General chemistry Flashcards
E = hf = hc/wavelength
Paramagnetic: at least one unpaired electron
Diamagnetic: all paired
Chromium and copper are weird
Equations to know
Coulomb’s law
Fe = Zeff + C / r^2
Zeff= Z - core electron
Formal charge= (valence electrons) - (1/2 bonding electrons) - (lone pairs)
Geometry
Sp = linear (180 deg)
Sp2 = trigonal planar (120 deg)
AX2E = bent
Sp3 = tetrahedral (109.5 deg)
AX4 = tetrahedral
AX3E = trigonal pyramidal
AX2E2 = bent
Breaking bond = endothermic
Compounds with covalent bonds and ionic bonds = insulators
Compounds with metallic bonds, aqueous solution of an ionic compounds = conductors
Hydrogen bonds on FON
Enthalpy
Change in enthalpy = bonds broken - bonds formed
Change in enthalpy formation = nHf products - nHf reactants
Free energy equation
DeltaG = deltaH - T(deltaS)
Phase change:
Q= n(deltaH phase change)
Temp change:
q= mc (deltaT)
Solubility rules of electrolytes
Always soluble: group 1 ions, H+, NH4+, NO3-, CH3COO-, ClO4-
Usually insoluble: Ag+, Pb2+, Pb4+, (Hg2)2+, Hg2+, CO3-2, PO4-3, S-2
Ideal gas laws
- Avogadro’s law: V = n regardless of identity of gas
- Boyle’s law: P1V1= P2V2
- Charles’ law: V1/ T1 = V2/T2
- Gay-Lussac’s law: P1/ T1 = P2/ T2
Ideal gas law: 22.4L / mol and 1 atm and 273K
Real gas law
(P + an^2 / V^2)(V - nb) = nRT
A= IMF
B= size
Dalton’s law
Ptotal = sum of partial pressures
Pgas = (mole fraction)(Ptotal)
Graham’s law of diffusion/ effusion
Rate of gas 1/ rate of gas 2 = square root of molar mass of gas 2 / molar mass of gas 1
Reaction rate
Rate = (-1/r)(delta [R] / delta t) = (+1/p) (delta [P] / delta t)
Rate laws
Oth order: double concentration but same rate (M/s)
1st order: double conc and double rate (1/s)
2nd order: everything else (1/M*s)
Equilibrium constant Kc
Temp changes K
Kc or Kp = [products]^p / [reactants]^r
Partial pressures can also be used
Q= instance from equilibrium