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Chapter 4 from Chem 1303
review for final
42
Chemistry
Undergraduate 1
12/08/2014

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Term
solution
Definition
homogeneous (uniform) mixture of two or more substances, consisting of:
1. solvent
2. solute(s)
3. aqueous soln
Term
solvent
Definition
the bulk medium, ex: H2O (usually the larger amount)
Term
solute(s)
Definition
the dissolved substance(s), ex: NaCl (usually present in lesser quantities)
Term
aqueous soln
Definition
H2O is the solvent
Term
concentration
Definition
measure of relative solute/solvent ratio
Term
standard solution
Definition
accurately known concentration
Term
saturated solution
Definition
contains maximum amount of solute
Term
solubility
Definition
concentration of a saturated solution, ex:,
solubility of NaCl is about 36 g NaCl/ 100 g H2O ("soluble")
solubility of CuS is about 10^-5 CuS/ 100 g H2O ("insoluble")
Term
precipitate
Definition
an "insoluble" reaction product
Ex: a precipitation reaction where the precipitate is AgCl:
NaCl (aq) + AgNO3 (aq) --> AgCl (s) + NaNO3 (aq)
Term
electrolytes
Definition
solutes that produce ions in solution via dissociation (these solutions can conduct electricity)
Ex: NaCl (s) --> Na+ (aq) + Cl- (aq)
(NH4)2SO4 (s) --> 2 NH4+ (aq) + SO42- (aq)
Term
hydration
Definition
process of surrounding ions by H2O
Term
"strong" electrolytes
Definition
100% ionized
-salts and acids can be electrolytes
HCl (g) --> H+ (aq) + Cl- (aq)
Term
"weak" electrolytes
Definition
substances that are partially ionized (<100%)
weak acid (acetic acid)
Term
non-electrolytes
Definition
substances that are not ionized and do not conduct electricity
C6H12O6 + H2O --> C6H12O6 + H2O (No ions are present!)
Term
Strong Electrolytes
Definition
HCl
HBr
HI
HNO3
HClO4
H2SO4
soluble bases with OH- (i.e., NaOH, Ba(OH)2
Term
weak electrolyte
Definition
CH3COOH
HF
HNO2
NH3
H2O
Term
nonelectrolyte
Definition
C6H12O6 (glucose)
C12H22O6 (sucrose)
CH3OH (methanol)
C2H5OH (ethanol)
(NH2)2CO (urea)
Term
precipitation reactions
Definition
occur when aqueous solns are mixed and the reaction produces insoluble product (precipitate so ions are tied up)
Term
Solubility
Definition
maximum amount of solute that will dissolve in a given quantity of solvent
Term
How does formation of insoluble product make a reaction occur?
Definition
Because it prevents the products from reforming the original reactants
Term
Solubility Rules
Definition
Soluble:

Acetates
Bicarbonates
Chlorates and perchlorates
Group 1
Ammonium
Nitrates
Group 7 (halides)
-EXCEPT
Ag+
Hg2 2+
Pb 2+
Sulfates
- Except
Ag+
Ca 2+
Sr 2+
Ba 2+
Pb 2+
Hg2 2+

Insoluble

Carbonates
Phosphates
Chromates
Sulfides

Except Group I and NH4+

OH : hydroxides
Except: Grop I and Ba 2+
Term
Metathesis Reaction ("double displacement")
Definition
Ions from two different reactants simply trade partners, Ex: ,,
NaCl (aq) + AgNO3 (aq) --> AgCl (s) + NaNO3 (aq)
Term
spectator ions
Definition
appear uncharged on both sides of the equation
do not participate in the chemically important part of the reaction
Term
what is the net ionic equation?
What does it show?
Why is it useful?
Definition
-
- The net ionic equation shows that, in general, a precipitate of BaCO3 will form whenever the ions Ba 2+ and CO 3 2- are combined in aqueous solution, regardless of their sources

- The essential chemical process can be written without the spectator ions in the net ionic equation
Term
Molecular Equation
Definition
shows all compounds with complete,, neutral molecular formulas
useful in planning experiments and stoichiometry calculations
Term
Ionic Equation (complete)
Definition
- All strong electrolytes are show in their dissociated, ionic forms
- insoluble substances and weak electrolytes are shown in their molecular form
- spectator ions are included
- useful for showing all details of what is happening in the reaction
Term
Net Ionic Equation
Definition
- "spectator ions" are omitted
- only the essential chemical process is shown, ex: formation of it
- solid precipitate
- gaseous product, or
- weak electrolyte (ex: water)
- useful for generalizing the reaction--the same important part can often be formed from different sets of reactants
Term
Acid-Base Reactions
Definition
Occur when aqueous solns are mixed and the reaction produces a weak electrolyte (so ions are tied up)
Term
Arrhenius definition
Definition
Acids give H+ when dissolved in water and bases give OH-

Common acids: vinegar, lemon juice, aspirin
Common bases: milk of magnesia, lye
Term
Properties of acids
Definition
- taste sour
- cause color changes in dyes (litmus: blue to red)
- react with metals (Zn, Mg, Fe) to form H2 gas
2 HCl (aq) + Mg (s) --> MgCl2 (aq) + H2 (g)
- react with carbonates and bicarbonates to form CO2 gas
2 HCl (aq) + CaCO3 (s) --> CaCl2 (aq) + H2O (l) + CO2 (g)
- aqueous solutions conduct electricity (because there are ions present)
- react with bases to form salts and water
HCl (aq) + NaOH (aq) --> NaCl (aq) + H2O
Term
Properties of Bases
Definition
- taste bitter
- feel slippery (ex: soaps)
- cause color changes in dyes (litmus: red to blue)
- aqueous solutions conduct electricity (because there are ions present)
- react with acids to form salts and water
HCl (aq) + NaOH (aq) --> NaCl (aq) + H2O
Term
Bronsted definition (broader)
Definition
Acid- proton (H+) donor
Base- proton acceptor
Term
Bronsted Acid
Definition
HCl (aq) --> H+ (aq) + Cl- (aq)
more correctly
HCl (aq) + H2O (l) __> H3O+ (aq) + Cl- (aq)
H3O+ is a hydrated proton called the hydronium ion
Term
monoprotic acids
Definition
donate one hydrogen ion upon ionization

HCl (aq) --> H+ (aq) + Cl- (aq)
Term
diprotic acids
Definition
donate two hydrogen ions upon ionization

H2SO4 (aq) --> H+ (aq) + HSO4- (aq)

HSO4- (aq) ---> H+ (aq) + SO4 2- (aq)
<---
2 steps with the second being incomplete
Term
triprotic acids
Definition
donate three hydrogen atom (H3PO4)
Term
Acid-Base Neutralization
Definition
acid + base --> salt + water

(Neutralization reaction)

HCl (aq) + NaOH (aq) --> NaCl (aq) + H2O (l)
Term
Gas Formation Reaction
Definition
Occur when aqueous solns are mixed and the reaction produces gaseous product (gas so ions are tied up)
Term
Oxidation-Reduction Reactions
Definition
electron transfer reactions

Ex: burning fossil fuels, bleach, rusting, some occur in water, others don't
2 Na + Cl2 --> 2 NaCl

2 half reactions
oxidation---loss of electron(s)
reduction---gain of electron(s)

half reactions:
Na ---> Na+ + e- (oxidation)
Cl2 + 2e- ---> 2 Cl- (reduction)
Term
oxidizing agent
Definition
the substance that is reduced
Term
reducing agent
Definition
the substance that is oxidized
Term
Oxidation Number


Rules for assigning oxidation numbers
Definition
a "charge" that is assigned to an atom to aid in a lancing redox reactions

- Generally, oxidation number is the charge that would result if all of the bonding electrons around an atom were assigned to the more electronegative element(s).


1. Free elements--oxidation number = 0
2. Ions of one atom: oxidation number= charge
3. Oxygen--usually -2; in peroxides (H2O2), O= -1
4. Hydrogen is usually +1, except when bonded to metals, ex: LiH, NaH in which H= -1
5. F= -1; Cl, Br, I (ions) = -1, but as molecular compounds, the charge varies and is positive
6. Sum of oxidation numbers = 0 in neutral compounds and equals the charge in polyatomic ions
7. Oxidation numbers are not always integers, ex: O2- (superoxides) = -1/2
Thus for
S (s) + O2 (g) --> SO2 (g)
- S (s) =0
- O2 (g)- 0
- SO2 (g): S= +4 and O = -2
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