JC final test Flashcards
Titration Curves,ElectroChem, Orgo (173 cards)
1
Q
Wh at is Condensed Structural Formula
A
Representation without showing individual bonds.
2
Q
What is Central Atom
A
Atom bonded to surrounding atoms in a structure.
3
Q
What are Identical Groups
A
Represented with parentheses and subscripts.
4
Q
What are Nonbonding Electrons
A
Typically not shown in condensed formulas.
5
Q
What is a Voltaic Cell
A
Device converting chemical energy to electrical energy.
6
Q
Who is Alessandro Volta
A
Italian scientist, namesake of voltaic cells.
7
Q
WHo is Luigi Galvani
A
Italian scientist, discovered electricity, namesake of galvanic cells.
8
Q
What is a Spontaneous Redox Reaction
A
Chemical reaction releasing energy for electrical work.
9
Q
What is Electron Transfer
A
Movement of electrons through an external pathway.
10
Q
What is the Anode
A
Electrode where oxidation occurs, negative terminal.
11
Q
What is the Cathode
A
Electrode where reduction occurs, positive terminal.
12
Q
What is an Oxidation Half Reaction
A
Process where Zn(s) loses electrons to form Zn2+.
13
Q
What is a Reduction Half Reaction
A
Process where Cu2+ gains electrons to form Cu(s).
14
Q
What is a Salt Bridge
A
U-shaped tube maintaining electrical neutrality in cells.
15
Q
What is a Porous Glass Disc
A
Separates compartments, allows ion migration without mixing.
16
Q
What are Electromotive Force (EMF)
A
Driving force pushing electrons through the circuit.
17
Q
What are Potential Difference’s
A
Voltage difference between anode and cathode.
18
Q
Def of Cation Movement
A
Positive ions migrating to maintain electrical neutrality.
19
Q
Def of Anion Movement
A
Negative ions migrating to maintain electrical neutrality.
20
Q
What is an External Circuit
A
Pathway for electron flow from anode to cathode.
21
Q
What is the Oxidation Reaction for Zn(s)
A
Zn(s) → Zn2+(aq) + 2e-.
22
Q
What is the Reduction Reaction for Cu2+
A
Cu2+(aq) + 2e- → Cu(s).
23
Q
What is an Electrolyte Solution
A
Conductive solution in salt bridge for ion migration.
24
Q
WHat is the Waterfall effect
A
Potential energy decreases from top to bottom.
25
What is Standard Cell Potential
Denoted as Eº cell, measures cell voltage.
26
WHat are Standard Conditions
1M concentration, 1 atm pressure, 25°C temperature.
27
WHat is the Cell Potential Formula
E° cell = E° red (cathode) - E° red (anode).
28
What is a Volt (V)
Unit of electrical potential, 1 J/C.
29
WHat is a Voltmeter
Device to measure electrical cell potential.
30
What is a Potentiometer
Variable voltage device from external power.
31
What is the Driving Force for Reduction
More positive Eº indicates stronger reduction tendency.
32
What is the Standard Hydrogen Electrode (SHE)
Reference electrode assigned 0V potential.
33
WHat is a Spontaneous Reaction
Positive Eº indicates spontaneous forward reaction.
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WHat is a Nonspontaneous Reaction
Negative Eº indicates nonspontaneous forward reaction.
35
What are Standard Reduction Potentials
Measured at 1M solutes, 1 atm gases, 25°C.
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WHat is the Half-Reaction Reversal Rule
Reversing half-reaction changes E° sign.
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What is the Half-Reaction Multiplication Rule
Multiplying half-reaction does not change E°.
38
What is Line Notation
Describes electrochemical cells' components and phases.
39
WHat is the Anode Compartment
Listed on the left in line notation.
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WHat is the Cathode Compartment
Listed on the right in line notation.
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What are Phase Differences
Single vertical line separates different phases.
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WHat is a Salt Bridge
Double vertical line indicates connection between compartments.
43
WHat are Titration Curve
Plot of pH versus titrant amount added.
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WHat is the Equivalence Point
Equal moles of acid and base react.
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What is pH
Measure of hydrogen ion concentration in solution.
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What does a Strong Base do in a solution
Completely dissociates in solution, e.g., NaOH.
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what does a Strong Acid do in a solution
Completely dissociates in solution, e.g., HCl.
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what does a Weak Acid do in a solution
Partially dissociates in solution, e.g., CH3COOH.
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what does a Weak Base do in a solution
Partially dissociates in solution, e.g., NH3.
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what is Equivalence Point
Point where moles of acid equal moles of base.
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What is the Initial pH
pH before any titrant is added.
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How do you get Excess NaOH
Concentration of unreacted NaOH after equivalence.
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Def of a Conjugate Base
Species formed when an acid donates a proton.
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Def of a Conjugate Acid
Species formed when a base accepts a proton.
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WHat is the Buffering Effect
Resistance to pH change near equivalence point.
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WHat is pKa
Negative logarithm of the acid dissociation constant.
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WHat are Titration Curves
Graph of pH versus volume of titrant added.
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What is the Halfway Point
Point where weak acid equals conjugate base concentration.
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What is Phenolphthalein
Indicator that turns pink in basic solutions.
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What is the pH at Equivalence (WA-SB)
Always greater than 7.00 for weak acid titration.
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WHat is the pH at Equivalence (SA-SB)
Always equal to 7.00 for strong acid titration.
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What does Acid Strength determine
Determines the shape of the pH titration curve.
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WHat is Stoichiometry
Relationship between reactants in a chemical reaction.
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Indicator Detection Threshold
About 10% conversion needed for color change.
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Ka Expression
Ka = [In][H+]/[Hin] for acid dissociation.
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Redox Reactions
Reactions involving oxidation and reduction processes.
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Oxidation
Loss of electrons in a chemical reaction.
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Reduction
Gain of electrons in a chemical reaction.
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Oxidizing Agent
Substance that causes oxidation by accepting electrons.
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Reducing Agent
Substance that causes reduction by donating electrons.
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Oxidation State
Charge of an atom in a compound.
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Half-Reaction
Separation of oxidation and reduction processes.
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Conservation of Mass
Mass remains constant in chemical reactions.
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Conservation of Charge
Total charge remains constant in reactions.
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Balancing Redox Equations
Ensuring equal number of atoms and charges.
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Titration
Technique to determine concentration of a solution.
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Equivalence Point
Point at which reactants are in stoichiometric proportions.
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Electrons in Half-Reactions
Electrons are products in oxidation, reactants in reduction.
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MnO4- Reduction
MnO4- is reduced to Mn2+ in reactions.
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C2O42- Oxidation
C2O42- is oxidized to CO2 in reactions.
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Water Balance
Water added to balance oxygen in half-reactions.
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H+ Balance
H+ added to balance hydrogen in half-reactions.
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Charge Balance
Electrons added to balance charges in reactions.
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10 Electrons
Total electrons needed for balancing both half-reactions.
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Basic Solution Balancing
OH- added to neutralize H+ in reactions.
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Spontaneous Reaction Example
Zn(s) + 2H+(aq) → Zn2+(aq) + H2(g)
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Voltaic Cell
Device using spontaneous redox reactions for electricity.
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Salt Bridge
Connects half-cells, allowing ion movement.
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Anode
Electrode where oxidation occurs, loses mass.
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Cathode
Electrode where reduction occurs, gains mass.
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Oxidation Half-Reaction
Zn(s) → Zn2+(aq) + 2e-.
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Reduction Half-Reaction
Cu2+(aq) + 2e- → Cu(s).
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Cell EMF
Electromotive force driving electron flow.
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Standard Cell Potential
E°cell at standard conditions, measured in volts.
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Potential Difference
Difference in electrical potential, measured in volts.
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Electromotive Force (emf)
Force pushing electrons through an external circuit.
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Cations Movement
Cations move from anode to cathode.
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Anions Movement
Anions move from cathode to anode.
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Cell Voltage
Ecell, indicates spontaneity of reaction.
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Standard Reduction Potential
E°red measured against a standard.
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Driving Force
Electrons flow due to potential energy difference.
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Half-Cell
Each compartment in a voltaic cell.
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Spontaneous Reaction
Reaction that occurs without external energy.
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Zn Oxidation
Zn is oxidized to Zn2+ in the reaction.
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Cu Reduction
Cu2+ is reduced to Cu in the reaction.
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FAT CAT Mnemonic
Cathode gains mass during the reaction.
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Anorexic Anode Mnemonic
Anode loses mass during the reaction.
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1 Volt Definition
1 V = 1 J/C, potential difference.
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EMF
Electromotive force, driving voltage of a cell.
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Standard Reduction Potential
Potential measured under standard conditions, 1M, 1 atm.
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Standard Hydrogen Electrode
Reference electrode assigned 0 V standard potential.
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E°cell
Cell potential calculated from reduction potentials.
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Cathode
Electrode where reduction occurs in a cell.
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Anode
Electrode where oxidation occurs in a cell.
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Spontaneous Reaction
Reaction that occurs naturally without external energy.
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Nonspontaneous Reaction
Reaction that requires energy input to occur.
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Intensive Property
Property independent of the amount of substance.
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Stoichiometric Coefficient
Number indicating moles of reactants/products in a reaction.
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Oxidizing Agent
Substance that gains electrons, undergoes reduction.
120
Reducing Agent
Substance that loses electrons, undergoes oxidation.
121
Faraday's Constant
Charge of one mole of electrons, 96485 C/mol.
122
Nernst Equation
Calculates cell potential under nonstandard conditions.
123
Gibbs Free Energy
Energy available to do work in a system.
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E°red
Standard reduction potential for a half-reaction.
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Driving Force for Reduction
Greater positive E°red indicates stronger reduction tendency.
126
Electrode Potential
Voltage developed by an electrode in a solution.
127
Galvanic Cell
Device converting chemical energy into electrical energy.
128
Reaction Quotient (Q)
Ratio of products to reactants at any point.
129
Standard Conditions
1 M concentration, 1 atm pressure, 25°C.
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Cell Equilibrium
State when E = 0, no net reaction occurs.
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Ecell
Cell potential measured in volts (V).
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Concentration Cell
Cell generating emf from concentration differences.
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Lead-Acid Battery
12 V battery with six 2 V cells.
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PbO2 Reaction
Cathode reaction in lead-acid battery.
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Overall Reaction
Combined reaction of lead-acid battery components.
136
Rechargeable Battery
Battery that can be recharged and reused.
137
Alkaline Battery
Non-rechargeable battery using KOH solution.
138
Cell Potential
Voltage produced by an electrochemical cell.
139
Nickel-Cadmium Battery
Rechargeable battery with 1.30 V potential.
140
Cadmium Toxicity
Environmental concern regarding cadmium disposal.
141
Hydrogen Fuel Cell
Generates electricity from hydrogen and oxygen.
142
PEM Fuel Cell
Uses proton exchange membrane for ion transport.
143
Direct Methanol Fuel Cell
Uses methanol instead of hydrogen for reactions.
144
Corrosion
Undesirable redox reaction converting metal to compound.
145
Rusting of Iron
Oxidation of iron by oxygen in moisture.
146
E°red
Standard reduction potential measured in volts.
147
Oxidation
Loss of electrons during a chemical reaction.
148
Reduction
Gain of electrons during a chemical reaction.
149
Electrochemical Reaction
Chemical reaction producing electrical energy.
150
Anode
Electrode where oxidation occurs in electrochemical cells.
151
Cathode
Electrode where reduction occurs in electrochemical cells.
152
Standard Reduction Potential
Measure of tendency to gain electrons, in volts.
153
Galvanized Iron
Iron coated with zinc to prevent corrosion.
154
Cathodic Protection
Technique using sacrificial anodes to prevent corrosion.
155
Sacrificial Anode
Metal that oxidizes to protect another metal.
156
Electrolysis
Nonspontaneous reaction requiring external current.
157
Electrolytic Cell
Cell where electrolysis reactions occur.
158
Voltaic Cell
Cell generating electrical energy from spontaneous reactions.
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Active Electrode
Electrode participating in electrolysis reactions.
160
Electroplating
Process of depositing metal onto a surface.
161
Coulomb
Charge passing a point in one second at 1 ampere.
162
Faraday's Law
1 mol electrons deposits 1 mol metal.
163
Charge Calculation
q = I t, where q is charge.
164
Free Energy (G)
Maximum useful work obtainable from a system.
165
Electrical Work
Work done by the system on surroundings.
166
Oxidation of Iron
Iron reacts with oxygen, forming rust.
167
Rust Composition
Fe2O3.xH2O, formed from oxidized iron.
168
Electrolysis of NaCl
Produces Na and Cl2 from molten salt.
169
Electrolysis of Aqueous NaF
Water reduces more easily than fluoride ions.
170
Current (I)
Flow of electric charge, measured in amperes.
171
Energy Conversion
1 kWh = 3.6 x 10^6 J.
172
pH Influence
Affects corrosion rate of iron.
173
Name the 10 carbon chains
Methane, Ethane, Propane, Butane, Pentane, Hexane, Heptane, Octane, Nonane, Decane
