Learning Targets Unit 2 Atomic Model
1. Define, apply, and distinguish among the following terms
Atom
nucleus
Protons
Neutrons
electrons
Atomic number
Atomic mass
Mass number
Isotopes
Isotopic notation
Orbital
Electron configuration
Mole
Avogadro’s number
Molar mass
Valence electrons
ion
Cation
Anion
Period
Group (family)
ionic size
alkali metals
alkaline earth metals
transition metals
noble gases
halogens
metalloids
energy level
2. Describe the atom, its parts (protons, neutrons, and electrons) and location of these
parts and their characteristics (Binder Pg 43-45)
3. Write element symbols in isotopic notation (Binder Pg 43-45)
4. Distinguish between atoms and ions (Binder Pg 43-45)
5. Figure out the atomic number, mass number, and number of electrons in an atom or
ion. (Binder Pg 43-45)
6. Describe the mole as a counting unit and state “how much” a mole is - expressed in
scientific notation (Avogadro’s number) (Binder Pg 91-93)
7. Use the periodic table to determine molar mass. (Binder Pg 91-93)
8. Perform the following calculations (using dimensional analysis and considering sig figs)
with the mole (Binder Pg 91-93)
a. Grams to moles
b. Moles to grams
9. Explain what happens when electrons absorb/release different amounts of energy
(Electron Excitation Exploration)
a. Relate the change in energy to the color of light and the electromagnetic
spectrum (Ex: The greater the energy released the higher the energy of light
emitted.)
b. Represent the process visually
10. Explain the basics of the Quantum model of the atom (current view of the atom) and
how electrons behave (Electron Configuration Packet)
a. describe what an orbital is.
b. relate the energy level number to the types of orbitals
c. relate the types of orbitals to the number of electrons allowed in each orbital
11. Write complete and short-cut electron configurations for neutral atoms using the
periodic table (Electron Configuration Packet)
12. Explain the concepts and fill out orbital box diagrams. (Electron Configuration Packet)
a. Fill lower energy levels first
b. One electron in each orbital and then go back and pair them.
c. Place electrons with opposite spins in each orbital (up and down arrows) when
two electrons are occupying the orbital
13. Locate the different families of main group elements (metals and non-metals) on the periodic
table (Binder pg. 87-90)
14. Use the periodic table to predict the number of valence electrons for a main group element.
15. Write valence electron configurations for main group metals and non-metals. (Electron
Configuration Packet)
16. Write electron configs and draw box diagrams for ions (Electron Configuration Packet)
17. Use the periodic table to determine the predictable charge of main group elements
(Binder pg. 87-90)