Electronic Structure of Atoms

	6-1	Describe the wave properties and characteristic speed of propagation of radiant energy (electromagnetic radiation).
	6-2	Use the relationship (lambda)(nu)= c , which relates the wavelength (lambda) and the frequency (nu of radiant energy to its speed (c).
	6-3	Explain the essential feature of Planck's quantum theory, namely, that the smallest increment, or quantum, of radiant energy of frequency, nu, that can be emitted or absorbed is h(nu) , where h is Planck's constant.
	6-4	Explain the origin of the expression line spectra.
	6-5	List the assumptions made by Bohr in his model of the hydrogen atom.
	6-6	Explain the concept of an allowed energy state and how this concept is related to the quantum theory.
	6-7	Explain the concept of ionization energy.
	6-8	Calculate the energy differences between any two energy states of the electron in hydrogen.
	6-9	Calculate the characteristic wavelength of a particle from a knowledge of its mass and velocity (de Broglie's relationship).
	6-10	Describe the uncertainty principle and explain the limitation it places on our ability to define simultaneously the location and momentum of a subatomic particle, particularly an electron.
	6-11	Explain the concept of orbital, electron density, and probability as used in the quantum-mechanical model of the atom.
	6-12	Describe the quantum numbers, n, l, ml , used to define an orbital in an atom and list the limitations placed on the values each may have.
	6-13	Describe and draw the shape of the s, p, and d orbitals.
	6-14	Explain why electrons with the same value of the principle quantum number (n) but different values of the azimuthal quantum number (l) possess different energies.
	6-15	Explain the concept of electron spin and the electron spin quantum number.
	6-16	State the Pauli exclusion principle and Hund's rules, and illustrate how they are used in writing the electronic structures of the elements.
	6-17	Write the electron configuration for any element.
	6-18	Write the orbital block diagram representation for electron configurations of atoms.
	6-19	Describe what we mean by the s, p, d, and f blocks of elements.
	6-20	Write the electron configuration and valence electron configuration for any element once you know its place in the periodic table.

You are responsible for all material discussed in Lecture and all material
contained in the text (unless otherwise indicated) whether or not it appears here.

RETURN