EAR = (1 + .127/365)^365 - 1, or 13.2% Solution EAR = (1 + .127/365)^365 - 1, or 13.2%.

1. Percent error: |actual - experimental| / actual x 100%.
AMU, atomic mass unit, is 1 / (6.022 x 10^23) = 1.66 x 10^-24. Also, the molar masses found on
the periodic table are AMUs for that specific element. Ex. Hydrogen: 1.0079 amu per atom.
There are 4 types of quantum numbers.
Principle Quantum number (n) - describes the energy level of the electron; is a whole number
between 1 and 7, corresponding with the period on the periodic table. The total number of
electron orbitals per energy level = n^2.
Angular Momentum Quantum number (l) - describes the shape of the orbital in space; is a whole
number (0, 1, 2, or 3) corresponding with the orbital types (s, p, d, f).
Magnetic Quantum Number (ml) - describes the orientation of the orbital in space. If n = 1, ml =
0 (only 1 way to orient a sphere in space); if n = 2, ml = -1, 0, +1 (corresponding to the x, y, and
z axes); if n = 3, ml = -2, -1, 0, +1, +2 (5 possible spacial orientations for d orbitals); if n = 4, ml
= -3, -2, -1, 0, +1, +2, +5 (7 orientations for f orbitals).
Spin Quantum number (ms) - describes the 2 possible directions of electron spin (+1/2, -1/2; aka
clockwise or counterclockwise)
Refer to the periodic table for names of atoms. Memorize the polyatomic ions. Rules for naming
ionic compounds: 1. Balance charges 2. Cation is always written first (in name and formula) 3.
Change ending of the anion to -ide (unless polyatomic ion, then don't change). Ex. Na2S =
sodium sulfide. Rules for naming binary covalent compounds: 1. Name the element with the
lower group first (or higher period if same group) 2. Name the second element as if an anion,
adding -ide 3. Use greek prefixes (mono, di, tri, tetra, etc) indicate the number of atoms of each
nonmetal element in the chemical formula for the compound. Ex. chlorine trifluoride: ClF3
Solution
Percent error: |actual - experimental| / actual x 100%.
AMU, atomic mass unit, is 1 / (6.022 x 10^23) = 1.66 x 10^-24. Also, the molar masses found on
the periodic table are AMUs for that specific element. Ex. Hydrogen: 1.0079 amu per atom.
There are 4 types of quantum numbers.
Principle Quantum number (n) - describes the energy level of the electron; is a whole number
between 1 and 7, corresponding with the period on the periodic table. The total number of
electron orbitals per energy level = n^2.

2. Angular Momentum Quantum number (l) - describes the shape of the orbital in space; is a whole
number (0, 1, 2, or 3) corresponding with the orbital types (s, p, d, f).
Magnetic Quantum Number (ml) - describes the orientation of the orbital in space. If n = 1, ml =
0 (only 1 way to orient a sphere in space); if n = 2, ml = -1, 0, +1 (corresponding to the x, y, and
z axes); if n = 3, ml = -2, -1, 0, +1, +2 (5 possible spacial orientations for d orbitals); if n = 4, ml
= -3, -2, -1, 0, +1, +2, +5 (7 orientations for f orbitals).
Spin Quantum number (ms) - describes the 2 possible directions of electron spin (+1/2, -1/2; aka
clockwise or counterclockwise)
Refer to the periodic table for names of atoms. Memorize the polyatomic ions. Rules for naming
ionic compounds: 1. Balance charges 2. Cation is always written first (in name and formula) 3.
Change ending of the anion to -ide (unless polyatomic ion, then don't change). Ex. Na2S =
sodium sulfide. Rules for naming binary covalent compounds: 1. Name the element with the
lower group first (or higher period if same group) 2. Name the second element as if an anion,
adding -ide 3. Use greek prefixes (mono, di, tri, tetra, etc) indicate the number of atoms of each
nonmetal element in the chemical formula for the compound. Ex. chlorine trifluoride: ClF3