EXAM 2 Topics
Based on the Textbook: Chemistry, McMurry, Fay, Robinson 7e.
On Exam 2 students should be able to show that they can do the following:
Chapter 4 - Solutions
Assign oxidation numbers to atoms in a compound.
Identify redox reactions, oxidizing agents, and reducing agents.
Use the activity series to predict if a redox reaction will occur.
Use a redox titration to determine the concentration of a solute in a solution.
Chapter 5 - Periodicity and Electronic Structure of the Atom
Label the wavelength, frequency and amplitude in an electromagnetic wave and describe their meaning.
Interconvert between wavelength and frequency or wavelength, frequency and energy of electromagnetic
radiation.
Interconvert between energy of a photon and energy per mol (of photons).
Describe the photoelectric effect and explain how it supports the theory of particle-like properties of light.
Calculate the frequency or wavelength of radiation needed to produce the photoelectric effect given the work
function of a metal.
Compare the energy, wavelength and frequency of different electron transitions in the Bohr model of the atom.
Distinguish between electron transitions that emit and those that absorb energy.
Relate wavelengths calculated using the Balmer-Rydberg equation to energy levels in the Bohr model of the
atom.
Describe the deBroglie equation and why the wavelength of macroscopic objects is not observed.
Describe the Heisenberg uncertainty principle.
Identify and write valid sets of quantum numbers that describe electrons in different types of orbitals.
Identify an orbital based on its shape and describe it using a set of quantum numbers.
Visualize the nodal planes in different types of orbitals and different shells.
Assign a set four quantum numbers to specified electrons in an atom.
Write electron configurations for atoms in their ground state and draw corresponding orbital filling diagrams.
Also identify atoms from electron configurations or orbital filling diagrams.
Determine the number of unpaired electrons in an atom
Explain periodic trends in atomic radii based on shielding and trends in effective nuclear charge (Z eff).
Predict the relative size of atoms based upon their position in the periodic table.
Chapter 6 - Ionic Compounds: Periodic Trends and Bonding Theory
Write ground-state electron configurations for main group and transition metal ions and determine the number
of unpaired electrons in a transition metal ion.
Predict the relative size of anions, cations, and atoms.
Describe ionization energy an order elements from lowest to highest ionization energy.
Explain the periodic trend in ionization energy based on quantum theory.
Compare successive ionization energies for a given element and identify elements based on values of successive
ionization energies.
Describe electron affinity and compare the value of electron affinity for different elements.
Explain the periodic trend in electron affinity based on quantum theory.
Use the octet rule to predict charges on main group ions.
Write formulas for ionic compounds.
Visualize ionic compounds on the molecular level: describe the number of positive ions around each cation and
vice versa in an ionic lattice with like charges on the atoms.
Draw a Born-Haber cycle and calculate the energy of formation or the energy change associated with one of the
steps.
Based on the Textbook: Chemistry, McMurry, Fay, Robinson 7e.
On Exam 2 students should be able to show that they can do the following:
Chapter 4 - Solutions
Assign oxidation numbers to atoms in a compound.
Identify redox reactions, oxidizing agents, and reducing agents.
Use the activity series to predict if a redox reaction will occur.
Use a redox titration to determine the concentration of a solute in a solution.
Chapter 5 - Periodicity and Electronic Structure of the Atom
Label the wavelength, frequency and amplitude in an electromagnetic wave and describe their meaning.
Interconvert between wavelength and frequency or wavelength, frequency and energy of electromagnetic
radiation.
Interconvert between energy of a photon and energy per mol (of photons).
Describe the photoelectric effect and explain how it supports the theory of particle-like properties of light.
Calculate the frequency or wavelength of radiation needed to produce the photoelectric effect given the work
function of a metal.
Compare the energy, wavelength and frequency of different electron transitions in the Bohr model of the atom.
Distinguish between electron transitions that emit and those that absorb energy.
Relate wavelengths calculated using the Balmer-Rydberg equation to energy levels in the Bohr model of the
atom.
Describe the deBroglie equation and why the wavelength of macroscopic objects is not observed.
Describe the Heisenberg uncertainty principle.
Identify and write valid sets of quantum numbers that describe electrons in different types of orbitals.
Identify an orbital based on its shape and describe it using a set of quantum numbers.
Visualize the nodal planes in different types of orbitals and different shells.
Assign a set four quantum numbers to specified electrons in an atom.
Write electron configurations for atoms in their ground state and draw corresponding orbital filling diagrams.
Also identify atoms from electron configurations or orbital filling diagrams.
Determine the number of unpaired electrons in an atom
Explain periodic trends in atomic radii based on shielding and trends in effective nuclear charge (Z eff).
Predict the relative size of atoms based upon their position in the periodic table.
Chapter 6 - Ionic Compounds: Periodic Trends and Bonding Theory
Write ground-state electron configurations for main group and transition metal ions and determine the number
of unpaired electrons in a transition metal ion.
Predict the relative size of anions, cations, and atoms.
Describe ionization energy an order elements from lowest to highest ionization energy.
Explain the periodic trend in ionization energy based on quantum theory.
Compare successive ionization energies for a given element and identify elements based on values of successive
ionization energies.
Describe electron affinity and compare the value of electron affinity for different elements.
Explain the periodic trend in electron affinity based on quantum theory.
Use the octet rule to predict charges on main group ions.
Write formulas for ionic compounds.
Visualize ionic compounds on the molecular level: describe the number of positive ions around each cation and
vice versa in an ionic lattice with like charges on the atoms.
Draw a Born-Haber cycle and calculate the energy of formation or the energy change associated with one of the
steps.
