Reading...
Play button
Play button
Use LEFT and RIGHT arrow keys to navigate between flashcards;
Use UP and DOWN arrow keys to flip the card;
H to show hint;
A reads text to speech;
16 Cards in this Set
- Front
- Back
|
Hund's rule
|
orbitals of equal enery are each occupied by one electron before any orbital is occupied by a second electron and all electrons in singly occupied orbitals have the same spin
|
|
|
highest occupied level
|
the eletron-containing main energy level with the highest principal quantum number
|
|
|
inner-shell electrons
|
electrons that are not in the highest occupied energy level
|
|
|
noble gases
|
group 18 elements
|
|
|
heisenberg uncertainty principle
|
it is impossible to deteermine simultaneously both the position and velocity of an electron or any other particle
|
|
|
noble-gas configuration
|
an outer aim energy level fully occupied, in most cases, by 8 electrons
|
|
|
quantum theory
|
describes mathematically the wave properties of electrons and other very small particles
|
|
|
angular momentum quantum number
|
symbolized by l, indicates shape of the orbital
|
|
|
magnetic quantum number
|
symbolized by m, indicates the orientation of an orbital around the nucleus
|
|
|
spin quantum number
|
2 possible values, -1/2, +1/2
which indicate the two fundamental spin states of an electron in an orbital |
|
|
electron configuration
|
arrangement of electrons in an atom
|
|
|
Aufbau principle
|
an electron occupies the lowest energy orbital that can recieve it
|
|
|
Pauli Exclusion Principle
|
no two electrons in the same atom can have the same set of four quantum numbers
|
|
|
principal quantum number
|
symbolized by n, indicates the main energy level occupied by the electron
|
|
|
quantum numbers
|
specify the properties of atomic orbitals and the properties of electrons in orbitals
|
|
|
orbital
|
three dimensional region around the nucleus that indicates the probably location of an electron
|
