chemical reactions. chemical reactions objectives 1.classify and name compounds in chemical...
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Chemical Reactions Objectives1.Classify and name compounds in chemical reactions2.Describe chemical reactions in word and chemical
equations.3.Balance chemical equations based on the Law of
Conservation of Mass.4.Identify and classify types of chemical reactions
and energy changes involved.5.Predict products and energy changes in a chemical
reaction. 6.Identify and test factors that affect the rate of
chemical reactions.
Chemical Reactions
What is a chemical reaction? • Use your background knowledge to explain
what a chemical reaction is.• Think about chemical changes you have
observed in your surroundings.• Think about chemical changes on an atomic
level.
Chemical Reactions• Substances chemically interact to form different
substances. • A substance can be an element or a compound.
• Chemical bonds are broken and created.
Example: Iron chemically reacts with Oxygen to produce Iron(II) Oxide
Chemical Equations Fe + O2 ------> FeO
Reactants:
• Starting substances.• Chemically interact with one another.• Usually located to the left of the arrow.Products:• Ending substances.• Substances formed from the chemical reaction.• Usually located to the right of the arrow.
Chemical Equations
Fe(s) + O2 (g) ------> FeO (s)
• (s)= substance in solid state• (g)= substancein gaseous state• (l)= substance in liquid state• (aq)= substance dissovled in water.(aqueous solution)
Chemical Reactions Fe(s) + O2 (g) ------> FeO (s)
• Are atoms destroyed or created during a chemical reaction?
• No, they are just rearranged to produce new substances.
Law of Conservation Of Mass
• Matter is not created or destroyed.
• Matter is just rearranged.(mass of reactants = mass of products)
That is why it is important to balance chemical equations.
Conservation of Mass Lab
• Observe the conservation of mass lab, to understand why it is important to balance chemical equations.
Balancing Chemical Equations 2Fe(s) + O2 (g) ------> 2FeO (s)
Balancing Chemical Equations:1. Add coefficients in front of substances, do
NOT change subscripts.
2. First balance elements that only appear once on each side of the equation.
Chemical Reactions Bell Ringer1. N2 (g) + H2(g) --------> NH3(g)
a. What is the chemical name of one of the reactants?
b. What is the chemical name of the product?
c. What state of matter is all the substances in this reaction?
d. Balance the chemical equation if needed.
Type of Anion
Name of Acid
Monatomic anion (-ide ending)
hydro + stem + ic
Polyatomic anion(-ite ending)
stem + ous
Polyatomic anion(-ate ending)
stem + ic
Types of Chemical Reactions
1. Synthesis (A+ B ----> AB)2. Decomposition (AB------> A + B)3. Single Replacement (A+ BC ---> B + AC)4. Double Replacement (AB + CD ---> CB + AD)5. Combustion (CxHx + O2 ----> CO2 + H2O)
6. Neutralization (Acid + Base--> H2O + Salt)
Chemical Reactions Objectives1. Identify and classify types of chemical reactions.
2. Identify energy changes involved with chemical reactions.
3. Predict products and energy changes in a chemical reaction.
Synthesis (Combination) Reaction
• 2 or more substances chemically combine to form a single substance.
• A + B ---> AB + energy
• Energy released into surroundings is more than energy absorbed by the system.
( Energy of surroundings > Energy of system)
Decomposition Reaction
• A compound breaks down into simpler substances.
• AB + energy ----> A + B
• Energy of system > Energy of surroundingsWhy?
Single Replacement Reaction
• An element replaces another element in a compound.
• A + BC --------> B + AC + energy
• Energy of surroundings > Energy of system
Double Replacement Reaction
• Exchange of cations between two compounds. • AB + CD + energy ----> CB + AD + more energy
• Energy of Surrounding > Energy of System
Combustion Reaction
• Fuel (hydrocarbons) reacts with oxygen to produce predictable substances and energy.
• CxHx + O2 ----> CO2 + H2O + ENERGY
• Energy of Surroundings > Energy of System
Neutralization • Acid and Base react to produce predictable
products. • Changes the pH to 7 (neutral).
Acid + Base -------> H2O + Salt
Salt: An ionic compound. The cation comes from the base and the anion from
the acid.
Class Reminders:
• Acid Rain Article (15pts.)
• Balance Chemical Equations Worksheet (10pts.) (balance and classify equations)
• Word Equation Worksheet (10pts.)
*3rd Quarter Ends: March 8th*
Chemical Reaction Lab
Purpose: • Perform and observe types of chemical
reactions.• Determine reactants and predict products.• Classify chemical reactions.• Balance chemical reactions.• Write a formal lab report
Types of Chemical Reactions
1. Synthesis (A+ B ----> AB)2. Decomposition (AB------> A + B)3. Single Replacement (A+ BC ---> B + AC)4. Double Replacement (AB + CD ---> CB + AD)5. Combustion (CxHx + O2 ----> CO2 + H2O)
6. Neutralization (Acid + Base--> H2O + Salt)
Chemical Equations to Lab
Just need to check and see if they are balanced. 1. Mg + O2 ------>
2. Mg + HCl ----> 3. (NH4)2(CO3) -----> NH3 + CO2 + H2O
4. Ca(CO3) + HCl ----> CaCl2 + H2O + CO2
5. Zn + CuCl2 ---->
6. CuCl2 + Na3(PO4) --->
7. HCl + Na(OH) ----> H2O + NaCl
8. C2H6O + O2 ----->
Chemical Reaction Review1. What are the coefficients that will balance the
chemical equation below? AlCl3 + Na(OH) ----> Al(OH)3 + NaCl
a. 1,3,1,3b. 3,1,3,1c. 1,1,1,3d. 1,3,3,12. What type of chemical reaction is in question 1?
3. Predict the product and balance if needed: Ba (s) + O2 (g) ---------->
Chemical Equations to Lab
Just need to check and see if they are balanced. 1. Mg + O2 ------> MgO
2. Mg + HCl ----> MgCl + H2
3. (NH4)2(CO3) -----> NH3 + CO2 + H2O
4. Ca(CO3) + HCl ----> CaCl2 + H2O + CO2
5. Zn + CuCl2 ----> ZnCl2 + Cu
6. CuCl2 + Na3(PO4) ---> Cu3(PO4)2 + NaCl
7. HCl + Na(OH) ----> H2O + NaCl
8. C2H6O + O2 -----> CO2 + H2O
ConclusionNeeds to include the following:• Identify and explain the types of reactions obsvd. ?
• Which reaction(s) did you like the best and why?
• Based on data section explain which reactions were exothermic and endothermic.
• What did you learn from this lab?
Predicting Products in a Chemical Reaction
a. Ca + N2 --------> ?
b. Cu2S -------> ?
c. NaBr + F2 ------> ?
d.CH4 + O2 ----->
Balancing and Classifying Equations Quiz Types of Chemical Reactions 1. Synthesis 2. Decomposition 3. Single Replacement 4. Double Replacement 5. Combustion 6. Neutralization
Predicting Single Replacement Reactions• An Activity Series can help us predict if a single
replacement reaction will take place.
Activity Series Lab Hypothesis CuCl2(aq) Ag(NO3) HCl (aq) dH(OH) (l)
Copper (s)
Magnesium (s)
Zinc (s)
Calcium (s)
Activity Series Lab1. Using the Activity Series Table, predict whether
the following single replacement reactions would occur:
a. Li + MgCl
b. Hg + Na3P
c. Pb + HF
Predicting Single Replacement Reactions• An Activity Series can help us predict if a single
replacement reaction will take place.
Chemical Reaction Study Guide Changes
1. Vocabulary words: Thermochemistry10. HgO + energy ------> Hg + O211. Fe + F2 ----------> FeF3 + energy
12. CH4 + O2 ---------> CO2 + H2O + energy
15. K(OH) + H3(PO4) ------->
18. Omit last word equation.
Chemical Reaction Review1. What are the coefficients that will balance the
chemical equation below? AlCl3 + Na(OH) ----> Al(OH)3 + NaCl
a. 1,3,1,3b. 3,1,3,1c. 1,1,1,3d. 1,3,3,12. What type of chemical reaction is in question 1?
3. Predict the product and balance if needed: BaS + Mg ---------->
ThermochemistryEnergy changes that occur within reactions.
Endothermic Reactions Exothermic Reactions
Exothermic Reaction
• Energy absorbed < Energy released. • The chemical reaction becomes cooler and its
surroundings gets warmer. • Energy is on the product side.
• C8H18 + O2 -------> CO2 + H2O + energy
Endothermic Reactions• Energy absorbed > Energy released• Chemical reaction gets warmer and its
surroundings gets cooler. • Energy is on the reactant side.Ex. Photosynthesis
Chemical Reaction Energy Diagram• Activation Energy (Ea): The amount of kinetic energy needed to be absorbed from the surroundings for thechemical reaction to occur.
H : The amount of kinetic energy released into the into the surroundings.
Chemical Reactions Objectives1.Classify and name compounds in chemical reactions2.Describe chemical reactions in word and chemical
equations.3.Balance chemical equations based on the Law of
Conservation of Mass.4.Identify and classify types of chemical reactions and
energy changes involved.5.Predict products and energy changes in a chemical
reaction. 6.Identify and test factors that affect the rate of
chemical reactions. (Chpt. 18.1)
Chemical Reactions Rates• Reaction Rates = how fast the reactants
chemically change into the products. • Collision Theory: Reactant particles will react to
form products when they collide and exchange enough kinetic energy with one another.
Rates of Chemical Reactions
• What are factors that can affect the rates of reactions?
• Temperature• Concentration of Reactants• Surface Area of Reactants• Catalysts• Inhibitors
Temperature of Reaction
What if we increase the temperature of a reaction?
What if we decrease the temperature of a reaction?
Catalysts
• Catalysts speed up reactions, but they are not apart of the chemical reaction.
Ex. Enzymes keep your body temperature around 37oC (98 oF) by speeding up important biological reactions.
Inhibitors
• Inhibitors slow down a chemical reaction.• Inhibitors bind to a catalyst and prevent it
from speeding up a reaction. Ex. Preservation of food. Antioxidants prevent
foods from becoming stale or moldy.
Soln. A Concentration vs. Avg. Reaction Times
TimeConc
G1 G2 G3 G4 G5 G6 G7 Avg.
A1 7 6 9 9.4 5 3 4.0
A2 6.4 9 9.76 9.5 8 9 15.2
A3 4.8 12 9.4 13.4 12 6 22.6
A4 8.9 15 15.0 19.1 19.1 14 24.3
Activation Energy• Activation energy = minimum energy
colliding reactants must have for a reaction to occur. (Energy hump.)