Ppt chemical reactions
of 31
/31
-
Author
kstalke47 -
Category
Technology
-
view
939 -
download
1
Embed Size (px)
description
Transcript of Ppt chemical reactions
Chemical Reactions
Chemical Reaction
What is a chemical reaction? • Atoms rearrange to create one or more new compounds. • In other words, old bonds break and new bonds form.
Chemical Reaction
OLD NEW
Chemical Reaction
OLD NEW
Reactants
Products
Chemical Equation
Reactants Products YEILD OR =
Reactants and products can be represented by using chemical formulas or compound names.
Chemical Equation 2 H2 (g) + 1 O2 (g) 2
H2O (g) Reactants Products
Yield or =
Chemical Reactions can
1.Absorb or release energy.
2.Fast or Slow
Absorb energy or release energy?
Exothermic- release of energy.Exo- Think exit! Thermic – heat
Endothermic- absorption of energy Endo- Taken in Thermic – heat
Chemical Reactions can be…
2. Fast or slow The speed of a chemical reaction is different for all!
Depends on the reactants.
Chemical Reactions can be…
Reaction Rate
Activity
Reaction Rate Activity- the speed a reaction going from reactants to products.
Law of Conservation of MatterThe law of conservation of matter states that matter (mass) can neither be created nor destroyed. It can, however, can be rearranged.
In a chemical reaction, the mass of the reactants must equal the mass of the products.
Law of Conservation of MatterThe law of conservation of matter states that matter (mass) can neither be created nor destroyed. It can, however, can be rearranged.
In a chemical reaction, the mass of the reactants must equal the mass of the products.
WHAT??????
Think of a Balance Everything must be equal. When matter goes through a physical
or chemical change, the amount (or mass) of the substances that you begin with must equal the amount (or mass) of the substances that you end with.
BEFORE MASS MUST = THE AFTER MASS!
WHY you ask!!!!!!!
How do we balance chemical equations?!?!?!
1.USE A PENCIL!!
2.Identify reactants and products
3. Make a Table!!!
EXAMPLE:
H2O2 O2 + H2O
How do we balance chemical equations?!?!?!
How many of each element is in the reactants?
How many of each element is in the products?
Element w/o coeff. X coeff. Total
Element w/o coeff. X coeff. Total
EXAMPLE:
KClO3 KCl + O2
How do we balance chemical equations?!?!?!
How many of each element is in the reactants?
How many of each element is in the products?
Element w/o coeff. X coeff. Total
Element w/o coeff. X coeff. Total
EXAMPLE:
CH4 + O2 CO2 + H2O
How do we balance chemical equations?!?!?!
How many of each element is in the reactants?
How many of each element is in the products?
Element w/o coeff. X coeff. Total
Element w/o coeff. X coeff. Total
Types of Reactions
1. Synthesis- Two or more simple substances are
combined to form one new and more complex substance.
Types of Reactions
A + B AB
1. Synthesis- Two or more simple substances are
combined to form one new and more complex substance.
Types of Reactions
A + B AB 2Na + Cl2
2NaCl
2. Decomposition Reaction- A more complex substance breaks down into
its more simple parts.
Types of Reactions
AB A + B
2. Decomposition Reaction- A more complex substance breaks down into
its more simple parts.
Types of Reactions
AB A + B
H2O2 O2 + H2O
3. Single-Replacement- A free uncombined element replaces another
combined element in a compound.
Types of Reactions
AB + C AC + B
3. Single-Replacement- A free uncombined element replaces another
combined element in a compound.
Types of Reactions
AB + C AC + B
LiCl + Br2 LiBr + Cl2
4. Double Replacement Reaction- The reacting parts of two compounds switch
places to form two new compounds.
Types of Reactions
AB + CD AD + BC
4. Double Replacement Reaction- The reacting parts of two compounds switch
places to form two new compounds.
Types of Reactions
AB + CD AD + BC
CaF2 + LiSO4 CaSO4 + LiF
5. Combustion Reaction- OR Burning Reaction Involves the combination of a substance with
oxygen to give off heat and light.
Types of Reactions
AB + O2 Heat+ Light
5. Combustion Reaction- OR Burning Reaction Involves the combination of a substance with
oxygen to give off heat and light.
Types of Reactions
AB + O2 Heat+ Light CH4 + O2 CO2 +
H2O
Types of Reactions Use the code below to classify each reaction. S = Synthesis D = Decomposition SR = Single Replacement DR = Double Replacement ____ P + O2 → P4O10 ____ Mg + O2 →
MgO
____ HgO → Hg + O2 ____ Al2O3 → Al + O2
____ Cl2 + NaBr → NaCl + Br2 ____ H2 + N2 → NH3
