1 flashback! chemical reactions types of chemical equations balancing chemical equations reaction...
TRANSCRIPT
1
FLASHBACK!
Chemical ReactionsTypes of Chemical Equations
Balancing Chemical EquationsReaction Rates
Awareness of basic chemistry can save your life! Example: mixing certain cleaning solutions can
produce a poisonous gas Ammonia (Windex) + Bleach (Clorox)
Chloroamine (a poisonous gas) Chemistry is alive in our everyday life:
Ice Packs, Hot Packs, Air Bags in Cars, Foods
→
Compounds are groups of elements chemically bonded together
2 types we’ve studied: IONIC – bonding where electrons are gained or lost
COVALENT – bonding where electrons are shared
A reaction that releases energy and gives off heat/light/sound resulting in a raising of temperature
“energy” will be with the products side of a chemical equations
Examples: glow sticks, fire, lycopodium powder
A reaction that ABSORBES energy resulting in LOWERING of temperature.
“energy” will be with the REACTANTS side of a chemical equations
Examples: ANTACID & WATER, PHOTOSYNTHESIS
Changes in PHYSICAL properties1. Melting2. Boiling3. Condensation4. Evaporation5. Sublimation6. Change in Size or Shape
NO change occurs in the IDENTITY of the substance(s)
Examples: Ice, rain, and STEAM are all WATER
Atoms in the REACTANTS are REARRAGED to form one or more DIFFERENT substances
OLD chemical BONDS are BROKEN and NEW chemical BONDS are FORMED
Changes DO occur in the identity of the compounds since NEW compounds are formed
Examples:
Fe and O2 form RUST (Fe2O3)
Ag and S form TARNISH (Ag2S)
1. New substance produced
2. Production of a gas
3. Change in color
4. Change in smell
5. Change in heat or light
Classify each of the following as a
PHYSICAL CHANGE (P) or a
CHEMICAL CHANGE (C)
A. ____ a burning candle
B. ____ steam coming up from boiling H2O
C. ____ toasting a marshmallow
D. ____ cutting a pizza
E. ____ polishing silver
Classify each of the following as a
PHYSICAL CHANGE (P) or a
CHEMICAL CHANGE (C)
A. _C_ a burning candle
B. _P_ steam coming up from boiling H2O
C. _C _ toasting a marshmallow
D. _ P cutting a pizza
E. _ C _ polishing silver
A process in which AT LEAST
ONE NEW SUBSTANCE IS
PRODUCED AS A RESULT OF A
CHEMICAL CHANGE.
11
REACTANTS PRODUCTS
Draw the contents of these two boxes on your paper
A. Use the box drawing to determine, how does the equation indicate a change in the identity of the reacting substances?
B. Does the equation follow the Law of Conservation of Matter? How can you tell?
A. Use the box drawing to determine, how does an equation indicate a change in the identity of the reacting substances? The formulas of the reactants are different than the formulas of the products.
B. Does the equation follow the Law of
Conservation of Matter? How can you tell? Yes, there are the same number and kinds of symbols (atoms) on both sides of the chemical equation.
Chemical equations give a “BEFORE & AFTER” picture of a chemical reaction
Reactants Products
MgO + C CO + Mg
*magnesium oxide TO FORM *carbon monoxide
REACTS with carbon and magnesium
15
→
12 oz of dough, 4 oz mushrooms, 12 slices pepperoni, 8 oz cheese and 5 oz
tomato sauce are used to make a pizza.
A.How would you write the recipe above as an equation?
12 oz of dough, 4 oz mushrooms, 12 slices pepperoni, 8 oz cheese and 5 oz tomato
sauce are used to make a pizza.
A.How would you write the recipe as an equation?
12 oz dough + 4 oz mshrm + 12 pep + 8 oz chse 1 pizza
+ 5 oz tom sauce
4NH3 + 5O2 → 4NO + 6H2O ________ molecules of NH3 REACT with
________ molecules O2 TO PRODUCE
________ molecules of NO and ________
molecules of H2O
FOURFIVE
FOUR SIX
SAME numbers of EACH TYPE OF ATOM on each side of the equation
Al + S → Al2S3
2Al + 3S → Al2S3
When balancing an equation, _______change subscripts; _________ change ______________
Not Balanced
Balanced
NEVERCOEFFICIENTS
ALWAYS
H2 + Cl2 → 2HCl
Total Atoms = Total Atoms H = 2, Cl = 2 H = 2, Cl = 2
Total Mass = Total Mass 2 (1.0) + 2 (35.5) 2 (1.0 + 35.5) 73.0 amu = 73.0 amu
→+ +
In any ordinary chemical
reaction, MATTER IS
NOT CREATED or
DESTROYED
Add Coefficients IN FRONT of compounds to BALANCE the equation
4NH3 + 5O2 4NO + 6H2O
N = & N = H = & H = O = & O =
41210
41210
Fe3O4 + H2 Fe + H2O
Fe: Fe3O4 + H2 3Fe + H2O
O: Fe3O4 + H2 3Fe + 4H2O
H: Fe3O4 + 4H2 3Fe + 4H2O
Fe3O4 + 4H2 3Fe + 4H2O
A. Number of H atoms in the reactants?
B. Number of O atoms in the reactants?
C. Number of Fe atoms in the reactants?
Fe3O4 + 4H2 3Fe + 4H2O
A. Number of H atoms in the reactants? 8
B. Number of O atoms in the reactants? 4
C. Number of Fe atoms in the reactants? 3
6CO2 + 6H2O + sunlight C6H12O6 + 6O2
A. Number of carbon atoms in the reactants?
B. Number of oxygen atoms in the reactants?
C. Number of hydrogen atoms in the reactants?
D. Is this a endo or exothermic reaction? What important biological process does this chemical equation represent?
6CO2 + 6H2O + sunlight C6H12O6 + 6O2
A. # of carbon atoms in the reactants? 6
B. # of oxygen atoms in the reactants? 18C. # of hydrogen atoms in the reactants? 12D. Is this a endo or exothermic reaction? What important
biological process does this chemical equation represent? Endothermic Reaction; Photosynthesis
Balance each equation. SHOW YOUR WORK!
A. Mg + N2 Mg3N2
B. Al + Cl2 AlCl3
C. Fe2O3 + C Fe + CO2
D. Al + FeO Fe + Al2O3
Balance each equation. SHOW YOUR WORK!
A. Mg + N2 Mg3N2
B. Al + Cl2 AlCl3
C. Fe2O3 + C Fe + CO2
D. Al + FeO Fe + Al2O3
22 3
32 3
42 3 3
3
1. Synthesis
Getting Together
A + B → AB
___Fe + ___O2 → ___Fe2O3
Iron reacts with Oxygen to produce rust
234
2. Decomposition Breaking Apart AB → A + B
___H2O2 → ___H2O + O2 + energy
Hydrogen Peroxide reacts with Oxygen to produce water & oxygen & energy
22
3. Single Replacement Reaction
One Exchange
AB + C → A + BC or A + BC → AB + C
Ag + H2S → AgS + H2
Silver Tarnishing
4. Double Replacement Reaction Two Exchanges
AB + CD → AC + BD
HCl + NaOH → NaCl + H2OAcid + Base → Salt + Water
CH3COOH + NaHCO3 → CH3COON2 + H2O + CO2
Vinegar + Baking Soda → Sodium Acetate Salt + Water + Carbon Dioxide
(Neutralization)
(Neutralization)
Determine which type of chemical reaction is shown:
A.CuCl2 + H2 S → CuS + 2HCl
B.2H2O → 2H2 + O2
C.MgO + Fe → FeO3 + Mg
D.P4 + 5O2 → P4O10
DR
DSR
S
E. Ag + H2S → AgS + H2
F. Fe3O4 + 4H2 → 3Fe + 4H2O
G. 3Mg + N2 → Mg3N2
H. 3Al + 3Cl2 → 2AlCl3
I. HCl + NaOH → NaCl + H2O
J. 2Fe2O3 + 3C → 4Fe + 3CO2
K. 2Al + 3FeO → 3Fe + Al2O3
L. 2Fe2O3 → 4Fe + 3O2
SRSR
SS
DRSR
SRD
• “Reaction Rates” refers to HOW FAST A REACTION OCCURS
• Factors that Influence Reaction Rates
1. Temperature Examples: o Glow sticks in HOT water glow brighter than
one in cold water o Antacid dissolves faster in HOT water than
cold water
• Factors that Influence Reaction Rates2. Surface Area
Refers to how much of the outside of a substance is exposed
The greater surface area, the faster the reaction Examples: o Lycopodium Powdero Headache medicine reacts faster in powder form
than solid form (ex. Goodie Powder versus Tylenol Pill)
• Factors that Influence Reaction Rates3. Concentration
Refers to how much of a substance there is The greater concentration of a reactant,
the faster the reaction Example: o Vinegar & Baking Soda in Beaker – more
vinegar produces a faster reaction
• Factors that Influence Reaction Rates4. Presence of a Catalyst
Refers to a substance that speeds up a reaction but is NOT used up by the reaction
The catalyst can be recovered unchanged, and re-used indefinitely
Examples: o Yeast in our “chemiluminescent elephant’s
toothpaste” reactiono Enzymes found in animals that speed up digestion
• Factors that Influence Reaction Rates5. Presence of an Inhibitor
Refers to something that slows down or stops a chemical reaction
Examples: o Why do we cover our left over foods?o Why do we even put food in the fridge?o Why do we use food preservatives like salts?
List 4 ways to make a reaction occur faster
(increase the speed): 1.
2.3.4.
List 4 ways to make a reaction occur slower (decrease the speed):
1. 2.3.4.
See Study Guide From Chapter 7
Test