Atomic and Molecular Structure

1. The periodic table displays the elements in increasing atomic number and shows
how periodicity of the physical and chemical properties of the elements relates to
atomic structure. As a basis for understanding this concept:
a. Students know how to relate the position of an element in the periodic table to its
atomic number and atomic mass.
b. Students know how to use the periodic table to identify metals, semimetals, nonmetals,
and halogens.
c. Students know how to use the periodic table to identify alkali metals, alkaline
earth metals and transition metals, trends in ionization energy, electronegativity,
and the relative sizes of ions and atoms.
d. Students know how to use the periodic table to determine the number of electrons
available for bonding.

e. Students know the nucleus of the atom is much smaller than the atom yet contains
most of its mass.
f.* Students know how to use the periodic table to identify the lanthanide, actinide,
and transactinide elements and know that the transuranium elements were
synthesized and identified in laboratory experiments through the use of nuclear
accelerators.
g.* Students know how to relate the position of an element in the periodic table to its
quantum electron configuration and to its reactivity with other elements in the
table.
h.* Students know the experimental basis for Thomson’s discovery of the electron,
Rutherford’s nuclear atom, Millikan’s oil drop experiment, and Einstein’s explanation
of the photoelectric effect.
i.* Students know the experimental basis for the development of the quantum theory
of atomic structure and the historical importance of the Bohr model of the atom.
j.* Students know that spectral lines are the result of transitions of electrons between
energy levels and that these lines correspond to photons with a frequency related
to the energy spacing between levels by using Planck’s relationship (EÊ=Ê hv).