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Chemical Reactions Physical Science.

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Presentation on theme: "Chemical Reactions Physical Science."— Presentation transcript:

1 Chemical Reactions Physical Science

2 Chemical Reactions When 2 or more elements chemically combine to form a “new” substance

3 Chemical Equation Is a representation of a chemical reaction Two Parts
Reactants Products

4 The arrow () divides an equation in half
Reactants vs Products C + O2  CO2 The arrow () divides an equation in half Reactants The substance(s) that undergo the change All things on the left side of the “” Ex: C & O2 Products The new substance(s) that form All things on the right side of the “” Ex: CO2

5 Id the Reactants and Products
2Cu + O2  2CuO 2KClO3  2KCl + 3O2 HCl + NaOH  NaCl + H2O N2H4 + O2  N2 + 2H2O

6 Endothermic vs Exothermic
Reaction absorbs energy from its surrounding Surrounding becomes cooler Exothermic Reaction releases energy to the surrounding Surrounding becomes warmer

7 Signs of a Reaction Production of a GAS Formation of a Precipitate
Fizzing, bubbling Formation of a Precipitate Insoluble solid Energy is released EX: Light, heat Color Change

8 Counting Atoms Number in front is called a coefficient
Coefficients are multiplied to all elements behind it Subscripts go to what they follow

9 Counting Atoms Practice
Mg(OH)2 3Ca(NO3)2 NH4OH

10 End of Day One

11 How Do I Balance an Equation?
ID the elements present Count the amount of atoms on both sides of the “” for each element Place coefficients in front of compounds and multiply to any subscript Recount the atoms on both sides of the “” to see if they are equal. If not equal, adjust the coefficients LEFT has to equal RIGHT

12 ____Cu + ____O2  ____CuO
Balancing Practice #1 ____Cu + ____O2  ____CuO

13 ____N2H4 + ____O2  ____N2 + ____H2O
Balancing Practice #2 ____N2H4 + ____O2  ____N2 + ____H2O

14 ____KClO3  ____KCl + ____O2
Balancing Practice #3 ____KClO3  ____KCl + ____O2

15 Choose the Balanced Equation
KClO2  KCl + 2O2 4Al + 3O2  2Al2O3 N2 + 3H2  2NH3 H2 + O2  H2O 2NaCl  2Na + Cl2

16 Why Balance? The Law of Conservation of Matter
Matter is neither created nor destroyed Start = Finish

17 End of Day Two

18 Types of Reactions 4 Main Types 2 Special Types Synthesis
Decomposition Single Replacement Double Replacement 2 Special Types Combustion Reaction Neutralization Reaction

19 Synthesis Reaction A + B  AB
When 2 or more substances react to form a single substance 21 Dating: Becoming a Couple

20 Decomposition Reaction AB  A + B
When a compound breaks down into two or more substances 12 Dating: Breaking Up

21 Single Replacement Reaction A + BC  B + AC
A reaction in which one element trades places with another element in a compound Element and Compound Dating: CHEATING

22 Double Replacement Reaction AB + CD  AD + BD
Where two different compounds exchange positive ions (cations) to form two new compounds All compounds (4 of them) Dating: Swingers

23 Type Of Reaction Practice
Na3PO4 + 3KOH  3NaOH + K3PO4 P4 + 3O2  2P2O3 Pb + FeSO4  PbSO4 + Fe CaCO3  CaO + CO2

24 Special Reaction: Combustion Reaction
When a hydrocarbon (hydrogen and carbon together) reacts with Oxygen Products are always CO2 & H2O Ex: CH4 + 2O2  CO2 + H2O

25 End of Unit!


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