Chemistry MCAT Review
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25 Terms
Atomic number (Z)
The number of protons in an atom.
Mass number (A)
The sum of protons and neutrons in an atom.
Avogadro’s number
The number of particles in one mole of a substance, equal to 6.02 × 10²³.
Atomic weight
The weighted average of naturally occurring isotopes of an element.
Energy of the quantum (Planck relation)
E = hf.
Ground state
The lowest energy state of an atom.
Excited state
When an electron moves to a higher energy level than its normal state.
Absorption or emission
Energy difference between any two energy levels; energy of absorbed/emitted light.
Orbitals
Regions around the nucleus where electrons move.
Pauli exclusion principle
No two electrons in an atom can have the same set of four quantum numbers.
Principal quantum number (n)
Indicates the energy level and size of an orbital.
Azimuthal quantum number (l)
Describes the shape and number of subshells within an energy level.
Magnetic quantum number (mi)
Specifies the orientation of an orbital in space.
Spin quantum number (ms)
Describes the spin of an electron in an orbital.
Hund’s rule
Orbitals are filled to maximize the number of half-filled orbitals with parallel spins.
Paramagnetic
Materials with unpaired electrons attracted to a magnetic field.
Diamagnetic
Materials with all paired electrons slightly repelled by a magnetic field.
Valence electrons
Electrons farthest from the nucleus with the highest potential energy.
Metals
Elements on the left-middle of the Periodic Table, known for malleability.
Nonmetals
Elements on the right of the Periodic Table, often brittle and poor conductors.
Metalloids
Elements with properties intermediate between metals and nonmetals.
Effective nuclear charge (Zeff)
Net positive charge experienced by the outermost electron.
Ionization energy
Energy required to remove an electron from a gaseous species.
Electron affinity
Energy released when a gaseous species gains an electron.
Electronegativity
Measure of an atom's ability to attract electrons in a chemical bond.
