Chem Ch. 6

Wavelength

Lambda: distance in meters

Frequency

V: repitition (Hz, 1/s, s^-1)

Relationship of wavelength and frequency

c = wavelength * frequency

Quantized energy

E = planck’s constant * frequency

Photoelectric Effect

Minimum light frequency is required for emission of one electron off a metal surface

Energy of a photon

E = (planck’s constant * speed of light) / wavelength

Absorption

Energy is absorbed (higher quanta)

Emission

Energy is emitted (lower quanta)

Spectra

Produced from absorption and emission

Orbitals

Most likely location of electron

N Quantum Number

Size and energy, can be 1,2,3, etc

L quantum number

Shape of orbital, 0 - n-1

ML quantum number

Orientation, -L - L

Spin quantum number

Determines spin, +1/2 or -1/2

S orbitals

L=0, mL= 0

P orbitals

L=1 mL=-1,0,1

D orbitals

L=2, mL=-2,-1,0,1,2

F orbitals

L=3, mL= -3,-2,-1,0,1,2,3

Pauli exclusion principle

No two electrons have the same set of quantum numbers

Hund’s rule

Spin up first then spin down

Electron configuration anomalies

D^4 and d^9 orbitals turn into d^5 and d^10 orbitals

Isoelectronic Ions

Ions become isoelectronic with a noble gas (minus charges add electrons and plus charges lose electrons)