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Chem 111- Unit 2

DeBroglie's wave-particule duality electrons have wave-like motion, -> only certain allowable frequencies and energies
as mass ___, wavelength ____ (DeBroglie) increases, decreases
The uncertainty principle it is impossible to know the exact position and momentum of a particle simultaneously
if uncertainty is >___, then ____ 1x10^-9, we have no idea where the electron is
principle quantum number (n) (size) positive integers
angular momentum (l) (shape) **subshell -> 1, n-1
s subshell 0, circular
p subshell 1, two lobes
d subshell 3, 4 lobes
f subshell 4, 8 lobes
magnetic quantum number (m(sub)l) (orientation) -l, 0, l
electron spin quantum number (m(sub)s) can be +1/2 or -1/2
nuclear charge higher nuclear charge= increases nucleus-electron interactions **lowers energy of the sublevel
shielding electron-electron repulsions counteract nuclear attraction **raises energy
Zeff effective nuclear charge- the net positive charge experienced by an electron
penetration certain shells allow electrons to get closer to the nucleus than others
Hunn's rule electrons prefer unoccupied orbitals before filling occupied ones
Pauli exclusion principle no 2 electrons can share the same quantum numbers
larger atom trend down, to the left
two electron configuration exceptions Cr: [Ar] 4s1 3d5 Ag: [Kr] 5s1 4d10
main group valence electrons electrons with the highest n value
transition metal valence electrons highest n value + d-electrons
ionization energy the energy required to remove an electron from an atom
ionization energy trend top, to the right
transition metal ionization comes out of s subshell first! (then d)
cations (size) smaller than parent atom
anions (size) larger than parent atom
isoelectronic same electron configuration
binary ionic compound (naming) cation+anion(ide)
transition metal ionic compound (naming) transmetal+charge+anion(ide)
"higher" electron affinity most negative (top right)
Created by: melaniebeale