AP Chemistry Fall 2013 Final Review Chapters
You should be able to do the following:
- Calculate
- o Density
- o Significant figurations
- Define precision and accuracy
- Relate atomic structure to the model of the atom
- Classify materials in terms of element, compounds, and mixtures
- Name chemical compounds & acids
- Perform mole calculations
- Calculate empirical and molecular formula from percent composition
- Perform stoichiometric calculations including limiting reactant and percent yield
- Define the terms concentration and molarity.
- Calculate the molarity of a solution and describe how the solution is made (in DETAIL).
- Perform calculations using stoiciometry and limiting reagent problems from Unit 3, given initial amounts of reactants (or products) in terms of molarity and volume of solution.
- Know general solubility rules and prediction of precipitate production.
- Be able to write molecular or ionic equations
- Predict the products from single displacement or double displacement reaction
- Know strong vs. weak acids and bases
- Write the neutralization equation for a reaction between an acid and a base, either as a molecular equation or as a net ionic equation
- Be able to assign oxidation numbers to all elements in any compound
- Define the terms oxidation, reduction, oxidizing agent and reducing agent.
- Balance oxidation-reduction reactions in acidic or basic solutions using the method of half- reactions (ion-electron method).
- You need to know how to do dilutions and titration calculations.
- AP EQUATIONS – NET IONICS
- define the term atmospheric pressure and describe how a mercury barometer works.
- state the units for measuring pressure and carry out conversions between different pressure units.
- state the mathematical relationship for Boyle's Law and carry out calculations using the relationship.
- state the mathematical relationship for Charles' Law and carry out calculations using the relationship.
- describe one experiment that yields a value for absolute zero.
- write the ideal gas equation and define each variable.
- use the ideal gas equation to solve for any of its variables or a ratio of variables, such as denisity.
- determine the molecular weight of an unknown gas, and determine the molecular formula of that gas using that info.
- extract Boyle's Law, Charles' Law and Avagadro's Law from the ideal gas equation.
- use the ideal gas law to calculate the amount of product formed, or reactant consumed, in a chemical reaction, given the initial amount of one reactant (or product) and assuming the other reactant is in excess.
- display the relationship between Dalton's Law of partial pressures and the ideal gas equation and solve problems using Dalton's Law of partial pressures.
- state the postulates of the kinetic-molecular theory.
- explain the relationship between the temperature of a sample of gas and the kinetic energy of the particles of the gas.
- relate the macroscopic behavior of an ideal gas to the kinetic-molecular model of a gas.
- calculate relative effusion or diffusion rates of gases.
- explain the shortcomings of the ideal gas model when dealing with real gases.
- define the terms thermodynamics and thermochemistry.
- describe the difference between temperature and heat
- distinguish between the system and the surrounding in a chemical process.
- define the terms exothermic and endothermic as they apply to chemical reactions.
- define the terms specific heat and heat capacity and use both concepts to calculate heat flow.
- calculate heat flow in a coffee-cup calorimetry experiment.
- calculate heat flow in a bomb calorimeter experiment.
- state the first law of thermodynamics.
- write the mathematical equation defining the internal energy change in a chemical reaction.
- calculate the internal energy change for a chemical process in terms of heat flow and work.
- write the mathematical equation for heat flow in chemical reactions at constant volume and constant pressure.
- define the term enthalpy (H) and distinguish it from internal energy (E).
- list the important characteristics of enthalpy of a chemical reaction.
- describe and recognize state functions.
- calculate the enthalpy change in a chemical reaction using Hess's Law.
- define the term standard state as it is applied to an element or compound.
- write a chemical equation describing the formation of any compound and look up its heat of formation in table of standard heats of formation.
- calculate the enthalpy change in any chemical reaction using standard enthalpies of formation.
- define these terms: electromagnetic radiation; wave; wavelength; frequency; amplitude; and velocity.
- state the mathematical relationship between wavelength and frequency. and calculate the wavelength of light, given its frequency and the speed of light.
- define the terms quantum, quantized and photon in terms of the interaction of matter with electromagnetic radiation.
- state the mathematical relationship between energy and frequency for light and calculate the energy of photons of light at a given frequency or wavelength.
- state the postulates Bohr used to account for the experimentally observed emission spectrum of hydrogen.
- explain the importance of the principal quantum number.
- calculate the Bohr radius and the energy of an electron in the Bohr atom, given the principal quantum number.
- define the terms: excited state; ground state
- describe the properties of matter waves and calculate the wavelength of an object, given its velocity and mass.
- explain how the uncertainty principle relates to our knowledge of the properties of electrons in atoms.
- compare and contrast the Bohr model and the quantum mechanical model for describing the properties of electrons in atoms.
- define the term orbital.
- define principal quantum number, azimuthal quantum number and magnetic quantum number and describe how each of these numbers relate to the energy, shape and orientation of an electronic orbital in an atom.
- write the full set of quantum numbers for an electron in a particular energy level.
- draw a complete energy level diagram (through n = 4) for the hydrogen atom, based on the quantum mechanical model of the atom and label the diagram with the correct orbital designations.
- draw the shape of 's', 'p' and 'd' orbitals.
- define the terms effective nuclear charge and screening effect and explain how the energy of the atomic orbitals are effected by the presence of more than one electron.
- describe the electron spin quantum number.
- define and apply the Pauli exclusion principle to the process of building up a multi-electron atom.
- list the four quantum numbers associated with each electron in multi-electron atoms and write the electron configuration for any element in the periodic table.
- define and apply Hund's rule.
- define valence electrons and core electrons and distinguish between them for any element in the periodic table.
- identify the sections of the periodic table that contain s orbital, p orbital, d orbital and f orbital valence electrons.
- identify electron configurations for elements from these regions of the periodic table: alkali metals, alkaline earth metals, transition metals, chalcogen, halogen, noble gas, lanthanide and actinides.
- identify electron configurations for charged atoms and explain why they form those charges
- describe the trend in atomic radii among elements within groups and periods of the periodic table.
- describe the trend in ionization energy among elements within groups and periods of the periodic table.
- describe the trend in electron affinity among elements within groups and periods of the periodic table.
- Explain how intermolecular forces such as surface tension, capillary action, viscosity, vapor pressure, and boiling point affect the properties of liquids.
- Rank a substance in order of increasing/decreasing properties such as boiling points.
- Understand the different types of solids and know examples of each.
- Know characteristic points of heating curves and phase diagrams.
- Perform calculations with different solution concentrations such as molarity, mass percent, molality, and mole fraction.
- Discuss effects of temperature, pressure, and structure on solubility.
- Understand colligative properties such as boiling point elevation, freezing point depression, and vapor pressure lowering.
- Use colligative properties to determine the molar mass of a solute.