Chapter 6

Question 1

The intensity of a light is a function of the waves______

Answer 1

Amplitude

Question 2

A point of zero amplitude

Answer 2

A node

Question 3

Unit of frequency

Answer 3

Cycles per second or hertz

Question 4

As wavelength increases, frequency and energy ________

Answer 4

Decrease

Question 5

Max Planck proposed that light waves existed as discrete packets of energy known as…

Answer 5

Quanta

Question 6

Ultraviolet catastrophe

Answer 6

According to classical physics, the intensity of emitted light approaches infinity as the wavelength approves zero (incorrect)

Predictions failed in the UV region

Question 7

Light acts as….

Answer 7

Waves and particles

Question 8

An object can gain or lose energy by absorbing or emitting radiant energy in…..

Answer 8

Quanta

Question 9

Quanta of energy

Answer 9

Smallest unit of energy that may be emitted as radiation

Question 10

Electrons can only go up or down_____levels

Answer 10

Entire

Question 11

Quantization is the….

Answer 11

Only specific energies that are allowed

Question 12

Certain metals will____electrons when light strikes the metal surface

(Excited electrons, think of flame test)

Answer 12

Release (energy must exceed a threshold energy first)

Question 13

Blackbody radiation

Answer 13

Theory that a body absorbs all of the radiation that falls on it

Question 14

Packets of energy

Answer 14

Photons

Question 15

There is a 1:1 correspondence between ejected electrons and______

Answer 15

Light waves

Question 16

Credited with the first modern model of the hydrogen atom based on the “line spectra” of atomic emission sources

Answer 16

Bohr

Question 17

Proposed a “planetary” structure for the atom where the electrons circled the nucleus in….

Answer 17

Defined orbitals

(Attractive electrostatic forces of the electron and nucleus were balanced by the centripetal forces of the orbiting electron)

Question 18

When ______light passes through a prism, all of the colors of the rainbow are observed

Answer 18

White

Question 19

When the light from a discharge tube containing a pure element is passed through the same prism….

Answer 19

Only certain colors are observed (emission spectrum)

Question 20

Wavelength red presents the distance between one complete______
(Wavelength)

Answer 20

Cycle

Question 21

The lines on the line spectrum indicate…

Answer 21

Jumps between allowed energy levels

Question 22

Wave duality

Answer 22

Electron has the properties of lights and waves

De brogli

Question 23

Heisenberg uncertainty principle

Answer 23

Impossible to determine exact position and velocity of electron

Question 24

Schrodinger

Answer 24

Determined that matter could be described as a wave, came up with orbitals

Question 25

The behavior of an electron in the atom can be described as....

Answer 25

Is standing wave

Question 26

Pauli exclusion principal

Answer 26

No 2 electrons have the same quantum numbers

Question 27

The importance of E =mc ^2

Answer 27

Energy has mass

Question 28

Electromagnetic radiation can be thought of as..:

Answer 28

A stream of particles called photons

Question 29

Diffraction results when...

Answer 29

Iight is scattered from a regular array of points or lines

Question 30

T or F All matter exhibits either particulate or wave properties exclusively

Answer 30

F

Question 31

The 4 lines observed in the visible emission spectrum for hydrogen tell us that...

Answer 31

Only certain energies are allowed for the electron in a hydrogen atom

Question 32

Criticism of the Bohr model of the atom

Answer 32

Does not adequately predict the ionization energy of the valence electrons for elements other than H

Question 33

Bohr's model correctly describes....

Answer 33

Only the H atom

Question 34

Orbital

Answer 34

Space where electrons are most likely to be found

Question 35

Can the movement of electrons be determined?

Answer 35

No

Question 36

The size of an orbital is_____defined

Answer 36

Arbitrarily

Question 37

How to find electrons in n=___

Answer 37

n^2 * 2 (electrons)

Question 38

The lowest energy configuration for an atom is the one having the maximum number of unpaired electrons allowed by the Pauli principle in a particular set of degenerate orbitals

Answer 38

Hund's rule

Question 39

n describes the.... | Principle quantum number

Answer 39

Energy level, row on periodic table, size of orbital

Question 40

n represents the...

Answer 40

Subshell

Question 41

l is the_____quantum number

Answer 41

Angular momentum

Question 42

l represents the

Answer 42

Subshell (shape of orbital)

Question 43

l equals...

Answer 43

0 to n-1 values The # of nodes (space that no electrons occupy)

Question 44

ml represents the _______quantum number

Answer 44

Magnetic

Question 45

ml equals

Answer 45

-l to +l

Question 46

ms represents the_____quantum number ms equals...

Answer 46

Spin -1/2 or +1/2

Question 47

The number of orbitals having a given value of l is equal to...

Answer 47

2l + 1