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Principles of Chemistry 1 > U4- Module 1: Modeling Chemical Reactions > Flashcards

U4- Module 1: Modeling Chemical Reactions Flashcards

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1
Q

Double Replacement Reaction

A

The anions and cations switch molecules, causing two new compounds to be formed.

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2
Q

Insoluble Precipiate

A

A compound formed in a double replacement reaction, that either does not follow charge rules or is stated as insoluble on the guideline sheet.

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3
Q

What are the 4 signature features of chemical reactions?

A
  1. Chemical reactions involve reactants and products.
  2. Chemical processes always have some transfer of energy going on.
  3. Chemical reactions occur at varying speeds.
  4. Chemical reactions can include both reactants and products in the final state of the reaction.
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4
Q

Reactants

A

The initial substances in a chemical process that react with each other.

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5
Q

Products

A

The new substances created in a reaction from the reactants.

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6
Q

What are two examples of energy exchange in a chemical reaction?

A

Endothermic and Exothermic

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7
Q

What would a reaction that is endothermic look like?

A

The glass would feel cold because the energy is being absorbed.

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8
Q

What would a reaction that is exothermic look like?

A

The glass would feel warm because the energy is being released.

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9
Q

What are the 6 assumptions of chemical reactions?

A
  1. Particles with different composition and structures are formed due to atoms of the reactants being rearranged.
  2. The rearrangements of atoms can produce changes in the potential energy.
  3. For a chemical reaction to occur, reactants must collide.
  4. For a chemical reaction to occur, particles must be oriented in a specific way that allows the reactants to interact correctly.
  5. For a chemical reaction to occur, colliding particles must have enough energy to reach a transition state that leads to the formation of products.
  6. As reactants interact to form products, particles of the products can interact and create more reactants until the chemical interaction is at an equilibrium.
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10
Q

Chemical reactions

A

Processes in which the atoms that make up the reactants are rearranged
- conversion of reactants to products

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11
Q

How do you correctly label the two sides of a reaction?

A

“Start of reaction” and “End of reaction”

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12
Q

What is true about the numbers of each atoms and the mass of the reaction?

A

They are conserved by being kept in the same container throughout the entire reaction.

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13
Q

Stoichiometric Coefficients

A

The number in front of a molecule in the chemical formula that shows how much of the molecule is in the reaction.

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14
Q

Excess Molecule

A

Reactants that did not react and ended up in the product side of the equation

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15
Q

Is the excess molecule apart of the chemical equation?

A

No
- Subtract from the reactant side to determine that there is no excess molecules in the reaction

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16
Q

What should you always make sure you do when writing the chemical formula?

A

Write it in the lowest ratio
(divide by common factors)

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17
Q

Limiting Reactant

A

The reactant that is used up first and limits the amount of excess reactant that can be used.

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18
Q

What does the limiting reactant determine?

A

The maximum amount of products.

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19
Q

Chemical Changes

A

The generation of new substances from existing substances

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20
Q

Chemical Equation

A

Represent the proportions of reactants to products

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21
Q

What is the limiting reactant used to calculate?

A

The theoretical yield of reactions

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22
Q

Combustion Reaction

A

Forms CO2 as a product

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23
Q

What does an incomplete combustion reaction form?

A

CO

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24
Q

What happens to the energy in an exothermic reaction?

A

Energy is released

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25
Is an exothermic reaction a heat or cool pack?
Heat pack - energy given off
26
What happens to the energy in an endothermic reaction?
Energy is absorbed/taken in
27
Is an endothermic reaction a heat or cool pack?
Cool pack
28
Where is heat placed in the chemical equation of an exothermic reaction?
Product side
29
Where is heat placed in the chemical equation of an endothermic reaction?
Reactant side
30
How do you draw the PEC diagram for an exothermic reaction?
The mixed state has to have a lower potential energy level than the UM state. -give off energy
31
How do you draw the PEC diagram for an endothermic reaction?
The mixed state has to have a higher potential energy level than the UM state. -take in energy
32
Are bonds stronger on the reactant or product side of an exothermic reaction?
product side
33
Are bonds stronger on the reactant or product side of an endothermic reaction?
reactant side - need to add energy to overcome bonds
34
When energy is needed for a reaction to occur, it energy a reactant or product?
Reactant
35
When asked for the molecules used in the reaction, what should you include?
The true ratio of the reactants in the balanced equation (do not simplify) - Do not include the excess reactants.
36
When asked for the molecules at the start of the reaction, what should you include?
The true ratio of the reactants in the balanced equation (do not simplify) - Include the excess reactants
37
What is the relationship between number of collisions and chemical process speed?
The more collisions in a given time, the faster the process.
38
What variables can be changed to control collision frequency?
- Temperature - Pressure - Volume - Number of reactant particles
39
Which way can you alter these variables to increase the reaction rate? - Temperature - Pressure - Volume - Number of reactant particles
- Increase the temperature; speeds up particles. - Increase the pressure; correlated to volume. - Decrease the volume; smaller space for particles to avoid each other. - Increase number of reactant particles; more chances for collisions to occur.
40
How is the configuration effectiveness in a complicated molecule?
Complicated molecules have lower effectiveness due to it being harder for the molecule to correctly interact with the right portion of another molecule.
41
What is the relationship between % of configurations and reaction speed?
The higher % of effective configurations leads to a faster reaction process.
42
Summarize the 2 general rules for reaction speed.
1. The fewer number of gas particles in the reactants and 2. The simpler the composition and structure is of reactants = Faster reaction process.
43
What must happen for a chemical reaction between A and B?
A and B must collide
44
Activation Energy
The initial energy that needs to be supplied to allow the reacting particles to transition into products.
45
Transition State
The unstable state of energy that represents the point in transformation between reactants and products.
46
Net Energy Change
The energy difference between the reactants and products
47
Catalysts
Additives to chemical reactions that can speed up the process by lowering the activation energy.
48
What do catalysts not do?
1. Change the energy of the reaction 2. Be consumed during the reaction (not a reactant)
49
How do you determine which reaction is more favored by collision effectiveness?
The reaction that either has fewer gas particles reacting or simpler molecules.
50
How do you determine which reaction is more favored by activation energy?
The one that has the smaller Ea value in the graph.
51
How do you determine which reaction is faster?
The one with less gas particles/simpler molecules and lower activation energy.
52
Which reaction is faster when all variables are the same between them?
They are the same reaction rate.
53
What are the 3 factors that influence reaction rate?
1. Collision Frequency 2. Configuration Effectivness - less gas particles 3. Activation energy - lower is better
54
What does a higher temperature do?
Increase the number of particles that have enough energy to react. - Higher reaction rate
55
What must be available to form the transition state between two particles?
Activation Energy
56
How is the final state of a chemical system determined?
The balance between the forward and backward reaction rate.
57
What symbolizes a chemical equilibrium?
The forward and backwards arrow
58
Product favored reaction
The forward reaction rate is faster/stronger than the backwards reaction rate - more products than reactants
59
Reactant Favored Reaction
The backwards reaction rate is stronger/faster than the forward reaction rate - More reactants than products
60
What does the graph between forward reaction and backward reaction look like in a product favored reaction?
The rate of the forward line starts at the top, but the backwards line switches spot with it once there are more products.
61
What does the graph between forward reaction and backward reaction look like in a reactant favored reaction?
The line of the forward reaction starts above the backward line but the two even out in the middle (do not switch spots)
62
What is an example of a reactant favored equilibrium?
Weak acids
63
What indicates that a reaction goes to completion?
Single forward arrow
64
What indicates a reaction that is at equilibrium?
Double facing arrow
65
What does it mean when a reaction is at equilibrium?
The rate of the forward and reverse reactants are equal - does not mean that there is the same number of reactants and products.
66
What happens when the number of effective configurations and activation energy support different sides of the reaction?
The reaction is conditional and temperature plays a role in differentiating them.
67
What are the 4 types of reaction favors?
- Reactant favored - Product favored Conditional: - Product favored at low temperature - Product favored at high temperature
68
What are acids classified by?
The extent of their dissociation in the reaction
69
Strong Acids
Fully dissociate in water to generate H3O+ = 100% product
70
How is an acid strong?
When it has enough energy advantage to force all H+ ions of the acid into the solvent H2O to form H3O+
71
What is this equation an example of? HCl + H2O -> H3O+ + Cl-
Strong acid - forward facing arrow indicates only products are leftover
72
Weak Acids
Acids that partially dissociate in water to generate H3O+ = <100% product
73
What is this equation an example of? HF + H2O <-/-> H3O+ + F
Weak acid - forward and backwards arrow indicates the acid did not fully dissociate into ions
74
What does the graph of a strong acid look like?
The line of reactants starts at the top and the line of products start at the bottom. Due to fully dissociating, the two switch positions and end up leveling out, with the products now on the top.
75
What does the graph of a weak acid look like?
The reactant line starts at the top and the product line starts at the bottom. Based on how much the acid dissociates, the lines will slowly dip down/up, but even out to a straight line immediately.
76
What type of acid is more ionized and why?
Strong Acids - Fully dissociate into ions.
77
What do chemical processes usually lead to?
A net transfer of energy between a system and its surroundings
78
What are usually indications of chemical change?
- Color change - Precipitates - Bubbles - Temperature change
79
Why do chemical reactions occur at fixed ratios?
Mass is conserved throughout the reaction

Principles of Chemistry 1 (16 decks)

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