name the key experimental observations that led to the development of quantum mechanics

convert between velocity, kinetic energy or momentum and wavelength of a free electron (or other particle of known mass)

identify the components of the wave equation

convert between the wavelength, frequency and energy of light

calculate the allowed energy of a hydrogen-like atom of atomic number Z and quantum number n, and the wavelength of a transition between energy levels.

appreciate how the wave nature of an electron leads to discrete energy levels

draw out the electron configuration for atoms in the s-and p-blocks of the Periodic Table, including unpaired electrons

explain why the orbitals with the same principal quantum number but different angular momentum quantum numbers have different energies in multi-electron atoms

explain periodic trends in atomic radii and ionization energies in terms of quantum theory

define electron affinity and explain some features of its periodic trends in terms of electronic configurations derived from quantum theory.

Textbook and eBook References

Wave Theory of Electrons and Resulting Atomic Energy Levels -
Section 4.2

Shape of Atomic Orbitals and Quantum Numbers -
Sections 4.3 and 4.4

Filling Energy Levels in Atoms Larger than Hydrogen -
Sections 4.5 and 4.6

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Wave Theory of Electrons and Resulting Atomic Energy Levels -