Emission Spectra and Orbitals

Question 1

concept of energy quanta comes from

Answer 1

the experiments emission spectra of hydrogen

Question 2

Excited atoms emit

Answer 2

light of only certain wavelength

Question 3

wavelengths of emitted light depend on the e..

Answer 3

element

Question 4

visible series of lines called-

Answer 4

Balmers series

Question 5

scientist who did experiment on hydrogen

Answer 5

bohr

Question 6

Electrons can only exist in

Answer 6

discrete orbits / stationary states/quantized energy states

Question 7

energy state of an atom=

Answer 7

• R/n^2

Question 8

sharp line spectra = evidence for //// ////

Answer 8

energy levels

Question 9

calculation of 🔺E

Answer 9

understood?

Question 10

Problems with bohr’s theory
• theory only /////// for H
• introduced quantum idea ///////

Answer 10

succesful, artifcially

Question 11

orbitals & e-configurations

Answer 11

understood

Question 12

each orbital

Answer 12

no more than 2 electrons!

Question 13

Diamagnetic is not .

Answer 13

attracted to a magnetic field

Question 14

Paramagnetic:

Answer 14

substance is attracted to a magnetic field

Question 15

Substances with unpaired electrons

Answer 15

paramagnetic

Question 16

n

Answer 16

energy level number

Question 17

l

Answer 17

energy sublevel number staring with 0 for s

Question 18

mi

Answer 18

orbital number given in the range -l to l

Question 19

ms

Answer 19

electron spin number (±1/2)

Question 20

AUFBAU

Answer 20

WHEN BUILDING UP THE E CONFIGURATION OF AN ATOM, THE ELCTRONS OCCUPY THE LOWEST AVAILABLE ENERGY LEVELS FIRST

Question 21

Pauli

Answer 21

no more than two electrons can occupy a single orbital and those two must have opposite spins. Also electrons must occupy the orbitals single before filling them in pairs.