š Key Concepts
Subatomic particles: proton (pāŗ), electron (eā»), neutron (n)Thomson's model: "Plum pudding" - electrons embedded in positive sphereRutherford's model: Nuclear model with concentrated positive chargeBohr's model: Quantized energy levels, fixed orbitsQuantum mechanical model: Probability of finding electron (orbitals)ā
šÆ Key Formulas
Energy of electron in nth orbit: En = -13.6/nĀ² eVWavelength: Ī» = h/mvde Broglie wavelength: Ī» = h/ā(2mE)Heisenberg's Uncertainty: ĪxĪp ā„ h/4ĻPrincipal quantum number (n): Energy levels (1,2,3...)Azimuthal quantum number (l): Subshell shape (0 to n-1)Magnetic quantum number (m): Orbital orientation (-l to +l)Spin quantum number (s): Electron spin (Ā±Ā½)ā
ā ļø Common Mistakes to Avoid
Confusing orbit (Bohr) vs orbital (quantum)Mixing up quantum numbers and their rangesWrong electron configurations for exceptions (Cr, Cu)Incorrect application of Aufbau principleā
š Knowledge Prerequisites
Basic atomic structureWave nature of matterElectromagnetic radiation conceptsMathematical skills for quantum numbersā
š” Tips for Students
Learn quantum number rules systematicallyMemorize electron configuration exceptionsPractice drawing orbital diagramsUnderstand rather than memorize mathematical derivationsā
š Practice Recommedations
Write electronic configurationsCalculate wavelengths using de Broglie equationDetermine quantum numbers for electronsDraw orbital diagramsSolve numerical problems on Bohr's modelā
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