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Intro to Reactions. Ch. 7 – Chemical Reactions. A.Signs of a Chemical Reaction. Change in heat and light Formation of a gas Formation of a precipitate Color change Odor. B.Law of Conservation of Mass. In a chemical reaction, matter is not created or destroyed. Atoms can only rearrange. - PowerPoint PPT Presentation
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I. Intro to Reactions
Ch. 7 – Chemical Reactions
A.Signs of a Chemical Reaction Change in heat and light Formation of a gas Formation of a precipitate Color change Odor
B.Law of Conservation of Mass In a chemical reaction, matter is not
created or destroyed. Atoms can only rearrange. Discovered by Lavoisier.
4H
2O
4H
2O
C. Chemical Reaction
A change in which one or more substances are converted to different substances.
A+BC+DREACTANTS PRODUCTS
C. Chemical Equations
Reactants = Starting substances Products = Substances Formed
C. Chemical Equationsp. 635
C. Chemical Equations
A chemical equation is a way to describe a chemical reaction using chemical formulas and other symbols.
Chemical equations written with symbols makes it much easier to tell what is happening in the reaction.
C. Chemical Equations
Aqueous lead(II) nitrate plus two units
of aqueous potassium iodide
produces solid lead(II) iodide and two
units of aqueous potassium nitrate.
Pb(NO3)2+ KI PbI2 + KNO32 2
Coefficient - # of units of each substance
C. Chemical Equations
Describing Coefficients:
individual atom = “atom”
2Mg 2 atoms of magnesium
covalent substance = “molecule”
3CO2 3 molecules of carbon dioxide
ionic substance = “unit”
4MgO 4 units of magnesium oxide
C. Johannesson
II. Balancing Equations
Ch.7– Chemical Reactions
A. Balancing Steps
1. Write the unbalanced equation.
2. Count atoms on each side.
3. Add coefficients to make #s equal.
Coefficient subscript = # of atoms
4. Reduce coefficients to lowest possible ratio, if necessary.
5. Double check atom balance!!!
B. Helpful Tips
Balance one element at a time. Update ALL atom counts after
adding a coefficient. If an element appears more than
once per side, balance it last. Balance polyatomic ions as single
units. “1 SO4” instead of “1 S” and “4
O”
Al + CuCl2 Cu + AlCl3
33 2
C. Balancing Example
Aluminum and copper(II) chloride react to form copper and aluminum chloride.
2
Determine the reactants and products
Write the reactants on the left side of the equation and the products on the right
Show an equal number of atoms for each element on both sides of the equation.
D. Writing Balanced Equations
When propane gas burns in the air, the reactants are propane (C3H8)and oxygen (O2). The products formed are carbon dioxide (CO2)and water (H2O).
Step 1: Find the reactants and products.
Example
Example
Step 2: Write a chemical equation
C3H8 + O2 CO2 + H2O
Example
Step 3: Balance the chemical equation
*In balancing a chemical equation, change only the coefficients. Never change the subscripts.
C3H8 + O2 CO2 + H2O5 3 4
Homework Assignment
Page 235: 33-36 Show inventory and balance the
reactions
D. Writing Reactions Identify the reactants and products
and write the equation for each of the following chemical reactions.
The key to getting this right is to balance each of the pieces correctly (Write the balanced formula. Remember from chapter 4?)
After writing the reactions balance them.
D. Writing Reactions
There are a few elements that need to be treated in a special way because of how they bond with each other.
Example: Elemental oxygen, is never found by itself. It is always found as O2. Oxygen is one of the diatomic elements. This means they are always paired up.
There are 7 diatomic elements: H, I, Br, O, N, Cl, F. (Remember
HI BrONClF!) These elements are all gases!
• The Seven Diatomic Elements
Br2 I2 N2 Cl2 H2 O2 F2
HIBrONClF
D. Writing Reactions
Writing Reactions
When writing the balanced formula for elemental metals they are always written by themselves.
Example: Elemental Copper is just Cu. Elemental Aluminum is just Al.
This will be the case for all elemental metals.
Writing Reactions
Example 1:
Solid magnesium metal reacts with liquid water to form solid magnesium hydroxide and hydrogen gas.
Step 1: Find the reactants and products
Writing Reactions
The reactants are Mg metal and Water, the products are Mg hydroxide and H gas.
Step 2: Write the balanced formula for each piece.Mg (s) = Magnesium MetalH2O (l) = Water
Mg(OH)2 (s) = Magnesium Hydroxide
H2 (g)= Hydrogen gas
Writing Reactions
The reactants are Mg metal and Water, the products are Mg hydroxide and H gas.
Step 2: Write the balanced formula for each piece.
Mg (s) = Magnesium MetalH2O (l) = Water
Mg(OH)2 (s) = Magnesium Hydroxide
H2 (g)= Hydrogen gas
Writing Reactions
Step 3: Put the reactants and products into a chemical reaction.
Mg(s) + H2O(l) Mg(OH)2 (s) + H2(g)
Step 4: Balance the reaction
D. Writing Reactions
Write the following reactions and then balance them:
1. Solid Ammonium dichromate decomposes to form solid chromium (III) oxide, gaseous nitrogen, and gaseous water.
2. Gaseous ammonia (NH3) reacts with gaseous oxygen to form gaseous nitrogen monoxide and gaseous water.
Assignment
Page 234 #’s 9-11, 13, 18, 21, 25-28
I want you to write the question, circle the reactants, underline the products. Then write out the reaction in symbol form and balance it.
Ch. 8 – Chemical Reactions
III. Types of Chemical Reactions
A. Combustion
CH4(g) + 2O2(g) CO2(g) + 2H2O(g)
the burning of any substance in O2 to produce heat
A + O2 B
Na(s)+ O2(g)
C3H8(g)+ O2(g) 5 3 4
A. Combustion
Products:contain oxygenhydrocarbons form CO2 + H2O
CO2(g)+ H2O(g)
Na2O(s) 4 2
B. Synthesis
the combination of 2 or more substances to form a compound
only one product
A + B AB
C. Johannesson
B. Synthesis
H2(g) + Cl2(g) 2 HCl(g)
Al(s)+ Cl2(g) AlCl3(s)2 3 2
B. Synthesis
Products: ionic - cancel chargescovalent - hard to tell
C. Decomposition
a compound breaks down into 2 or more simpler substances
only one reactant
AB A + B
C. Johannesson
C. Decomposition
2 H2O(l) 2 H2(g) + O2(g)
KBr(l) K(s) + Br2(l) 2 2
C. Decomposition
Products:binary - break into elementsothers - hard to tell
C. Johannesson
D. Single Replacement
one element replaces another in a compoundmetal replaces metal (+)nonmetal replaces nonmetal (-)
A + BC B + AC
C. Johannesson
D. Single Replacement
Cu(s) + 2AgNO3(aq) Cu(NO3)2(aq) + 2Ag(s)
C. Johannesson
Fe(s)+ CuSO4(aq) Cu(s)+ FeSO4(aq)
D. Single Replacement
Products:metal metal (+)nonmetal nonmetal (-) free element must be more active (check activity series)
Br2(l)+ NaCl(aq) N.R.
C. Johannesson
AB + CD AD + CB
E. Double Replacement
ions in two compounds “change partners” cation of one compound combines with
anion of the other
C. Johannesson
E. Double Replacement
Pb(NO3)2(aq) + K2CrO4(aq) PbCrO4(s) + 2KNO3(aq)
Pb(NO3)2(aq)+ KI(aq) PbI2(s)+ KNO3(aq)
E. Double Replacement
Products:switch negative ions
NaNO3(aq)+ KI(aq) N.R.
2 2
Decide the RXN TypeWOWO33 + 3H + 3H22 W + 3H W + 3H22OO
RbCl + 2ORbCl + 2O22 RbClO RbClO44
RbBr + AgCl RbBr + AgCl AgBr + RbCl AgBr + RbCl
2KNO2KNO33 2KNO 2KNO2 2 + O+ O22
3Mg + N3Mg + N22 Mg Mg33NN22
2C2C22HH66 + 7O + 7O22 4CO 4CO22 + 6H + 6H22OO
Chemical reactions can be Chemical reactions can be classified into 5 different types.classified into 5 different types.These 5 types are Single These 5 types are Single Displacement, Double Displacement, Double Displacement, Decomposition, Displacement, Decomposition, Synthesis, and Combustion. Synthesis, and Combustion. You will be given the general form You will be given the general form for each of the 5 reactions.for each of the 5 reactions.
Chemical Changes
In a single displacement reaction one In a single displacement reaction one element displaces or changes places with element displaces or changes places with another element in a compound.another element in a compound.General Form:General Form:Element + CompoundElement + Compound Element + Element + CompoundCompoundEx. ClEx. Cl22 + 2KBr + 2KBr 2KCl + Br 2KCl + Br22
Chlorine changes places with BromineChlorine changes places with Bromine
Single Replacement
Look at the reactants in the following single Look at the reactants in the following single displacement reaction and decide which displacement reaction and decide which elements will change places: Al + Feelements will change places: Al + Fe22OO33 Be sure to find the charges of all the Be sure to find the charges of all the elements.elements.Which ones will switch?Which ones will switch?
Single Replacement
In a double displacement reaction the In a double displacement reaction the positive and negative parts of two positive and negative parts of two compounds switch places.compounds switch places.General form: General form: Compound + Compound Compound + Compound Compound + Compound + Compound Compound Ex: PbClEx: PbCl22 + Li + Li22SOSO44 PbSO PbSO44 + 2LiCl + 2LiCl
Double Replacement
Look at the reactants for the following Look at the reactants for the following double displacement reaction and predict double displacement reaction and predict what will happen.what will happen.ZnBrZnBr2 2 + AgNO+ AgNO33
Double Replacement
In a decomposition reaction a compound In a decomposition reaction a compound break up or decompose down into simpler break up or decompose down into simpler substances.substances.General form: Compound General form: Compound two or two or more elements or compoundsmore elements or compoundsEx: 2AgEx: 2Ag22O O 4Ag + O 4Ag + O22
Decomposition
In a synthesis reaction two or more In a synthesis reaction two or more substances combine to form one new substances combine to form one new substance.substance.General form: Element or compound + General form: Element or compound + Element or compound Element or compound Compound CompoundEx: CaO + SiOEx: CaO + SiO22 CaSiO CaSiO33
Ex: 2HEx: 2H22 + O + O22 2H 2H22OO
Synthesis
Combustion
Combustion occurs when an organic Combustion occurs when an organic compound (a compound of Carbon) reacts with compound (a compound of Carbon) reacts with oxygen in the air and burns. When this occurs oxygen in the air and burns. When this occurs the products are the products are alwaysalways Carbon dioxide and Carbon dioxide and Water.Water.General form: Hydrocarbon + oxygen General form: Hydrocarbon + oxygen Carbon dioxide + Water Carbon dioxide + Water Ex: CHEx: CH44 + 2O + 2O22 CO CO22 + 2H + 2H22OO
Examples:Decide the RXN Type
WO3 + 3H2 W + 3H2O
RbCl + 2O2 RbClO4
RbBr + AgCl AgBr + RbCl 2KNO3 2KNO2 + O2
3Mg + N2 Mg3N2
2C2H6 + 7O2 4CO2 + 6H2O