Test Objectives: Atomic Structure II – The Electron

Use the Periodic Table to determine the correct number of protons & electrons in a
particular atom

Know the basic features of the Bohr model of the atom

Know what is meant by the valence level of electrons

Using the reference tables, determine the correct number of valence electrons for the
representative elements

Distinguish between valence electrons & kernel electrons (inner shell electrons)

Recognize the ground state configuration of an element

Distinguish between ground state & excited state configurations of an atom

Explain the cause of spectral lines in terms of electrons & energy levels. Spectral lines are
produced when electrons jump down from a high energy level to a low energy level

Understand that electrons absorb heat, light, or electric energy when they move to an
excited state (endothermic process) and release light energy when they return to the
ground state configuration (exothermic process)

Recognize that each line in the bright-light spectrum of an element can be used to calculate
the energy of a particular electron “jump” or transition

Understand that the bright line spectrum of an element can be used to determine if a given
element is present in a sample, by matching the spectral lines in the emission spectrum

Know how to draw Lewis Dot structures for atoms and their ions

Describe the modern model of the atom (orbital model)

Define the term principal energy level

Know the maximum number of electrons (2n2) in a given principal energy level

Know the number of sublevels for a given principle energy level

Know how many orbitals in a given sublevel

Define orbital (a region of space in the modern model that holds two electrons); know the
difference between orbit and orbital