Chapter 3 (Orbitals) Flashcards
symbol: n
principle shell, only has positive integers, tells the orbital size and energy level, equation is 2n^2
symbol: l
orbital shape (subshell), has intergers from zero up to n-1, corresponds with orbital types
l=0 is s orbital
l=1 is p orbital
l= 2 is d orbital
l= 3 is f orbital
symbol: ml (subscript)
tells the orbital orientation, intergers from -l to +l, numbers the boxes in an energy level diagram
symbol: ms (subscript)
tells the spin orientation of the electrons, +1/2 or -1/2 depending on order of entry (first gets +1/2).
pauli exclusion principle
only two electrons of opposite spin can occupy one orbital
Heisenberg’s Uncertainty Principle
it is impossible to predict both the position AND momentum of an electron with certainty
Aufbau Principle
number of electrons in an atom is equal to the atomic number, start filling the orbital with the lowest energy
Hund’s Rule
every orbital in a subshell is occupied by one electron before any one can gain two (bus principle).
electromagnetic radiation
Waves of electric and magnetic fields moving at the speed of light through space
Frequency
The number of wave cycles that pass in a specific amount of time with the unit being hertz (Hz).
Photon
A packet or quantum of electromagnetic energy. It is the smallest possible amount.
emission spectra
A series of lines of different colours of light that are emitted by atoms of a specific element as they transition from higher energy level to a lower energy level.
ground state
The arrangement of electrons in atoms or ions with lower energy levels. The most stable state of an atom.
Excited state
When an electron temporarily occupies an energy state greater than its ground state.
Quantum/quantized
A single packet of energy that must be fully absorbed or emitted with none left over.
