1. Unit 6 – Chemical Reactions
Chemical equations, Molar mass, Rates of reactions, Limiting reactants

2. Intro Vocabulary
Chemical reaction is the changing of substances to other substances by breaking bonds in reactants and forming new bonds in the products.
-when some chemicals come into contact, they break apart, join, or rearrange to form new chemicals (always to become more stable)
-produce new substances with new properties
Chemical equations are shorthand representations of chemical reactions.

3. Some more vocabulary Reactant(s) yield product(s) A + B  AB
Reactants are the elements or compounds that enter into a reaction
Products are the elements or compounds that are formed as a result of a chemical reaction
Arrow () means yields, produces or forms
Reactant(s) yield product(s)
A + B  AB

4. Al2(SO4)3 + Ca(OH)2  Al(OH)3 + CaSO4
Skeleton equation (Unbalanced equation)
Consists of symbols and subscripts
Symbols: element, yield (), combining (+)
Subscript: small number found below the element symbol representing the number of atoms of each element present

5. Al2(SO4)3 + Ca(OH)2  Al(OH)3 + CaSO4
Name the reactants (everything left of arrow)
Aluminum sulfate & Calcium hydroxide
Types & number of atoms in each reactant
Aluminum sulfate
Al = 2 S = 3 O = 12
Calcium hydroxide
Ca = 1 O = 2 H = 2

6. Al2(SO4)3 + Ca(OH)2  Al(OH)3 + CaSO4
Name the products (everything right of arrow)
Aluminum hydroxide & Calcium sulfate
Types & number of atoms in each reactant
Aluminum hydroxide
Al = 1 O = 3 H = 3
Calcium sulfate
Ca = 1 S = 1 O = 4

7. Al2(SO4)3 + Ca(OH)2  Al(OH)3 + CaSO4
Notice that the number of atoms is not the same on both sides of the equation.
Al = 2 S = 3 O = 14 Ca = 1 H = 2
On the reactant side
Al = 1 S = 1 O = Ca = 1 H = 3
On the product side

8. Balancing equations why & how
Why do we balance equations?
Law of conservation of mass
-atoms are not created or destroyed in an ordinary chemical reaction, just rearranged to form new substances
What is used to balance chemical equations?
Coefficients
-the number before the chemical formula (the number is written normal size – not superscript or subscript)

9. Steps to Balancing Equations
1. Determine the number of atoms of each element in reactants and products
2. Balance by adding coefficients
A. Polyatomic ions (if same poly. ion on both sides  balance as a chunk)
B. Metals
C. Nonmetals
D. “O” & “H”
3. Recheck your count!!!

10. H2 + O2  H2O 2 2 H O * Only add coefficients, NEVER Δ subscripts
Recount total number of each type of atom
Only 1 oxygen atom “out” (2 “in”)
 place 2 in front of H2O
Only 2 hydrogen “in” (4 “out”)
 place 2 in front of H2
* Only add coefficients, NEVER Δ subscripts
Can you ever make just 1 molecule of water?

11. 2 NaOH  Na2O + H2O Na O H Only 1 sodium atom “in” (2 “out”)
 place 2 in front of NaOH
Recount total number of each type of atom

12. 2 4 Fe + O2  Fe2O3 3 2 Fe O Recount total number of each type of atom
Only 1 iron atom “in” (2 “out”)
 place 2 in front of Fe
Only 2 oxygen atom “in” (3 “out”)
 place 2 in front of Fe2O3
and place 3 in front of O2
Only 2 iron atom “in” (4 “out”)
 change 2 in front of Fe into a 4

13. Counting molecules/compounds
How many molecules of each of the following compounds are present in this equation?
Al2(SO4)3 + 3Ca(OH)2  2Al(OH)3 + 3CaSO4
Reactants:
Al2(SO4)3 = 1 (when only 1 = no number)
Ca(OH)2 = 3 (large 3 in front)
Products:
Al(OH)3 = 2 (large 2 in front)
CaSO4 = 3 (large 3 in front)

14. 2H20  2H2 + O2
How many molecules of oxygen are formed when 2 molecules of water are broken down?
one
How many molecules of water would be required to form 3 molecules of oxygen?
Six
The number of molecules does not have to be the same!
2 molecules in, 3 molecules out.

15. Using state symbols
When writing chemical equations, the state of each product or reactant may be labeled with the following abbreviations
(s) = solid
(g) = gas
(l) = liquid
(aq) = aqueous (solid dissolved in a liquid usually water)
NOTE: If the states of matter are not included, you will NOT need to include them. If the states of matter are present, you MUST include them!

16. 7 Diatomic elements
7 elements can not exist as single elements – must exist in pairs if it is JUST that element
HONClBrIF
These 7 are always H2, O2, N2, Cl2, Br2, I2, F2
Never just write H, O, N, Cl, Br, I, F without being bonded to another element.
H20 is okay – WHY?
Because O is bonded to another element

17. Steps to using word equation to form formula equations:
1)     Write formulas / symbols
2)    Check for diatomic elements
3)    Add state symbols (if given)
4) Balance (if can’t balance, then recheck formulas!!)

18. Writing chemical equation from word equations
Na+1
Br-1
Solid sodium bromide reacts with chlorine gas to yield solid sodium chloride and bromine gas.
Na+1
Cl-1
Recheck
Check for diatomics (HONClBrIF)
Write formulas & element symbols
Add state symbols
Balance 2
NaBr + Cl  2
NaCl + Br
(s)
(g)
(g) 2
(s) 2
NaBrCl

19. Another word equation 2 4 Al + 3 O  2 Al2O3
Solid aluminum metal reacts with oxygen gas to form solid aluminum oxide.
O-2
Al+3
Check for diatomics (HONClBrIF)
Write formulas & element symbols
Add state symbols
Balance
Recheck 2 4 Al + 3 O  2
Al2O3
(s)
(g) 2
(s)
AlO

20. Writing Word Equations
Na2O(s) + CO2(g)  Na2CO3(s)
Solid sodium oxide combines with (reacts with / and) carbon dioxide gas to form (yields/produces) solid sodium carbonate.
NaCl(s) + AgNO3(aq)  NaNO3(aq) + AgCl(s)
Solid sodium chloride and (combines with / reacts with) aqueous silver nitrate forms (yields / produces) aqueous sodium nitrate and solid silver chloride.

21. 5 Basic Types of Reactions
Synthesis Reaction
Two or more substances combine to form a single substance.
Also known as a combination reaction.
A + B  AB
always forming 1 product
Example: 2K + Cl2  2KCl

22. 5 Basic Types of Reactions
Decomposition Reaction
A single compound is broken down into two or more products.
AB  A + B
always having 1 reactant
Example: CaCO3  CaO + CO2

23. 5 Basic Types of Reactions
Single Replacement Reaction
one element replaces another element in a compound (also called single displacement)
AB + C  AC + B
Always a compound + element as reactants
Example:
Mg + Zn(NO3)2  Mg(NO3)2 + Zn
(Mg is Cation so replaces the cation in the compound)

24. 5 Basic Types of Reactions
Double Replacement Reaction
the positive ions are exchanged between two reacting compounds (also called double displacement)
AB + CD  AD + CB
Always a compound + compound as reactants
Example: BaCl2 + K2CO3  BaCO KCl
(Ba & K are the cation that switch places forming the new compounds)

25. 5 Basic Types of Reactions
Combustion Reaction
an element or a compound reacts with oxygen often producing energy as heat and light
CxHy + O2  CO2 + H2O
Always has oxygen as a reactant
Is an exothermic reactions (gives off heat)
Example: CH4 + 2O2  CO2 + 2H2O

26. Calculating Gram Formula Mass
Formula mass can be calculated in amu’s or g’s of a substance by multiplying the number of atoms of each element by the mass in amu’s or g’s of the element. Then add the values together. (YES, sig figs COUNT!!!)
Example: CaSO4
(# atoms each element x mass = total mass of element in compound)
1 Ca x g =
1 S x g =
4 O x g =
Then add masses of all elements together + + =

27. The Mole
To make a quantity that is measurable in lab, we use the mole.
In chemistry one mole is equal to x 1023 particles (Avogadro’s number).
The gram formula mass of any compound is the mass of 1 mole of the compound in grams.
1 mole = x 1023 is similar to
12 eggs = 1 dozen
52 weeks = 1 year
1 gross = 144

28. Limiting Reactants
The limiting reactant is the reactant that determines the maximum amount of product that is formed.
The limiting reactant will be completely used up in a reaction. This makes the reaction stop.
The other reactant will have some unchanged so it is said to be the excess reactant.
For example, if you need to make 10 chicken sandwiches. You have 10 slices of bread and 10 pieces of chicken. If each sandwich requires 2 slices of bread and 1 piece of chicken, which is the limiting reactant? Excess reactant?

29. Rates of Reactions
The reaction rate is the change in concentration of reactants and products in a certain amount of time.
Rate at which the reactants disappear and the products appear.
Combining two substances (causing a reaction) means forcing their particles to hit, or collide with, one another
Collision Theory states that molecules must collide in order to react

30. Activation Energy
The activation energy is the energy needed to start the reaction.
When particles collide with sufficient energy – at least equal to the activation energy – existing bonds may be disrupted and new bonds can form
Endothermic reaction – the energy of the product is greater than that of the reactants (energy is absorbed into the reaction)
Exothermic reaction – the energy of the products is lower than that of the reactants (energy is released from the reaction)

31. Factors Affecting Reaction Rates
Nature of Reactants
Depends on the state of particular reactants and the complexity of the bonds that have to be broken and formed in order for the reaction to proceed
The more bonds to be broken then the longer the reaction takes
A reaction between two gases will be quicker than a reaction between two liquids or two solids.

32. Factors Affecting Reaction Rates
Temperature
The higher the temperature at which a reaction occurs, the faster the particles will move
The faster the particles move the higher the frequency of collisions
For example, food spoils faster at room temperature than when it is refrigerated.

33. Factors Affecting Reaction Rates
Concentration
Deals with how many particles are there
An increase in concentration means that there are more particles within a given volume and thus smaller spaces between the reacting particles.
Thus, the higher the concentration of reactants, the greater the frequency of collisions among their particles.
For example, the more people there are in a room the more people you will bump into as you walk through the room.

34. Factors Affecting Reaction Rates
Surface Area
Surface area deals with the number of particles that are exposed for reaction.
The larger the surface area the greater the number of particles that are exposed for reaction.
For example, many small pieces of coal will burn faster than a lump of coal (small pieces have more particles exposed to react with more oxygen particles)

35. Factors Affecting Reaction Rates
Catalysts
A catalyst is a substance that increases the rate of the reaction without itself being used up in the reaction (doesn’t appear as a reactant or a product)
Catalysts lower the activation energy required for a reaction to occur.
Thus a catalyst creates a different pathway from reactants to products – one that requires less energy.
Catalysts in the body are enzymes – there to speed up reactions in the body that are essential to life.