Chapter 4: Ionic Theory of Solution and Solubility Roles

Question 1

Electrolyte

Answer 1

A substance that dissolves in water to give an electrically conducting solution. Ionic solids that dissolve in water are electrolytes.

Question 2

Nonelectrolyte

Answer 2

A substance that dissolves in water to give a nonconducting or very poorly conducting solution.

Question 3

Strong electrolyte

Answer 3

A solute that completely, or almost completely, ionizes or dissociates in a solution. These ions are good conductors of electric current in the solution.

Example: NaCl –> Na+(aq) + Cl-(aq)

Question 4

Weak electrolyte

Answer 4

An electrolyte that dissolves in water to give a relatively small percentage of ions. Generally are molecular substances

Example: NH3(aq)+H2O(l) –> NH4^+(aq) + OH-(aq)

Question 5

Molecular Equation

Answer 5

Which is a chemical equation in which the reactants and products are written as if they were molecular substances, even though they may actually exist in solution as ions.

Question 6

Complete Ionic Equation

Answer 6

Written in stand-alone ionic form.

Question 7

Spectator Ions

Answer 7

An ion in an ionic equation that does not take part in the reaction. You can cancel such ions from both sides to express essential reactions that occur.

Question 8

Strong acid

Answer 8

An acid that ionizes completely ion water and is also a strong electrolyte.

Question 9

Strong base

Answer 9

Base that is present in aqueous solution entirely as ions, one of which is OH-. A strong electrolyte

Question 10

Weak base

Answer 10

A base that is only partly ionized in water; it is a weak electrolyte.

Question 11

Common Strong Acids

Answer 11

HClO4
H2SO4
HI
HBr
HCl
HNO3

Question 12

Strong Bases

Answer 12

LiOH
NaOH
KOH
RbOH
CsOH
Ca(OH)2
Sr(OH)2
Ba(OH)2

Question 13

Weak Acids

Answer 13

CO(2)H (Carboxylic Acids.)

Question 14

Rules for Assigning Oxidation Numbers: Elements

Answer 14

Oxidation = 0

Question 15

Rules for Assigning Oxidation Numbers: Monoatomic Ions

Answer 15

Oxidation number always = 0

Question 16

Rules for Assigning Oxidation Numbers: Oxygen

Answer 16

Oxidation # = -2 in most compounds. Except in H2O2 and other peroxides, it is 1.

Question 17

Rules for Assigning Oxidation Numbers: Hydrogen

Answer 17

Oxidation # = 1 unless it is in a binary compound with metal, it is -1.

Question 18

Rules for Assigning Oxidation Numbers: Halogens

Answer 18

Flourine always = 1
Chlorine, Bromine, Iodine, Astitine = -1 in binary compounds, except when the other element is another halogen above it on PT or is O.

Question 19

Rules for Assigning Oxidation Numbers: Compounds and Ions

Answer 19

• The sum of the Ox# = 0.

- The sum of the Ox# of polyatomic ion equals the charge on the ion.

Question 20

Ease of Oxidation

Answer 20

Bottom-Up on PT

Question 21

Calculating Molarity:

Answer 21

Molarity: Moles of Solute/Liters of the Solution

Question 22

Concentration

Answer 22

Moles/Volume in Liters

Same as molarity

Question 23

Monoprotic

Answer 23

One ionizable acid

Question 24

Diprotic

Answer 24

Two ionizable acids

Question 25

Intensive property

Answer 25

Bulk property, not depending on the system size or amount of material in the system. Properties include temperature, refractive index, density, hardness. I.e., maintained properties

Question 26

Extensive properties

Answer 26

Proportional to the amount of material in the system, e.g., energy, entropy, length, mass, particle number, momentum, moles, volume.

Question 27

Dissociation reaction

Answer 27

Reversible

Question 28

Decomposition reaction

Answer 28

Irreversible

Question 29

Titration

Answer 29

Neutralization, often indicated by a color change.

Question 30

Carbonates and HCO3 with acids produce...

Answer 30

...H2O! Examples: CaCO3 + HCl --> CaCl2 + CO2 + H2O NaHCO3 + HBr --> NaBr + CO2 + H2O The CO2 and H2O in these equations creates Hydrogen Carbonate (HCO3).

Question 31

Gas forming reactions for | NH4OH -->

Answer 31

NH3 + H2O Ammonium, salt + strong base = NH4OH Example NH4Cl + NaOH --> H2O + NH3 + NaCl

Question 32

Gas forming reactions of | H2SO3 -->

Answer 32

SO2 + H2O Decomposes to create H2SO3 Example SrSO3 + 2HI --> SrI2 + SO2 + H2O

Question 33

Gas forming reactions for | H2CO3 -->

Answer 33

``` CO2 + H2O Produces Hydrogen Carbonates (H2CO3) when added with acid. Examples: CaCO3 + HCl --> CaCl2 + CO2 + H2O NaHCO3 + HBr --> NaBr + CO2 + H2O ```

Question 34

Ionic equations

Answer 34

An equation in which ions are specifically shown

Question 35

Spectator Ion

Answer 35

An ion that appears unchanged on both sides of a reaction arrow

Question 36

Net ionic equation

Answer 36

An equation that does not include spectator ions.

Question 37

The gas-forming compounds

Answer 37

NH4OH H2SO3 H2CO3

Question 38

Naming acids: SO4^2-

Answer 38

-ate = -ic | Sulfate --> H2SO4 = Sulfuric Acic

Question 39

Naming acids: NO2^-

Answer 39

-ite = -ous | Nitrite --> HNO2^- = Nitrous acid

Question 40

Naming acids: Cl^-

Answer 40

-ide = hydro- -ic | Chloride --> HCl^- = Hydrochloric acid