Deck 7: The Quantum-Mechanical Model of the Atom

Question 1

Calculate the frequency of the green light emitted by a hydrogen atom with a wavelength of 486.1 nm.

A)1.46 × 10¹⁴ s^-1
B)6.86 × 10¹⁴ s^-1
C)4.33 × 10¹⁴ s^-1
D)6.17 × 10¹⁴ s^-1
E)1.62 × 10¹⁴ s^-1

Answer 1

6.17 × 10¹⁴ s^-1

Question 2

Calculate the wavelength (in nm)of the red light emitted by a neon sign with a frequency of
4.74 × 10¹⁴ Hz.

A)633 nm
B)158 nm
C)142 nm
D)704 nm
E)466 nm

Answer 2

633 nm

Question 3

Place the following types of electromagnetic radiation in order of increasing wavelength.
Ultraviolet light gamma rays radio waves

A)gamma rays < radio waves < ultraviolet light
B)radio waves < ultraviolet light < gamma rays
C)radio waves < gamma rays < ultraviolet light
D)ultraviolet light < gamma rays < radio waves
E)gamma rays < ultraviolet light < radio waves

Answer 3

gamma rays < ultraviolet light < radio waves

Question 4

Which of the following visible colors of light has the highest frequency?

A)green
B)red
C)blue
D)yellow
E)orange

Question 5

Calculate the energy of the orange light emitted,per photon,by a neon sign with a frequency of
4.89 × 10¹⁴ Hz.

A)3.09 × 10^-19 J
B)6.14 × 10^-19 J
C)3.24 × 10^-19 J
D)1.63 × 10^-19 J
E)5.11 × 10^-19 J

Question 6

Identify the location of the visible range of light.

A)between X-ray and ultraviolet
B)between microwave and radio
C)between gamma ray and ultraviolet
D)between X-ray and gamma ray
E)between ultraviolet and infrared

Question 7

Calculate the frequency of the red light emitted by a neon sign with a wavelength of 659.9 nm.

A)2.20 × 10¹⁴ s^-1
B)1.98 × 10¹⁴ s^-1
C)4.55 × 10¹⁴ s^-1
D)5.05 × 10¹⁴ s^-1
E)3.32 × 10¹⁴ s^-1

Question 8

Calculate the energy of the red light emitted by a neon atom with a wavelength of 703.2 nm.

A)3.54 × 10^-19 J
B)4.27 × 10^-19 J
C)2.34 × 10^-19 J
D)6.45 × 10^-19 J
E)2.83 × 10^-19 J

Question 9

Calculate the energy of the violet light emitted by a hydrogen atom with a wavelength of 410.1 nm.

A)4.85 × 10^-19 J
B)2.06 × 10^-19 J
C)1.23 × 10^-19 J
D)8.13 × 10^-19 J
E)5.27 × 10^-19 J

Question 10

Place the following types of electromagnetic radiation in order of increasing frequency.
Visible light microwaves X-rays

A)microwaves < visible light < X-rays
B)X-rays < visible light < microwaves
C)microwaves < X-rays < visible light
D)X-rays < microwaves < visible light
E)visible light < X-rays < microwaves

Question 11

Which of the following visible colors of light has the longest wavelength?

A)blue
B)green
C)yellow
D)red
E)violet

Question 12

Which of the following visible colors of light has the shortest wavelength?

A)blue
B)violet
C)orange
D)green
E)yellow

Question 13

Which of the following visible colors of light has the lowest frequency?

A)yellow
B)blue
C)orange
D)green
E)purple

Question 14

Place the following types of electromagnetic radiation in order of decreasing energy.
Ultraviolet light radio waves microwaves

A)radio waves > microwaves > ultraviolet light
B)ultraviolet light > microwaves > radio waves
C)radio waves > ultraviolet light > microwaves
D)ultraviolet light > radio waves > microwaves
E)microwaves > radio waves > ultraviolet light

Question 15

Calculate the wavelength (in nm)of the blue light emitted by a mercury lamp with a frequency of
6.88 × 10¹⁴ Hz.

A)229 nm
B)436 nm
C)206 nm
D)485 nm
E)675 nm

Question 16

Which of the following occurs as the energy of a photon increases?

A)The frequency decreases.
B)The speed increases.
C)The wavelength increases.
D)The wavelength gets shorter.
E)None of the above occurs as the energy of a photon increases.

Question 17

How many photons are contained in a burst of yellow light (589 nm)from a sodium lamp that contains 609 kJ of energy?

A)3.37 × 10¹⁹ photons
B)3.06 × 10³⁰ photons
C)1.80 × 10²⁴ photons
D)4.03 × 10²⁸ photons
E)2.48 × 10²⁵ photons

Question 18

How many photons are contained in a flash of green light (525 nm)that contains 189 kJ of energy?

A)5.67 × 10²³ photons
B)2.01 × 10²⁴ photons
C)1.25 × 10³¹ photons
D)4.99 × 10²³ photons
E)7.99 × 10³⁰ photons

Question 19

Calculate the energy of the green light emitted,per photon,by a mercury lamp with a frequency of 5.49 × 10¹⁴ Hz.

A)2.75 × 10^-19 J
B)3.64 × 10^-19 J
C)5.46 × 10^-19 J
D)1.83 × 10^-19 J
E)4.68 × 10^-19 J

Question 20

Which of the following occurs as the wavelength of a photon increases?

A)The frequency decreases.
B)The energy increases.
C)The speed decreases.
D)Planck's constant decreases.
E)None of the above occurs as the wavelength of a photon increases.

Question 21

It is possible to determine the ionization energy for hydrogen using the Bohr equation.Calculate the ionization energy for an atom of hydrogen,making the assumption that ionization is the transition from
N = 1 to n = ∞.

A)-2.18 × 10^-18 J
B)+2.18 × 10^-18 J
C)+4.59 × 10^-18 J
D)-4.59 × 10^-18 J
E)+4.36 × 10^-18 J

Question 22

Which of the following transitions represent the emission of a photon with the largest energy?

A)n = 2 to n = 1
B)n = 3 to n = 1
C)n = 6 to n = 3
D)n = 1 to n = 4
E)n = 2 to n = 5

Question 23

What value of l is represented by a d orbital?

A)1
B)2
C)0
D)3

Question 24

Determine the longest wavelength of light required to remove an electron from a sample of potassium metal,if the binding energy for an electron in K is 1.76 × 10³ kJ/mol.

A)147 nm
B)68.0 nm
C)113 nm
D)885 nm
E)387 nm

Question 25

Which of the following transitions (in a hydrogen atom)represent absorption of the smallest frequency photon?

A)n = 5 to n = 6
B)n = 5 to n = 4
C)n = 4 to n = 1
D)n = 1 to n = 3
E)n = 1 to n = 2

Question 26

Choose the transition (in a hydrogen atom)below that represents the absorption of the shortest wavelength photon.

A)n = 1 to n = 2
B)n = 2 to n = 3
C)n = 4 to n = 5
D)n = 6 to n = 3
E)n = 3 to n = 1

Question 27

How much energy (in kJ)do 3.0 moles of photons,all with a wavelength of 655 nm,contain?

A)183 kJ
B)303 kJ
C)394 kJ
D)548 kJ
E)254 kJ

Question 28

Determine the shortest frequency of light required to remove an electron from a sample of Ti metal,if the binding energy of titanium is 3.14 × 10³ kJ/mol.

A)7.87 × 10¹⁵ Hz
B)4.74 × 10¹⁵ Hz
C)2.11 × 10¹⁵ Hz
D)1.27 × 10¹⁵ Hz
E)6.19 × 10¹⁵ Hz

Question 29

Which of the following transitions (in a hydrogen atom)represent emission of the longest wavelength photon?

A)n = 1 to n = 2
B)n = 3 to n = 1
C)n = 3 to n = 4
D)n = 4 to n = 2
E)n = 5 to n = 4

Question 30

Give all possible orbitals for n = 4.

A)1s
B)2s,2p
C)3s,3p,3d
D)4s,4p,4d,4f

Question 31

Calculate the wavelength of a baseball (m = 155 g)moving at 32.5 m/s.

A)7.60 × 10^-36 m
B)1.32 × 10^-34 m
C)2.15 × 10^-32 m
D)2.68 × 10^-34 m
E)3.57 × 10^-32 m

Question 32

Give the principal level for a 2p sublevel.

A)2
B)1
C)0
D)-1
E)-2

Question 33

Each of the following sets of quantum numbers is supposed to specify an orbital.Which of the following sets of quantum numbers contains an error?

A)n = 2,l = 1 ,m_l = -1
B)n = 4,l = 2,m_l = 0
C)n = 3,l =3 ,m_l = -2
D)n = 1,l = 0,m_l = 0
E)n = 3,l = 0,m_l = 0

Question 34

Determine the velocity of a marble (m = 8.66 g)with a wavelength of 3.46 × 10^-33 m.

A)45.2 m/s
B)11.3 m/s
C)22.1 m/s
D)38.8 m/s
E)52.9 m/s

Question 35

Determine the velocity of a medicine ball (m = 10.0 kg)with a wavelength of 1.33 × 10^-35 m.

A)8.81 m/s
B)12.3 m/s
C)2.21 m/s
D)4.98 m/s
E)6.44 m/s

Question 36

What total energy (in kJ)is contained in 1.0 mol of photons,all with a frequency of 2.75 × 10¹⁴ Hz?

A)182 kJ
B)219 kJ
C)457 kJ
D)326 kJ
E)110 kJ

Question 37

For n = 3,what are the possible sublevels?

A)0
B)0,1
C)0,1,2
D)0,1,2,3

Question 38

What are the possible orbitals for n = 3?

A)s,p,d
B)s,p,d,f
C)s
D)s,p

Question 39

Which of the following statements is true?

A)The emission spectrum of a particular element is always the same and can be used to identify the element.
B)Part of the Bohr model proposed that electrons in the hydrogen atom are located in "stationary states" or particular orbits around the nucleus.
C)The uncertainty principle states that we can never know both the exact location and speed of an electron.
D)An orbital is the volume in which we are most likely to find an electron.
E)All of the above are true.

Question 40

Calculate the wavelength of an electron (m = 9.11 × 10^-28 g)moving at 3.66 × 10⁶ m/s.

A)1.99 × 10^-10 m
B)5.03 × 10^-10 m
C)1.81 × 10^-10 m
D)5.52 × 10^-9 m
E)2.76 × 10^-9 m

Question 41

Which of the following statements are true?

A)The principal quantum number (n)describes the shape of an orbital.
B)The angular momentum quantum number (l)describes the size and energy associated with an orbital.
C)The magnetic quantum number (m_l)describes the orientation of the orbital.
D)An orbital is the path that an electron follows during its movement in an atom.
E)All of the above are true.

Question 42

In which orbital below would an electron (on average)be farthest from the nucleus?

A)1s
B)4f
C)3s
D)3d
E)2p

Question 43

Each of the following sets of quantum numbers is supposed to specify an orbital.Choose the one set of quantum numbers that does not contain an error.

A)n = 4,l = 4,m_l = 0
B)n = 3,l = 2,m_l = +3
C)n = 4,l = 0,m_l = -1
D)n = 3,l = 1,m_l = -2
E)n = 5,l = 3,m_l = -3

Question 44

Calculate the wavelength of light associated with the transition from n = 1 to n = 3 in the hydrogen atom.

A)103 nm
B)155 nm
C)646 nm
D)971 nm
E)136 nm

Question 45

Each of the following sets of quantum numbers is supposed to specify an orbital.Choose the one set of quantum numbers that does not contain an error.

A)n = 2,l = 2,m_l = -1
B)n = 2,l = 2,m_l = 0
C)n = 3,l = 2,m_l = -3
D)n = 4,l = 3,m_l = -2
E)n = 4,l = 2,m_l = +4

Question 46

How many different values of m_l are possible in the 4f sublevel?

A)1
B)7
C)3
D)5
E)2

Question 47

Calculate the energy change associated with the transition from n = 4 to n = 1 in the hydrogen atom.

A)+4.89 × 10^-18 J
B)+1.64 × 10^-18 J
C)-6.12 × 10^-18 J
D)+3.55 × 10^-18 J
E)-2.04 × 10^-18 J

Question 48

It is possible to determine the ionization energy for hydrogen using the Bohr equation.Calculate the ionization energy (in kJ)for a mole of hydrogen atoms,making the assumption that ionization is the transition from n = 1 to n = ∞.

A)7.62 × 10³ kJ
B)2.76 × 10³ kJ
C)1.31 × 10³ kJ
D)3.62 × 10³ kJ
E)5.33 × 10³ kJ

Question 49

How many different values of l are possible in the third principal level?

A)1
B)2
C)3
D)0
E)4

Question 50

Determine the energy change associated with the transition from n = 3 to n = 2 in the hydrogen atom.

A)+3.03 × 10^-19 J
B)-1.82 × 10^-19 J
C)+5.51 × 10^-19 J
D)-3.03 × 10^-19 J
E)+2.69 × 10^-19 J

Question 51

In which orbital below would an electron (on average)be closest to the nucleus?

A)2p
B)4s
C)2s
D)5d
E)3p

Question 52

How many orbitals are contained in the third principal level (n = 3)of a given atom?

A)9
B)3
C)18
D)7
E)5

Question 53

Which of the following quantum numbers describes the shape of an orbital?

A)principal quantum number
B)magnetic quantum number
C)spin quantum number
D)Schrödinger quantum number
E)angular momentum quantum number

Question 54

Which of the following statements are true?

A)We can sometimes know the exact location and speed of an electron at the same time.
B)All orbitals in a given atom are roughly the same size.
C)Since electrons have mass,we must always consider them to have particle properties and never wavelike properties.
D)Atoms are roughly spherical because when all of the different shaped orbitals are overlapped,they take on a spherical shape.
E)All of the above are true.

Question 55

How many sublevels are contained in the second shell (n = 2)of a given atom?

A)1
B)2
C)9
D)4
E)3

Question 56

Determine the energy change associated with the transition from n=2 to n=5 in the hydrogen atom.

A)-2.18 × 10^-19 J
B)+6.54 × 10^-19 J
C)+4.58 × 10^-19 J
D)-1.53 × 10^-19 J
E)+3.76 × 10^-19 J

Question 57

Calculate the frequency of light associated with the transition from n = 2 to n = 3 in the hydrogen atom.

A)2.19 × 10¹⁴ s^-1
B)5.59 × 10¹⁴ s^-1
C)4.57 × 10¹⁴ s^-1
D)1.79 × 10¹⁴ s^-1
E)3.28 × 10¹⁴ s^-1

Question 58

If two electrons in the same atom have the same value of "l",they are

A)in the same sublevel,but not necessarily in the same level.
B)in the same level,but different sublevel.
C)in the same orbital.
D)in different levels and in different shaped orbitals.
E)None of the above

Question 59

Which of the following quantum numbers describes the orientation of an orbital?

A)magnetic quantum number
B)principal quantum number
C)angular momentum quantum number
D)spin quantum number
E)Schrödinger quantum number

Question 60

How many different values of m_l are possible in the 3d sublevel?

A)2
B)1
C)3
D)5
E)7

Question 61

Match the following.
n = 6 to n = 5

A)103 nm
B)657 nm
C)7460 nm
D)122 nm
E)1280 nm

Question 62

Match the following.
n = 1 to n = 2

A)103 nm
B)657 nm
C)7460 nm
D)122 nm
E)1280 nm

Question 63

Electromagnetic radiation with a wavelength of 525 nm appears as green light to the human eye.The energy of one photon of this light is ________ J.

A)1.04 × 10^-31
B)3.79 × 10^-28
C)3.79 × 10^-19
D)1.04 × 10^-22
E)2.64 × 10¹⁸

Question 64

Define constructive interference.

Question 65

What is the photoelectric effect?

Question 66

Give the numbers for m_l for a d orbital.

A)0,1,2,3,4
B)1,2,3,4,5
C)1,2,3
D)-2,-1,0,1,2

Question 67

Describe how a neon light works.

Question 68

How many orbitals are contained in the n = 2 level? Give the l and m_l values of each of them.

Question 69

Describe the shape of a p orbital.

A)a ball
B)two balls
C)three balls
D)four balls

Question 70

Electromagnetic radiation with a wavelength of 525 nm appears as green light to the human eye.The frequency of this light is ________ s^-1.

A)5.71 × 10¹⁴
B)5.71 × 10⁵
C)1.58 × 10²
D)1.58 × 10¹¹
E)1.75 × 10^-15

Question 71

Match the following.
n = 5 to n = 3

A)103 nm
B)657 nm
C)7460 nm
D)122 nm
E)1280 nm

Question 72

Why do atoms only emit certain wavelengths of light when they are excited? (Why do line spectra exist?)

Question 73

In the electromagnetic spectrum,identify the highest energy radiation

Question 74

Why don't we observe the wavelength of everyday macroscopic objects?

Question 75

What is the maximum number of f orbitals that are possible?

A)1
B)3
C)7
D)5

Question 76

Match the following.
n = 3 to n = 1

A)103 nm
B)657 nm
C)7460 nm
D)122 nm
E)1280 nm

Question 77

An FM radio station broadcasts electromagnetic radiation at a frequency of 100.6 MHz.The wavelength of this radiation is ________ m.

A)2.982 × 10⁶
B)2.982
C)3.018 × 10¹⁶
D)3.018 × 10¹⁰
E)0.3353

Question 78

Describe the shape of one of the d orbitals.

A)four lobes in one plane
B)three lobes in one plane
C)two lobes in one plane
D)one sphere

Question 79

Match the following.
n = 3 to n = 2

A)103 nm
B)657 nm
C)7460 nm
D)122 nm
E)1280 nm

Question 80

How much energy,in kJ,is required to ionize 2.78 moles of hydrogen atoms?

A)2.74 × 10³ kJ
B)4.72 × 10³ kJ
C)1.66 × 10³ kJ
D)3.65 × 10³ kJ
E)5.89 × 10³ kJ