Unit 3

Question 1

1 meter is equal to

Answer 1

10^9 nanometers

Question 2

Violet light color frequency

Answer 2

400 x 10^-9 meters

Question 3

Red light color frequency

Answer 3

700 x 10^-7 meters

Question 4

frequency symbol

Answer 4

cursive v

Question 5

wavelength symbol

Answer 5

upside down y

Question 6

formula to find frequency

Answer 6

v = E/h

Question 7

formula to find wavelength

Answer 7

y = c/v

Question 8

frequency and wavelength relationship

Answer 8

inversely proportional

Question 9

frequency and energy relationship

Answer 9

directly proportional

Question 10

wavelength and energy relationship

Answer 10

inversely proportional

Question 11

Planck’s assumption

Answer 11

heated object emits energy in specific amounts (quanta) not continuously

Question 12

discrete packet of energy emitted by objects

Answer 12

quanta

Question 13

a quanta of light

Answer 13

a photon

Question 14

minimum quantity of energy that can be lost or gained by an atom

Answer 14

quantum

Question 15

according to planck, light has ___ properties

Answer 15

particle-like

Question 16

according to broglie, electrons have ____ properties

Answer 16

wave-like

Question 17

bohr model

Answer 17

electrons can only have certain orbits around the nucleus to be able to orbit around the atom

Question 18

the ground state is

Answer 18

when the electrons are in the lowest energy state possible (closest to the atom) (normal orbital notation)

Question 19

the excited state is

Answer 19

when the electrons absorb different quanta of energy and jump to the next energy level (not closest to the atom)

Question 20

first energy level is

Answer 20

closest to the nucleus, lowest amount of energy, most stable

Question 21

higher energy levels are

Answer 21

father away from the nucleus, higher amounts of energy, less stable

Question 22

electrons in excited state return to ground state by

Answer 22

emitting specific quanta of energy

Question 23

electrons in ground state move to excited state by

Answer 23

absorbing specific quanta of energy

Question 24

how much energy does an electron need to jump

Answer 24

exact amount, no more and no less

Question 25

emission of light from an atom occurs when

Answer 25

an electron goes from upper to lower energy level

Question 26

absorption of light from an atom occurs when

Answer 26

an electron goes from lower to higher energy level

Question 27

the pattern formed when photons are emitted from the electron shifting from higher to lower energy state is called

Answer 27

bright line spectra

Question 28

bright line spectra are

Answer 28

like a fingerprint for elements

Question 29

the pattern formed when photons are emitted from the electron shifting from lower to higher energy state is called

Answer 29

dark line spectra

Question 30

total energy absorbed by electrons when they go from ground to excited state is ____ to the total energy released when electrons go from excited to ground state

Answer 30

exactly equal

Question 31

each orbital can hold max

Answer 31

2 electrons

Question 32

principle quantum number

Answer 32

describes the energy level of an electron (2s, 4p, etc)

Question 33

angular momentum quantum number

Answer 33

describes the type of sublevel (2s, 4p, etc)

Question 34

s orbital shape

Answer 34

spherical

Question 35

p orbital shape

Answer 35

peanut/figure 8

Question 36

d orbital shape

Answer 36

square/double peanut

Question 37

f orbital shape

Answer 37

flower

Question 38

s orbital number

Answer 38

1 on each s sublevel

Question 39

Pauli Exclusion principle

Answer 39

two electrons in the same orbital must have opposite spins