Chemistry: Review for Second Semester Exam
Atomic Structure: Students will:
 Identify the main attributes of the currently accepted model of the atom.
 Identify the number of protons, neutron and electrons in an element or ion.
 Construct an atomic symbol given the number of protons, neutron and electrons in an element or ion.
 Distinguish between average atomic mass and mass number.
 Calculate the average atomic mass of an element by using mass number and percent abundance of its isotopes.
 Calculate the percent abundance given the average atomic mass and mass numbers of the isotopes (only 2 stable isotopes).
 Explain why certain elements are radioactive using the concepts of nuclear stability.
 Identify alpha, beta, and gamma particles
 Write a nuclear decay equation for a given radioactive isotope.
Electron Configurations: Students will:
 Identify light as a wave that has specific energy.
 Explain how electrons change energy states in an atom by absorbing or emitting light.
 Identify the ground state as the lowest energy location of electrons in an atom or ion.
 Identify the principle energy levels, sublevels and orbitals for an electron configuration of an atom or ion.
 Draw an orbital diagram for the highest principle energy level in any atom or ion using the 3 rules (Aufbau, Pauli
Exclusion, Hund's rule).
 Determine the number of unpaired electrons in an electron configuration of an atom or ion.
 Determine the number of valence electrons in an atom or ion.
 Write a complete electron configuration for any atom or ion using the 3 rules (Aufbau, Pauli Exclusion, Hund's rule).
 Write an abbreviated electron configuration for any atom or ion using the 3 rules (Aufbau, Pauli Exclusion, Hund's rule).
Periodic Trends: Students will:
 Interpret a graph of atomic trends compared to atomic number.
 Define effective nuclear charge.
 Describe the shielding effect.
 Explain how effective nuclear charge and shielding effect determine atomic/ionic radius.
 Explain how effective nuclear charge and shielding effect determine electronegativity.
 Explain how effective nuclear charge and shielding effect determine ionization energy.
 Compare elements and their reactivity based on atomic trends (atomic/ionic radius, electronegativity, ionization energy).
 Identify the named groups on the periodic table (Alkali, Alkaline Earth metals, Transition metals, Halogens, Noble gases).
 Arrange elements on the periodic table (s and p block) based on their atomic trends and group names.
Chemical Bonding: Students will:
 Describe the distinguishing characteristics of an ionic bond.
 Define cation, anion, polyatomic ions.
 Describe the distinguishing characteristics of a covalent bond.
 Compare and contrast the properties of ionic and covalent compounds.
 Relate the atomic trends to the number of valence electrons.
 Use the atomic trends to explain ionic charges and the octet rule.
 Use the knowledge of electron configurations to explain the formation of ionic and covalent bonds.
Molecular Shapes: Students will:
 Construct Lewis structures for small molecules (single central atom).
 Identify the common shapes of small molecules (tetrahedral, pyramidal, bent (v-shaped), linear, trigonal planar).
 Interpret a Lewis structure to determine the 3-dimensional shape of a molecule.
 State the VSEPR theory.
 Apply the VSEPR theory to explain the 3-dimensional shape of a molecule.
 Apply the VSEPR theory to predict bond angles of various molecules.
 Determine the polarity of a covalent bond using the difference in electronegativity between the bonded atoms.
 Predict the polarity of a molecule using the symmetry of its bonds and unshared pairs around the central atom.
Condensed Matter (Solids and Liquids): Students will:
 State the kinetic molecular theory.
 Define the different types of intermolecular forces (dispersion, dipole-dipole, hydrogen bonding) affecting covalent
compounds.






Explain how the kinetic-molecular theory and intermolecular forces account for the physical properties of liquids and
solids. (state of matter, M.P., B.P.)
Define viscosity and surface tension.
Relate viscosity and surface tension to intermolecular forces.
Compare crystalline and amorphous substances.
Explain what is happening to a substance on the macroscopic scale when it is heated (heating curve).
Explain what is happening to a substance on the microscopic scale when it is heated (intermolecular forces, kinetic and
potential energy changes on a heating curve).
Gases: Students will:
 Describe the kinetic molecular theory of gases (6 postulates).
 Describe what causes gas pressure and identify the units used to measure it.
 Define STP.
 Define the variables of temperature, pressure, volume, and quantity (moles) in terms of gas behavior.
 Explain how temperature, pressure, volume, and quantity (moles) of gas are related using the terms directly and inversely
proportional.
 Perform calculations using Boyle’s, Charles’, Gay-Lussac’s, Combined, Ideal and Avogadro’s gas laws.
 Calculate the density of gases at different temperatures and pressures.
 Calculate the molar mass of a gas given the mass, volume, temperature and pressure.
 Label a phase diagram including the states of matter, phase changes, and triple point.
 Interpret a phase diagram.
Solutions and Solubility: Students will:
 Define the terms: solvent, solute, solution, electrolytes, and alloy
 Define the terms: saturated, unsaturated, and supersaturated solutions
 Interpret a solubility curve in terms of saturation, temperature and pressure.
 Describe the process of dissolving.
 Identify factors that affect the rate of dissolving.
 Define and calculate molarity and molality.
 Calculate the concentration of a solution when it has been diluted.
 Describe the factors that affect solubility.
 Use the polarity of a solute to determine if it will dissolve in a given solvent.
 Define colligative properties of a solvent. (boiling point elevation and freezing point depression).
 Explain how concentration affects colligative properties.
 Calculate the boiling point elevation or the freezing point depression of a solution. (ionizing and non-ionizing solutes)
Equilibrium: Students will:
 Define an equilibrium reaction.
 Write an equilibrium expression for any reversible reaction.
 Calculate the equilibrium constant for a given reversible reaction.
 Determine if products or reactants are favored given the equilibrium constant.
 Identify the stresses that affect the equilibrium of a reaction (temperature, concentration, pressure).
 State Le Chatlier's Principle.
 Determine the effect a stress has on the position of equilibrium by applying Le Chatlier's Principle.
Acids and Bases: Students will:
 Identify common physical and chemical properties of acids and bases.
 Compare the Arrhenius definitions to the Brønsted-Lowry definitions for acids and bases.
 Identify the acid, base, conjugate acid, and conjugate base in a reaction.
 Define a salt and how it is produced by a neutralization reaction.
 Distinguish between strong and weak when referring to acid/bases.
 List the 6 strong acids (HCl, HBr, HI, HNO3, HClO4, H2SO4) and 6 strong bases (hydroxides of Li, Na, K, Ca, Sr, Ba).
 Write the dissociation reaction equations for acids/bases in water.
 Write the Ka/Kb expressions from acid/base dissociation reactions in water.
 Identify the ion concentrations in pure water and relate to K w.
 Perform calculations involving concentrations of hydronium/hydroxide ions and pH/ pOH.
 Calculate Ka/Kb using initial concentration of acid and pH/pOH.
 Explain what is happening in a titration between a strong acid and strong base and identify the endpoint.
 Calculate the initial concentration of an unknown strong acid/base by performing a titration.
 Describe the purpose of the indicator and how they are chosen.