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This course can help prepare students who wish to continue their scientific education after high school, as well as students who wish to perform exceptionally well on the SAT exam. The level of aptitude in this subject will assist students wishing to excel on the SAT and in college courses. Students who wish to go into a career in science or even enter a science-related field of study in college should strongly consider getting a jump start on their education and take AP Chemistry.
According to the College Board, AP Chemistry is an introductory college level course designed to be the equivalent of a student’s first year of college chemistry. It may also fulfill a lab requirement and free students from having to take other science classes. Students should attain a depth of understanding of fundamentals and a reasonable competence in dealing with chemical problems and solutions.
AP Chemistry is a course geared toward highly motivated students with interests in chemical and physical sciences. AP Chemistry builds on concepts covered in a regular or "honors" chemistry course, using greater detail in concept exploration and laboratory investigation. This course prepares students to take the AP Chemistry exam toward the end of the academic year. AP Chemistry topics include atomic theory, chemical bonding, phases of matter, solutions, types of reactions, equilibrium, reaction kinetics, and thermodynamics.
Anyone wishing to take an AP Chemistry course should take at least two years of high school math before enrolling in this course. Their math experience should also include a second year Algebra course in order to ensure that students are familiar with the types of functions that will be used during experiments. A basic first year chemistry course (Chemistry I) should also be completed in order to provide students with the foundation they need to succeed with higher levels of chemistry. Additionally, while AP Chemistry is a desirable course, universities also recommend that students take a basic physics course while in high school as well as higher math classes to prepare students for college.
AP Chemistry is a serious course and includes many course goals. According to the College Board’s website, by the time students take their AP Chemistry exam (or the SAT exam) they should be prepared to do the following:
Students who choose to take Advances Placement courses should remember that they’re just that: Advanced. Students should be prepared to challenge themselves in order to develop above average study skills and discipline. Students who do this and commit themselves to their education will see a definite payoff. Their grades and academic confidence will improve tremendously, as will their preparedness for college.
Advanced placement courses are not only important for a student’s development, but they can look excellent on high school transcripts. Students that wish to get into the college or university of their choice should talk to their counselor about enrolling in an AP course (or several). Most importantly, students can save valuable time, energy, and money by earning college credit while still in high school! The more a student does to prepare themselves for college, the more it will pay off in the end. Advanced Placement courses are the perfect answer to students who want to get the most out of their education.
Here you will find AP Chemistry outlines and slides. We are working to add more AP Chemistry resources such as vocabulary terms, unit notes, topic notes, study questions, practice quizzes and glossary terms.
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These chemistry notes and outlines will help you study for specific chemistry topics.
See included chemistry topics below:
SI units - set of 7 basic units from which all other units are derived
prefixes of metric system
derived SI units - uses a combination of SI units
matter - physical material of the universe
states of matter - gas, liquid, or solid
pure substances - has distinct properties and doesn't vary from sample to sample
properties of matter - can be physical or chemical
separation of mixtures - possible by using the components' different properties
scientific method - guidelines for the practice of science
numerical uncertainty - measurements are ALWAYS inexact
significant figures - all digits of a quantity, including an uncertain one
dimensional analysis - guarantees that the result has the proper units
See included chemistry topics below:
atomic theory of matter - developed by John Dalton
cathode ray tubes - vacuum tube through which high voltage creates radiation
radioactivity - spontaneous emission of radiation
nuclear atom - final view of atom discovered by Rutherford
subatomic particles - determine the atom's characteristics
basic forces - 4 basic interactions in nature
isotope - elements that differ in number of neutrons
periodic table - developed in 1869
molecules - combination of 2+ atoms bound tightly together
ammonium NH4+
acetate C2H3O2-
acetic HC2H3O2
hydronium H3O+
hydrogen carbonate HCO3-
carbonic H2CO3
hypochlorite ClO-
hypochlorous HClO
phosphite PO33-
chlorite ClO2-
chlorous HClO2
phosphate PO43-
chlorate ClO3-
chloric HClO3
perchlorate ClO4-
perchloric HClO4
carbonate CO32-
bromate BrO3-
chromic H2CrO4
chromate CrO42-
hydroxide OH-
hydrobromic HBrO3
dichromate Cr2O72-
nitrite NO2-
nitrous HNO2
oxalate C2O42-
nitrate NO3-
nitric HNO3
sulfite SO32-
iodate IO3-
oxalic H2C2O4
sulfate SO42-
permanganate MnO4-
phosphorous H3PO3
peroxide O22-
cyanide CN-
phosphoric H3PO4
thiocyanate SCN-
sulfurous H2SO3
sulfuric H2SO4
hydrocyanic HCN
chemical nomenclature - naming of substances
naming positive ions
naming negative ions
naming ionic compounds
naming acids
naming binary molecular compounds
alkanes - most basic class of hydrocarbons, each carbon atom is bonded to 4 other atoms
See included chemistry topics below:
stoichiometry - used to find quantitative information about the substances in reactions
chemical equations - represents chemical reactions
combination reaction - 2+ substances react to form 1 product
decomposition reaction - 1 substance reacts to produce 2+ substances
combustion reaction - rapid reactions that produce a flame
formula weight - sum of the atomic weights in each chemical formula
Avogadro's number (mole) - number of atoms in 12g of pure carbon-12
moles to number of representative particles
number of representative particles to moles
mass (grams) to mole
moles to mass (grams)
number of representative particles to mass (grams)
mass (grams) to number of representative particles
empirical formula - tells relative number of atoms of each element in a compound
quantitative information - available from the coefficients of a balanced equation
limiting reactant - restricts how much of the excess substance can be used
See included chemistry topics below:
aqueous solution - solutions in which water is the dissolving medium
electrolytic properties - conducts electricity due to the ions floating in the solution
precipitation reaction - reactions that result in the formation of an insoluble product
soluble ionic compounds
insoluble ionic compounds
metathesis (exchange) reactions - reactions where ions exchange partners
ionic equations - sometimes useful to show if the dissolved substances are ions or molecules
acids - substances that ionize to form hydrogen ions
bases - substances that accept hydrogen ions, produce hydroxide ions in reactions
strength of acids/bases
neutralization reactions - mixing an acidic and base solution
oxidation-reduction (redox) reactions - involve transfer of electrons between reactants
oxidation number - aka oxidation state; actual chargeof the atom as a monoatomic ion
displacement reaction - ion in a solution gets replaced through oxidation of an element
activity series - list of metals arranged in order of decreasing oxidation
concentration - amount of solute dissolved in a given quantity of solvent
dilution - lowers the concentration of a solution by adding water
chemical analysis - convert to moles to find relationships between reactants/products
titration - determines concentration of a particular solute in a solution
See included chemistry topics below:
energy - ability to do work or transfer heat
internal energy - sum of all kinetic/potential energy in a system
system - area isolated for study
state function - property of system determined by its condition/state
enthalpy - describes heat flow in chemical changes
Hess's Law - DH for reaction equals sum of DH for its parts
Calculate DH for 2C(s) + H2(g) >> C2H2(g)
enthalpy of formation - aka heat of formation, DHf
Find standard enthalpy change for combustion of C6H6(l) into CO2(g) and H2O(l)
calorimetry - measurement of heat flow
Find amount of heat needed to warm 250 g of water from 22°C to 98°C
constant-pressure calorimetry - heat gained by solution same as heat lost by reaction
Find enthalpy change for reaction if temperature of solution in calorimeter changed from 21.0°C to 27.5°C when 50mL of 1.0M HCl was mixed with 50mL of 1.0M NaOH
bomb calorimetry (constant-volume calorimetry) - studies combustion reactions
Find heat of reaction for comubstion of 4.00g of CH6N2 if its combustion in a calorimeter w/ heat capacity of 7.794 kJ/ °C changes temperature from 25.00°C to 39.50°C
fuel value - energy released when 1g of material is combusted
See included chemistry topics below:
electromagnetic radiation - aka radiant energy
Planck's constant - 6.63 x 10-34 J-s
Find energy of 1 photon light w/ wavelength 589 nm
line spectra - spectrum containing radiation of specific wavelengths
Rydberg equation - allowed calculation of wavelengths of all spectral lines
Bohr's Model - electrons moving in circular paths lose energy and spiral towards nucleus
Find the de Broglie wavelength of an electron w/ velocity 5.97 x 106 m/s
matter waves - describes wave characteristics of material particles
quantum (wave) mechanics - studies w/ subatomic particles
orbitals
Pauli exlusion principle - no 2 electrons can have same set of quantum numbers (n, l, ml, ms)
Hund's rule - in degenerate orbitals, lowest energy obtained if max # of electrons have same spin
electron configuration - way electrons are distributed among atoms' orbitals
See included chemistry topics below:
periodic table development - ordered according to atomic mass by Mendeleev/Meyer
effective nuclear charge - electric field created by nucleus and surrounding electron density
atomic radii - nonbonding/bonding radius
ionization energy - measures amount of energy needed to lose an electron
ion electron configurations - electrons removed from largest available quantum number first
electron affinity - energy change when electron is added to a gaseous atom
metals - make up 3/4 of the periodic table, in left/middle part
nonmetals - on right side of periodic table
metalloids - have properties intermediate between metals/nonmetals
See included chemistry topics below:
chemical bond - attraction between atoms or ions
ionic bonding - ions held in 3D array
electron configurations of ions of representative elements
electron configurations of metal ions
covalent bonding - sharing of electron pairs
electronegativity - ability of atom in a molecule to attract electrons
dipole moment - measure of dipole’s magnitude
Calculate the dipole moment of HCl if the H and Cl are separated by 1.27Å
In units of e, what is the charge on the atoms of a compound if they're separated by 2.74Å and have a measured dipole moment of 1.97 D?
drawing Lewis structures -
formal charge - charge of an atom if all atoms had the same electronegativity
resonance structures - placement of electrons changes, but atom placement doesn’t
exceptions to octet rule -
Draw Lewis Structures for PCl3, PO33-, XeFl4, BCl3
bond enthalpy - enthalpy change for breaking of a bond
Find the DH for 2C2H6 + 7O2>> 4CO2 + 6H2O
Find the DH for N2H4 >> N2 + 2H2
See included chemistry topics below:
VSEPR model - valence-shell electron-pair repulsion model
linear electron-domain geometry
trigonal planar electron-domain geometry
tetrahedral electron-domain geometry
trigonal bipyramidal electron-domain geometry
octahedralelectron-domain geometry
bond polarity - measure of electron sharing
valence-bond theory - explains covalent bonding
hybrid orbitals - new orbitals formed by a mix of other orbitals
multiple bonds - overlap of p orbitals
molecular orbital theory - describes electrons in terms of molecular orbitals
molecular properties of electron configurations
See included chemistry topics below:
characteristics of gas -
pressure - force acted upon a given area
Boyle’s Law - pressure-volume relationship
Charle’s Law - temperature-volume relationship
Avogadro’s Law - quantity-volume relationship
ideal-gas equation - describes hypothetical gas (ideal gas)
Find the temperature of gas at which 0.407 mol takes up 3.23 L of space at 118 in Hg
gas density - unit mass per unit volume
Find the density of carbon tetrachloride at 714 torr at 125° C
Dalton ’s law of partial pressures
Find the partial pressures and total pressure of a mixture made from 6.00 g O2 and 9.00 g CH4 in a 15.0 L container at 0° C
collecting gases over water - gases produced by chemical reactions often collected over water
kinetic-molecular theory - explains behavior of gases
effusion - escape of gas molecules through a tiny opening
behavior of real gases - different than behavior of ideal gases
van der Waals equation - takes into account the gas volume and attractive forces
Find the pressure in atm that O2 exerts at 70.6° C if 1.850 moles occupies 16.5 L.
See included chemistry topics below:
3 phases - dependent on the intermolecular forces
intermolecular forces - much weaker than ionic/covalent bonds
phase changes - changes of the state of a substance
Find the enthalpy change as 10 g of a liquid at 70° C goes to a gas at 100° C
vapor pressure - pressure exerted by vapor during dynamic equilibrium
phase diagrams - graphic representation of equilibrium between phases
liquids - properties explained by intermolecular forces
solid structures - either crystalline or noncrystalline (amorphous)
bonding in solids - arrangement of particles determines melting point, hardness, etc
See included chemistry topics below:
solution process - like molecules dissolve like molecules
spontaneous solution formation - usually exothermic
crystallization - opposite of solvation
solute-solvent interactions - determines tendency of substances to mix
pressure effects - doesn’t affect liquid/solid as much as gas
temperature effects - different for gas/solid
concentration - dilute (small solute concentration), concentrated (large solute concentration)
Find the mass percentage of a KCl solution if it's supposed to be isotonic w/ a 9% NaCl solution
In a certain ore, there is 1g of Silver for every 500kg of ore. What is the concentration in parts per million? parts per billion?
Find the molality of chloride ions if 1 g of CaCl2 is dissolved in 750 mL of water
Find the molarity of H2SO4 in a 95% by mass solution if the solution's density is 1.84 g/cm3
colloids (colloidal dispersions) - in between heterogeneous mixtures and solutions
colligative properties - depends on quantity of solute, not the type
Arrange the following solutions from lowest to highest freezing point, lowest to highest boiling point, and lowest to highest vapor pressure: 0.35 m antifreeze, 0.20 m KBr, 0.20 m K2CO3, 0.12 m NaCl, 0.20 m sugar
How many grams of NaCl should be added to 3kg of water to get a water-salt solution that freezes at -10 C?
What is the boiling point of a solution w/ 44.4 g CaCl2 in 2L water?
Find the molar mass of tabitol if 2.5g of tabitol in a 100mL solution produces an osmotic pressure of 1.79atm at 25C.
See included chemistry topics below:
factors affecting reaction rates -
rate law - shows how rate depends on concentrations
first-order reaction - reaction where rate depends on concentration of single reactant
second-order reaction - reaction where rate depends on concentrations of 2 reactants
For the following data and the reaction X + Y >> Z, what is the order for X and Y?
initial X concentration
initial Y concentration
initial rate
0.200
0.200
7.50
0.400
0.200
30.00
0.200
0.800
30.00
For a second order reaction, the rate constantis 25 L/mol-s at 20 C. Find the time it takes for the concentration to go from 0.025 M to 0.010 M
For a first order reaction involving popcorn, 6 kernels pop every 5 seconds when there are 150 kernels. How long until 75 of the kernels pop?
half-life (t1/2) - time needed for concentration of reactant to drop to 1/2 or original value
Find the half-life of a substance that decomposes by 20% after 5 years.
Find the age of a piece of wood whose carbon-14 count is 35/min, when a new piece of wood has a count of 125/min.
Find the half life of a substance if 95% of it disappears after 10 years.
collision model - based on kinetic-molecular theory
activation energy (Ea) - minimum amount of energy needed for reaction to occur
reaction mechanisms - process by which reaction occurs
catalyst - substance that changes reaction rate
See included chemistry topics below:
equilibrium in reactions - when forward/reverse reactions occur at same rate
Haber Process - synthesizing ammonia from hydrogen/nitrogen
equilibrium constant - only changed by temperature, not by reaction mechanism
For the reaction CaCo3(s) >> CaO(s) + CO2(g), K = 0.0108. Find the equilibrium weight of CO2 if 2g of CaCo3, 2g of CaO, and 0.5g of CO2 were placed in a 1 liter flask.
At equilibrium for the reaction 2NO(g) + Cl2(g) >> 2NOCl, K = 51. If [NOCl] = 0.10 and [Cl2] = 0.20, find [NO]
Le Châtelier’s Principle - equilibrium position changed when outside force disturbs the system
Describe the effect on CaCO3(s) >> CaO(s) + CO2(g) when:
For reaction PCl5(g) >> PCl3(g) + Cl2(g), K = 0.015 and DH = -375. What happens when Cl2 is removed?
For endothermic equation N2(g) + O2(g) >> 2NO(g), K = 4.0 x 10-4. What happens when pressure is increased?
For endothermic equation N2(g) + O2(g) >> 2NO(g), K = 4.0 x 10-4. What happens when temperatre is increased?
See included chemistry topics below:
definition - increases the concentration of H+ ions when dissolved in water
Find the pH of a 0.001 M solution of acetic acid
Find the pH of 0.1 M solution of HCl
definition - increases the concentration of OH- ions when dissolved in water
Find the pH of 0.0030 M solution of ammonia
conjugate acid-base pairs - HX + H2O >> X- + H3O+
Find the pH for 0.25 M of sodium lactate
hydrolysis - ability of ions to react w/ water to make H+, OH- ions
See included chemistry topics below:
common-ion effect - ionization of electrolyte decreases if common ion added
Find the pH in a solution of 0.1 M lactic acid and 0.1 M sodium lactate
Find the pH of a 500mL solution containing 1.00 g propionic acid and 1.0 g sodium propionate
complex ions - made up of metal ion and Lewis base
amphoterism - able to act as acid or base
precipitation/separation of ions - occurs when product of ion concentrations > Ksp
buffered solutions - contains weak conjugate acid-base pair
If the buffer system in blood is made up of carbonic acid and sodium bicarbonate, what is the base to acid ratio if the pH is measured to be 7.41?
How many moles of NaOBr should be added to 1.00 L of 0.050 M HOBr to form a buffer w/ pH 8.80?
In a buffer of acetic acid and sodium acetate where the pH is 5, find the molarity of sodium acetate if the molarity of acetic acid is 0.10
titration - known concentration of base is added to acid (or acid to base)
Find the pH of solution formed when 45.0 mL of 0.100 M NaOH is added to 50.0 mL of 0.100 M acetic acid.
Find the pH at the equivalence point in the titration of 50.0 mL of 0.100 M acetic acid w/ 0.100 M NaOH
When titrating a 0.1 M acetic acid solution with 0.005 M NaOH, what is the pH 1/2 way through the titration?
solubility product - Ksp
Find the Ksp for a saturated solution of Mg(OH)2 if the pH is 10.17
Find the molar solubility of Mn(OH)2 if the Ksp is 1.6 x 10-13
Find the molar solubility of Ba(IO3)2 in a solution of 0.010 M NaIO3
Find the molar solubility of Ba(IO3)2 in a solution of 0.01 M NaNO3
See included chemistry topics below:
parts of atmosphere - 4 regions
atmospheric composition - made up of mostly nitrogen, oxygen
troposphere composition - like atmosphere, mostly nitrogen/oxygen
seawater - contains 97.2% of world's water, aka saline water
freshwater - amount of oxygen = quality of water
green chemistry - using chemical products that preserve the environment
water purification - water chlorination produces trihalomethanes (THM)
See included chemistry topics below:
spontaneous reaction - occurs w/o any outside intervention
Find the conditions surrounding H2O(l) >> H2O(s)
entropy - the amount of disorder in a system
Arrange the following changes from least increase in entropy to greatest increase in entropy: 1g of ice warmed by 1°, 1g of ice melted, 1g of water frozen, 1g of water evaporated.
Gibbs free energy - free energy
Find the conditions surrounding the stretching of a rubber band.
Calculate DG (in kJ) for Mg(s) + 1/2O2 >> MgO(s) at 300K
nonstandard free energy - value differs from standard value at different conditions
Calculate the Keq for 2NO2 (g) >> N2O4 (g) at 25°C
See included chemistry topics below:
oxidation-reduction reactions - oxidation states change
For the following equations, determine the oxidizing agent and reducing agent.
steps for balancing a redox reaction
Balancing MnO4-1 + Fe+2 >> Mn+2 + Fe+3
voltaic (galvanic) cells - electrons transferred through external pathway instead of directly
cell EMF (electromotive force) - aka cell potential/voltage
For the following batteries, determine the anode/cathode and voltage
effect of concentration on cell EMF - depends on Nernst equation
concentration cell - cell based on emf generated from difference in concentration
battery - portable, self-contained electrochemical power source w/ 1 or more voltaic cells
corrosion - metal converted to unwanted compound due to environment
electrolysis - nonspontaneous redox reactions started by outside energy source
See included chemistry topics below:
radioactivity - tendency to decay, emit particles
nuclear stability - depends on multiple factors
nuclear transmutations - changing the atom’s identity
Xenon-118 undergoes electron capture to become what?
Carbon-14 undergoes betay decay to produce what?
radioactive decay rates - 1st-order kinetic process
An old piece of wood has carbon-14 activity of 11.7 disintegrations per minute per gram. Current carbon-14 activity is 15.3 disintegrations per minute per gram. The half-life of carbon-14 is 5714 years. How old is that old piece of wood?
radioactivity detection - radioactivity found everywhere
nuclear fission - fragmenting heavy nuclei to generate energy
nuclear fusion - combining/fusing light nuclei
biological effects of radiation - radiation >> excitation or ionization of matter
These AP Chemistry outlines correspond to chapters of Zumdahl's Chemistry (5th Edition) textbook
Here you find AP Chemistry outlines for Zumdahl's Chemistry, 5th Edition Textbook. These will help you study for your AP Chemistry Exam or any other Chemistry test.
Additional Information:
Please click below to download the AP Chemistry outline for 'Chapter 1 - Chemical Foundations', from the Zumdahl's Chemistry, 5th Edition Textbook. These AP Chemistry notes will cover the key topics discussed in this chapter.
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Chapter 1 - Chemical Foundations | 37.66 KB |
Please click below to download the AP Chemistry outline for, 'Chapter 2 - Atoms, Molecules, and Ions', from the Zumdahl's Chemistry, 5th Edition Textbook. These AP Chemistry notes will cover the key topics discussed in this chapter.
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Chapter 2 - Atoms, Molecules, and Ions | 28.88 KB |
Please click below to download the AP Chemistry outline for, 'Chapter 3 - Stoichiometry', from the Zumdahl's Chemistry, 5th Edition Textbook. These AP Chemistry notes will cover the key topics discussed in this chapter.
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Chapter 3 - Stoichiometry | 20.8 KB |
Please click below to download the AP Chemistry outline for, 'Chapter 4 - Types of Chemical Reactions and Solution Chemistry, from the Zumdahl's Chemistry, 5th Edition Textbook. These AP Chemistry notes will cover the key topics discussed in this chapter.
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Chapter 4 - Types of Chemical Reactions and Solution Chemistry | 37.03 KB |
Please click below to download the AP Chemistry outline for, 'Chapter 5 - Gases', from the Zumdahl's Chemistry, 5th Edition Textbook. These AP Chemistry notes will cover the key topics discussed in this chapter.
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Chapter 5 - Gases | 37.89 KB |
Please click below to download the AP Chemistry outline for, 'Chapter 6 - Thermochemistry', from the Zumdahl's Chemistry, 5th Edition Textbook. These AP Chemistry notes will cover the key topics discussed in this chapter.
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Chapter 6 - Thermochemistry | 47.96 KB |
Please click below to download the AP Chemistry outline for, 'Chapter 7 - Atomic Structure and Periodicity', from the Zumdahl's Chemistry, 5th Edition Textbook. These AP Chemistry notes will cover the key topics discussed in this chapter.
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Chapter 7 - Atomic Structure and Periodicity | 151.46 KB |
Please click below to download the AP Chemistry outline for 'Chapter 8 - Bonding: General Concepts', from the Zumdahl's Chemistry, 5th Edition Textbook. These AP Chemistry notes will cover the key topics discussed in this chapter.
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Chapter 8 - Bonding: General Concepts | 60.4 KB |
Please click below to download the AP Chemistry outline for 'Chapter 9 - Covalent Bonding: Orbitals', from the Zumdahl's Chemistry, 5th Edition Textbook. These AP Chemistry notes will cover the key topics discussed in this chapter.
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Chapter 9 - Covalent Bonding: Orbitals | 78.43 KB |
Please click below to download the AP Chemistry outline for 'Chapter 10 - Liquids and Solids', from the Zumdahl's Chemistry, 5th Edition Textbook. These AP Chemistry notes will cover the key topics discussed in this chapter.
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Chapter 10 - Liquids and Solids | 47.43 KB |
Please click below to download the AP Chemistry outline for 'Chapter 11 - Properties of Solutions', from the Zumdahl's Chemistry, 5th Edition Textbook. These AP Chemistry notes will cover the key topics discussed in this chapter.
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Chapter 11 - Properties of Solutions | 43.07 KB |
Please click below to download the AP Chemistry outline for 'Chapter 12 - Chemical Kinetics', from the Zumdahl's Chemistry, 5th Edition Textbook. These AP Chemistry notes will cover the key topics discussed in this chapter.
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Chapter 12 - Chemical Kinetics | 44.69 KB |
Please click below to download the AP Chemistry outline for 'Chapter 13 - Chemical Equilibrium', from the Zumdahl's Chemistry, 5th Edition Textbook. These AP Chemistry notes will cover the key topics discussed in this chapter.
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Chapter 13 - Chemical Equilibrium | 32.62 KB |
Please click below to download the AP Chemistry outline for 'Chapter 14 - Acids and Bases', from the Zumdahl's Chemistry, 5th Edition Textbook. These AP Chemistry notes will cover the key topics discussed in this chapter.
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Chapter 14 - Acids and Bases | 49.32 KB |
Please click below to download the AP Chemistry outline for 'Chapter 15 - Applications of Aqueous Equilibria', from the Zumdahl's Chemistry, 5th Edition Textbook. These AP Chemistry notes will cover the key topics discussed in this chapter.
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Chapter 15 - Applications of Aqueous Equilibria | 159.44 KB |
Please click below to download the AP Chemistry outline for 'Chapter 16 - Spontaneity, Entropy, and Free Energy', from the Zumdahl's Chemistry, 5th Edition Textbook. These AP Chemistry notes will cover the key topics discussed in this chapter.
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Chapter 16 - Spontaneity, Entropy, and Free Energy | 31.97 KB |
Please click below to download the AP Chemistry outline for 'Chapter 17 - Electrochemistry', from the Zumdahl's Chemistry, 5th Edition Textbook. These AP Chemistry notes will cover the key topics discussed in this chapter.
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Chapter 17 - Electrochemistry | 54.4 KB |
Please click below to download the AP Chemistry outline for 'Chapter 18 - The Representative Elements: Groups 1A Through 4A', from the Zumdahl's Chemistry, 5th Edition Textbook. These AP Chemistry notes will cover the key topics discussed in this chapter.
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Chapter 18 - The Representative Elements: Groups 1A Through 4A | 65.38 KB |
Please click below to download the AP Chemistry outline for 'Chapter 21 - The Nucleus: A Chemist's View', from the Zumdahl's Chemistry, 5th Edition Textbook. These AP Chemistry notes will cover the key topics discussed in this chapter.
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Chapter 21 - The Nucleus: A Chemist's View | 39.36 KB |
Please click below to download the AP Chemistry outline for 'Chapter 22 - Organic Chemistry', from the Zumdahl's Chemistry, 5th Edition Textbook. These AP Chemistry notes will cover the key topics discussed in this chapter.
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Chapter 22 - Organic Chemistry | 61.97 KB |
Please click below to download the AP Chemistry outline for 'Chapter 23 - Amino Acid Structures', from the Zumdahl's Chemistry, 5th Edition Textbook. These AP Chemistry notes will cover the key topics discussed in this chapter.
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Chapter 23 - Amino Acid Structures | 8.79 KB |
These AP Chemistry unit notes correspond with Holt's Modern Chemistry. These unit notes, along with the AP Chemistry outlines and glossary terms can be used to prepare for the AP Chemistry exam.
These unit notes correspond with Holt's Modern Chemistry. These unit notes cover a wide variety topics that will help you prepare for the AP Chemistry Exam or any other Chemistry test.
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Unit 0 - Observations, Measurements, and Calculations | 124.54 KB |
Please click below to download the AP Chemistry unit notes for the Holt’s Modern Chemistry Textbook. These AP Chemistry unit notes will cover the key topics discussed in this unit.
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Unit 1 - Atomic Structure | 157.01 KB |
Please click below to download the AP Chemistry unit notes for the Holt’s Modern Chemistry Textbook. These AP Chemistry unit notes will cover the key topics discussed in this unit.
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Unit 2 - Electrons and Periodic Behavior | 145.62 KB |
Please click below to download the AP Chemistry unit notes for the Holt’s Modern Chemistry Textbook. These AP Chemistry unit notes will cover the key topics discussed in this unit.
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Unit 3 - Chemical Bonding and Molecular Structure | 195.34 KB |
Please click below to download the AP Chemistry unit notes for the Holt’s Modern Chemistry Textbook. These AP Chemistry unit notes will cover the key topics discussed in this unit.
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Unit 4 - Conservation of Mass and Stoichiometry | 210.17 KB |
Please click below to download the AP Chemistry unit notes for the Holt’s Modern Chemistry Textbook. These AP Chemistry unit notes will cover the key topics discussed in this unit.
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Unit 5 - Gases and Gas Laws | 144.33 KB |
Please click below to download the AP Chemistry unit notes for the Holt’s Modern Chemistry Textbook. These AP Chemistry unit notes will cover the key topics discussed in this unit.
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Unit 6 - Liquids, Solids and Solutions | 232.08 KB |
Please click below to download the AP Chemistry unit notes for the Holt’s Modern Chemistry Textbook. These AP Chemistry unit notes will cover the key topics discussed in this unit.
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Unit 7 - Kinetics and Thermodynamics | 138.88 KB |