1. States of Matter ↔ Chemical Bonding Intermolecular forces (H-bonding, dipole-dipole, London) determine physical properties. These forces arise from the electronic structure studied in Chemical Bonding. Strong H-bonding in $H_{2}O$, HF, $NH_{3}$ explains anomalously high boiling points.

2. States of Matter ↔ Thermodynamics KE = (3/2)RT links directly to internal energy (U = f/2 × RT for f degrees of freedom). Joule-Thomson effect involves enthalpy considerations. Real gas deviations affect work calculations in PV work (w = −P_ext × $\Delta V$).

3. States of Matter ↔ Electrochemistry Gas laws appear in electrochemistry: Faraday's laws give moles of gas produced, then PV = nRT gives volume at given conditions. Example: 1 F of charge liberates 1 mol of $H_{2}$ gas; find volume at 27°C, 1 atm → V = (1 × 0.0821 × 300)/1 = 24.63 L.

4. States of Matter ↔ Solutions Henry's Law (gas solubility ∝ partial pressure) uses Dalton's Law concept. Vapour pressure lowering (Raoult's Law) for solutions links to liquid state vapour pressure concepts.

5. States of Matter ↔ Kinetics Activation energy and reaction rates: Maxwell-Boltzmann distribution explains why rate increases with T — more molecules have E > E_a (activation energy) at higher T (tail of distribution extends further).

6. States of Matter ↔ Atomic Structure Atomic/ionic radii → van der Waals radius → molecular volume → 'b' constant. Polarisability (electronic cloud size) → London dispersion forces → 'a' constant. Electronegativity → H-bonding ability → high boiling points.