|SC (9-12) Chemistry || |
3. Use the periodic table to identify periodic trends, including atomic radii, ionization energy, electronegativity, and energy levels. Utilizing electron configurations, Lewis dot structures, and orbital notations to write chemical formulas Calculating the number of protons, neutrons, and electrons in an isotope Utilizing benchmark discoveries to describe the historical development of atomic structure, including photoelectric effect, absorption, and emission spectra of elements
Example: Thompson's cathode ray, Rutherford's gold foil, Millikan's oil drop, and Bohr's bright line spectra experiments
|SC2015 (9-12) Physical Science || |
1. Use the periodic table as a model to predict the relative properties and trends (e.g., reactivity of metals; types of bonds formed, including ionic, covalent, and polar covalent; numbers of bonds formed; reactions with oxygen) of main group elements based on the patterns of valence electrons in atoms.
|SC2015 (9-12) Chemistry || |
3. Use the periodic table as a systematic representation to predict properties
of elements based on their valence electron arrangement.
a. Analyze data such as physical properties to explain periodic trends of
the elements, including metal/nonmetal/metalloid behavior, electrical/heat
conductivity, electronegativity and electron affinity, ionization energy, and
atomic-covalent/ionic radii, and how they relate to position in the periodic
b. Develop and use models (e.g., Lewis dot, 3-D ball-and-stick, space-filling, valence-shell electron-pair repulsion [VSEPR]) to predict the type of bonding and shape of simple compounds.
c. Use the periodic table as a model to derive formulas and names of ionic
and covalent compounds.