heat homes and run automobiles (octane, as in gasoline, is C 8 H 18 )

24 Edgar Allen Poe’s drooping eyes and mouth are potential signs of CO poisoning.

25 Example C 5 H 12 (l) + 8 O 2(g)  5 CO 2(g) + 6 H 2 O (l) Write the products and balance the following combustion reaction: C 10 H 22 (l) + O 2 (g) 

26 State the type of reaction, predict the products, and balance the following reactions: 1. BaCl 2 + H 2 SO 4  2. C 6 H 12 + O 2  3. Zn + CuSO 4  4. Cs + Br 2  5. FeCO 3 

27  https://www.youtube.com/watch?v=g-biRwAVTV8 https://www.youtube.com/watch?v=g-biRwAVTV8 Good Overall Review:  https://www.youtube.com/watch?v=d58UcB_Yb2Q https://www.youtube.com/watch?v=d58UcB_Yb2Q


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