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Chemistry 1A > Chapter 4: Ionic Theory of Solution and Solubility Roles > Flashcards

Chapter 4: Ionic Theory of Solution and Solubility Roles Flashcards

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1
Q

Electrolyte

A

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

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2
Q

Nonelectrolyte

A

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

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3
Q

Strong electrolyte

A

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)

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4
Q

Weak electrolyte

A

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)

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5
Q

Molecular Equation

A

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.

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6
Q

Complete Ionic Equation

A

Written in stand-alone ionic form.

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7
Q

Spectator Ions

A

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.

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8
Q

Strong acid

A

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

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9
Q

Strong base

A

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

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10
Q

Weak base

A

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

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11
Q

Common Strong Acids

A 
HClO4
H2SO4
HI
HBr
HCl
HNO3
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12
Q

Strong Bases

A 
LiOH
NaOH
KOH
RbOH
CsOH
Ca(OH)2
Sr(OH)2
Ba(OH)2
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13
Q

Weak Acids

A

CO(2)H (Carboxylic Acids.)

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14
Q

Rules for Assigning Oxidation Numbers: Elements

A

Oxidation = 0

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15
Q

Rules for Assigning Oxidation Numbers: Monoatomic Ions

A

Oxidation number always = 0

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16
Q

Rules for Assigning Oxidation Numbers: Oxygen

A

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

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17
Q

Rules for Assigning Oxidation Numbers: Hydrogen

A

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

18
Q

Rules for Assigning Oxidation Numbers: Halogens

A

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.

19
Q

Rules for Assigning Oxidation Numbers: Compounds and Ions

A
  • The sum of the Ox# = 0.

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

20
Q

Ease of Oxidation

A

Bottom-Up on PT

21
Q

Calculating Molarity:

A

Molarity: Moles of Solute/Liters of the Solution

22
Q

Concentration

A

Moles/Volume in Liters

Same as molarity

23
Q

Monoprotic

A

One ionizable acid

24
Q

Diprotic

A

Two ionizable acids

25
Q

Intensive property

A

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

26
Q

Extensive properties

A

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

27
Q

Dissociation reaction

A

Reversible

28
Q

Decomposition reaction

A

Irreversible

29
Q

Titration

A

Neutralization, often indicated by a color change.

30
Q

Carbonates and HCO3 with acids produce…

A

…H2O!
Examples:
CaCO3 + HCl –> CaCl2 + CO2 + H2O
NaHCO3 + HBr –> NaBr + CO2 + H2O

The CO2 and H2O in these equations creates Hydrogen Carbonate (HCO3).

31
Q

Gas forming reactions for

NH4OH –>

A

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

32
Q

Gas forming reactions of

H2SO3 –>

A

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

33
Q

Gas forming reactions for

H2CO3 –>

A 
CO2 + H2O
Produces Hydrogen Carbonates (H2CO3) when added with acid.
Examples: 
CaCO3 + HCl --> CaCl2 + CO2 + H2O
NaHCO3 + HBr --> NaBr + CO2 + H2O
34
Q

Ionic equations

A

An equation in which ions are specifically shown

35
Q

Spectator Ion

A

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

36
Q

Net ionic equation

A

An equation that does not include spectator ions.

37
Q

The gas-forming compounds

A

NH4OH
H2SO3
H2CO3

38
Q

Naming acids: SO4^2-

A

-ate = -ic

Sulfate –> H2SO4 = Sulfuric Acic

39
Q

Naming acids: NO2^-

A

-ite = -ous

Nitrite –> HNO2^- = Nitrous acid

40
Q

Naming acids: Cl^-

A

-ide = hydro- -ic

Chloride –> HCl^- = Hydrochloric acid

Chemistry 1A (14 decks)

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