Chem I Test 2

J or kgm2/s2

m (nm)

s-1

E

v (nu)

lamda

electrons leave atom or rings when light hits them

show wavelengths of light emitted when electrons jump rings

shows orbitals, orbits, and levels

Idea that if light acts as both a particle and a wave, it can behave as both a particle and a wave

wavelength associated with momentum and mass

idea that one can't see an electron as a wave and a partcile at the same time because they are complimentary principles and cancel each other out

Idea that we know where the electron is likely to be, but not really

short-hand numbers to describe e- configuration

n, shell number, determined by row #

l, subshell, describes shape of orbital; determined by block

0

1

2

3

ml, orientation of orbital in space; determined by -l through +l

1/2 positive (spin up) vs -1/2 negative (spin down)

No two elecctrons in an atom have the same set of 4 quantum numbers

n^2 = # of orbitals

# of orbitals * 2

electrons will fill empty spin up and spin down orbitals before they'll fill full ones

outermost electrons, used in bonding; use ns + nblock

electrons deep inside atom

Cr, Mo, Cu, Ag

[Ar] 4s13d5

[Kr] 5s14d5

[Ar] 4s14d10

[Kr] 5s14d10

alkali metals

alkalines earth metals

Chalcogens

Halogens

noble gases

columns 3-12

#57-71

#89-102

metal and nonmetal

nonmetal and nonmetal

tendency of an atom to attract electrons

0.4 or less

0.4-2.0

2.00 or more