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Transcript of CHEMICAL REACTIONS. SO FAR... So far we have looked at the properties of individual atoms and...
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CHEMICAL REACTIONS
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SO FAR . . . So far we have looked at the
properties of individual atoms and molecules Atomic number Atomic mass Ions Lewis dot structures Molecular shapes Naming Moles
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HOW DO THESE ATOMS AND MOLECULES INTERACT?
The way that these atoms and molecules interact with each other is through chemical reactions
Chemical reaction: Change of one or more substances into a different substance.
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BEFORE WE BEGIN Important concept (by Antoine
Lavosier):Conservation of mass: Matter is
neither created or destroyed in a chemical reaction
In other words, you must have the same components in the beginning and end or a chemical reaction
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GENERAL TYPES OF REACTIONS
1. Gas evolution reactions: these are reactions that occur in liquids and produce a gaseous product
For example – Alka Seltzer in H2O
2. Oxidation-reduction reactions: electrons are transferred from one substance to another
For example – rust formation, batteries
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GENERAL TYPES OF REACTIONS
3. Precipitation reactions: reactions that occur in liquid that produce a solid substance
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IN MORE DEPTH . . .
We will discuss these reactions more in depth at a later time
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HOW DO WE KNOW THAT A CHEMICAL REACTION HAS TAKEN
PLACE?
Many chemical reactions produce easily detectable changesColor changeFormation of a solid Formation of a gasHeat absorption or emission (uses
up or produces heat)Light absorption or emission
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HOW DO WE KNOW THAT A CHEMICAL REACTION HAS TAKEN
PLACE?
The previous are only INDICATIONS of a chemical reaction
Chemical analysis is needed to verify if a reaction is actually occurring. For example: Boiling water looks like a
gas is being produced, but this is a physical change, NOT A CHEMICAL CHANGE
H2O(l) H2O(g) NO NEW SUBSTANCE
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SHOWING CHEMICAL REACTIONS
Chemical equations are a way that chemists summarize a chemical reaction that takes place
Reactions take the following general format
Reactants ProductsA set of chemicals react to form
a set of products
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REACTIONS AND ENERGYChemical reactions either absorb
energy/heat from their surroundings or they release energy/heat:
EXOTHERMIC: a chemical reaction that produces heat (ie. Burning gas in your car)
ENDOTHERMIC: a chemical reaction that absorbs heat (ie. Icy hot)
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SHOWING CHEMICAL REACTIONS
In chemical reactions, the state of matter is usually described:
1. Solid (s)2. Liquid (l)3. Gas (g)4. Aqueous (aq)
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PRACTICE For each of the following, translate
the sentence into a chemical reaction:
1. Solid zinc is mixed with aqueous hydrochloric acid to form zinc chloride and hydrogen gas
2. Aqueous sulfuric acid is combined with solid gold to produce aqueous gold(I) sulfate and hydrogen gas
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ANSWER
1. Zn(s) + HCl(aq) ZnCl2(aq) + H2(g)
2. H2SO4(aq) + Au Au2SO4(aq) + H2(g)
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HOW DO WE APPLY CONSERVATION OF MATTER TO CHEMICAL
REACTIONS?
C3H8(l) + O2(g) CO2(g) + H2O(l)
Let’s examine this reaction closer: How many atoms of each element are on
each side of the reaction?Reactants Products
C CH HO O
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BALANCING THE REACTION
According the law of conservation of matter, you must have the same number of each atom on each side
NO MATTER is created or destroyed
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BALANCING THE REACTION
Therefore, we must BALANCE the reaction to get the same number of atoms on the reactant side and the product side
To balance we can add more MOLECULES, but you cannot change the molecule
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BALANCING THE REACTION
C3H8(l) + O2(g) CO2(g) + H2O(l)
Therefore, we CAN add more C3H8
For example: we can have 3 C3H8
But we CANNOT change the molecule itself Cannot make C3H8 into CH8
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TRY TO BALANCE THE EQUATION
C3H8(l) + O2(g) CO2(g) + H2O(l)
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ANSWER C3H8(l) + 5O2(g) 3CO2(g) + 4H2O(l)
Let’s look at each atom on the reactant and product side:
Reactant ProductC 3 C 3H 8 H 8O10 O 10 Same number on each side =
BALANCED
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WHAT ARE THE NUMBERS IN FRONT OF EACH
COMPOUND? C3H8(l) + 5O2(g) 3CO2(g) + 4H2O(l)
The numbers in the front of each compound tells you how many MOLES you combine.
How many moles of each compound do you have in this reaction?
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BALANCING TIPS Just balancing the equation is
fairly difficultTherefore there are some tips to
help you balance the equation
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TIP #1 The first thing to do is to write the
skeletal reaction with just the compounds involved:
For example: Aqueous sodium hydroxide and aqueous
sulfuric acid mix to form liquid water and aqueous sodium sulfate
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TIP #2 H2SO4(aq) + NaOH(aq) H2O(l) +
Na2SO4(aq)
If an element occurs in only 1 compound on both sides of the reaction, balance it first. Otherwise, balance metals before nonmetals
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TIP #3 H2SO4(aq) + 2NaOH(aq) H2O(l) +
Na2SO4(aq) Not balanced yet
Save diatomic molecules and/or water for last H2SO4(aq) + 2NaOH(aq) 2H2O(l) +
Na2SO4(aq)
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SIDE NOTE SIDE NOTE: Most times, when you have a
polyatomic ion, do not break it up. Think of the polyatomic ion as one atom for balancing. It will save you some grief.
H2SO4(aq) + 2NaOH(aq) 2H2O(l) + Na2SO4(aq)
The SO4 in the reactant is balanced by the SO4 in the product. Don’t balance all the S and the O
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TIP #4 If a balanced equation contains
coefficient fractions, clear these by multiplying the entire equation by the appropriate number
C8H18 + O2 CO2 + H2O C8H18 + O2 8CO2 + 9H2O C8H18 + (25/2)O2 8CO2 + 9H2O 2C8H18 + 25O2 16CO2 +18 H2O
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TIP #5 Check to make sure the equation is
balanced by summing the atoms on each side of the reactionReactant Product
C 16 C 16H 36 H 36O 50 O 50
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TRY THESE1. Solid aluminum and aqueous sulfuric
acid combine to form aqueous aluminum sulfate and hydrogen gas
2. Solid iron combines with gaseous oxygen to form solid iron(III) oxide
3. Liquid ethanol (C2H6O) combines with gaseous oxygen to form gaseous carbon dioxide and liquid water
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ANSWER1. 2Al(s) + 3H2SO4(aq) Al2(SO4)3(aq) +
3H2(g)
2. 4Fe(s) + 3O2(g) 2Fe2O3(s)
3. C2H6O(l) + O2(g) 2CO2(g) + 3H2O(l)
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SPECIAL NOTE All reactions are reversible. They can
go forwards or backwards. For example:
4Fe(s) + 3O2(g) 2Fe2O3(s)
2Fe2O3(s) 4Fe(s) + 3O2(g)
To show this, we write reactions with double arrows 4Fe(s) + 3O2(g) 2Fe2O3(s)
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SPECIFIC TYPES OF CHEMICAL REACTIONS
There are 4 specific types of chemical reactions.
1. Synthesis (combination) reactions2. Decomposition reactions3. Displacement reactions4. Double displacement reactions5. Combustion reactions (special)
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SYNTHESIS REACTIONS A synthesis reaction is when you take
simpler molecules and combine them to form more complex molecules
They have the following general set up A + B AB Example: 2Na(s) + Cl2(g) 2NaCl(aq)
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DECOMPOSITION REACTIONS These are the opposite of the synthesis
reactions. A more complex compound breaks down to form simpler compounds.
They have the following general set up AB A + B Example: 2H2O(l) 2H2(g) + O2(g)
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DISPLACEMENT REACTIONS (SINGLE DISPLACEMENT)
One element displaces (or takes the place of) another element in a compound.
They have the following general set up A + BC AC + B Example: Zn(s) + CuCl2(aq) ZnCl2(aq) + Cu(s)
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DOUBLE DISPLACEMENT REACTION
Two elements, in separate compounds, displace (or switch places with) each other.
They have the following general set up AB + CD AD +BC Example: AgNO3(aq) + NaCl(aq) AgCl(s) +
NaNO3(aq)
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COMBUSTION REACTIONS When a compound combines with
oxygen to form carbon dioxide, water and heat
They have the following general set up Molecule + O2 CO2 + H2O + heat
Example: 2C2H6 + 7O2 4CO2 + 6H2O + heat
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TRY THESE Translate, balance and tell what type
of reactions the following are:1. Chlorine gas combines with
sodium bromide to form sodium chloride and bromine gas.
2. Mercury(II) oxide breaks apart to form mercury and oxygen gas.
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ANSWER1. Cl2 + 2NaBr Br2 + 2NaCl
The chlorine displaces the bromine in sodium bromide
This is a SINGLE DISPLACEMENT reaction
2. 2HgO 2Hg + O2
The mercury(II) oxide breaks apart into mercury and oxygen
This is a DECOMPOSITION reaction
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GENERAL TYPES OF REACTIONS (EXPANDED)
Before we can describe the general types of reactions, in detail, we have to visit the concept of solubility
Soluble: the substance in question will dissolve in water
Insoluble: the substance in question will not dissolve in water
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WHY SOLUBILITY If you know what compounds are
soluble, you can figure out if a reaction is: Gas evolution reaction Precipitation reaction
If soluble, the reaction will not form a precipitate or evolve a gas
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SOLUBLE (VERY IMPORTANT – MAKE SURE YOU COPY)
Soluble1. All acetates (C2H3O2
-) except Fe+3
2. All ammonium (NH4+) compounds
3. All bromides (Br-) except Ag+, Hg2+2,
and Pb+2
4. All chlorates (ClO3-)
5. All chlorides (Cl-) except Ag+ and Pb+2
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SOLUBLE (VERY IMPORTANT – MAKE SURE YOU COPY)
6. All iodides (I-) except Ag+, Hg2+2, and
Pb+2
7. All nitrates (NO3-)
8. All perchlorates (ClO4-)
9. All sulfates (SO4-2) except Ca+2, Ba+2,
Pb+2, Sr+2, Hg2+2
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INSOLUBLE Insoluble
1. Carbonates (CO3-2), except group 1 and
NH4+
2. Chromates (CrO4-2), except group 1 and
NH4+
3. Hydroxides (OH-), except group 1, Ca+2, Sr+2, and Ba+2
4. Oxalates (C2O4-2), except group 1 and
NH4+
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INSOLUBLE5. Oxides (O-2), except group 1, Ca+2, Sr+2,
and Ba+2
6. Phosphates (PO4-3), except group 1 and
NH4+
7. Sulfides (S-2), except those of group 1, group 2, and NH4
+
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SOLUBLE OR INSOLUBLE?1. H2SO4
2. Ca(C2H3O2)2
3. AgNO3
4. Na2O
5. Li2CO3
6. BaC2O4
7. Mg(OH)2
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ANSWER1. Soluble2. Soluble3. Soluble4. Soluble5. Soluble6. Insoluble7. Insoluble
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WHY DO WE CARE ABOUT SOLUBILITY?
By knowing the solubility rules, you will be able to do further analysis to determine if a chemical reaction will form a precipitate
If a chemical does not precipitate out of solution (have the product insoluble), then the reaction will not be a precipitation reaction
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EXAMPLE Examine the reactions below,
determine which reaction produces a precipitate or not
1. Ba(OH)2 + K2O BaO + 2KOH
2. 2H3PO4 + 3BaO Ba3(PO4)2 + 3H2O
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ANSWER1. Ba(OH)2(aq) + K2O(aq) BaO(aq) +
2KOH(aq) 1. BaO is soluble2. KOH is soluble3. Since both products are soluble, there is no
precipitate2. 2H3PO4(aq) + 3BaO(aq) Ba3(PO4)2(s) +
3H2O(l)1. Ba3(PO4)2 is insoluble.2. This means that as the reaction progresses,
the Ba3(PO4)2 is a precipitate that is produced.
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GENERAL TYPES OF REACTIONS (REVISITED)
Precipitation reactions
Only nonsoluble compounds form precipitates
If any product is insoluble, it forms a precipitate
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PRECIPITATION REACTION How to determine:1. Write the two compounds in question
as reactants1. Na2CO3 + CuCl2
2. Write the formulas of the potential products of the reaction
1. Na2CO3 + CuCl2 NaCl + CuCO3
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PRECIPITATION REACTION3. Look at the solubility rules to
determine the solubility of the products
1. NaCl soluble2. CuCO3 insoluble
4. Write the equation with states of matter
1. Na2CO3(aq) + CuCl2(aq) NaCl(aq) + CuCO3(s)
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PRECIPITATION REACTION5. Balance the equation
1. Na2CO3(aq) + CuCl2(aq) 2NaCl(aq) + CuCO3(s)
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GAS EVOLUTION REACTIONS Whenever a reaction produces a gas,
that gas will leave the reaction (bubble forms)
If a product is a gas, then you have a gas evolution reaction HCl(aq) + NaHCO3(aq) H2O(l) +
NaCl(aq) + CO2(g) This is the reaction of Alka Seltzer with
your stomach acid
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OXIDATION-REDUCTION REACTIONS
These reactions (redox) involve the transfer of electrons from one element to another
In order to understand these reactions better, we must look at the charges of the elements in a chemical reaction
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DEFINITIONS Oxidation: when an element loses
electrons (the atom becomes +) Reduction: when an element gains
electrons (the charge is reduced, becomes -)
Oxidation and reduction must occur together so the electrons can travel from one element to another
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OXIDATION-REDUCTION REACTIONS
Example 4Na(s) + O2(g) 2Na2O
4 Na (s) 4 Na+ + 4e- 4e- + 2O 2O-2
In this example, Na goes from a neutral charge to a +1, it needed to lose an electron
O goes from a neutral charge to a -2, it had to gain electrons
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TRY THESE In each of the following reactions,
identify the element that is oxidized and the element that is reduced:
1. 2Na + Cl2 2NaCl
2. 4Fe + 3O2 Fe2O3
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ANSWER1. 2Na + Cl2 2NaCl
1. 2Na 2Na+ + 2e- (oxidized)2. 2e- + 2Cl 2Cl- (reduced)
2. 4Fe + 3O2 2Fe2O3
1. 4Fe 4Fe+3 + 12e-2. 12e- + 6 O 6 O-2
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SUMMARY There are 3 general types of reactions
Precipitation One of the products must be insoluble Use the solubility rules
Gas evolution If a gas is produced, it will come out of solution
Oxidation-reduction Involves the movement of electrons Something must be oxidized (lose electrons)
and something must be reduced (gain electrons)
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SUMMARY There are 5 specific types of
reactions Synthesis
A + B AB Decomposition
AB A + B Displacement
A + BC AB + C Double displacement
AB + CD AD + BC Combustion
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SUMMARY With any sort of chemical reaction, we
must follow the law of conservation of mass
Therefore, every chemical reaction must have the same number of atoms in the reactants and products
To balance, use the following tips
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SUMMARY
1. Write the skeletal reaction with just the compounds involved.
2. If an element occurs in only 1 compound on both sides of the reaction, balance it first. Otherwise, balance metals before nonmetals
3. Save diatomic molecules and/or water for last
4. If a balanced equation contains coefficient fractions, clear these by multiplying the entire equation by the appropriate number
5. Check to make sure the equation is balanced by summing the atoms on each side of the reaction