L = nh

      2Π

E = -R_H

        n²

E = hc

      λ

E = hc/λ = -R_H ( 1/n²_i - 1/n²_f)

FC = V - N_nonbonding - (1/2)N_bonding

where V = valence e^-

Equivalents = mass of compound(g)/Gram

                    equivalent weights (g)

Molarity = Normality/n

where n = number of ions produced or consumed per mole of compound in the rxn

% comp = (mass of X in formula/formula    

                   weight of compound) X 100%

rate = k[A]^x[B]^y

K_eq = [C]^c[D]^d

         [A]^a[B]^b

µ = qr

q is the charge magnitude, r is the distance between partial charges

ΔS = Q_rev

        T

where Q = heat gained or lost in a reversible process

Q_c = [C]^c[D]^d

        [A]^a[B]^b

ΔG_rxn = RT ln (Q)

                        (K_eq)

µ_rms = (3RT)^1/2

      (MM)

r₁/r₂ = (MM₂)^1/2

       (MM₁)

d = m/V = P(MM)

                 (RT) 

V/T = k or V₁/T₁ = V₂/T₂

or

V/T = nR/P

(P + n^₂a) (V - nb) = nRT

(V2)_____________

ΔG = G(g) - G(s) = 0

or 

G(g) = G(s)

In a solution dissolving A_mB_n(s) ↔ mAⁿ⁺(aq) + nB^m-(aq)

K_sp = [Aⁿ⁺]^m[B^m-]ⁿ

K_a = [H₃O⁺][A^-] 

       [HA]

K_b = [B+][OH-]

        [BOH]

pH = pKa + log [conjugate base]

                    [weak acid]

pOH = pK_b + log [conjugate acid]

                         [weak base]

E_cell = E°_cell - (RT) (ln Q)

            (nF)

ΔG° = -nFE°_cell = -RT ln K_eq

or more simply

nFE°_cell = RT ln K_eq