chapter 7. chapter 7 day 1 objective : interpret chemical reactions for reactants and products,...
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Chapter 7 Day 1OBJECTIVE:
Interpret chemical reactions for reactants and products,
energy needs and conservation of mass. Do Now: Chapter 7 Vocabulary TURN IN: Model Molecule Lab
Today: Chapter 7 – Chemical Reactions notes
Types of Chemical Reactions Cartoon Chemistry
Homework: Finish Cartoon Chemistry
Unit 2 Chapter 7 Day 2 OBJECTIVE:
Interpret chemical reactions for reactants and products,
energy needs and conservation of mass.
Do Now: Types of Chemical Reactions
Today: The Balancing Act packet –
Notes and Worksheets Homework:
Balancing Equations
Unit 2 Chapter 7 Day 3 OBJECTIVE:
Interpret chemical reactions for reactants and products,energy needs and conservation of mass.
• Do Now: • Balancing Review
• Today:• Homework review – Balancing Equations• DVD Field Trips – Chapters 6 & 7• Test review / Study Guide…
What did we learn again?• START Test Review packet
• Homework:• COMPLETE Test Review packet
Unit 2 Chapter 7 Day 4 OBJECTIVE:
Demonstrate knowledge of matter, phase, atomic structure, the periodic table, chemical reactions and
conservation of mass.
• Do Now: • Vocabulary Bingo - Chapters 4,5,6,7
• Today:• Review Chemistry Unit Study Guide• Spring Balance Challenge
• Homework:• STUDY FOR CHEMISTRY UNIT TEST
Unit 2 Chapter 7 Day 5OBJECTIVE:
Demonstrate knowledge of matter, phase, atomic structure, the periodic table, chemical reactions and
conservation of mass.• Do Now:
• Do Now Folder #6-7 (8 pages)• Today:
• Chemistry Unit Test • Unit 2 Notebook Chap 6 & 7 (21 pages)
• Homework: Current Events – 2nd Chance
Experiments
Extra Credit Balance Challenges
A) ____ CoBr3 + ____ CaSO4 ____ CaBr2 + ____ Co2(SO4)3
B) ____ S + ____ HNO3 ____ H2SO4 + ____ NO2 + ____ H2O
C) ____ Cu + ____ HNO3 ____ Cu(NO3)2 + ____ NO + ____ H2O
A 2 CoBr3 + 3 CaSO4 3 CaBr2 + Co2(SO4)3
B S + 6 HNO3 -> H2SO4 + 6 NO2 + 2 H2O
C 3 Cu + 8HNO3 -> 3 Cu(NO3)2 + 2 NO + 4 H2O
Unit 2 Chapter 6/7 OBJECTIVE:
Investigate five indicators of chemical reations.
• Do Now: • ASK Review
• Today:• Identifying Chemical Reaction Lab
• Homework:• Missing Assignments for MP1?
Wednesday 11/12and Thursday 11/13
Indicators of chemical reactions
Formation of a gas
Emission of light or heat
Formation of a precipitate
Color change
Emission of odor
All chemical reactions:
Create 1 or more new substancesHave two partsReactants - the substances you start
withProducts- the substances you end up
with
The reactants turn into the products.Reactants ® Products
In a chemical reaction…
Bonds between atoms in reactants are brokenAtoms rearrange and form new bonds in the productsAtoms aren’t created or destroyed…Mass is CONSERVED in a chemical reaction..This is called…
Law of Conservation of Mass
All chemical reactions are accompanied by a change in energy. It takes energy to break bonds AND energy is released when bonds are broken!
Exothermic - reactions that release energy to their surroundings (usually in the form of heat)
Endothermic - reactions that need to absorb heat from their surroundings to proceed.
Reaction Energy
Synthesis ReactionsTWO elements combine to make one compound. (Polyatomics count as one)
A + B ® AB
Na + Cl2 ® NaCl
Ca +O2 ® CaO
SO3 + H2O ® H2SO4 We can predict the products if there are two elements.
Mg + N2 ®
Mg3N2
Decomposition Reactionsdecompose = fall apart, Falls apart into its elementsMade up of only two elementsone compound (reactant) falls apart into two or more elements or compounds.Usually requires energy
AB ® A + B
NaCl ® Na + Cl2
CaCO3 ® CaO + CO2
Single Replacement
One element replaces anotherReactants must be an element and a compound.Products will be a different element and a different compound.
A + BC ® AC + B 2Na + SrCl2 ® Sr + 2NaCl
F2 + LiCl ® LiF + Cl2
Double Replacement
Two things replace each other.Usually in water solution
AB + CD ® AD + CB
AgNO3 + NaCl ® AgCl + NaNO3
ZnS + 2HCl ® ZnCl + H2S
How to recognize which typeLook at the reactants
Element(E), Compound(C)
E + E CE + CC + C
Synthesis
Decomposition
Single replacement
Double replacement
Examples
Synthesis
Decomposition
DecompositionSingle replacement
Single replacement
Double replacement
Double replacement
H2 + O2 ®
H2O ® AgNO3 + NaCl ®
Zn + H2SO4 ® HgO ®
KBr +Cl2 ®
Mg(OH)2 + H2SO3 ®
Examples
Decomposition
Single replacement
Synthesis
Single replacement
Double replacement
CaPO4 ®
AgBr + Cl2 ®
Zn + O2 ®
HgO + Pb®
Cu(OH)2 + KClO3 ®
Identifying Chemical Reactions
_____ P + O2 → P4O10
____ Mg + O2 → MgO
____ HgO → Hg + O2
____ Al2O3 → Al + O2
____ Cl2 + NaBr → NaCl + Br2
____ H2 + N2 → NH3
S = Synthesis D = Decomposition SR = Single Replacement DR = Double Replacement
____ Na + Br2 → NaBr
____ CuCl2 + H2S → CuS + HCl
____ HgO + Cl2 → HgCl + O2
____ C + H2 → CH4
____ KClO3 → KCl + O2
____ S8 + F2 → SF6
____ BaCl2 + Na2 SO4 → NaCl + BaSO4
Chemical Reactions Review…1. Is the process where physical and
chemical properties of the original substance change into a new substance with different physical and chemical properties If there is no new substance there has
been no reactionReactants enter into the reactionProducts are produced by the reaction
Chemical Reactions Review…2. Chemical equations describe
chemical reactions using symbols and numbers.
2Na + SrCl2 ® Sr + 2NaCla) Coefficients (in red)
The large numbers in front of chemical formulas.
The number of molecules of the substance in the reaction
Chemical Reactions Review…2. Chemical equations describe
chemical reactions using symbols and numbers.
2Na + SrCl2 ® Sr + 2NaClb) Subscripts (in Green)
The small numbers to the lower right of chemical symbols
Represent the number of atoms of each element is in the molecule
Chemical Reactions Review…3. Atoms can neither be created nor
destroyed during a chemical reaction…Mass MUST remain constant
You have to end up with the same number of atoms you started with, but in a different arrangement
So balanced equations have the same number of atoms on each side of the YIELDS “®“ sign
Law of Conservation of Mass
Balancing Chemical Equations
(ALWAYS USE PENCIL)1. Check for DIATOMIC molecules H2 , N2 , O2 , F2 , Cl2 , Br2 , I2 , and At2
You cannot change the subscripts of these elements in an equation… whenever they are by themselves, these must be written with the subscript 2.
Balancing Chemical Equations
2. Count the number of atoms on each side of the reaction:
___Na + ___MgCl2 ® ___Mg + ___NaCl
Sodium=____ ® Sodium=____
Magnesium=____ ® Magnesium
=____ Chlorine=____ ®
Chlorine=____
1
1
2
1
1
1
Balancing Chemical Equations
2. Balance the metals first then the nonmetals
___Na + ___MgCl2 ® ___Mg + ___NaCl
Sodium=____ ® Sodium=____
Magnesium=____ ® Magnesium
=____ Chlorine=____ ®
Chlorine=____
1
1
2
1
1
1X 2
2
X 2
2
X 2
Balancing Chemical Equations
3. If they are in your equation, balance OXYGEN
then HYDROGEN last4. Recount all atoms and check your work!
Work from the bottom to top until you find any error.
5. If every coefficient will reduce, rewrite in the simplest whole number ratio
Balancing Chemical EquationsLets try an easy one:
___H2 + ___O2 ® ___H2O
Hydrogen=____ ® Hydrogen=____
Oxygen=____ ® Oxygen =____
2
2
2
1X 2
2
X 4
2
X 4
Balancing Chemical EquationsLets try one more:
___Na + ___HCl ® ___H2 + ___NaCl
Sodium=____ ® Sodium =____
Hydrogen=____ ® Hydrogen=____
Chlorine=____ ® Chlorine =____
1
1
1
1
2
1
X 2
2
X 2 X 2
2
X 2X 2
2
Balancing Act
1. ___Mg + ___O2 ® ___MgO
2. ___Ca + ___O2 ® ___CaO
3. ___H2O2 ® ___H2O + ___O2
4. ___N2 + ___H2 ® ___NH3
5. ___Cu2O + ___C ® ___Cu+ ___CO2
• Spontaneous Reactions - Reactions that proceed immediately when two substances are mixed together. Not all reactions proceed spontaneously.
Reaction Energy
• Activation Energy – the amount of energy that is required to start a chemical reaction.
• Once activation energy is reached the reaction continues until you run out of material to react.
Diatomic elements
There are 8 elements that never want to be alone.They form diatomic molecules.H2 , N2 , O2 , F2 , Cl2 , Br2 , I2 , and At2
What is a catalyst?
A substance that can help the reactants in a chemical reaction react with each other fasterSpeeds up a reaction without being changed by the reaction…it does NOT become part of the reaction.Enzymes are biological or protein catalysts.