AP Chemistry

Pages
- Class
  Laboratory report rubric
  Notes
  1. Chemical foundations
  2. Atoms, molecules, and ions
  3. Stoichiometry
  4. Types of chemical reactions and solution stoichiometry
  5. Gases
  6. Thermochemistry
  7. Atomic structure and periodicity
  8. Bonding: general concepts
  9. Covalent bonding: orbitals
  10. Liquids and solids
  11. Properties of solutions
  12. Chemical kinetics
  13. Chemical equilibrium
  14. Acids and bases
  15. Acid-base equilibria
  16. Solubility and complex ion equilibria
  17. Spontaneity, entropy, free energy
  18. Electrochemistry
  Drug unit
  Basics
  Analgesics
  Antacids
  Anesthetics
  Depressants
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  Antibiotics
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  Mind-altering drugs
- Textbook (incomplete)
  1. Chemical foundations
  2. Atoms, molecules, and ions
  3. Stoichiometry
  4. Types of chemical reactions and solution stoichiometry
  5. Gases
  6. Thermochemistry
  7. Atomic structure and periodicity
  8. Bonding: general concepts
- CED
  1. Atomic structure and properties
  2. Compound structure and properties
  3. Properties of substances and mixtures
  4. Chemical reactions
  5. Kinetics
  6. Thermochemistry
  7. Equilibrium
  8. Acids and bases
  9. Thermodynamics and electrochemistry

AP Chemistry

...

18. Electrochemistry

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18. Electrochemistry

electrochemistry: chemistry of flowing electrons

oxidation-reduction reaction

oxidation involves loss, reduction involves gain

example:

⁠

Galvanic cell

galvanic cell: converts chemical energy into electrical energy

ions in liquid must match metal

metals connected with wire

voltmeter: measures voltage between two points in electric circuit

volt (V): number of electrons flowing past a point in an amount of time

V = 0 at equilibrium

salt bridge: piece of paper soaked in ionic compound

⁠

anode: side of galvanic cell where oxidation occurs

cathode: side of galvanic cell where reduction occurs

Cell potential

cell potential (E): the pull of electrons through a wire (volts)

total cell potential must be positive for the cell to work

flip equation: E changes sign

do not multiply E if you multiply coefficients

half-cell: just the anode or just the cathode

hydrogen standard: E = 0

example:

reaction and total cell potential?

⁠

flip Mg reaction (make positive)

⁠

need to add the values of E

total cell potential: 0.71 V

balance electrons by multiplying equations by constant

voltage does not multiply

add equations together

⁠

Mg is anode, Al is cathode

⁠

ΔG: Gibb’s free energy (J)

n: moles of electrons (mol)

F: Faraday’s constant (96485 C/mol e⁻)

coulomb = C = J/V

faraday (unit): moles of electrons

E: cell potential (V)

changing the amount of metal does not do anything, only changing concentrations

Nonstandard cell potential

standard cell potential (E°): cell potential under standard conditions (1 M)

nonstandard cell potential (E): cell potential not under standard conditions

Nernst equation:

⁠

E: nonstandard cell potential

E°: standard cell potential

R: gas constant (J/K)

T: temperature (K)

n: electrons (mol)

F: Faraday’s constant (96485 C/mol e⁻)

Q: reaction quotient

adding to the left increases E, adding to the right decreases E

example:

⁠

if [Al³⁺] = 2.0 M, [Mn²⁺] = 1.0 M: E would be less

if [Al³⁺] = 1.0 M, [Mn²⁺] = 3.0 M: E would be greater

Electrolysis

electrolysis: adding electricity to reverse the reaction in a galvanic cell

e.g. charging devices, plating metals

ampere (amp): speed of electron current (coulombs per second)

use Faraday’s constant to convert to moles of electrons

⁠

I: flow of electrons (A)

q: charge (C)

t: time (s)

example:

⁠

, add 10.0 amps of electricity for 30 min; how much Cu(s) is made (g)?

amperes → coulombs:

⁠

coulombs → moles of electrons:

⁠

moles of electrons → moles of copper:

⁠

moles → grams

⁠

Galvanic cell

Cell potential

Nonstandard cell potential

Electrolysis

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