Product or Reactant?
• H2SO4 + BaCl2
1. BaCl2

Reactant
Product

2. HCl
3. BaSO4
4. H2SO4

Product
Reactant

2HCl + BaSO4
Review
Chemical Reactions
Law of Conservation of

Matter
1. Synthesis Reactions
Combining of several

simple substances to
form a more complicated
substance
Synthesis Reactions
A + B  AB
A = element
B = element
AB = compound
Synthesis Reactions
2Mg + O  2MgO
2

Magnesium (A) + Oxygen (B)
Magnesium oxide (AB)
2. Decomposition Reactions
The break down of a

compound into simpler
substances
AB  A + B
Opposite of synthesis
Decomposition Reactions
2H O 
2

2H2 + O2

Done by electrolysis
3. Single Replacement
A free element takes the place

of, or replaces, another element
Takes place between an
element an...
Single Replacement
A + BC  AC + B

A – free element
BC - compound
AC – new compound
B - new free element
Single Replacement
Zn + 2HCl 

ZnCl2 + H2

Hydrogen is set free
4. Double Replacement
 Two elements in two different

compounds switch places with
each other
 Takes place between two
c...
Double Replacement
AB + CD  AD + CB
AB – compound 1
CD – compound 2
AD – new compound 1
CB – new compound 2
Double Replacement
 Na(OH) + HCl

 NaCl +

H(OH)
 (OH) and Cl change places
 2 new compounds form
 NaCl and H O
2
These reactions can be…

ExothermicHeat is given
off
It feels hot!
These reactions can be…

EndothermicHeat is
absorbed
It feels cold!
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Types of Chemical Reactions

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Types of Chemical Reactions

  1. 1. Product or Reactant? • H2SO4 + BaCl2 1. BaCl2 Reactant Product 2. HCl 3. BaSO4 4. H2SO4 Product Reactant 2HCl + BaSO4
  2. 2. Review Chemical Reactions Law of Conservation of Matter
  3. 3. 1. Synthesis Reactions Combining of several simple substances to form a more complicated substance
  4. 4. Synthesis Reactions A + B  AB A = element B = element AB = compound
  5. 5. Synthesis Reactions 2Mg + O  2MgO 2 Magnesium (A) + Oxygen (B) Magnesium oxide (AB)
  6. 6. 2. Decomposition Reactions The break down of a compound into simpler substances AB  A + B Opposite of synthesis
  7. 7. Decomposition Reactions 2H O  2 2H2 + O2 Done by electrolysis
  8. 8. 3. Single Replacement A free element takes the place of, or replaces, another element Takes place between an element and a compound
  9. 9. Single Replacement A + BC  AC + B A – free element BC - compound AC – new compound B - new free element
  10. 10. Single Replacement Zn + 2HCl  ZnCl2 + H2 Hydrogen is set free
  11. 11. 4. Double Replacement  Two elements in two different compounds switch places with each other  Takes place between two compounds  Two new compounds form
  12. 12. Double Replacement AB + CD  AD + CB AB – compound 1 CD – compound 2 AD – new compound 1 CB – new compound 2
  13. 13. Double Replacement  Na(OH) + HCl  NaCl + H(OH)  (OH) and Cl change places  2 new compounds form  NaCl and H O 2
  14. 14. These reactions can be… ExothermicHeat is given off It feels hot!
  15. 15. These reactions can be… EndothermicHeat is absorbed It feels cold!
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