Memly's AP® Chemistry Core Concepts: 300 Study Cards

300 concepts, with 40 cards naming the misreading to avoid.

300 cardsLast updated 2026-08-22

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Most of this course is a small number of ideas asked in many disguises. Coulomb's law explains atomic radius, ionization energy, electronegativity and lattice energy. Le Chatelier explains solubility in acid, the common ion effect and why a catalyst changes nothing. A state function is why Hess's law works at all. Once you can name the underlying reason, an unfamiliar comparison becomes a question you have already answered in another form. So these 300 cards are built around the reason rather than the result. 298 open with a definition, 249 add why it matters, and 40 carry an explicit warning where the usual misreading is predictable: that weak describes ionization and not concentration, that a catalyst shifts nothing, that bond energies are averages, that a negative enthalpy change does not mean fast. The weighting is 36 cards on bonding and structure, 34 on acids and bases, 32 each on atomic structure, thermodynamics and equilibrium, 30 each on stoichiometry and kinetics, 28 each on intermolecular forces and electrochemistry, and 18 on gases. Element facts and ion formulas are not here. Symbols, atomic numbers and categories live in the Periodic Table Elements deck, and formulas and charges in the Polyatomic Ions deck, so the three fit together without repeating a card. Cards are tagged by topic and sub-topic, so you can drill just equilibrium, just the rate laws, or just the titration curves. Import it and the deck joins your spaced-repetition schedule, and what you should end up with is the ability to say not only what happens but which principle makes it happen.

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What's inside

Showing 100 representative cards from the full 300-card deck.

Front	Back
Atomic number and mass number	Definition: The atomic number is the proton count and fixes the element. The mass number is protons plus neutrons for one particular atom. Why it matters: Changing neutrons gives a different isotope of the same element, while changing protons gives a different element entirely.
Mass spectrum of an element	Definition: A plot of relative abundance against mass-to-charge ratio, with one peak per isotope. Reads out: Peak position gives isotope mass and peak height gives abundance, so the average atomic mass can be calculated from the spectrum alone.
Photon energy and wavelength	Definition: Photon energy is proportional to frequency and therefore inversely proportional to wavelength. Why it matters: Shorter wavelength means higher energy, so ultraviolet photons can drive transitions that visible light cannot.
Limitations of the Bohr model	Definition: It treats electrons as travelling in fixed circular orbits at set radii. Why it matters: It predicts the hydrogen spectrum well and fails for every atom with more than one electron, because it ignores electron-electron repulsion and wave behaviour.
Aufbau principle	Definition: Electrons fill the lowest available energy subshell first. Watch out: The 4s subshell fills before 3d, but once occupied the 3d electrons are lower in energy, which is why 4s electrons are removed first on ionization.
Pauli exclusion principle	Definition: No two electrons in an atom can have the same set of four quantum numbers, so one orbital holds at most two electrons with opposite spins. Why it matters: It is the reason shells have fixed capacities rather than accepting unlimited electrons.
Noble gas shorthand	Definition: Replacement of the inner configuration by the preceding noble gas in brackets, followed by the remaining electrons. Why it matters: What follows the bracket is the valence portion, which is the part that governs chemistry.
Valence electrons	Definition: The electrons in the outermost shell, which take part in bonding. Why it matters: For main group elements the count matches the group, which is why elements in one column behave alike.
Effective nuclear charge	Definition: The net positive pull an outer electron feels, reduced from the full nuclear charge by shielding from inner electrons. Why it matters: It rises across a period and stays nearly constant down a group, which is the single idea most periodic trends rest on.
Ionic radius	Definition: The size of an ion, which differs from the neutral atom. Trend: Cations are smaller than their parent atoms because a shell is often lost entirely, and anions are larger because added electrons increase repulsion.
Irregularities in ionization energy	Definition: Small dips where a new subshell begins and where a subshell first pairs electrons. Why it matters: The dips are evidence for subshell structure, which a smooth trend based on nuclear charge alone would not produce.
Electronegativity	Definition: The tendency of an atom in a bond to draw the shared electrons toward itself. Trend: Rises across a period and falls down a group, with fluorine the highest. Watch out: Values come from a scale rather than a direct measurement, so different scales give slightly different numbers.
Ionic bonding	Definition: Electrostatic attraction between oppositely charged ions formed by electron transfer, typically between a metal and a nonmetal. Why it matters: The attraction extends in all directions through a lattice rather than between one pair, which is why ionic compounds have no molecules.
Metallic bonding	Definition: Cations in a fixed array surrounded by electrons free to move throughout the structure. Why it matters: Mobile electrons explain conductivity, and non-directional bonding explains why metals deform rather than shatter.
Bond length and bond strength	Definition: The distance between bonded nuclei, and the energy required to break the bond. Relationship: Shorter bonds are stronger, because the nuclei and the shared electrons are closer. Watch out: Tabulated bond energies are averages across many compounds, so a calculation from them is an estimate rather than an exact value.
Bond polarity versus molecular polarity	Definition: A molecule can contain polar bonds and still be non-polar overall if the bond dipoles cancel by symmetry. Example: Carbon dioxide is linear with two polar bonds that cancel, while water is bent so its bond dipoles do not. Why it matters: Geometry decides the outcome, so polarity cannot be judged from the bonds alone.
Lewis structure	Definition: A diagram showing bonding pairs and lone pairs, drawn so that the total valence electron count is conserved. Why it matters: The count comes first and the arrangement second, so a structure with the wrong total is wrong regardless of how reasonable it looks.
Formal charge	Definition: The charge an atom would carry if bonding electrons were shared equally, calculated from valence electrons minus lone pair electrons minus half the bonding electrons. Why it matters: The preferred structure keeps formal charges near zero and places any negative charge on the more electronegative atom.
Expanded octet	Definition: More than eight valence electrons around a central atom, possible from the third period onward. Why it matters: The availability of d orbitals is the usual explanation, which is why second period elements never expand.
Electron domain geometry versus molecular geometry	Definition: Electron domain geometry counts every domain, while molecular geometry describes only where the atoms sit. Why it matters: Lone pairs occupy space but are invisible in the shape name, which is why the same domain arrangement produces several molecular shapes.
Trigonal planar geometry	Definition: Three electron domains arranged in a flat triangle. Angle: About 120 degrees. With one domain a lone pair, the molecular shape becomes bent.
Trigonal bipyramidal geometry	Definition: Five electron domains, three in an equatorial plane and two axial. Why it matters: Lone pairs occupy equatorial positions because there is more room there, which is why the derived shapes are seesaw, T-shaped, then linear.
Effect of lone pairs on bond angle	Definition: Lone pairs repel more strongly than bonding pairs, compressing the angles between the remaining bonds. Why it matters: A lone pair is held by one nucleus rather than two, so it spreads out more, which is why bond angles fall slightly below the ideal value.
Sigma and pi bonds	Definition: A sigma bond has electron density along the internuclear axis from end-on overlap. A pi bond comes from side-on overlap above and below that axis. Why it matters: A single bond is one sigma, a double is one sigma and one pi, and a triple is one sigma and two pi.
Molecular orbital theory	Definition: A model in which atomic orbitals combine into orbitals belonging to the whole molecule. Why it matters: It explains properties the Lewis picture cannot, most obviously why oxygen is attracted into a magnetic field.
Paramagnetism and diamagnetism	Definition: A paramagnetic substance has unpaired electrons and is attracted into a magnetic field. A diamagnetic one has all electrons paired and is weakly repelled. Why it matters: It is an experimental test of electron pairing, which is how molecular orbital predictions are checked.
Alloys	Definition: A mixture of metals, either substitutional with similar-sized atoms replacing one another or interstitial with small atoms filling gaps. Why it matters: Disrupting the regular array makes layers harder to slide, so alloys are generally harder than the pure metal.
Types of crystalline solid	Definition: Ionic, metallic, network covalent, and molecular solids, distinguished by what holds the particles together. Why it matters: Melting point and conductivity follow directly from the category, so classifying the solid predicts both.
Intermolecular versus intramolecular forces	Definition: Intramolecular forces are the bonds within a molecule. Intermolecular forces act between separate molecules. Why it matters: Boiling breaks intermolecular forces only, which is why boiling points are far lower than bond energies and why a substance keeps its identity when it boils.
Dipole-dipole forces	Definition: Attraction between the permanent partial charges of polar molecules. Why it matters: They act in addition to dispersion, so a polar molecule generally boils higher than a non-polar one of similar size.
Ion-dipole forces	Definition: Attraction between an ion and the oppositely charged end of a polar molecule. Why it matters: It is what dissolves an ionic solid in water, since the released energy offsets the lattice energy that must be overcome.
Boiling point and intermolecular forces	Definition: Boiling occurs when vapour pressure equals the external pressure, which requires enough energy to separate particles. Why it matters: Stronger intermolecular forces raise the boiling point, so comparing boiling points is a way of comparing those forces.
Heat of fusion and heat of vaporization	Definition: The energy required to melt or to vaporize a given amount of substance at its transition temperature. Why it matters: Vaporization takes far more energy than fusion, because melting only loosens the particles while vaporizing separates them completely.
Like dissolves like	Definition: Substances dissolve best in solvents whose intermolecular forces resemble their own. Why it matters: Solution forms when solute-solvent attractions repay the energy of separating solute and solvent particles, so mismatched forces do not repay it.
Henry's law	Definition: The solubility of a gas is proportional to its partial pressure above the liquid. Why it matters: It explains why a carbonated liquid releases gas when the container is opened and the pressure above it drops.
Molality	Definition: Moles of solute per kilogram of solvent. Why it matters: Mass does not change with temperature, so molality is used where temperature varies, as in freezing and boiling point calculations.
Dilution relationship	Definition: Moles of solute are unchanged on dilution, so concentration times volume before equals concentration times volume after. Why it matters: Only the solvent is added, so the relationship follows from conservation of solute rather than being a separate rule.
Freezing point depression	Definition: The lowering of freezing point when a solute is present. Why it matters: Solute particles disrupt the ordered arrangement the solid requires, so more energy must be removed before it can form.
Saturated, unsaturated and supersaturated	Definition: A saturated solution is at equilibrium with undissolved solute. An unsaturated one can dissolve more. A supersaturated one holds more than the equilibrium amount and is unstable. Why it matters: A supersaturated solution crystallizes suddenly when disturbed, because it was never at equilibrium.
Distillation	Definition: Separation of a mixture by differences in boiling point, vaporizing one component and condensing it separately. Why it matters: It works because vapour above a mixture is richer in the more volatile component, so intermolecular forces are what make the separation possible.
The mole	Definition: The amount of substance containing a fixed number of particles, defined by the Avogadro constant. Why it matters: It links a countable number of particles to a mass that can be weighed, which is what makes stoichiometry possible.
Molar mass	Definition: The mass of one mole of a substance, numerically equal to its formula mass in atomic mass units. Why it matters: It is the conversion factor between grams and moles, which is the first step of most calculations.
Molecular formula	Definition: The actual number of each kind of atom in one molecule, a whole-number multiple of the empirical formula. Why it matters: Finding the multiplier requires the molar mass, which is why empirical data alone cannot give it.
Significant figures in calculation	Definition: Multiplication and division keep the fewest significant figures of the inputs, while addition and subtraction keep the fewest decimal places. Watch out: Exact counts and defined constants do not limit the result, so they are treated as having unlimited precision.
Limiting reactant	Definition: The reactant that runs out first and therefore sets how much product can form. Why it matters: It is identified by comparing available moles against the mole ratio, not by comparing masses or by which is present in smaller amount.
Theoretical and percent yield	Definition: Theoretical yield is the maximum from the limiting reactant. Percent yield is actual divided by theoretical, times one hundred. Why it matters: Yields fall short through incomplete reaction, competing reactions, and losses in handling, so a value near one hundred indicates a clean process rather than a careful measurement.
Equivalence point versus endpoint	Definition: The equivalence point is where stoichiometrically equal amounts have reacted. The endpoint is where the indicator changes. Why it matters: They are close but not identical, and the difference is a source of systematic error.
Precipitation reaction	Definition: A reaction in which two solutions combine and an insoluble solid forms. Why it matters: Whether a precipitate forms is predicted from solubility patterns, so the ions present decide the outcome rather than the compounds added.
Oxidation number rules	Definition: A bookkeeping charge assigned by convention, with elements at zero, monatomic ions at their charge, oxygen usually at minus two, and hydrogen usually at plus one. Watch out: Peroxides and metal hydrides break the usual oxygen and hydrogen assignments.
Oxidizing and reducing agents	Definition: The oxidizing agent is reduced and causes oxidation. The reducing agent is oxidized and causes reduction. Watch out: Each is named for what it does to the other, so the agent undergoes the opposite change to its name.
Combustion reaction	Definition: Reaction with oxygen releasing energy, with complete combustion of a hydrocarbon giving carbon dioxide and water. Why it matters: Incomplete combustion gives carbon monoxide or soot instead, so the products report how much oxygen was available.
Single and double replacement	Definition: Single replacement has one element displacing another from a compound. Double replacement exchanges the partners of two compounds. Why it matters: Single replacement is always redox because an element changes oxidation state, while double replacement usually is not.
Kinetic molecular theory	Definition: Gas particles are in constant random motion, occupy negligible volume, exert no forces between collisions, and collide elastically, with average kinetic energy proportional to absolute temperature. Why it matters: Every gas law follows from these assumptions, so departures from ideal behaviour are departures from one of them.
Boyle's law	Definition: At constant temperature and amount, pressure and volume are inversely proportional. Why it matters: Halving the volume doubles the collision frequency with the walls, so the relationship follows from the model rather than being an empirical accident.
Avogadro's law	Definition: At the same temperature and pressure, equal volumes of gases contain equal numbers of particles. Why it matters: It makes volume ratios equal to mole ratios for gases, so a balanced equation gives volume relationships directly.
Ideal gas constant	Definition: The proportionality constant in the ideal gas law, whose numerical value depends on the units chosen for pressure and volume. Watch out: Using a value whose units do not match the data is the most common error, so check the pressure unit before substituting.
Dalton's law of partial pressures	Definition: The total pressure of a gas mixture is the sum of the pressures each gas would exert alone. Why it matters: It follows from particles not interacting, so each gas behaves as if the others were absent.
Collecting a gas over water	Definition: The measured pressure includes water vapour, so the vapour pressure of water at that temperature is subtracted to get the pressure of the dry gas. Why it matters: Omitting the correction overstates the amount of gas collected, and the size of the error grows with temperature.
Molecular speed and molar mass	Definition: At a given temperature, average kinetic energy is the same for all gases, so heavier molecules move more slowly. Why it matters: Equal kinetic energy with unequal mass forces unequal speed, which is the basis of both effusion and diffusion differences.
Reaction rate	Definition: The change in concentration of a reactant or product per unit time. Why it matters: Rate is defined as a positive quantity, so a reactant's rate of change carries a negative sign that is removed by convention.
Molecular orientation in collisions	Definition: The requirement that colliding particles meet in a geometry allowing the new bonds to form. Why it matters: It is why complex molecules react more slowly than energy considerations alone would predict.
Rate law	Definition: An equation giving rate as the rate constant times reactant concentrations each raised to an experimentally determined power. Watch out: The exponents come from experiment, not from the coefficients in the balanced equation, and the two agree only for an elementary step.
First-order reaction	Definition: Rate proportional to the first power of the concentration. Reads out: A plot of the natural logarithm of concentration against time is linear. Why it matters: Its half-life is constant regardless of starting concentration, which is unique to first order.
Half-life and reaction order	Definition: The time for concentration to fall by half, which depends on order. Why it matters: Only for first order is it constant. For zero order it shortens as reaction proceeds and for second order it lengthens.
Catalyst	Definition: A substance that increases reaction rate by providing an alternative pathway with a lower energy barrier, and is not consumed overall. Watch out: It changes the rate in both directions equally and does not shift the position of equilibrium or change the overall energy released.
Molecularity	Definition: The number of particles taking part in one elementary step, described as unimolecular, bimolecular, or termolecular. Why it matters: Three particles colliding simultaneously is very improbable, so termolecular steps are rare and mechanisms are built from one- and two-particle steps.
System and surroundings	Definition: The system is the part under study. The surroundings are everything else that can exchange energy with it. Why it matters: Signs are written from the system's point of view, so energy leaving the system is negative even though the surroundings gain it.
Heat versus temperature	Definition: Heat is energy transferred because of a temperature difference. Temperature measures average kinetic energy per particle. Why it matters: A large object at low temperature can hold more energy than a small one at high temperature, so the two are not interchangeable.
State function	Definition: A property depending only on the current state, not on how it was reached. Examples: Enthalpy, entropy, free energy, internal energy, temperature and pressure. Heat and work are not state functions. Why it matters: Path independence is what allows Hess's law to work at all.
Manipulating thermochemical equations	Definition: Reversing an equation reverses the sign of its enthalpy change, and multiplying an equation multiplies the change by the same factor. Why it matters: These two operations are what make Hess's law usable, since given equations rarely appear in the needed direction.
Entropy as dispersal of energy	Definition: A measure of how many ways the energy of a system can be arranged among its particles. Why it matters: More available arrangements means higher entropy, which is why the idea is described as dispersal rather than simply disorder.
Third law of thermodynamics	Definition: A perfect crystal at absolute zero has zero entropy. Why it matters: It is what provides the fixed reference point that makes absolute entropy values possible.
Enthalpy and entropy combinations	Definition: Negative enthalpy with positive entropy is favoured at all temperatures, and the reverse is never favoured. Mixed cases depend on temperature. Why it matters: Only the two mixed cases have a crossover temperature, so those are the ones where heating or cooling changes the answer.
Free energy away from standard conditions	Definition: The actual free energy change depends on the reaction quotient as well as the standard value. Why it matters: A reaction with a positive standard value can still proceed forward if the reactant concentrations are high enough, which is how unfavourable steps run in practice.
Dynamic equilibrium	Definition: A state in which forward and reverse reactions continue at equal rates, so concentrations no longer change. Watch out: Equal rates, not equal concentrations, and the reactions have not stopped.
Magnitude of the equilibrium constant	Definition: A large value means products dominate at equilibrium and a small value means reactants do. Watch out: It says nothing about how fast equilibrium is reached, which is a kinetic question.
Manipulating equilibrium expressions	Definition: Reversing a reaction inverts its constant, multiplying by a factor raises the constant to that power, and adding reactions multiplies their constants. Why it matters: These rules are the equilibrium counterpart of Hess's law for enthalpy.
Effect of adding an inert gas	Definition: Adding an unreactive gas at constant volume raises total pressure but does not shift the equilibrium. Why it matters: Partial pressures of the reacting species are unchanged, so the quotient is unchanged.
Solubility product	Definition: The equilibrium constant for a slightly soluble ionic solid dissolving into its ions. Watch out: The solid does not appear in the expression, so the constant contains only the ion concentrations raised to their coefficients.
Common ion effect	Definition: The solubility of a salt falls when a solution already contains one of its ions. Why it matters: The constant is unchanged, so raising one ion concentration forces the other down and less solid dissolves.
Complex ion formation and solubility	Definition: A ligand binding the metal ion lowers its free concentration, allowing more solid to dissolve. Why it matters: It is another way of removing a product, which is why solubility can be increased without changing temperature.
Coupled equilibria	Definition: Two equilibria sharing a species, so a change in one shifts the other. Why it matters: The overall constant is the product of the individual constants, which is how a very unfavourable step can be pulled forward by a favourable one.
Arrhenius acid and base	Definition: An acid produces hydrogen ions in water and a base produces hydroxide ions. Why it matters: It is the narrowest of the three definitions, since it applies only in aqueous solution and only to substances containing those ions.
Conjugate acid-base pair	Definition: Two species differing by one proton. Why it matters: Every proton transfer produces two such pairs, so identifying them is the first step in analysing any acid-base equation.
Weak acid	Definition: An acid that ionizes only partly, establishing an equilibrium with its conjugate base. Watch out: Weak describes the extent of ionization, not the concentration, so a concentrated weak acid is entirely possible.
Acid strength and conjugate base strength	Definition: The stronger an acid, the weaker its conjugate base. Why it matters: The conjugate base of a strong acid has effectively no basic character, which is why a salt of a strong acid does not make a solution basic.
Autoionization of water	Definition: Water transfers a proton between its own molecules, producing small equal amounts of hydronium and hydroxide. Why it matters: It is why pure water conducts slightly and why hydroxide is present even in acidic solution.
pOH and its relationship to pH	Definition: The negative logarithm of the hydroxide concentration, with pH and pOH summing to a constant at a given temperature. Why it matters: It lets a base problem be solved in hydroxide terms and converted at the end rather than working in hydronium throughout.
pKa	Definition: The negative logarithm of the acid dissociation constant. Why it matters: A lower value means a stronger acid, so the direction is opposite to that of the constant itself. Watch out: Tabulated values vary slightly between sources and with conditions, so use the value a question supplies.
Base dissociation constant	Definition: The equilibrium constant for a weak base accepting a proton from water. Why it matters: The expression contains hydroxide rather than hydronium, so the calculation gives pOH first.
Salt hydrolysis	Definition: Reaction of a salt's ions with water, producing an acidic or basic solution. Why it matters: The ions are conjugates of the acid and base that formed the salt, so their strengths determine the result.
Choosing a buffer	Definition: A buffer works best when the pKa of its weak acid is close to the target pH, so the ratio of the two components is near one. Why it matters: Far from that ratio one component runs out quickly, so capacity is lost in one direction first.
Oxidation and reduction at electrodes	Definition: Oxidation is loss of electrons and reduction is gain, occurring at separate electrodes connected by a circuit. Why it matters: Separating the halves is what forces the electrons through an external path where their flow can be used.
Salt bridge	Definition: A connection allowing ions to move between half cells to maintain electrical neutrality. Why it matters: Without it charge builds up in each compartment and current stops almost immediately, so it completes the circuit rather than merely joining the containers.
Standard reduction potential	Definition: The potential of a half reaction written as a reduction, measured against the reference electrode under standard conditions. Why it matters: A more positive value means a greater tendency to be reduced. Watch out: Values come from a table and depend on the conditions and conventions used, so take them from the reference a question provides.
Effect of concentration on cell potential	Definition: Cell potential shifts from its standard value as concentrations depart from standard, in the direction that the reaction quotient predicts. Why it matters: Raising a reactant concentration raises the potential, which is the same Le Chatelier reasoning applied to a cell.
Faraday constant	Definition: The electric charge carried by one mole of electrons. Why it matters: It converts between charge measured in the circuit and moles of electrons transferred, which is the link between electrical and chemical quantities.
Electroplating	Definition: Depositing a thin metal layer onto an object made the cathode of an electrolytic cell. Why it matters: The thickness is controlled by the total charge passed, so time and current together set the amount deposited.
Fuel cell	Definition: A galvanic cell supplied continuously with reactants from outside rather than holding them internally. Why it matters: It does not run down as its electrodes are not consumed, so operation is limited by supply rather than by capacity.
Intensive and extensive properties in cells	Definition: Cell potential is intensive and does not change when a half reaction is multiplied. Free energy and charge are extensive and do. Why it matters: It is why balancing electrons changes the free energy calculation but never the potential.

Frequently asked

How does it fit with the Periodic Table and Polyatomic Ions decks?

They sit underneath it and share no cards. The Periodic Table deck gives each element its symbol, atomic number, category, group and period. The Polyatomic Ions deck gives formulas and charges. This deck is the reasoning built on top of those: why the radius trend runs the way it does, why a lattice energy is large, why a salt solution turns out acidic.

What is on each card?

A concept on the front. On the back, a definition on 298 of the 300, then on 249 the reason it matters, most often the principle a question would actually turn on. 40 cards add an explicit warning where the common misreading is predictable. Each line is labeled, so the back reads as a short structured answer rather than a paragraph.

Which topics get the most cards?

Bonding and structure 36, acids and bases 34, then atomic structure, thermodynamics and equilibrium at 32 each, stoichiometry and kinetics at 30 each, intermolecular forces and electrochemistry at 28 each, and gases 18. The weighting follows where the reasoning is hardest rather than where the content is longest to list.

Why are there no bond energy or reduction potential tables in it?

Because those values differ between sources and reference conditions, and an exam supplies them anyway. A card quoting one number would be wrong for anyone using a different table. So the cards teach what the quantity means and how the calculation is set up, including which direction to subtract in, and leave the numbers to whatever reference you are given.

How is it organized for studying one topic at a time?

Every card carries a topic tag and a finer sub-topic tag, across atomic structure, bonding, intermolecular forces, stoichiometry, gases, kinetics, thermodynamics, equilibrium, acids and bases, and electrochemistry. Filter by a tag to drill one topic, or by the finer tag for a single block such as rate laws, solubility equilibria or buffers and titration.

Can I import the whole deck on the free plan?

Yes. Importing a saved deck runs no new AI generation and spends no AI credits, so the free plan imports every card. You can study, edit and delete them afterwards.

Will importing it twice create duplicates?

No. Cards you already have are skipped and only cards added in a revision come through. Including re-imports after deleting it, one official deck can be imported three times per account.

Can I edit the cards after importing?

Yes. Once imported they are your cards: edit either side, delete the ones you already know cold, retag them, or move them into another deck.