Ch2. Atomic Structure
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Definitions
Atomic emission spectra: The characteristic line spectrum that occurs as a result of energy being released by individual elements. Coloured lines on a black background.
Atomic absorption spectra: The characteristic line spectrum that occurs as a result of energy being absorbed by individual elements. Black lines on a continuum (coloured) background.
Atomic number: Number of protons in the nucleus.
Mass number: Number of nucleons (protons and neutrons) in the nucleus
Aufbau principle: The principle that states that lowest energy levels are filled first.
Hund’s rule: Orbitals within the same sub-shell are filled singly first.
Ionization energy, first: Energy required to remove one mole of electrons from an atom in its gaseous state.
Isotopes: Atoms that contain the same number of protons but a different number of neutrons.
Orbital: A region of space around the nucleus of an atom that is occupied by a maximum of two electrons at any given time.
Pauli’s exclusion principle: electrons in single orbital must have opposite spin.
Relative abundances: The percentage of natural occurrence of an isotope of an element.
Relative atomic mass: The weighted mean of all the naturally occurring isotopes of the element relative to 12C. No units.
Valence electrons: The electrons in the highest main energy level.
•Basic concepts of atomic theory [.pdf]
•Electromagnetic spectrum [.jpg]
•Ionization energies of Sodium [.gif]
•Shapes of orbitals: s & p, d, f [.gif]
•Emission/absorption spectra [.pps]
•Quantum theory and periodicity [.pps]
Mass spectrometer [.swf]
Powers of ten [link]
