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Types of Chemical Reactions Unit 5A. Synthesis Reaction 2 or more substances combining to form a single compound 2 or more substances combining to form.

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Presentation on theme: "Types of Chemical Reactions Unit 5A. Synthesis Reaction 2 or more substances combining to form a single compound 2 or more substances combining to form."— Presentation transcript:

1 Types of Chemical Reactions Unit 5A

2 Synthesis Reaction 2 or more substances combining to form a single compound 2 or more substances combining to form a single compound A + B AB A + B AB N 2 (g) + 3H 2 (g) 2NH 3 (g) N 2 (g) + 3H 2 (g) 2NH 3 (g)

3 Decomposition Reaction A single reactant breaks down into simpler substances. A single reactant breaks down into simpler substances. CD C + D CD C + D 2H 2 O 2 (l) 2H 2 O(l) + O 2 (g) 2H 2 O 2 (l) 2H 2 O(l) + O 2 (g)

4 Single- replacement Reaction An element replaces another in an ionic compound. An element replaces another in an ionic compound. E + FG F + EG E + FG F + EG L + JK K + JL L + JK K + JL 2Na(s) + MgCl 2 (aq) Mg(s) + 2NaCl(aq) 2Na(s) + MgCl 2 (aq) Mg(s) + 2NaCl(aq) 2F 2 (g) + 2FeBr 3 (aq) 3Br 2 (l) + 2FeF 2 (aq) 2F 2 (g) + 2FeBr 3 (aq) 3Br 2 (l) + 2FeF 2 (aq)

5 Single- replacement Reactions Only occur if the element doing the replacing is more active (reactive) than the other element! Only occur if the element doing the replacing is more active (reactive) than the other element!

6 Activity Series of the Elements METALS NON-METALS (halogens) Lithium Fluorine Potassium Chlorine Calcium Bromine Sodium Iodine Magnesium Aluminum Zinc Chromium Iron Nickel Tin Lead Hydrogen Copper Mercury Silver Platinum Each element can replace all the other elements below it!

7 Double- replacement Reactions The cations of 2 ionic compounds exchange anions. The cations of 2 ionic compounds exchange anions. QR + ST QT + SR QR + ST QT + SR BaBr 2 (aq) + 2AgNO 3 (aq) Ba(NO 3 ) 2 (aq) + 2AgBr(s) BaBr 2 (aq) + 2AgNO 3 (aq) Ba(NO 3 ) 2 (aq) + 2AgBr(s)

8 Combustion Reaction A hydrocarbon is burned with oxygen to produce carbon dioxide, water and light/ heat. A hydrocarbon is burned with oxygen to produce carbon dioxide, water and light/ heat. C x H y + O 2 (g) CO 2 (g) + H 2 O(g) C x H y + O 2 (g) CO 2 (g) + H 2 O(g) 2C 4 H 10 (l) + 13O 2 (g) 8CO 2 (g) + 10H 2 O(g) 2C 4 H 10 (l) + 13O 2 (g) 8CO 2 (g) + 10H 2 O(g) 2C 2 H 5 OH(l) + 7O 2 (g) 4CO 2 (g) + 6H 2 O(g) 2C 2 H 5 OH(l) + 7O 2 (g) 4CO 2 (g) + 6H 2 O(g)


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