Chem - Quantum Flashcards
S sublevel
1 s orbital, 2 electrons; spherical
P sublevel
3 p orbitals, 6 electrons; 2 lobes (dumbell)
D sublevel
5 d orbitals, 10 electrons; 4 lobes (clover)
F sublevel
7 f orbitals, 14 electrons; 8 lobes
Electromagnetic Spectrum
Series of waves that travel at the speed of light
Wavelength
The distance a wave travels in 1 cycle; the distance between corresponding points on adjacent waves
Frequency
Cycles per second; number of complete waves that pass a given point per second
Amplitude
Height or depth of a wave crest or trough, related to intensity of radiation or light
Wavelength and frequency
Inversely proportional, c = lambda × nu (c = speed of light)
Blackbody radiation
A solid object emits visible light when heated to 1000K, demonstrates that energy is related to frequency and wavelength
Energy and frequency
Directly proportional, E = h × nu (h = Plank’s constant
Quantum Theory of Energy
Any object can emit or absorb only certain quantities of energy
Quantum
A fixed quantity of energy
Photoelectric effect
The emission of electrons from a material when light of certain frequencies shines on the surface of the material, there must be a minimum or threshold frequency to cause the photoelectric effect
Photon
Bundle of energy
Atomic Emission Spectrum
A set of frequencies of electromagnetic waves given off by atoms of an element when they release energy as electrons return to a non-excited state; each element gives off a characteristic pattern
Heisenberg Uncertainty Principle
It is impossible to know both the velocity and the position of a moving particle at the same time
Quantum number: n
Energy level; positive integer
Quantum number: L
Sublevel; ranges from 0 to n-1; s=0 p=1 d=2 f=3
Quantum number: mL
Orbital; ranges from -L to +L
Quantum number: ms
Spin; +/- 1/2 (upspin first)
Paulu Exclusion Principle
An orbital can hold up to 2 electrons and they must have opposite spin
Hund’s Rule
When filking orbitals of equal energy (same sublevel), each orbital receives one electron prior to pairing
Aufbau Principle
Electrons enter orbitals of lowest energy first
