AP Chemistry Review Flashcards

This set of flashcards covers key concepts and principles from AP Chemistry, organized by units and essential definitions.

What is the formula used for dilutions in chemistry?

M1V1 = M2V2

What is the equation for gas laws relating pressure, volume, and temperature?

(P1V1)/(n1T1) = (P2V2)/(n2T2)

What should you aim for on the multiple choice section of the AP Chemistry exam?

Aim to answer 37 out of 60 questions correctly.

When you get stuck on a question in the FRQ section, what should you do?

Assume a number for the stuck part and proceed with subsequent parts.

What does the empirical formula rhyme help you with?

It helps you find the simplest whole number ratio of moles in a compound.

What is measured in mass spectroscopy?

The relative abundance of isotopes.

What does electronegativity measure?

The tendency of an atom to attract electrons.

What does each electron domain represent in VSEPR theory?

Bonds (single, double, triple) and lone pairs.

How does atomic radius change across a period?

It decreases due to increasing nuclear charge.

How do ionization energy trends change down a group?

Ionization energy decreases as the atomic radius increases.

What happens to the radius of cations compared to neutral atoms?

Cations are smaller due to less electron-electron repulsion.

What impact does the electronegativity difference have on bond polarity?

Higher difference results in more polar bonds.

What type of force do dipole-dipole interactions describe?

Intermolecular forces between polar molecules.

How do ionic compounds behave at solid versus liquid states?

Ionic compounds do not conduct electricity as solids, but do as liquids or in aqueous solution.

Define the term 'molar mass'.

The mass of one mole of a substance, typically expressed in grams per mole.

What is a resonance structure?

A way to depict the delocalization of electrons in a molecule where two or more valid structures can be drawn.

What principle does Le Chatelier's relate to?

Shifts in equilibrium when conditions such as concentration, temperature, or pressure change.

What does Hess’s Law state?

The total enthalpy change for a reaction is the sum of individual changes, regardless of the pathway taken.

What is the function of a catalyst in a reaction?

To increase the rate by lowering activation energy.

What is the primary difference between thermodynamic and kinetic control?

Thermodynamic control favors stability at equilibrium, while kinetic control favors the formation of products based on reaction rate.

What happens to the temperature during a phase change?

The temperature remains constant as the energy is used to overcome intermolecular forces.

Where do oxidation and reduction occur in a galvanic cell?

Oxidation occurs at the anode; reduction occurs at the cathode.

How do you define pH?

pH = -log[H+], where [H+] is the concentration of hydrogen ions.

What are colligative properties?

Properties that depend on the number of solute particles in a solution, not their identity.

What does the term ‘activity series’ refer to?

A list of metals ranked by their reactivity.

What type of reaction occurs when two ionic solutions form an insoluble product?

A precipitation reaction.

What defines a strong acid?

An acid that completely ionizes in solution.

How can you determine the limiting reactant in a reaction?

By comparing the mole ratio of reactants with the balanced equation.

What is a buffer solution?

A solution that resists changes in pH upon the addition of small amounts of acid or base.

What happens at the equivalence point in a titration?

The amount of titrant added is stoichiometrically equivalent to the amount of analyte.

What is the Henderson-Hasselbalch equation used for?

To calculate the pH of a buffer solution.

How do weak acids behave in solution?

They only partially ionize and exist in equilibrium.

What are the key characteristics of gases described by the ideal gas law?

They have no fixed volume or shape and are highly compressible.

What happens to solubility in the presence of a common ion?

Solubility decreases due to the common ion effect.

What does an increase in temperature favor in an endothermic reaction?

The forward reaction, as it absorbs heat.

What information can be gleaned from a reaction energy profile?

It shows the energy change throughout the reaction, including activation energy.

What does q = cm∆T compute?

The heat transferred in a calorimetry experiment.

What factors influence the speed of a chemical reaction?

Temperature, concentration, surface area, and the presence of catalysts.

What is the effect of pressure changes on gas equilibrium?

Pressure changes can shift equilibrium if there is a difference in the number of gas particles on either side.

Define enthalpy of formation.

The change in enthalpy when one mole of a compound is formed from its elements in their standard states.

What is Gibbs free energy?

A thermodynamic quantity used to predict the spontaneity of a process.

What is the general trend for entropy in chemical processes?

Entropy tends to increase with the dispersal of energy and matter.

What does it mean when ∆G is negative?

The reaction is thermodynamically favored and will occur spontaneously.

What do the letters ICE stand for in the context of equilibrium problems?

Initial, Change, Equilibrium.

What is denoted by Ksp?

The solubility product constant for a saturated solution at equilibrium.

What is vapor pressure?

The pressure exerted by a vapor in equilibrium with its liquid or solid phase.

Define a strong base.

A base that completely dissociates in water to produce OH- ions.

What does the term polarity refer to?

The distribution of electrical charge over the atoms joined by the bond.

What is the relationship between molecular weight and speed of gas molecules?

Higher molecular weight gases move slower at a given temperature.

What is oxidation in terms of electron transfer?

The loss of electrons by a substance.

What equation relates pressure, volume, and moles of a gas?

PV=nRT (Ideal gas law).

What defines the term stoichiometry?

The calculation of reactants and products in chemical reactions.

How do catalysts affect activation energy?

They lower the activation energy required for the reaction to proceed.

What does the term 'exothermic' mean?

A process that releases heat and enthalpy changes that are negative.

What is the structure of an ionic compound?

A crystal lattice formed by alternating positive and negative ions.

What information can you gather from a mass spectrum?

The relative abundance and mass of isotopes in a sample.

What does the term 'electron configuration' describe?

The distribution of electrons in an atom’s orbitals.

What is the function of a salt bridge in galvanic cells?

It maintains electrical neutrality by allowing the movement of ions.

What is the significance of Lewis structures in chemistry?

They represent the arrangement of atoms, bonds, and lone pairs in a molecule.

What does a high specific heat capacity indicate about a substance?

It requires a lot of energy to change its temperature.

What are intermolecular forces?

Forces that act between molecules, influencing physical properties.

What is the purpose of chromatography in chemistry?

To separate mixtures based on differing polarities.

How can reaction rates be affected?

By changing temperature, concentration, surface area, or adding catalysts.

What is the relationship between bond length and bond strength?

Shorter bonds are generally stronger due to greater overlap between orbitals.

When can a reaction be considered at equilibrium?

When the rate of the forward reaction equals the rate of the reverse reaction.

What does adsorption refer to in a chemical context?

The process of molecules adhering to a surface.

How does temperature influence the solubility of solids in liquids?

In general, solubility increases with temperature.

What is Boyle's law?

A principle stating that the pressure of a gas is inversely proportional to its volume at a constant temperature.

Define kinetic molecular theory.

A model that explains the behavior of gases in terms of particles in constant motion.

What is the Arrhenius equation?

An equation used to calculate the effect of temperature on reaction rates.

What does it mean for a solution to be saturated?

It contains the maximum concentration of solute that can dissolve under given conditions.

What defines an endothermic process?

One that absorbs heat, resulting in a positive change in enthalpy.

What role does water play in many chemical reactions?

It often acts as a solvent or medium for reactions.

What does the term 'dynamic equilibrium' refer to?

The state where the rates of forward and reverse reactions are equal.

What does Charles's law state?

The volume of a gas is directly proportional to its temperature in Kelvin, at constant pressure.

What safety equipment is important when conducting chemistry experiments?

Safety goggles, gloves, and lab coats.

How are the properties of acids different from bases?

Acids taste sour and turn litmus red, while bases taste bitter and turn litmus blue.

What is Le Chatelier’s principle?

If a system at equilibrium is subjected to a change, the system will shift to counteract that change.

What are specific examples of strong acids?

HCl, HNO3, H2SO4.

What is a half-life in the context of chemical reactions?

The time it takes for half of a reactant to be consumed in a reaction.

What does increasing concentration do to the rate of a reaction?

It generally increases the rate of reaction.

What does the term 'thermodynamics' refer to in chemistry?

The study of energy changes in chemical reactions.

What is the purpose of a titration?

To determine the concentration of a solution by reacting it with a standard solution.

How does pressure affect gas solubility?

Increased pressure increases the solubility of gases in liquids.

What does Gibb's free energy indicate about a reaction?

Whether a reaction is spontaneous or non-spontaneous at constant temperature and pressure.