Unit 2: Chapter 3

Question 1

Wave-particle duality

Answer 1

light can behave as a
wave or a particle

Question 2

Light has both ____-like and _____-like properties

Answer 2

wave, particle

Question 3

an oscillation or periodic movement that can transport energy from one point in space to another

Answer 3

wave

Question 4

distance between two corresponding points in a wave

Answer 4

Wavelength (λ)

Question 5

number of successive wavelengths that pass a given point per second (units = Hz, which are s–1)

Answer 5

frequency (v)

Question 6

2.998 ✕ 108 m/s

Answer 6

speed of light

Question 7

Light can behave as streams of tiny particles

Answer 7

photons

Question 8

light shone on metal causes ejection of e–

Answer 8

Photoelectric effect

Question 9

A photon’s energy depends on its _______

Answer 9

frequency

Question 10

6.626 ✕ 10–34 J⋅s

Answer 10

Plank’s constant

Question 11

_______ energy photons correspond to light with a ↑λ (↓ν)

Answer 11

Low

Question 12

____energy photons correspond to light with a ↓λ (↑ν)

Answer 12

high

Question 13

True or False: λabsorbed = λemitted

Answer 13

true

Question 14

Matter and ______ are constantly interacting with one another

Answer 14

energy

Question 15

True or False: Every element has a unique absorption and emission spectrum

Answer 15

true

Question 16

Visible light affects an element’s _______

Answer 16

electrons

Question 17

Ground state

Answer 17

lowest energy level

Question 18

Excited states

Answer 18

higher energy levels

Question 19

Quantized energy levels (shells)

Answer 19

areas of specific energies where e– are most likely to be found

Question 20

Absorption

Answer 20

e– absorbs energy and moves to excited state (λabs ≥ E gap)

Question 21

Emission

Answer 21

e– falls from excited state, emitting energy equal to difference between shells

Question 22

True or False: The Balmer-Rydberg Equation only works to explain the emission spectrum of hydrogen

Answer 22

true

Question 23

Wave-particle duality of light/matter

Answer 23

quantum theory

Question 24

e– in atoms exist only in ______ energy levels, not between them

Answer 24

discrete

Question 25

e– can _____ from one energy level to another but not transition ______ or stay between these levels

Answer 25

jump, smoothly

Question 26

mathematical solutions that provide an atomic “address” for an e–

Answer 26

quantum numbers

Question 27

specific notation for the arrangement and number of e– in an atom

Answer 27

electron configuration

Question 28

What helps us describe a particular e– associated with an atom

Answer 28

quantum numbers

Question 29

regions of space surrounding nucleus where an e– is likely to be found

Answer 29

orbitals

Question 30

Each orbital holds how many electrons?

Answer 30

≤ 2 e–

Question 31

What are the 4 classes of orbital shapes?

Answer 31

s,p,d,f

Question 32

What happens as n increases?

Answer 32

energy of e– in shell increases distance between e– and nucleus increases capacity to hold e– increases

Question 33

Identifies the energy level or shell of the e–

Answer 33

principal quantum number, n

Question 34

If n=1 ℓ =___

Answer 34

0

Question 35

If n=2 ℓ =___

Answer 35

0 or 1

Question 36

If n=3 ℓ =___

Answer 36

0,1,or 2

Question 37

How many orbitals are in the s subshell?

Answer 37

1

Question 38

How many orbitals are in the p subshell?

Answer 38

3

Question 39

How many orbitals are in the d subshell?

Answer 39

5

Question 40

How many orbitals are in the f subshell?

Answer 40

7

Question 41

What values of mℓ are in the s subshell?

Answer 41

0

Question 42

What values of mℓ are in the p subshell?

Answer 42

-1,0,1

Question 43

What values of mℓ are in the d subshell?

Answer 43

-2,-1,0,1,2

Question 44

What values of mℓ are in the f subshell?

Answer 44

-3,-2,-1,0,1,2,3

Question 45

Every ___ has spin

Answer 45

e-

Question 46

According to the _______ _______ ______ no two e– in an atom can have the same set of four quantum numbers

Answer 46

The Pauli exclusion principle

Question 47

as n ↑, the size of each type of orbital ___

Answer 47

↑

Question 48

within a shell, subshells _____ in energy

Answer 48

increase

Question 49

orbitals within a subshell at the same energy level are called _____ ______

Answer 49

degenerate orbitals

Question 50

The _____ _____ is the process of filling the subshells with e– from the lowest energy upward

Answer 50

Aufbau principle

Question 51

According to _____ ______ e– within a subshell (degenerate orbitals) remain as unpaired as possible

Answer 51

Hund’s rule

Question 52

______ ______ is the specific notation for the arrangement and number of electrons in an atom by increasing energy levels

Answer 52

Electron configuration

Question 53

e– occupying outermost shell orbitals are _____ ______

Answer 53

Valence electrons

Question 54

Atomic and ionic size is determined by:

Answer 54

electronic structure interactions between oppositely charged nucleus and electrons

Question 55

_______ _______ govern interactions between electrons (–) and nucleus (+)

Answer 55

Electrostatic principles

Question 56

Oppositely charged particles _____ each other.

Answer 56

attract

Question 57

Like-charged particles _____ each other.

Answer 57

repel

Question 58

As the charges ______, so does the attraction or repulsion.

Answer 58

increase

Question 59

As the two charged bodies get closer to each other, the force of attraction or repulsion gets ____.

Answer 59

stronger

Question 60

Electrons are electrostatically attracted to ______

Answer 60

nucleus

Question 61

the net positive charge from the nucleus an e– experiences

Answer 61

Effective nuclear charge (Zeff)

Question 62

Valence e– have a lower Zeff than core electrons because:

Answer 62

Further distance from nucleus Shielding by core electrons

Question 63

_____ _____ is ½ the distance between 2 nuclei in covalently bonded molecule

Answer 63

Atomic radius

Question 64

All cations = ______ radius than neutral atom

Answer 64

smaller

Question 65

All anions = _____ radius than neutral atom

Answer 65

larger

Question 66

A cation has a ______ charge

Answer 66

positive

Question 67

An anion has a _____ charge

Answer 67

negative

Question 68

energy required to remove the highest-energy electron from an atom in the gaseous state

Answer 68

Ionization energy, IE

Question 69

the energy change when an electron is added to an atom in the gaseous state

Answer 69

Electron affinity, EA

Question 70

______ EA: energy is released when an e– is added

Answer 70

negative

Question 71

______EA = energy is required when an e– is added

Answer 71

positive