Chapter 6 – Electronic Structure of Atoms

Types of electromagnetic radiation

Wavelength (λ); frequency ( γ   ) and energy related to the types of electromagnetic radiation

Units for frequency: cycles per second, s^-1, or Hz (Hertz)

Speed of light calculations (c = λ ^. γ) and placement in electromagnetic spectrum

Emission Spectra: Light as wave and particle; line spectrum vs. continuous spectrum;

quanta, photons, E= h^.  γ   (h = Planck’s constant: 6.63x10^-34J^.s)

Interpretation of the chart showing electron transitions related to energy, frequency and Wavelength of line spectra.

Limitations of the Bohr Model

Quantum Mechanical Model of the Atom:

Schrodinger’s equation tells an electron’s location within an energy state, called “probability density”, or “electron density”, or “orbitals”.

An orbital is described with 3 quantum numbers:

Principal quantum number, “n” (energy level or shell), n = 1,2,3, . . .

            Azimuthal quantum number “ℓ” (shape of the orbital or subshell)

            ℓ = 0 ... n-1;    0=s,1=p,2=d,3=f.

            Magnetic quantum number “m_ℓ” (orientation in space or one box)

m_ℓ = -ℓ. . 0 . .+ ℓ

            Spin Magnetic quantum number “m_s” (electron spin) 

m_s = +1/2 or -1/2.

Hund’s Rule (bus stop rule)

Pauli Exclusion Principle- no 2 electrons can have the same set of quantum numbers

Electron configuration notation – full and condensed (using the pervious noble gas)

Orbital notation

Electron dot notation

Valence electrons

Core electrons

Lowest energy states for electron filling

Relationship to periodic table

Predicting unpaired electrons

Assigning quantum numbers to each electron

Electron configuration for “excited” atoms