MCAT Gen. Chem. Review - Ch. 1 + 2: Atomic Structure; The Periodic Table

Protons + Neutrons

Nucleus
Atomic mass unit (amu)
Atomic number (Z)
Mass number (A)
Isotopes
Atomic weight
Avogadro’s number, N_A = 6.02 × 10²³

Electrons

Electron shells
Valence electrons
Cation
Anion

Rutherford

Quanta
Energy
Planck equation (E = hf)
Planck’s constant = 6.626 × 10^-34 J × s

Bohr Model

Angular momentum of electron (L = nh/2pi)
Energy of the electron (E = -R_H/n²)
Rydberg unit of energy = 2.18 × 10^-18 J/electron
Orbit
Ground state
Excited state
AHED

Atomic Emission + Absorption Spectra

Line spectrum
Atomic emission spectrum
Lyman/Balmer/Paschen series
Absorption spectrum

Quantum Mechanical Model of Atoms

Heisenberg uncertainty principle
Pauli exclusion principle
Principal quantum number n
Shell

Azimuthal Quantum Number

Azimuthal (angular momentum) quantum number I
Subshells
Spectroscopic notation

Magnetic + Spin Quantum Number

m_I, Orbital
m_s spin quantum number
Paired electrons vs. parallel spins

Electron configuration

Aufbau principle (building-up principle)
n + I rule

Hund’s Rule

Paramagnetic
Diamagnetic
Allotrope

The Periodic Table

Periodic law
Periods
Groups and families
Valence shell + electrons
A (representative) elements
B (nonrepresentative) elements (transition, lanthanide, actinide)

Metals

Lustrous
Ductile
Malleability
Electropositivity
Oxidation states
Conductors

Nonmetals + Metalloids

Semimetals

Periodic Properties of Elements

Effective nuclear charge (Z_eff)
Noble/inert gases
Octet rule
Atomic radius
Ionic radii

Ionization Energy (IE)

Ionization potential
Endothermic process
First + second ionization energy
Active metals
Exothermic
Electron affinity
Electronegativity/Pauling electronegativity scale

Chemistry of Groups

Alkali metals
Alkaline earth metals
Chalcogens
Halogens
Noble gases
Transition metals (hydration complexes, subtraction frequencies, complementary color)