Transcript Classifying Reactions PowerPoint

Chapter 6: Chemical Reactions
 Classify chemical reactions.
 A synthesis reaction is a reaction in
which two or more substances react to
produce a single product.
 When two elements react, the reaction
is always a synthesis reaction.
 Two compounds can also react to create
one compound in a synthesis reaction.
 All synthesis reactions follow this
general equation:
 A + B  AB
 A decomposition reaction is one in
which a single compound breaks down
into two or more elements or new
compounds.
 Decomposition reactions often require
an energy source, such as heat, light, or
electricity, to occur.
 Decomposition reactions follow this
general equation:
 AB  A + B
 In a single-displacement reaction, one
element displaces another in a
compound.

Usually a metal will replace another metal,
or a halogen will replace another halogen in
single displacement reactions

Single displacement reactions follow this
general equation:
 A + BC  AC + B
 Double displacement reactions occur
when ions exchange between two
compounds.
 Double displacement reactions will
always produce either a precipitate,
water, or a gas.
 A double-displacement reaction follows
the general form
 AB + CD  AD + BC
 Classify the following reactions:
 Na2O(s) + H2O(l) ⟶ 2 NaOH(aq)
 Ba(NO3)2(aq) + K2SO4(aq) ⟶ BaSO4(s) + 2
KNO3(aq)
 2 Al(s) + Fe2O3(s) ⟶ Al2O3(s) + 2 Fe(l)
 2 H2O2(aq) ⟶ 2 H2O(l) + O2(g)
 Solid calcium reacts with chlorine gas to
produce solid calcium chloride.
 Write a balanced chemical equation for
each synthesis reaction:
 Ag(s) + Br2(g)
 Mg(s) + Cl2(g)
 Write a balanced chemical equation for
each decomposition reaction:
 Al2O3(s) 
 H2O(l) 