Module 6 - Electronic Structure of Atoms V5

Question 1

Electromagnetic radiation refers to waves that move through a vacuum at the speed of light.

Answer 1

true

Question 2

A nanometer is how many meters?

Answer 2

10-9

Question 3

A wavelength refers to the number of waves passing through a given point in a specific amount of time.

Answer 3

false

Question 4

A quantum is a fixed amount of the smallest amount of electromagnetic radiation that can be absorbed or released by an object.

Answer 4

true

Question 5

Which of the following multiples of h\nu are allowed?

Answer 5

3 h/nu

Question 6

The unit for energy is Hz.

Answer 6

false

Question 7

Ground state is the highest energy state for an electron.

Answer 7

false

Question 8

Each element has its own unique atomic emission spectrum.

Answer 8

true

Question 9

Which scientist came up with the concept of principal quantum numbers?

Answer 9

Bohr

Question 10

All orbitals that have the same values of n and l are known as e-shells.

Answer 10

false

Question 11

An orbital is where electrons can be found inside an atom, each one having its own unique set of energies and shapes.

Answer 11

true

Question 12

What does the quantum number “ml” represent?

Answer 12

the orientation of the orbital

Question 13

The following energy diagram is drawn correctly.

Answer 13

false

Question 14

The Aufbau principle states that electrons must fill orbitals of __________ energy before occupying orbitals of __________ energy.

Answer 14

lower; higher

Question 15

A many-electron atom is an atom with two or more electrons.

Answer 15

true

Question 16

Valence electrons are the electrons used in bonding.

Answer 16

true

Question 17

What is the electron configuration for chlorine?

Answer 17

1s22s22p63s23p5

Question 18

The electrons not involved in bonding are known as __________ electrons.

Answer 18

core

Question 19

The speed of light is used to calculate…

Answer 19

wavelength and frequency.

Question 20

All electromagnetic radiation is visible light.

Answer 20

false

Question 21

Which type of radiation has the lowest energy?

Answer 21

red

Question 22

Atoms move to a higher level when they__________energy and move to a lower level when they__________energy.

Answer 22

absorb; release

Question 23

What is the wavelength (in meters) of blue light that has a frequency of 4.60 x 109 Hz?

Answer 23

0.0065m

Question 24

Who is responsible for the explanation of the photoelectric effect?

Answer 24

Albert Einstein

Question 25

Photons have a quantum amount of energy.

Answer 25

true

Question 26

Based on the photoelectric effect, if you shine high-frequency light on a clean sheet of metal…

Answer 26

electrons are emitted from the metal

Question 27

What is the energy of a photon with a frequency of 1.1 x 1026 Hz?

Answer 27

7.3 x 10-8

Question 28

What is the energy of radiation with a wavelength of 3.4 x 10-5 meters?

Answer 28

5.842 x 10-21

Question 29

Elements in the same period have the same atomic emission spectrum.

Answer 29

false

Question 30

Based on Bohr’s model, which is the lowest energy level?

Answer 30

n = 4

Question 31

While the__________quantum number tells the shape of the orbital, the __________quantum number tells the orientation of the orbital shape.

Answer 31

angular momentum; magnetic

Question 32

As the principal quantum number, n, increases…

Answer 32

the number of orbitals increases.

Question 33

What are the quantum numbers for an electron in the 3p orbital (+1 orientation)?

Answer 33

n = 3, l = 1, ml = 1

Question 34

What are the quantum numbers for an electron in the 4d orbital (-2 orientation)?

Answer 34

n = 4, l = 2, ml = -2

Question 35

The Pauli exclusion principle states that…

Answer 35

no two electrons can have the same four quantum numbers.

Question 36

What element is represented by the following electron configuration? 1s22s22p63s23p5

Answer 36

chlorine

Question 37

Planck concluded that objects...

Answer 37

absorb a fixed amount of energy.

Question 38

The Aufbau principle states that orbitals of the lowest energy must be filled first.

Answer 38

true

Question 39

Which list correctly shows visible light in increasing energy?

Answer 39

red, orange, green, violet

Question 40

Which list correctly shows electromagnetic radiation in decreasing energy?

Answer 40

gamma, x-ray, visible light, infrared

Question 41

Which form of electromagnetic radiation listed here has the highest energy?

Answer 41

x-ray

Question 42

What is the speed for the constant c (speed of light constant)?

Answer 42

3.0 x 108 m/s

Question 43

What is the wavelength (in meters) of blue light that has a frequency of 6.3 x 1014 Hz?

Answer 43

4.8 x10-7 meters

Question 44

Within the equation E = hv, h stands for what?

Answer 44

Planck’s constant

Question 45

Which of the following provides the best explanation for the photoelectric effect?

Answer 45

When light of a certain frequency is shined on a clean metal surface, electrons are emitted from the surface.

Question 46

Within the equation E = hv, v stands for what?

Answer 46

frequency

Question 47

What is the energy of a photon with a frequency of 3.8 x 1014 Hz?

Answer 47

2.5 x 10-19 J

Question 48

What is the frequency of a photon whose energy is 9.2 x 10-18 joules?

Answer 48

1.4 x 1016 Hz

Question 49

__________ refers to the generic lab for observing light being emitted from excited electrons within an atom.

Answer 49

a flame test

Question 50

Line spectra observed through gaseous elements in a glass tube being sent energy in the form of electricity is...

Answer 50

an atomic emission spectrum.

Question 51

Which of the following would give a continuous spectrum when its light is broken up by a prism?

Answer 51

sunlight

Question 52

Which principal quantum number has the lowest energy?

Answer 52

n=1

Question 53

An electron in its __________ can absorb energy and jump up to an __________.

Answer 53

ground state, excited state

Question 54

What does the quantum number "l” represent?

Answer 54

the shape of the orbital

Question 55

What specific orbital aligns with the following quantum numbers? n=2 l = 0 ml = 0

Answer 55

2s

Question 56

The following picture represents which orbital shape?

Answer 56

s

Question 57

What are the quantum numbers for an electron in 3d orbital (+1 orientation)?

Answer 57

n=3, l = 2, ml = +1

Question 58

What are the quantum numbers for an electron in 5p orbital (0 orientation)?

Answer 58

n=5, l = 1, ml = 0

Question 59

The two quantum numbers for electron spin are...

Answer 59

-½ , and +½.

Question 60

The Pauli exclusion principle states that no __________ electrons can have the same set of __________ quantum numbers.

Answer 60

2; 4

Question 61

Identify the correct order for the following orbitals in order of lowest energy to highest energy for a many-electron atom: “4s, 2p, 3s, 5d, 4f, 6s.”

Answer 61

2p, 3s, 4s, 6s, 4f, 5d

Question 62

The electron circled in the energy level diagram is found in the _________ energy level and has an electron spin of __________.

Answer 62

2; +½

Question 63

A diagram showing relative energies of shells, subshells, and orbitals of a hydrogen or many-electron atom is a(n)...

Answer 63

energy level diagram.

Question 64

How many valence electrons does carbon have? Carbon’s electron configuration is 1s22s22p2.

Answer 64

4

Question 65

Fluorine has __________ paired electron(s) and __________ unpaired electron(s) in the 2p subshell.

Answer 65

2;1

Question 66

Calcium has __________ valence electrons.

Answer 66

2

Question 67

What element has the following electron configuration: 1s22s22p4?

Answer 67

oxygen

Question 68

Potassium has __________ valence electron(s) and __________ core electron(s).

Answer 68

1;18