Chapter 8 Key Terms Flashcards
Aufbau principle
Principle that indicates the pattern of orbital filling in an atom
Core electrons
Those electrons in a complete principle energy level and those in complete d and f subshells
Covalent radius / bonding atomic radius
In nonmetals, one half the distance of two bonded elements, in metals, one half distance between two atoms in a crystal of the metal
Degenerate
A term describing two+ orbitals with the same value of n that have the same energy
Diamagnetic
The state of an atom that contains only paired electrons, repelled by magnetic feild
Effective nuclear charge (Zeff)
Actual nuclear charge experienced by an electron - protons + inner electrons
electron affinity (EA)
Energy change associated with gaining of an electron by an atom in its gaseous state
Electron configuration
A notation that shows the orbitals that are occupied
Hund’s Rule
Principle that when electrons fill degenerate orbitals, they first fill singly with parallel spins
Ionization Energy (IE)
The energy required to remove an electron from an atom
Orbital diagram
A diagram that gives information similar to an electron configuration but symbolizes an electron as an arrow in a box representing an orbital, and the direction representing spin
Paramagnetic
An atom that contains unpaired electrons
Pauli exclusion principle
No two electrons in an atom can have the same 4 quantum numbers
Penetration
the phenomenon of some higher level orbitals having a significant amount of probability within the orbitals of lower levels
Periodic property
A property of an element that is predictable based on an element’s place on the periodic table
