Course review
Review each learning objective in this topic, then open its concept explanation or question set.
Learning objective
• Produced when electrons in excited states return to lower energy levels • Relationship: colour, wavelength, frequency, energy across electromagnetic spectrum • Continuous vs. line spectrum
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Learning objective
• Evidence for discrete energy levels • Energy transitions to n=1, n=2, n=3 • Describe convergence at higher energies; series names are not assessed
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Learning objective
• Integer n, holds maximum 2n² electrons • Deduce maximum electrons in each main energy level
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Learning objective
• Main energy levels divided into s, p, d, f sublevels • Shapes: s orbital (spherical), three p orbitals (dumbbell) • Link sublevels to s, p, d, f blocks in the periodic table
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Learning objective
• Each orbital holds 2 electrons of opposite spin • Aufbau principle, Hund's rule, Pauli exclusion principle • Electron configurations for atoms and ions up to Z=36 • Use full, condensed, and orbital box diagrams; include Cr and Cu exceptions
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Learning objective
• Convergence limit = ionization • Trends in 1st IE across period and down group • Calculate 1st IE from spectral data (wavelength/frequency)
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Learning objective
• Provide information about electron configuration • Deduce element's group from successive IE data
Start with the concept explanation, then practise to create mastery evidence.