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FINAL Flashcards

1
Q

What is a combination reaction?

A

Is a reaction in which two or more substances combine to form a single new substance Example: A+B→AB

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2
Q

What is a decomposition reaction?

A

A reaction in which a compound breaks down into two or more simpler substances. Example: AB→A+B

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3
Q

What is a displacement reaction?

A

Where an atom or a set of atoms are displaced by another atom in a molecule. Example: A + B-C → A-C + B

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4
Q

What is an exchange reaction?

A

It is where the elements that were partners on one side are then interchanged and switch partners on the other side. Example: AgNO3 + NaCl → AgCl + NaNO3

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5
Q

What is a combustion reaction?

A

a reaction in which a substance reacts with oxygen, releasing energy in the form of light and heat.

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6
Q

Identify the category of the following reaction.

4HNO3 → 4NO2 + 2H2O + O2
a.Combination reaction
b.Decomposition reaction
c.Single-replacement reaction
d.Double-replacement reaction

A

b. Decomposition reaction

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7
Q

What is a redox reaction?

A

A reaction that involves a transfer of electrons from one reactant to another

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8
Q

What is a nonredox reaction?

A

A reaction where there are no transfer of electrons from one reactant to another

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9
Q

What is the difference between oxidation and reduction in a redox reaction?

A

Oxidation: A reactant loses one or more electrons
Reduction: A reactant gains one or more electrons

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10
Q

What is an oxidizing agent and what is a reducing agent in redox reactions?

A

Oxidizing agent: the substance that gained electrons
Reducing agent : the substance that lost electrons

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11
Q

What is the molecular collision theory?

A

It is a theory that all molecules, ions, or atoms must come into contact (collide) with one another for any chemical change to occur

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12
Q

What is activation energy?

A

The combined kinetic energy that occurs when particles collide that they must have in order for their collision to be a chemical reaction

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13
Q

What is collision orientation?

A

It is where molecules or atoms or ions must collide in a certain way in order to successfully to get a product. If not then no product is produced

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14
Q

What are the three factors necessary for a
chemical reaction to occur?
a.Proper temperature, pressure, and concentration
b.Proper temperature, pressure, and low activation energy
c.Proper temperature, low activation energy, and proper
orientation of colliding particles
d. Molecular collisions, low activation energy, and proper
orientation of particles

A

d. Molecular collisions, low activation energy, and proper
orientation of particles

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15
Q

How can you tell the difference between exothermic chemical reactions and endothermic chemical reactions?

A

Exothermic chemical reactions: Energy is released as a product, and products are more stable than reactants

Endothermic chemical reactions: Input of energy is needed for the reaction to occur. Energy is the reactant. Additional energy must be put in so the reaction process can happen. Products are less stable than reactants

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16
Q

What are some examples of exothermic chemical reactions, and endothermic chemical reactions?

A

Exothermic chemical reactions: Burning fuel

Endothermic chemical reactions: Photosynthesis of plants

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17
Q

Which of the following statement(s) is(are) correct?
a.During an exothermic reaction, the average energy of the products is
higher than the average energy of the reactants.
b.During an endothermic reaction, the average energy of the products
is lower than the average energy of the reactants.
c.During an exothermic reaction, the average energy of the products is lower than the average energy of the reactants.
d.Both (a) and (b)

A

c.During an exothermic reaction, the average energy of the products is lower than the average energy of the reactants.

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18
Q

How does the reactant concentration affect the reaction rate?

A

When you increase the concentration of the reactant it increases the reaction rate. this is because it creates more molecules and when you have more molecules more collisions occur

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19
Q

What is physical nature of reactants?

A

It is where the physical state of a reactant and the particle size affects the reaction rate

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20
Q

Between the physical states of matter. Which ones make the reaction rate go slow? and what make the reaction rate go fast?

A
  1. The slowest are between solids
  2. The next fastest are between liquids
  3. And the fastest are between gasses
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21
Q

How does temperature affect the reaction rate?

A

As the temperature rises the reactant rate increases. This is because the molecules gain more speed and cause more collisions

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22
Q

How does the presence of catalysts affect the reaction rate?

A

It increases the reaction rates by providing different pathways that have lower activation energies

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23
Q

What are the catalysts called in human bodies?

A

Enzymes

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24
Q

What is the function of a catalyst in a chemical
reaction?
a.It increases the rate of the reaction by increasing the activation
energy.
b.It increases the rate of the reaction by decreasing the activation
energy.
c.It decreases the rate of the reaction by increasing the activation
energy.
d.It decreases the rate of the reaction by decreasing the activation
energy.

A

b.It increases the rate of the reaction by decreasing the activation
energy.

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25
What is a oxidizing agent?
The element that gains electrons and helps the other element lose electrons
26
What is a reducing agent?
The element that loses electrons and helps the other element gain electrons
27
What is the reversible chemical reaction?
Where the reactions form the products and simultaneously the products form the reactants
28
What is chemical equilibrium?
Where forward and reverse chemical reactions go at the same rate. The concentrations of the reactants and products no longer change
29
What do the brackets mean in the equilibrium constant expression?
The molar concentration
30
Where do the products ALWAYS GO in the equilibrium constant expression?
On top as the numerator
31
Where do the reactants ALWAYS GO in the equilibrium constant expression?
On bottom as the denominator
32
If Keq is greater than 1 are there more products or reactants?
More products
33
If Keq is Less than 1 are there more products or reactants?
More reactants
34
If more products are produced than reactants, which way does the equilibrium shift?
To the right
35
If more reactants are produced than products, which way does the equilibrium shift?
To the left
36
What is the Le Châtelier’s Principle?
If a stress is applied to a system at equilibrium the system will readjust in the direction that best reduces the stress on the system (Left or Right).
37
What type of things change Keq And what things don't change Keq?
Things that change Keq: Temperature Things that Don't change Keq: * Reactant or product concentration * Pressure (only gas reactions) * Catalysts (including enzymes!)
38
What is the concentration of change in the equilibrium system?
If the concentration of a substance is increased, the reaction that consumes that substance is favored, and the equilibrium shifts away from that substance
39
What is the pressure of change in the equilibrium system?
increasing the pressure shifts the equilibrium toward the side with fewer moles of gas. Decreasing the pressure shifts the equilibrium towards the side with greater number of moles.
40
What is the addition of catalysts in the equilibrium system?
It just speeds up the process as a whole and no shifting happens
41
What is an Arrhenius acid?
Hydrogen-containing compound that produces H+ ions in solution
42
What is an Arrhenius base?
Hydroxide-containing compound that produces OH– ions in solution
43
What kind of compound does Ionization use?
Molecular compound
44
What kind of compound does dissociation use?
Ionic compound
45
What is ionization?
Is which individual positive and negative ions are produced from a molecular compound that is dissolved in a solution
46
What is dissociation?
Is which individual positive and negative ions are released from an ionic compound (a metal and a nonmetal) that is dissolved in a solution
47
What is a Bronsted-Lowry acid classified as?
A proton donor
48
What is a Bronsted-Lowry base classified as?
A proton acceptor
49
How can you tell apart the acid and the base in an acid base pair?
Acid- The acid in the acid-base pair will always have one fewer negative charges (or electrons) than the base Base- The base in the acid-base pair will always have one more negative charge (or electron) than the acid
50
What is an amphiprotic substance?
A substance that can either lose or accept a proton so it can be either a Bronsted-Lowry acid or a Bronsted-Lowry base Ex: Water
51
What is a monoprotic acid?
Is an acid that supplies one proton (H+ ion) per molecule during an acid-base reaction
52
What is a Diprotic acid?
Is an acid that supplies two protons (H+ ion) per molecule during an acid-base reaction
53
What is a Triprotic acid?
Is an acid that supplies three protons (H+ ion) per molecule during an acid-base reaction
54
What is a Polyprotic acid?
Is an acid that supplies two or more protons (H+ ion) per molecule during an acid-base reaction (this include the diprotic acid and triprotic acid)
55
If polar bonds are greater between the two atoms in an acid. Is the acid stronger or weaker?
The acid is stronger. Stronger the polar bond = Stronger the acid
56
What does the acid compound H-X produce?
It is broken to form H+ and X- ions
57
What are some examples of acidic protons?
O-H, F-H, N-H, S-H
58
What are some examples of non acidic protons?
C-H
59
What are the three central concepts associated with the collision theory?
Molecular collisions, Low activation energy, and collision orientation
60
How do you identify the acidic hydrogen in a formula?
It is the hydrogen that is first or last in the formula
61
What is the difference between a strong acid and a weak acid?
Strong Acid: Equilibrium will be far to the right and will completely break apart and want to share its protons Weak Acid: Equilibrium will be far to the left and does not want to share share its protons
62
What is the difference between a strong base and a weak base?
Strong Base: Equilibrium will be far to the right and will dissociate completely Weak Base: Equilibrium will be far to the left and it will NOT dissociate completely
63
What is a salt in chemistry terms?
It is a positive ion and a negative ion EXCEPT the negative ion cannot be OH-
64
How do you make a salt?
React an Acid with a Base
65
What is self ionization?
It is where water reacts with each other to make a different ion
66
What is the acid ionization constant?
It is a fraction that has the products as the numerator and the reactants as the denominator BUT YOU DO NOT PUT THE WATER INTO THE EQUATION EXAMPLE: HA + H2O ........ H3O+ + A- Ka = (H3O+) (A-)/(HA)
67
What is the base ionization constant?
It is a fraction that has the products as the numerator and the reactants as the denominator
68
What does it mean when the Ka value in the acid ionization constant is high?
It means that it is a strong acid
69
What does it mean when the Ka value in the acid ionization constant is low?
It means it is a weak acid
70
What does it mean when the Kb value in the base ionization constant is high?
It means it is a strong base
71
What does it mean when the Kb value in the base ionization constant is Low?
It means it is a weak base
72
How can you tell if the product is a salt or not?
if it does not have an H+ proton or OH- in the molecule
73
What does H3O+, and OH- equal when added together in the Ion Product Constant of Water?
1.00 X 10 -14 M
74
What does H3O+ equal in the Ion Product Constant of Water?
1.00 X 10 -7M
75
What does OH- equal when in the Ion Product Constant of Water?
1.00 X 10 -7M
76
If H3O+ is greater than OH- in the ion product constant of water, What solution will it be?
An acidic solution
77
If OH- is greater than H3O+ in the ion product constant of water, What solution will it be?
A basic solution
78
What do H3O+, and OH- have to equal in the Ion Product Constant of Water?
1.00 X 10 -14 M
79
If OH- and H3O+ are the same in the ion product constant of water, What solution will it be?
Neutral (10 to the negative 7)
80
What is the PH equation for H3O+ and OH-?
H3O+ = -log(H3O+) OH- = -log(H+)
81
How do you solve -log(H3O+)?
Just plug in the number that H3O+ equals into the calculator and you are all good to go
82
How do you solve -log(H+)?
You find the number that equals OH-. Then you plug that number into the equation that you use for the ion product constant of water for OH- (Kw = [H3O+][OH–] = 1.00 × 10–14 M). Then after you get that answer you plug it into the -log(H3O+) equation into the calculator and the answer that you get into the calculator is correct
83
If the PH levels are at a 7 for a substance. Than what is the substance classified as? (neutral, acidic, or basic)
Neutral
84
If the PH levels are higher than a 7 for a substance. Than what is the substance classified as? (neutral, acidic, or basic)
Basic
85
If the PH levels are lower than a 7 for a substance. Than what is the substance classified as? (neutral, acidic, or basic)
Acidic
86
How do you solve -log(ka)?
Just plug in the number that Ka equals into the calculator and you are all good to go
87
If pKa is small what does that mean?
It means it is a strong acid. The smaller the pKa the stronger the acid
88
What is a buffer?
It prevents major changes in pH levels
89
What is a buffer composed of?
A weak acid and its conjugate base, or a weak base and its conjugate acid
90
What does the buffer do? Explain
the base in the buffer vacuums up the H+ and the acid in the buffer vacuums up in the OH-.
91
What is the Henderson–Hasselbalch Equation?
The relationship between pKa and pH for buffer solutions.
92
What is an electrolyte in chemistry?
Substance whose aqueous solution conducts electricity
93
What other substances can make electrolytes?
Acids, bases, and soluble salts
94
Why can Acids, bases, and soluble salts make electrolytes?
Because they produce ions
95
What are nonelectrolytes?
Substances that can not conduct electricity
96
What are some examples of nonelectrolytes?
Table sugar (sucrose) and glucose
97
What are strong electrolytes?
They produce ions and completely dissociate to make ions
98
What are some examples of strong electrolytes?
Strong acids, bases, and soluble salts Strong Electrolytes
99
What are weak electrolytes?
They do not completely make themselves into ions they do not completely dissociate
100
What are some examples of weak electrolytes?
Weak acids and bases Weak Electrolytes
101
What is Acid-Base titrations?
It is a neuralization reaction that happens between measured acids and bases
102
What is an Acid-Base Indicator?
A solution that changes colors based on the pH level
103
What does the Henderson-Hasselbalch equation help determine? (pKa)
How strong or weak an acid is
104
If pKa value is low what does that mean is it a strong acid or a weak acid?
It is a strong acid
105
If pKa value is high what does that mean is it a strong acid or a weak acid?
it is a weak acid
106
If Ka value is high what does that mean is it a strong acid or a weak acid?
it is a strong acid
107
If Ka value is low what does that mean is it a strong acid or a weak acid?
it is a weak acid
108
When determining the concentration of an acid or base, a(n) _____ is performed using a(n) _____ to visualize the desired pH of the solution. a) acid–base indicator; acid base titration b) acid–base titration; acid–base indicator c) acid titration; base indicator d) base titration; acid indicator
b) acid–base titration; acid–base indicator
109
25 mL of acid requires 14.8 mL of 0.351 M base for complete neutralization. What is the molarity of the acid and what two products are formed after neutralization? a) 0.208 M; a salt and water b) 4.81 M; a salt and water c) 0.208 M; not enough information is provided to determine the products. d) 4.81 M; not enough information is provided to determine the products. 85Copyright ©2016 Cengage Learning. All Rights Reserved.
a) 0.208 M; a salt and water
110
Calculate the pKa for HF given that the Ka for this acid is 6.8 × 10–4.
3.17 is the final answer
111
Which of the following is the correct mathematical expression for pH? a) pH = –log [H3O+] b) pH = log [H3O+] c) pH = –log [OH–] d) pH = log [OH–]
a) pH = –log [H3O+]
112
Calculate the pH for 0.040 M OH-
Final answer 12.60
113
Calculate the pH for 1.0 x 10-4 M H3O+
Final answer is 4
114
An acidic solution is defined as? a) An aqueous solution in which the concentration of H3O+ ion is lower than that of OH– ion. b) An aqueous solution in which the concentration of H3O+ ion is equal to that of OH– ion. c) An aqueous solution in which the concentration of H3O+ ion is higher than that of OH– ion. d) An aqueous solution in which the concentration of OH– ion is higher than that of H3O+ ion. 50Copyright ©2016 Cengage Learning. All Rights Reserved.
c) An aqueous solution in which the concentration of
115
Calculate [H3O+] or [OH–] as required for each of the following solutions at 24°C. a) 1.0 × 10–4 M OH–
final answer is 1.0 x 10-10
116
Which of the following equations would be a correct representation of a strong acid when placed in water? a. HA + H2O H3O+ + A– b. HA + H2O H3O+ + A– c. HA + H2O H3O+ + A– d. Not enough information is provided. 28Copyright ©2016 Cengage Learning. All Rights Reserved.
b. HA + H2O H3O+ + A–
117
Identify a conjugate acid–base pair in the following equation. HF(aq) + H2O(l) H30+(aq) + F–(aq) a. HF(aq) and H30+(aq) b. HF(aq) and F–(aq) c. H2O(l) and F–(aq) d. HF(aq) and H2O(l)
b. HF(aq) and F–(aq)

Chemistry (4 decks)

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