AP Chemistry General Review

Vocabulary practice flashcards covering AP Chemistry memorization topics, including strong acids/bases, solubility rules, VSEPR molecular shapes, reaction kinetics orders, and spectroscopy/molecular motion types.

SNAP Soluble Ions

Ionic compounds containing $Na^+$ (Sodium), $NO_3^-$ (Nitrate), $NH_4^+$ (Ammonium), or $K^+$ (Potassium) are always soluble in water without exception on the AP exam.

Diatomic Elements (7-up)

The seven elements that exist naturally as homonuclear diatomic molecules: $N_2$, $O_2$, $F_2$, $Cl_2$, $Br_2$, $I_2$, and $H_2$.

Strong Acids

The seven strong acids to memorize for AP Chemistry: $HCl$ (hydrochloric acid), $HNO_3$ (nitric acid), $H_2SO_4$ (sulfuric acid), $HBr$ (hydrobromic acid), $HI$ (hydroiodic acid), $HClO_3$ (chloric acid), and $HClO_4$ (perchloric acid).

Strong Bases

The eight strong bases listed for AP Chemistry: Lithium hydroxide ($LiOH$), Sodium hydroxide ($NaOH$), Potassium hydroxide ($KOH$), Rubidium hydroxide ($RbOH$), Cesium hydroxide ($CsOH$), Calcium hydroxide ($Ca(OH)_2$), Strontium hydroxide ($Sr(OH)_2$), and Barium hydroxide ($Ba(OH)_2$).

VSEPR Model

Valence Shell Electron Pair Repulsion model, a method used to predict 3D molecular geometry and bond angles by counting electron domains (steric number) around a central atom.

Steric Number and Hybridization

The relationship between steric number (# electron domains) and orbital hybridization: 1 domain ($s$), 2 domains ($sp$), 3 domains ($sp^2$), and 4 domains ($sp^3$).

VSEPR Molecular Geometries Summary

A chart detailing molecular shapes, electron regions (2 through 6), lone pairs, and predicted bond angles across linear, trigonal planar, bent, tetrahedral, trigonal pyramid, trigonal bipyramid, see-saw, T-shaped, octahedral, square pyramid, and square planar geometries.

Zero-Order Reaction

A reaction with rate law $-\frac{d[A]}{dt} = k$ where the rate is constant and independent of reactant concentrations. The rate constant $k$ has units of $\frac{\text{M}}{\text{s}}$, and plotting $[A]$ vs. time yields a straight line.

First-Order Reaction

A unimolecular reaction with rate law $-\frac{d[A]}{dt} = k[A]$ where rate depends on the concentration of one reactant. The rate constant $k$ has units of $\frac{1}{\text{s}}$, and plotting $\text{ln}[A]$ vs. time yields a straight line.

Second-Order Reaction

A reaction with rate law $-\frac{d[A]}{dt} = k[A]^2$ or $k[A][B]$ where rate depends on one second-order reactant or two first-order reactants. The rate constant $k$ has units of $\frac{1}{\text{M}\times\text{s}}$, and plotting $\frac{1}{[A]}$ vs. time yields a straight line.

Reaction Kinetics Summary

A overview of zero-order, first-order, and second-order reactions comparing their rate laws, reactant dependencies, real-world examples, and rate constant $k$ units.

Kinetics Linear Graphs (vs. Time)

Graphical tests for reaction order against time: zero-order is linear for $[A]$, first-order is linear for $\text{ln}[A]$, and second-order is linear for $\frac{1}{[A]}$.

Translational Motion

Movement of a molecule from one place to another, causing electrons to move to different energy levels; associated with Ultraviolet (UV) and Visible light spectroscopy.

Rotational Motion

Molecular motion in which a molecule spins on one of its axes; associated with Microwave radiation.

Vibrational Motion

Molecular motion where atoms vibrate in place while keeping their relative positions within a molecule (smaller atoms tend to vibrate faster); associated with Infrared (IR) spectroscopy.

Units of Rate Constant (k)

Order-dependent units for $k$: zero-order is $\frac{\text{M}}{\text{s}}$, first-order is $\frac{1}{\text{s}}$, and second-order is $\frac{1}{\text{M}\times\text{s}}$.

Polyatomic Ion Naming Rules

Guidelines for memorizing key polyatomic ions (Nitrate, Carbonate, Chlorate, Sulfate, Chromate, Phosphate, Hydroxide, Acetate) as well as their corresponding '-ite', 'hypo-', and 'per-' ion variants.