IndietroGeneral Chemistry Core Concepts and Formulas
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Dalton's model described atoms as indivisible spheres. Bohr's model introduced quantized electron orbits explaining hydrogen spectra.
Series include Lyman (UV), Balmer (visible), Paschen, Brackett, and Pfund (infrared), corresponding to electron transitions to different energy levels.
Calculates wavelengths of hydrogen spectral lines: \(\frac{1}{\lambda} = R \left( \frac{1}{n_1^2} - \frac{1}{n_2^2} \right)\), where R is Rydberg constant.
Energy of photon: \(E = h\nu\). Photoelectric effect shows light ejects electrons only above threshold frequency.
Particles have wave nature: \(\lambda = \frac{h}{mv}\), where m is mass and v velocity.
It is impossible to simultaneously know exact position and momentum of a particle: \(\Delta x \Delta p \geq \frac{h}{4\pi}\).
n: principal energy level; l: orbital shape; m_l: orbital orientation; m_s: electron spin (+1/2 or -1/2).
Electrons fill orbitals starting from lowest energy to higher energy levels.
No two electrons in an atom can have the same set of four quantum numbers.
Electrons occupy degenerate orbitals singly with parallel spins before pairing.
Net positive charge experienced by an electron after shielding by other electrons; calculated using Slater's rules.
Atomic radius decreases across a period and increases down a group; ionic radius depends on charge and electron configuration.
Generally increases across a period and decreases down a group; exceptions occur due to electron configurations (e.g., Be/B, N/O).
Thermodynamic cycle to calculate lattice energy of ionic compounds using Hess's law.
Predict covalent character in ionic bonds based on cation size, charge, and polarizability.
Atomic orbitals mix to form hybrid orbitals (sp, sp2, sp3, etc.) explaining molecular shapes and bonding.
Atomic orbitals combine to form molecular orbitals (bonding and antibonding); bond order predicts bond strength.
One mole contains 6.022 × 1023 entities; relates mass to number of particles.
\(PV = nRT\), relates pressure, volume, moles, gas constant, and temperature.
Total pressure of a gas mixture equals the sum of partial pressures of individual gases.
Explains gas properties based on particle motion, collisions, and energy distribution (Maxwell-Boltzmann speeds).
Limiting reagent is the reactant that runs out first; percentage yield = (actual/theoretical) × 100%.
Includes molarity (M), molality (m), normality (N), ppm, mole fraction, and % w/v.
Boyle: \(P \propto \frac{1}{V}\); Charles: \(V \propto T\); Gay-Lussac: \(P \propto T\); Avogadro: equal volumes contain equal moles.
Corrects ideal gas law for particle volume and intermolecular forces: \(\left(P + \frac{a}{V_m^2}\right)(V_m - b) = RT\).
Measure of bond polarity calculated from dipole moment and theoretical values.
Hydrogen bonding is a strong dipole-dipole interaction involving H bonded to N, O, or F; van der Waals includes dipole-induced dipole and London dispersion forces.