Chapter 6

Question 1

interference pattern

Answer 1

when light passes through two closely spaced slits

Question 2

constructive interference

Answer 2

result of adding waves that are in phase

Question 3

destructive interference

Answer 3

result of adding waves that are out of phase

Question 4

speed of light (c)

Answer 4

3.00e8 m/s

Question 5

speed of light equation

Answer 5

c = (wavelength)(frequency)
- (wavelength) = meters
- (frequency) = s^-1

Question 6

blackbody radiation

Answer 6

when a solid is heated, it emits electromagnetic radiation over a wide range of wavelengths

Question 7

Max Planck

Answer 7

suggested that radiant energy is only emitted or absorbed in discrete quantities or bundles

Question 8

quantum (of energy)

Answer 8

smallest quantity of energy that can be emitted (or absorbed)

Question 9

quantum theory formula

Answer 9

E = h(nu)
- E = energy in Joules
- nu = frequency
- h = Planck’s constant = 6.63e-34 Jxs

Question 10

photoelectric effect

Answer 10

Einstein; electrons are ejected from the surface of a metal exposed to light of a certain threshold frequency

Question 11

photons

Answer 11

Einstein proposed; light is a stream of particles

Question 12

photon quantum theory equation

Answer 12

Photon = h(nu)
- where nu is at the threshold frequency

Question 13

Heisenberg uncertainty principle

Answer 13

it is impossible to know simultaneously both the momentum and the position of a particle with certainty

Question 14

Heisenberg uncertainty principle formula

Answer 14

(delta)x x (delta)p >= h/4(pi)
- (delta)x = uncertainty in position in meters
- (delta)p = uncertainty in momentum (mass x velocity)

Question 15

Planck’s constant

Answer 15

6.63e-34 Jxs

Question 16

Pauli exclusion principle

Answer 16

no two electrons can have the same four quantum numbers

Question 17

Electron configuration

Answer 17

describes how the electrons are distributed in the atomic orbitals

Question 18

Aufbau principle

Answer 18

electrons are added to the lowest energy orbitals first before moving to higher energy orbitals

Question 19

Bohr’s Theory of the hydrogen atom

Answer 19

All wavelengths of visible light are present in the emission spectra of sun light and a heated solid

Question 20

Line spectra

Answer 20

emission of light only at specific wavelengths

Question 21

Bohr showed that the energies of the electron in a hydrogen atom are given by the equation

Answer 21

En = -2.18x10^18J(1/n^2)

Question 22

Lowest energy state (n=1)

Answer 22

ground state

Question 23

The stability of the electron decreases…

Answer 23

as n increases

Question 24

n>1

Answer 24

excited state

Question 25

Louis De Broglie

Answer 25

if light can behave like a
stream of particles (photons), then electrons could exhibit
wavelike properties.

Question 26

According to deBroglie, electrons behave like

Answer 26

standing waves

Question 27

The particle and wave properties are related by the
following expression:

Answer 27

lambda = h/mu
- m = mass (kg)
- u - velocity (m/s)

Question 28

Quantum numbers describe

Answer 28

the distribution of electron
density in an atom

Question 29

Principal quantum number

Answer 29

(n) - specifies size

Question 30

Angular moment quantum number

Answer 30

(l) - specifies shape

Question 31

Magnetic quantum number

Answer 31

(ml) - specifies orientation

Question 32

s orbitals

Answer 32

spherical

Question 33

p orbitals

Answer 33

hourglass shaped

Question 34

d orbitals

Answer 34

two hourglasses

Question 35

f orbitals

Answer 35

christmas lights

Question 36

electron spin quantum number

Answer 36

(ms) - used to specify an electrons spin
- either +1/2 or -1/2