General Chem Things

Gas Laws (not on sheet)

(P1)(V1) = (P2)(V2) - Boyles

(V1)(T2) = (V2)(T1) - Charles

(P1)(T2) = (P2)(T1) - Gay Lussac

(V1)(n2) = (V2)(n1) - Avogadro

Percent Composition

(part/whole)x100

Empirical formula

1. % to grams

2. grams to moles

3. divide by small

4. multiply until whole

Percent Yield

(actual / theoretical) x 100

Solubility Rules

• SNAP

  • Compounds containing sodium, nitrate, ammonium, potassium are ALWAYS soluble

Formal Charge

Valence - lone pairs (EACH ELECTRON COUNTS AS ONE (1 lone pair = 2!!!!!)) - bond (each bond counts as their own (ex. double bond = 1))

Valence - (Dots + Lines)

Coulombs Law

• Small radius and big charge = strong attraction

Henderson Hasselbalch

pH = pKa + log ([A^-]/[HA])

• [A^-] = conjugate base

• [HA] = weak acid

Faraday’s Law

q = I * t

(remember as quit)

Strong Acids

So I Brought No Clean Clothes

H₂SO₄

HI

HBr

HNO₃

HClO₃

HClO₄

Delta G equations

Standard conditions: Delta G = Delta H - T*Delta S

Nonstandard conditions: Delta G = Delta G + RTlnQ

• Thermo R = 8.314

Equilibrium: Delta G = -RTlnK

Electrochemistry: Delta G = -nFE

• n = moles

• F = Faraday’s constant (96485)

• E = cell potential

MAKE SURE DELTA S, H, G ALL HAVE MATCHING UNITS!!!!!!!!!!

Spontaneous Conditions

• Think: Both positive H and S = HIGH temp and both negative = LOW temp

  • positive = high

  • negative = low

Rate Law

rate = k [A]ⁿ[B]^m

Electrochemistry

E_cell = E_cathode - E_anode

Electrolytic Cell

HIGHER E VALUE IS FLIPPED!!!!!

(lower E value is flipped in Galvanic)

Enthalpy change (delta H)

Delta H = reactants - products

Acid/Base Titration Curves

• Strong Acid + Strong Base

  • S shaped

  • pH=7 @ equiv point

  • Low starting pH

• Strong Acid + Weak Base

  • pH<7 @ equiv point

  • Higher starting pH

• Weak Acid + Strong Base

  • S shaped

  • pH>7 @ equiv point

  • higher starting pH

• Weak Acid + Weak Base

  • gradual

Linear

• 2 electron pairs

• 0 lone pairs

• linear electron geometry

• 180 bond angle

• sp hybridization

Trigonal planar

• 3 electron pairs

• 0 lone pairs

• trigonal planar electron geometry

• 120 bond angle

• sp² hybridization

Bent

• 3 electron pairs

• 1 lone pair

• trigonal planar electron geometry

• 119 bond angle

• sp² hybridization

Tetrahedral

• 4 electron pairs

• 0 lone pairs

• tetrahedral electron geometry

• 109.5 bond angle

• sp³ hybridization

Pyramidal

• 4 electron pairs

• 1 lone pair

• tetrahedral electron geometry

• 107.5 bond angle

• sp³ hybridization

Bent

• 4 electron pairs

• 2 lone pairs

• tetrahedral electron geometry

• 105.5 bond angle

• sp³ hybridization

Trigonal bipyramidal

• 5 electron pairs

• 0 lone pairs

• trigonal planar electron geometry

• 120, 90 bond angle

• sp³d hybridization

See-saw

• 5 electron pairs

• 1 lone pair

• trigonal planar electron geometry

• 119, 90 bond angle

• sp³d hybridization

T-shaped

• 5 electron pairs

• 2 lone pairs

• trigonal planar electron geometry

• 90 bond angle

• sp³d hybridization

Linear

• 5 electron pairs

• 3 lone pairs

• trigonal planar electron geometry

• 180 bond angle

• sp³d hybridization

Octahedral

• 6 electron pairs

• 0 lone pairs

• octahedral electron geometry

• 90 bond angles

• sp³d² hybridization

Square pyramidal

• 6 electron pairs

• 1 lone pair

• octahedral electron geometry

• 90 bond angle

• sp³d² hybridization

Square planar

• 6 electron pairs

• 2 lone pairs

• octahedral electron geometry

• 90 bond angle

• sp³d² hybridization