General Chemistry 2 Notes Pdf «99% RELIABLE»
Boiling Point $\propto$ Strength of IMF. 2. Solutions & Colligative Properties Molarity (M): $M = \fracmoles\ soluteL\ solution$ Molality (m): $m = \fracmoles\ solutekg\ solvent$ (Used for colligative props). Raoult’s Law (Vapor Pressure Lowering) $$P_solution = \chi_solvent \cdot P^0_solvent$$ (Where $\chi$ = mole fraction, $P^0$ = vapor pressure of pure solvent) Boiling Point Elevation ($\Delta T_b$) $$\Delta T_b = i \cdot K_b \cdot m$$ Freezing Point Depression ($\Delta T_f$) $$\Delta T_f = i \cdot K_f \cdot m$$ Osmotic Pressure ($\Pi$) $$\Pi = i \cdot M \cdot R \cdot T$$
| Type | Present in | Relative Strength | Example | | :--- | :--- | :--- | :--- | | | All molecules (temporary dipoles) | Weakest (increases with molar mass) | $F_2, CH_4$ | | Dipole-Dipole | Polar molecules | Moderate | $HCl, CH_3Cl$ | | Hydrogen Bonding | H bonded to F, O, or N | Strong (but weaker than ionic/covalent) | $H_2O, NH_3$ | | Ion-Dipole | Mixture of ions & polar molecules | Strongest (for IMF) | $NaCl$ in $H_2O$ | general chemistry 2 notes pdf