qm models, e- config

Question 1

the relation bw the wavelength of radiation w the frequency

Answer 1

as the wavelength of the radiation inc, the frequency dec

Question 2

continuous spectrum

Answer 2

shows all available colour of the spectrum

Question 3

higher amplitude =

Answer 3

greater intensity, determined by the number of e- ejected

Question 4

smallest particle of em energy

Answer 4

photons

Question 5

absorption spectrum

Answer 5

the wavelengths of light that hv been absorbed by the atom show up as dark bands

Question 6

emission spectrum

Answer 6

colours present are the same as those that are missing from the absorption spectrum

Question 7

process of exciting an e-

Answer 7

1. in ground state, atoms dont emit energy
2. e- can change from ground to excited state by ABSORBING A SPECIFIC AMT of energy (exactly equal to the diff bw the 2 states)

Question 8

process of emission of energy

Answer 8

1. after e- is excited, the e- transitions back to ground state after a while
2. this causes it to release energy equal to that absorbed

Question 9

pros of bohr model

Answer 9

1. correctly predicted line spectra for H and other elements
2. explains the line spectrum (evidence for quantization) and why the e- cant hit nucleus

Question 10

cons of bohr model

Answer 10

1. only worked for single electron orbitals, not multi electron orbitals
2. rigid lines and the assumption that electrons orbit a fine line , when instead they are spread out over discrete orbitals

Question 11

aufbau’s principle

Answer 11

tells us to fill in electron from lowest to highest energy
order: 1s (n=1, l=0), 2s2p(n=2, l=1), 3s3p3d, 4s4p4d4f, 5s5p5d5f, 6…etc.

Question 12

paulis exclusion prcinciple

Answer 12

paired e- must be opposite spin, no 2 identical wavefunctions can exist

Question 13

hunds rule

Answer 13

when filling out e- shells, leave unpaired for as long as possible

Question 14

exceptions for filling e- orbitals

Answer 14

chromium/molybdenum - full unpaired d shell is lower energy than fully paired s shell
cu, ag, au - fully paired d shell is lower energy than full s shell

Question 15

n codes for

Answer 15

avg distance from nucleus, is kinda like the base of the rest

Question 16

l codes for

Answer 16

the shape of the e- orbital, is js n-1
l=0: s (spherical)
l=1: p (peanut)
l=2: d (flower and ringpop looking ahh)

Question 17

ml (magneti quantum number) codes for

Answer 17

how many of each shaped orbital are allowed at that lvl
- [-l, l] e.g. l=1 ml = -1, 0, 1

Question 18

magnetic spin number (ms) codes for

Answer 18

how e- acts in magnetic field
-1/2 or 1/2