
Mass # and Atomic # positions on element
 mAss # on top left (pro+neut)
 Atomic # on bottom left (prot)
 (On periodic table, the atomic # is listed ontop of element)

Isotope calculating strategy
 ie: Chlorine35 and Chlorine37 are 3:1 ratio
 35(.66) + 37(.33) = atomic weight of chlorine = 32

Pauli exclusion principle
no 2 electrons in a given atom can have the same four quantum numbers

4 quantum numbers
 principal (n)
 2nd is azimuthal (angular momentum) (l)
 3rd is magnetic quantum number (ml)
 4th is spin quantum number (ms)

Spin quantum number rules
 2 electrons in SAME orbital must have opposite spins
 Electrons in diff orbitals with same ms values have parallel spins electron spin: can be +1/2 or 1/2 (have to fill orbitals with one electron first, then can pair up)

magnetic quantum number rules
possible values: can be range from l to l (for p, 1, 0, +1)

azdimuthal (angular momentum) quantum number rules
 refers to the subshells or sublevels (l)
 for value of n, subshell (l) can be from 0 to n1
 0,1,2,3, representing s,p,d,f
 max # of electrons in subshell = 4l +2

principal quantum number rules
 Max # of electrons in energy level n = 2n^2
 larger the n integer, the higher energy level and radius of electron orbit
 energy diff from 12 is greater than 23 and so on going higher up with the values of n

Bohr model
 E=hf
 h=Planck's constant (6.626 x 1034 Js)
 f = frequency of radiation

Atomic emissions spectra  energy of photons equation
 E = hc/wavelength
 h=Planck's constant
 c=speed of light (3x108m/s)

Planck's constant
6.626 x 1034 Js

Calculating energy emitted when going from n=3 to n=2
 E =  RH (1/[ni^2]  1/[nf^2])
 should be positive value due to going back towards ground state and energy is being released

Calculating energy emitted when n=2
E =  RH/n^2

Balmer vs Lyman series
 Balmer are emissions from n>2 to n=2 (4 wavelengths in visible region)
 Lyman series are from n>1 to n=1 (the UV region)

What are atoms with the same atomic number, but different atomic mass
Isotopes of each other

