Ch 4 Section 2

Question 1

Investigations into the photoelectric reflect and hydrogen a emission line spectrum revealed that

Answer 1

Light could behave as both a wave and a particle

Question 2

French scientist Louis de broglie suggested that electrons be considered

Answer 2

Waves confined to the space around an atomic nucleus

Question 3

It followed that the electron waves could only exist at

Answer 3

Specific frequencies

Question 4

According to the relationship E= hv these frequencies corresponded to

Answer 4

Specific energies, the quantized energies of Bohr’s orbits

Question 5

Electrons like light waves can be

Answer 5

Bent (diffracted)

Question 6

Diffraction reefers to the

Answer 6

Bending of a wave as it passes by the edge of an object or through a small opening

Question 7

Electron beams like waves can

Answer 7

Interfere with each other

Question 8

Interference occurs when

Answer 8

Waves overlap

Question 9

Overlapping results in a

Answer 9

Reduction of energy in some areas and an increase of energy in others

Question 10

Heisenbergs proposal answers question of

Answer 10

Where electrons are located if they are both particles and waves

Question 11

Heisenbergs idea involved the

Answer 11

Detection of electrons

Question 12

Electrons are detected by their

Answer 12

Interaction with photons

Question 13

Because photons have about the same energy as electrons any attempt to locate a specific electron with a photon

Answer 13

Knocks the electron off its course

Question 14

The Heisenberg uncertainty principle stated that it is impossible to

Answer 14

Determine simultaneously both the position and velocity of an electron or any other particle

Question 15

Heisenberg uncertainty principle is One of the fundamental principles of our

Answer 15

Present understanding of light and matter

Question 16

In 1926 Austrian physicist Erwin schrodinger used the hypothesis that electrons have a dual wave particle nature and

Answer 16

Developed an equation that treated electrons in atoms as waves

Question 17

To explain why atomic energy states are quantized scientists had to change

Answer 17

The way they viewed the nature of the electron

Question 18

Quantization I’d electron energies was a natural outcome of

Answer 18

Schrodingers equation

Question 19

Only waves of specific energies and therefore frequencies

Answer 19

Provided solutions to the equation

Question 20

Together with the Heisenberg uncertainty principle the schrodinger wave equation laid the

Answer 20

Foundation for modern quantum theory

Question 21

Quantum theory describes mathematically the

Answer 21

Wave properties of electrons and other very small particles

Question 22

Solutions to the schrodinger wave equation are known as

Answer 22

Wave functions

Question 23

Based on the Heisenberg uncertainty principle the early developers of quantum theory determined that wave functions give only the

Answer 23

Probability of finding an electron at a given place around the nucleus

Question 24

Electrons do not travel around the nucleus in

Answer 24

Neat orbits as Bohr had postulated

Question 25

Instead electrons. Exist in certain regions called

Answer 25

Orbitals

Question 26

Am ornital is a

Answer 26

3d region around the nucleus that indicates the probably location of an electron

Question 27

According to the schrodinger equation electrons in atomic orbitals also have

Answer 27

Quantized energies

Question 28

An electrons energy level is not the only characteristic of an orbital that is indicated by

Answer 28

Solving the schrodinger equation

Question 29

Quantum numbers specify the properties of

Answer 29

Atomic orbitals and the properties of electrons in orbitals

Question 30

The first 3 quantum numbers result from

Answer 30

Solutions to the schrodinger equation. They indicate the main energy level shape and orientation of an orbital

Question 31

The fourth, spin quantum number, describes a

Answer 31

Fundamental state of the electron that occupied the orbital

Question 32

The principal quantum number symbolized by n indicated the

Answer 32

Main energy level occupied by the electron

Question 33

Values of n are

Answer 33

Positive integers only

Question 34

As n increases the electrons energy and its average distance from the nucleus

Answer 34

Increase

Question 35

An electron for which n = 1 occupied the

Answer 35

First (lowest) main energy level and is located closest to the nucleus

Question 36

More than one electron can have the same

Answer 36

N value. These electrons are sometimes said to be in the same electron shell

Question 37

Total number of orbitals that exist in a given she’ll is

Answer 37

N^2

Question 38

Except at the first main energy level orbitals of different

Answer 38

Shapes–known as sublevels– exist for a given value of n

Question 39

The angular momentum quantum number symbolized by l indicates the

Answer 39

Shape of the orbital

Question 40

For a specific main energy level the number of orbital shapes possible is

Answer 40

Equal to n

Question 41

The values of l allowed are

Answer 41

zero and all positive integers less than or equal to n-1

Question 42

Depending on its value of l an orbital is

Answer 42

Assigned a letter

Question 43

S orbitals are

Answer 43

Spherical

Question 44

p orbitals have

Answer 44

Dumb bell shapes

Question 45

D orbitals are more

Answer 45

Complex

Question 46

In the first energy level n=1

Answer 46

There is only one sublevels possible an s orbital

Question 47

second energy level n=2 has

Answer 47

2 sublevels the s and p orbitals

Question 48

In the nth main energy level there are

Answer 48

N sublevels

Question 49

Each atomic orbital is designated by the

Answer 49

Principal quantum number followed by the letter of the sublevels

Question 50

Atomic orbitals can have the same

Answer 50

Shape but different orientations around the nucleus

Question 51

The magnetic quantum number symbolized by m indicated the

Answer 51

Orientation of an orbital around the nucleus

Question 52

Values of m are whole numbers including

Answer 52

Zero from -l to +l

Question 53

Because an s orbital is spherical and is centered around the nucleus it has

Answer 53

Only one possible orientation

Question 54

S Orientation corresponds to a magnetic quantum number of

Answer 54

M = 0

Question 55

Only one s orbital in each

Answer 55

Sublevels

Question 56

The loves of a p orbital extend along the

Answer 56

X y or z axis of s 3 dimensional coordinate system

Question 57

There are 3 p orbitals in each

Answer 57

P sublevel which are designation as px py pz

Question 58

The 3 p orbitals occupy different regions of space and those regions are related to values of

Answer 58

M = 0 m = -1 m =+ 1

Question 59

There are 5 different d orbitals in each

Answer 59

D sublevel

Question 60

Five different orientations of d correspond to values of

Answer 60

M = -2. M = -1 m = 0 m= 2 m= 1

Question 61

There are 7 different f orbitals in each

Answer 61

F sublevel

Question 62

The total number of orbitals in a main energy level increases with

Answer 62

The value of n

Question 63

Number of orbitals at each main energy level equals the

Answer 63

Square of the principal quantum number n^2

Question 64

The electron exists in one of two possible

Answer 64

Spin states which creates a magnetic field

Question 65

To account for the magnetic properties of the electron theoreticians created the

Answer 65

Spin quantum number

Question 66

The spin quantum number has only two values (+1/2, -1/2) which indicate

Answer 66

The two fundamental spin states of an electron in an orbital

Question 67

A single orbital can hold a maximum of

Answer 67

Two electrons but the two electrons must have opposite spin states

Question 68

Number of orbitals in sublevel

Answer 68

2l + 1

Question 69

Number of electrons possible in sublevel

Answer 69

[2(2l + 1)]

Question 70

Total electrons possible for energy level

Answer 70

2n^2