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## Q4 – Week  – 5/16 – 5/20

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5/16 – Monday –   A Day

Reminders:

1. Contact – email: grodskib@whbschools.org

Main Goal

1.  Complete the double replacement lab.

2.  Begin the Energy Unit 2, potential energy curves

potential energy curves worksheet.pdf

potential energy curves worksheet key.pdf

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5/17 – Tuesday – B Day

Reminders:

1. Contact – email: grodskib@whbschools.org

Main Goal

1.  Begin the Energy Unit 2, potential energy curves, enthalpy

2. effect of a Catalyst

3. factors that affect the rate of a reaction – effective collisions.

An effective collision is a physical collision between reacting elements, compounds, or ions that results in the breaking of old bonds and the formation of new ones.

An effective collision requires 2 conditions:

1.  High enough kinetic energy to overcome the repulsive forces of the
cloud of electrons all chemical species have on their outside.
– if the reactants are not free atoms then some energy is needed to be consumed to
break the bonds.

2.  Correct orientation of the reacting chemicals.  Larger molecules especially
have areas where chemical reactions can and cannot occur.  Thus the
collisions of the reacting particles can occur at certain positions allowed
by the second law of thermodynamic.

Kinetic Energy factor:
Orientation Factor:

When Effective collision are increased then the rate at which the chemical reactions occur also increases.
Now in general or statistically, if we increase the frequency of collisions, we will increase the number of effective collisions.  The factors that will increase the frequency of collisions include:

1.  Temperature – particle motion (velocity) is proportional to temperature:

Average Speed (velocity)    =    urms = √3RT/M

The faster reactants move the higher the frequency of collisions.

2.  Pressure – If a reactant is a gas then increasing its partial pressure or decreasing its volume of the                                   reactant container will increase the frequency of the collisions.

3. Catalyst –  Catalysts will provide a new reaction mechanism that will have a Net lower Ea (activation
energy)  or will help with the orientation like biological enzymes or metal catalysts.
Catalysts lowers the energy requirement to start reactions and thus makes the frequency                                 of effective collisions increases with increasing the the overall frequency of collisions.                                   It increases the percentage of effectiveness of total collisions.

Elephants toothpaste demo: https://youtu.be/8ZnNSTzl1lc

4.  Surface area –  powdered forms of reactants will increase the frequency of collisions more than reactants
in solid lumps because more reactants are exposed to collisions.

Elevator Explosion demohttps://youtu.be/u3CixGBlBN0
dragons breath demo: https://youtu.be/WLcEFWTXWpk

5.   Concentrations   The amount of available reacting particle. will affect the frequency of collisions.

5/17 – Homework/Classwork:

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5/18 – Wednesday – A Day

Main Goal

1. To identify the factors that affect the rate of a reaction.

Effective Collisions –  1. Enough Ke

2. Proper Orientation

5/18  – Homework/Classwork:

1.  None

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5/19 – Thursday – B Day

Main Goal

1. To complete the review of all the factors that affect rate of reaction.

2. To complete a review worksheet on the kinetics concept.

Surface area demo-

Surface area demo-

5/19  – Homework/Classwork:

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5/20 – Friday – A Day

Main Goal

Concepts:

1.  Predict the products of a double replacement reaction.

2. Balance a double replacement reaction.

3. Identify the precipitate if any.