Chapter 4

Question 1

Amounts of substances in a chemical reaction are considered what?

Answer 1

Reaction Stoichiometry

Question 2

The stoichiometric factor can be used as a mole ratio relating moles of one substance, to ________ of another.

Answer 2

Moles

Question 3

What is the amount of a product that is “theoretically” possible to obtain?

Answer 3

Theoretical yield

Question 4

The amount of a product actually obtained in an experiment is what?

Answer 4

Actual yield

Question 5

You can’t calculate the _________ yield.

Answer 5

Actual

Question 6

What is the percent yield equation?

Answer 6

Actual yield/Theoretical yield x 100

Question 7

The amount of absolute in a solution is given by its _____________.

Answer 7

Concentration

Question 8

What is the molarity equation?

Answer 8

Moles of solute/Liters of solution

Question 9

What equation do we use for dilution?

Answer 9

M(initial) x V(initial) = M(final) x V(final)

Question 10

Reactions of Ionic compounds that take place in water are what?

Answer 10

Aqueous solution

Question 11

How do we know ions are present in aqueous solutions?

Answer 11

The solutions conduct electricity (called electrolytes)

Question 12

HCl, KMnO4, MgCl2, and NaCl are all examples of what?

Answer 12

Strong electrolytes

Question 13

Acetic acid ionizes only to a small extent so it is a _________ electrolyte.

Answer 13

Weak

Question 14

Compounds in the reaction are written as if the cations and anions of the compound are together, even though they may be dissociated as ions is considered what?

Answer 14

A molecular equation

Question 15

In a complete ionic equation compounds which are dissociated are written as _________ ions.

Answer 15

Separate

Question 16

To write the net ionic equation cancel the __________ ions in the compounds.

Answer 16

Spectator

Question 17

Ions that do not participate in the reaction are what?

Answer 17

Spectator ions

Question 18

Spectator ions can be found in exactly the same form on _________ sides of the chemical equation.

Answer 18

Both

Question 19

Precipitation reactions produce an ___________ salt.

Answer 19

Insoluble

Question 20

A precipitation reaction is one type of __________ reaction.

Answer 20

Exchange

Question 21

The anions exchange places between cations in ___________ reactions.

Answer 21

Exchange

Question 22

The driving force in a precipitation reaction is the formation of an ____________ compound.

Answer 22

Insoluble

Question 23

Arrhenius acids produce ______ in water.

Answer 23

H+

Question 24

Arrhenius bases produce ______ in water.

Answer 24

OH-

Question 25

Brønsted-Lowry acid donates a __________.

Answer 25

Proton

Question 26

Brønsted-Lowry base accepts a __________.

Answer 26

Proton

Question 27

Strong acids and bases ionize completely in __________. They are strong electrolytes.

Answer 27

Water

Question 28

Weak acids and bases only ___________ ionize in water. They are weak electrolytes.

Answer 28

Partially

Question 29

Acid-based reactions are also called _______________ reactions.

Answer 29

Neutralization

Question 30

What is the driving force in acid-based (neutralization) reactions?

Answer 30

Formation of water

Question 31

What is the net ionic equation for all reactions of soluble strong acids and bases?

Answer 31

(OH-) + (H+) ——> H2O

Question 32

What are the products of an acid-based reaction?

Answer 32

Water and a salt

Question 33

The exception to the H2O production in a neutralization reaction is when _______ reacts with an acid.

Answer 33

NH3

Question 34

Gas-forming reactions come from a metal carbonate reacting with an _________.

Answer 34

Acid

Question 35

Carbonic acid is unstable and forms ______ and ______.

Answer 35

CO2 H2O

Question 36

Oxidation-reduction (redox) reactions involve the transfer of ___________ from one substance to another.

Answer 36

Electrons

Question 37

In a redox reaction if you lose electrons it’s ___________.

Answer 37

Oxidation

Question 38

In a redox reaction if you gain electrons it’s a _____________.

Answer 38

Reduction

Question 39

Redox reactions are characterized by electron transfer between electron __________ and electron __________.

Answer 39

Donor Acceptor

Question 40

An electron transfer leads to an increase in the oxidation number of one element = ____________.

Answer 40

Oxidation

Question 41

An electron transfer leads to a decrease in the oxidation number of another element = _____________.

Answer 41

Reduction

Question 42

The electric charge an element appears to have when electrons are counted by some arbitrary rules are what?

Answer 42

Oxidation numbers

Question 43

Each atom in a free element has an oxidation number of _______.

Answer 43

Zero

Question 44

In simple ions, the oxidation number is equal to the ___________ on the ion.

Answer 44

Charge

Question 45

Oxygen has an oxidation number of ______.

Answer 45

-2

Question 46

The oxidation number of hydrogen is _____.

Answer 46

+1

Question 47

The algebraic sum of oxidation numbers equals _____ for a neutral compound.

Answer 47

0

Question 48

The algebraic sum of oxidation numbers is equal to the overall charge on a polyatomic ______.

Answer 48

Ion