1. Bellringer:4/9/2018
In your bellringer notebook count how many atoms are in the following compounds:
H2SO4 b) KClO3 c) NH3 d) O2
STOTD
**QUIZ on Thursday: Balancing Equations & Types of Chemical Reactions
**Lab on FRIDAY

2. Chemical Reactions
Chapter 7

3. Chemical Reactions Chemical Reaction Evidence of a Chemical Reaction
Process that rearranges atoms into different substances
Evidence of a Chemical Reaction
Temperature change
Production of light
Color change
Production of gas
Creation of a precipitate (solid)
end

4. Chemical Equations Chemical Equations
There are 2 parts in a chemical equation:
Reactants
To the Left of the arrow
Products
To the Right of the arrow
The state of matter is shown with an:
(s), (l), (g), (aq)
aq- aqueous (dissolved in water)
2 H2(g) + O2(g) 
2 H2O(l)
Yields/Forms/Produces
end

5. Chemical Equations
Put a box around the reactants, and underline the products
2 H2 + O2  2 H2O
Zn + H2SO4  ZnSO4 + H2
2 HgO  2 Hg + O2
end

6. Chemical Equations The Law of Conservation of Matter
Matter cannot be created or destroyed!
Every atom at the start of a reaction, must be at the end!
To account for every atom you must balance the equation
end

7. Chemical Equations NEVER Change the Subscripts
Steps to balancing chemical equations:
Write the chemical equation
List the elements on each side of the equation
Place coefficients in front of each formula
Distribute (multiply) the element by the coefficient
Balance 1 element at a time!
If you need part of an atom, multiply everything by 2
Double check your work!!!
NEVER Change the Subscripts
end

8. Chemical Equations Lets practice: ___ N2 + ___ H2  ___ NH3
___ KClO3  ___ KCl + ___ O2
___ NaCl + ___ F2  ___ NaF + ___ Cl2
___ CH4 + ___ O2  ___ CO2 + ___ H2O
___ P + ___ O2  ___ P2O5
end

9. Chemical Equations Practice! Balance the following
___ Na + ___ I2  ___ NaI
___ N2 + ___ O2  ___ N2O
___ KI + ___ Cl2  ___ KCl + ___I2
___ N2 + ___ H2  ___ NH3

10. Chemical Equations Word Equations
Names are written out instead of the formulas.
To solve:
Box the Reactants and Underline the Products
Write the formula of each reactant and product
Don’t forget to separate:
Each formula with a “+”
The reactants and products with an “”
end

11. Chemical Equations Write and balance the following equations:
Potassium oxide combines with water to make potassium hydroxide
Aluminum plus oxygen gas forms aluminum oxide
Nitrogen gas plus oxygen gas react and form dinitrogen pentoxide
end

12. Chemical Equations Practice: Hydrogen plus oxygen yield water
Nitrogen plus hydrogen yield ammonium
Aluminum bromide plus chlorine yield aluminum chloride and bromine

13. Bellringer: 4/10/2018 Balance the following chemical equations:
___ NaBr + ___ Ca(OH)2  ___ CaBr2 + ___NaOH
___ Na + ___ I2  ___ NaI
Safety Tip of the Day

14. Chemical Reactions There are 5 basic chemical reactions: Synthesis
Decomposition
Single Replacement
Double Replacement
Combustion
end

15. Chemical Reactions Synthesis A + B  AB 2 Ca + O2  2 CaO
2 or more reactants combine to form 1 product
A + B  AB
2 Ca + O2  2 CaO
end

16. Chemical Reactions Decomposition AB  A + B NH4NO3  N2O + 2 H2O
1 reactants breaks down into 2 or more products
AB  A + B
NH4NO3  N2O + 2 H2O
CuCl2  Cu + Cl2
end

17. Chemical Reactions Single Replacement A + BC  AC + B
1 element replaces another element in a compound
A + BC  AC + B
Cu + 2 AgNO3  2 Ag + Cu(NO3)2
3 Mg + 2 AlCl3  2 Al + 3 MgCl2
end

18. Chemical Reactions Double Replacement AB + CD  AD + CB
The reactants switch partners
AB + CD  AD + CB
These reactions often produce water, a gas , or a solid
NaOH + HCl  NaCl + H2O
LiI + AgNO3  AgI + LiNO3
end

19. Chemical Reactions Combustion CH4 + 2 O2  CO2 + 2 H2O
Oxygen combines with a compound to give off heat and light
Forms CO2(g) and H2O(l)
CH4 + 2 O2  CO2 + 2 H2O
end

20. Chemical Reaction Classify the following: 2 H2 + O2  2 H2O
Zn + H2SO4  ZnSO4 + H2
2 HgO  2 Hg + O2
AgNO3 + NaCl  AgCl + NaNO3
2 C2H6 + 7 O2  4 CO2 + 6 H2O
end

21. Bellringer: 4/11/2018
What are the 5 basic chemical reactions and their general equations?
Classify the following:
SO3 + H2O  H2SO4
CaCl2 + F2  CaF2 + Cl2
2 NaCl  2 Na + Cl2
3. Safety Tip of the Day

22. Bellringer: How do you know if a reaction is endothermic?
How do you know if a reaction is exothermic?
Provide an example of an exothermic chemical reaction.
STOTD

23. Energy Changes Chemical Energy Energy stored in chemical bonds
2 Types:
Exothermic
Endothermic
end

24. Energy Changes Exothermic Reaction AB + CD  AD + CB + energy
gives off energy
produces heat and/or light
ex) burning paper, Instant heating pad, glow sticks
energy given off will be written as a product
AB + CD  AD + CB + energy
Na + Cl2  NaCl + 411kJ
Energy measured in kilojoules
end

25. Energy Changes In an exothermic reaction:
Reactants have more energy than the products
end

26. Energy Changes Endothermic Reaction AB + CD + energy  AD + CB
Absorbs energy
Surroundings get colder
Ex) Instant icepacks
energy taken in will be written as a reactant
AB + CD + energy  AD + CB
15000 kJ + 6 CO2 + H2O  C6H12O6 + 6 O2
Energy measured in kilojoules
end

27. Energy Changes In an endothermic reaction:
Reactants are lower in energy than products
end

28. Activity With a partner:
In your notes write the question, “How can you make a chemical reaction go faster?”
With your partner brainstorm answers to the question and write them down.
Be prepared to share your answers

29. Reaction Rates Reaction Rate How fast the reactants change to products
There are 5 ways to make a reaction go faster:
Temperature
Surface Area
Stirring
Concentration
Catalysts
end

30. Reaction Rates 1. Temperature Adding heat makes molecules move faster
Move Faster = Faster Reaction
2. Surface Area
Grind up a substance into a powder
More Surface Area = Faster Reaction
3. Stirring
Stirring makes things move around
More Movement = Faster Reaction
4. Concentration
Adding more reactants makes it easier for them to combine
More Reactants = Faster Reaction
end

31. Reaction Rates Catalyst
Speeds up a reaction without being used in the reaction
Lowers the amount of energy needed to get the reaction started (the size of the hill)
Less Energy Needed = Faster Reaction
end

32. Energy Changes
end