Learning Objectives
Explain how elements are organized into the periodic table.
Locate elements based on their atomic number.
Identify the period and group in which elements are found.
Classify elements as metals, non-metals, or metalloids.
Define energy level.
Define orbital.
Determine the number of valence electrons in an atom.
Draw an electron dot structure for an atom.
Developed electron configuration pattern.
Describe the locations of electrons in an atom using an electron configuration.
Draw out Bohr-Rutherford models of the atom
Compare Bohr model (orbits) and quantum mechanical model
(orbitals) of atom (look at
filling order
PowerPoint)
terms: orbital vs. orbit; (orbitals:
s, p,
d, f-orbitals) Pauli exclusion principle
(spin-up / spin-down); Aufbau principle (filling order from bottom of atom -->
out); Hund's rule (maximum number of occupied orbitals);
Demonstration: spring to show wave nature of light
Introduce quantum mechanical model of atom
orbit vs. orbitals
an orbit is a
fixed path an electron rotates in; an orbital is a probable region in space the
electron may be found in (e.g. s- p-, d-, f-orbitals)
write out electron configuration of first 20 elements.
Show 'crutch" for filling order
ENERGY LEVELS AND SUBLEVELS Objective: To state the energy sublevels within a
given energy level.
Objective: To state the maximum number of electrons that can occupy a
given energy level and sublevel. QUANTUM MECHANICAL MODEL OF THE ATOM Objective: To list the order of sublevels
according to increasing energy.
Objective: To write the predicted electron configurations for selected
elements.