Deck 7: A Quantum Model of Atoms: Waves and Particles

Question 1

In refraction, polychromatic light is dispersed into its component wavelengths by ________

A) constructive and destructive interference of light waves in air.
B) internal reflections within a prism.
C) differences in the bending of different wavelengths of light by a prism.
D) constructive and destructive interference of light waves in a prism.
E) the reduction in the intensity of white light to reveal the colors.

Answer 1

differences in the bending of different wavelengths of light by a prism.

Question 2

Which of the following is quantized?

A) the trajectory of a baseball hit from home plate
B) the speed of a Formula 1 race car
C) the diameter of a redwood tree
D) the number of marbles in a bag
E) your age

Answer 2

the number of marbles in a bag

Question 3

What is the wavelength ( $\lambda$ , in m) of a radio station operating at a frequency of 99.6 MHz?

A) 3.01 * 10⁶ m
B) 3.01 m
C) 3.32 *10 10^-7 m
D) 0.332 m
E) 3.32 m

Answer 3

3.01 m

Question 4

Which of the following occurs only in discrete (quantized) increments?

A) the speed a car drives on the interstate
B) the altitude that an airplane flies
C) time
D) the level of water in a sink
E) money

Question 5

The fact that the absorption and emission spectra of atoms and their ions are different is evidence that the spectra are due to ________

A) electrons.
B) protons.
C) neutrons.
D) the nuclei.
E) electromagnetic interactions.

Question 6

In comparing the dark Fraunhofer lines with light emitted by elements in a flame, Bunsen and Kirchhoff demonstrated that ________

A) atoms emit and absorb electromagnetic radiation at characteristic wavelengths.
B) the solar spectrum has dark lines.
C) helium may be found in minerals that contain uranium.
D) electrons are responsible for the absorption and emission of electromagnetic radiation.
E) the solar spectrum has bright lines.

Question 7

The Fraunhofer lines are evidence that ________

A) atoms contain nuclei.
B) atoms contain electrons.
C) waves interfere constructively.
D) elements absorb light.
E) elements emit light.

Question 8

Atomic spectra are due to the changes in the energy of ________

A) protons.
B) neutrons.
C) nuclei.
D) electrons.
E) electromagnetic radiation.

Question 9

The emission spectra of Na and Na⁺ are different because ________

A) Na⁺ has fewer electrons.
B) Na has fewer electrons.
C) Na⁺ has more protons.
D) Na has fewer neutrons.
E) Na has more protons.

Question 10

Fraunhofer lines are due to ________

A) emission of radiation.
B) absorption of radiation.
C) the photoelectric effect.
D) constructive interference.
E) destructive interference.

Question 11

Which statement about electromagnetic radiation is not correct?

A) Electromagnetic radiation consists of oscillating electric and magnetic fields.
B) Electromagnetic radiation is emitted by all stars.
C) All electromagnetic radiation is visible to the eye.
D) Electromagnetic radiation spans a very wide range of wavelengths from gamma rays to radio waves.
E) The frequency and wavelength of electromagnetic radiation are related to each other.

Question 12

What color will a red object appear when it is seen through a filter with the absorption spectrum shown below?

A) blue
B) yellow
C) red
D) black
E) white

Question 13

Which of the following types of electromagnetic radiation has the longest wavelength?

A) gamma rays
B) X-rays
C) radio waves
D) infrared
E) visible

Question 14

Which of the following types of electromagnetic radiation has the shortest wavelength?

A) gamma rays
B) X-rays
C) radio waves
D) infrared
E) visible

Question 15

Which of the following photons has the lowest frequency?

A) a photon from a Nd:YAG laser with $\lambda$ = 1,064 nm
B) a photon from an Ar⁺ laser with $\lambda$ = 514.5 nm
C) a photon from a Kr⁺ laser with $\lambda$ = 647 nm
D) a photon from an ArF laser with $\lambda$ = 193 nm
E) a photon from a He-Ne laser with $\lambda$ = 633 nm

Question 16

What color will a yellow object appear when it is seen through a filter with the absorption spectrum shown below?

A) blue
B) yellow
C) red
D) black
E) white

Question 17

Which of the following photons has the highest frequency?

A) a photon from a Nd:YAG laser with $\lambda$ = 1,064 nm
B) a photon from an Ar⁺ laser with $\lambda$ = 514.5 nm
C) a photon from a Kr⁺ laser with $\lambda$ = 647 nm
D) a photon from an ArF laser with $\lambda$ = 193 nm
E) a photon from a He-Ne laser with $\lambda$ = 633 nm

Question 18

What color will a blue object appear when it is seen through a filter with the absorption spectrum shown below?

A) blue
B) yellow
C) red
D) black
E) white

Question 19

Which statement about refraction or diffraction is not correct?

A) A beam of light is bent or refracted as it moves from air into a denser medium such as water or a glass prism.
B) When a beam of light passes through a narrow slit, it is bent or diffracted by the edges and spreads out in a circular pattern.
C) When a beam of light is diffracted by two slits that are close to each other, the two sets of resulting waves interfere with each other, producing a pattern of light and dark bands.
D) When the crests of two waves overlap, they interfere constructively and produce a light band in the interference pattern.
E) When the crest of one wave overlaps with the trough of another, they are said to be "in phase."

Question 20

What is the frequency (v, in Hz) of the photons emitted by a He-Ne laser with a wavelength ( $\lambda$ ) of 632.8 nm?

A) 4.738 * 10⁵ Hz
B) 1.897 * 10² Hz
C) 1.897 *10¹¹ Hz
D) 4.738 * 10¹⁴ Hz
E) 1.897 * 10¹⁴ Hz

Question 21

The study of light emitted by the hydrogen atom by Johann Balmer, Johannes Rydberg, Niels Bohr, and others revolutionized physics because it revealed that ________

A) energy is quantized.
B) light intensity does not affect the number of atoms excited.
C) the emitted light is produced by the electron making a transition between quantized energy levels.
D) blackbody radiation is continuous.
E) atomic spectra are continuous.

Question 22

What is the minimum frequency of a photon that can eject a photoelectron from Ba metal? (The work function of barium is = 4.3 *10^-19 J.)

A) 2.8 *10^-52 Hz
B) 6.5 * 10¹⁴ Hz
C) 6.5 * 10⁴ Hz
D) 6.5 * 10¹³ Hz
E) 2.8 * 10¹⁴ Hz

Question 23

Based on the following graph, which metal will emit the highest energy photoelectron when a photon with a frequency of 3.9*10¹⁴ Hz is incident on the metal?

A) a
B) b
C) c
D) d

Question 24

Indicate which of the following sources produces the lowest energy photons.

A) a radio station with v = 106.7 MHz
B) a dentist's X-ray source with $\lambda$ = 100 pm
C) the laser in a CD player with $\lambda$ = 650 nm
D) a microwave oven with v = 6.0 * 10¹⁰ Hz
E) your cell phone with v = 1.750 GHz

Question 25

Which of the following will lead to an increase in the kinetic energies of photoelectrons emitted when light is incident on a metal surface?

A) decrease in the light's wavelength
B) increase in the light's intensity
C) increase in the light's wavelength
D) decrease in the light's frequency
E) decrease in the light's intensity

Question 26

An atom in its ground state absorbs a single photon of light and then relaxes back to the ground state by emitting an infrared photon (1,200 nm) followed by an orange photon (600 nm). What is the wavelength of the photon that was absorbed initially?

A) 600 nm
B) 1,200 nm
C) 1,800 nm
D) 900 nm
E) 400 nm

Question 27

What is the photon energy of the yellow-orange light ( $\lambda$ = 589 nm) produced by sodium vapor streetlights?

A) 3.37 *10^-19 J
B) 6.63 *10^-18 J
C) 2.99*10^-20 J
D) 1.45 *10^-17 J
E) 7.45 * 10^-16 J

Question 28

Based on the following graph, which metal will emit the highest energy photoelectron when a photon with a wavelength of 650 nm is incident on the metal?

A) a
B) b
C) c
D) d

Question 29

What is the energy (E, in J) of a photon from a microwave oven with a frequency of
v = 6.0 * 10¹⁰ Hz?

A) 3.98 *10 10^-30 J
B) 3.98 *10^-39 J
C) 3.98*10^-23 J
D) 3.98 *10^-17 J
E) 3.98 *10^-13 J

Question 30

Indicate which metal requires the shortest wavelength photons to eject photoelectrons based on the following graph.

A) a
B) b
C) c
D) d

Question 31

If each of the following metals is exposed to light with a wavelength of 240 nm, which will emit photoelectrons with the greatest kinetic energy?

A) iron ( = 7.2 *10^-19 J)
B) platinum (11ef1a66_0479_eb58_a3cb_57e06677e6de_TB3834_11 = 9.1 *10^-19 J)
C) nickel (11ef1a66_0479_eb58_a3cb_57e06677e6de_TB3834_11 = 8.3 *10^-19 J)
D) palladium (11ef1a66_0479_eb58_a3cb_57e06677e6de_TB3834_11 = 8.2 *10^-19 J)
E) sodium (11ef1a66_0479_eb58_a3cb_57e06677e6de_TB3834_11 = 4.4 *10^-19 J)

Question 32

Which of the following sources produces the highest energy photons?

A) a doctor's X-ray source
B) the heat lamp in your bathroom
C) a microwave oven
D) gamma rays from a star
E) radio waves from your local station

Question 33

Indicate which of the following photons can cause emission of photoelectrons from a surface of gallium (= 6.7 *10^-19 J).

A) 350 nm
B) 400 nm
C) 200 nm
D) 650 nm
E) 500 nm

Question 34

The work function of sodium is = 2.9 * 10^-19 J. What is the maximum wavelength that can cause ejection of photoelectrons from a sodium surface?

A) 151 nm
B) 222 nm
C) 45.1 nm
D) 451 nm
E) 685 nm

Question 35

Which of the following photons has the lowest energy?

A) a photon from a Nd:YAG laser with $\lambda$ = 1,064 nm
B) a photon from an Ar⁺ laser with $\lambda$ = 514.5 nm
C) a photon from a Kr⁺ laser with $\lambda$ = 647 nm
D) a photon from an ArF laser with $\lambda$ = 193 nm
E) a photon from a He-Ne laser with $\lambda$ = 633 nm

Question 36

What is the energy (E, in J) of the photons emitted by an Ar⁺ laser with a wavelength of $\lambda$ = 488 nm?

A) 2.46 * 10¹⁸ J
B) 9.69 *10^-23 J
C) 1.36 *10^-36 J
D) 4.07 *10^-19 J
E) 2.46 * 10^-18 J

Question 37

Which of the following photons has the highest energy?

A) a photon from a Nd:YAG laser with $\lambda$ = 1,064 nm
B) a photon from an Ar⁺ laser with $\lambda$ = 514.5 nm
C) a photon from a Kr⁺ laser with $\lambda$ = 647 nm
D) a photon from an ArF laser with $\lambda$ = 193 nm
E) a photon from a He-Ne laser with $\lambda$ = 633 nm

Question 38

Indicate which of the following sources produces the highest energy photons.

A) a radio station with $\lambda$ = 106.7 MHz
B) a dentist's X-ray source with $\lambda$ = 100 pm
C) the laser in a CD player with $\lambda$ = 650 nm
D) a microwave oven with v= 6.0 * 10¹⁰ Hz
E) your cell phone with v = 1.750 GHz

Question 39

Which of the following sources produces the lowest energy photons?

A) a doctor's X-ray source
B) the heat lamp in your bathroom
C) a microwave oven
D) gamma rays from a star
E) radio waves from your local station

Question 40

The studies of light emitted by hot objects (Max Planck) and the photoelectric effect (Albert Einstein) revolutionized physics because they revealed ________

A) that energy is quantized.
B) that light intensity does not affect the number of electrons ejected from a metal.
C) that atomic spectra are due to the quantized transitions of electrons.
D) that blackbody radiation is continuous.
E) that atomic spectra are continuous.

Question 41

How much energy is required to ionize a He⁺ ion in its ground state?

A) 2.18 * 10^-18 J
B) 4.36 *10^-18 J
C) 8.72 *10^-18 J
D) 1.74 *10^-18 J

Question 42

Which of the transitions in the hydrogen atom energy-level diagram shown here is not possible?

A) a
B) b
C) c
D) d

Question 43

Electromagnetic radiation with a frequency of 8.6 *10¹⁴ Hz incident on an unknown metal surface causes ejection of photoelectrons with kinetic energies of 1.3 *10^-19 J. What is the unknown metal?

A) rubidium ( = 3.5 *10^-19 J)
B) gold (11ef1a66_0479_eb58_a3cb_57e06677e6de_TB3834_11 = 8.2 *10^-19 J)
C) nickel (11ef1a66_0479_eb58_a3cb_57e06677e6de_TB3834_11 = 8.3 *10^-19 J)
D) sodium (11ef1a66_0479_eb58_a3cb_57e06677e6de_TB3834_11 = 4.4 *10^-19 J)
E) platinum (11ef1a66_0479_eb58_a3cb_57e06677e6de_TB3834_11 = 9.1 *10^-19 J)

Question 44

Early photoelectric light detectors were based on cesium. Cesium metal has a work function of 3.43 *10^-19 J. What is the minimum frequency of electromagnetic radiation required to eject photoelectrons from a cesium surface?

A) 1.75 *10¹⁴/s
B) 3.15 * 10¹⁴/s
C) 5.17 * 10¹⁴/s
D) 1.55 * 10¹³/s
E) 7.24 * 10¹⁵/s

Question 45

Early photoelectric light detectors were based on cesium. Cesium metal has a work function of 3.43 *10^-19 J. What is the longest wavelength of light that could be detected with one of these detectors?

A) 759 nm
B) 579 nm
C) 679 nm
D) 767 nm
E) 455 nm

Question 46

Determine the wavelength of the line in the hydrogen atom spectrum corresponding to the n₁ = 3 to n₂ = 4 transition.

A) 1,094 nm
B) 1,875 nm
C) 656 nm
D) 335 nm
E) 109 nm

Question 47

Which of the transitions in the hydrogen atom energy-level diagram shown here requires the longest wavelength photon?

A) a
B) b
C) c
D) d

Question 48

What is the kinetic energy of the photoelectrons emitted from a sodium surface ( = 2.9 *10^-19 J) when it is irradiated by photons with a wavelength of 350 nm?

A) 2.9 *10^-19 J
B) 5.7 *10^-19 J
C) 0 J
D) 2.8 *10^-19 J
E) 3.6 * 10^-19 J

Question 49

Early photoelectric light detectors were based on cesium. Cesium metal has a work function of 3.43 *10^-19 J. What is the minimum photon energy needed to eject photoelectrons from a cesium surface?

A) 4.33 * 10^-17 J
B) 3.34 *10^-18 J
C) 3.43 *10^-20 J
D) 3.43 *10^-19 J
E) 1.99 *10^-21 J

Question 50

Which of the following metals would be an appropriate choice for the construction of a photon detector for 550 nm light?

A) sodium ( = 4.4 * 10^-19 J)
B) rubidium (11ef1a66_0479_eb58_a3cb_57e06677e6de_TB3834_11 = 3.5 *10^-19J)
C) barium (11ef1a66_0479_eb58_a3cb_57e06677e6de_TB3834_11= 4.3 *10^-19 J)
D) gold (11ef1a66_0479_eb58_a3cb_57e06677e6de_TB3834_11 = 8.2 *10^-19 J)
E) platinum (11ef1a66_0479_eb58_a3cb_57e06677e6de_TB3834_11 = 9.1 *10^-19 J)

Question 51

Early photoelectric light detectors were based on cesium. Cesium metal has a work function of 3.43 *10^-19 J. What is the kinetic energy of the photoelectrons ejected from a cesium surface when exposed to blue light at 400 nm?

A) 5.41*10^-18 J
B) 5.14 *10^-20 J
C) 2.54*10^-17 J
D) 1.54 *10^-19 J
E) 2.54 * 10^-19 J

Question 52

Which of the transitions in the following hydrogen atom energy-level diagram involves the shortest wavelength photon?

A) a
B) b
C) c
D) d

Question 53

Early photoelectric light detectors were based on cesium. Cesium metal has a work function of 3.43 *10^-19 J. What is the velocity of the photoelectrons ejected from a cesium surface when exposed to blue light at 400 nm?

A) 2.90 * 10⁸ m/s
B) 2.90 *10⁵ m/s
C) 5.81 * 10² m/s
D) 5.81 * 10⁸ m/s
E) 5.81 *10⁵ m/s

Question 54

The change in energy of a one-electron atom or ion for an electronic transition from the initial energy level n_i to the final energy level n_f is given by
$\Delta$ E = -(2.18*10^-18 J)
Z² $\left( \frac { 1 } { n _ { f } ^ { 2 } } - \frac { 1 } { n _ { i } ^ { 2 } } \right.$
Which of the following species will have the longest wavelength emission line for the transition between the n_i = 2 and n_f = 1 levels?

A) H
B) He⁺
C) Li²⁺
D) Be³⁺
E) B⁴⁺

Question 55

Which transition in a hydrogen atom will cause emission of the shortest wavelength photon?

A) n₁ = 4 to n₂ = 3
B) n₁ = 4 to n₂ = 2
C) n₁ = 3 to n₂ = 2
D) n₁ = 3 to n₂ = 1
E) n₁ = 10 to n₂ = 9

Question 56

Which transition in a hydrogen atom requires the largest change in energy?

A) n₁ = 2 to n₂ = 3
B) n₁ = 2 to n₂ = 4
C) n₁ = 1 to n₂ = 3
D) n₁ = 1 to n₂ = 2
E) n₁ = 9 to n₂ = 10

Question 57

Which of the following objects, all moving at the same speed, will have the largest de Broglie wavelength?

A) a proton
B) an electron
C) a bowling ball
D) a neon atom
E) a neutron

Question 58

What wavelength of light is required to cause the ejection of photoelectrons with kinetic energies of 5.0 *10^-20 J from a calcium surface ( = 4.60 * 10^-19 J)?

A) 485 nm
B) 390 nm
C) 308 nm
D) 632 nm
E) 480 nm

Question 59

How much energy is required to ionize one mole of hydrogen atoms in their ground state?

A) 1,312 kJ
B) 2.18 kJ
C) 218 kJ
D) 2,178 kJ
E) 131.2 kJ

Question 60

The energy of a one-electron atom is given by E = -(2.18 *10^-18 J) $$\left( \frac { z } { n } \right) ^ { 2 }$$ where Z is the atomic number of the element. Which of the following one-electron ions has the largest ionization energy?

A) Li²⁺
B) Be³⁺
C) He⁺
D) B⁴⁺
E) C⁵⁺

Question 61

A shell is defined by ________

A) the $\ell$
Quantum number.
B) the m_l quantum number.
C) the m_s quantum number.
D) the n quantum number.
E) both the $\ell$
And m_l quantum numbers.

Question 62

Which subshell only has five orbitals?

A) $\ell$ = 2
B) $\ell$ = 1
C) $\ell$ = 5
D) $\ell$ = 3
E) $\ell$ = 4

Question 63

What is the speed of an argon atom that has a de Broglie wavelength of 5.2 pm?

A) 0.52 m/s
B) 5.2* 10³ m/s
C) 1.9 *10³ m/s
D) 1.9 m/s
E) 25 m/s

Question 64

Which statement A-D about the wave function for a single electron is not correct?

A) A French graduate student named Louis de Broglie first had the idea that an electron should be described as a wave
B) Louis de Broglie postulated that the wavelength of an electron is given in terms of Planck's constant and its momentum, $\lambda$ = h/p.
C) The square of the amplitude of the wave function at a particular point in space gives the probability density of finding the electron at that point.
D) An electronic wave function can never be 0 because that would mean the electron does not exist.
E) Statements A-D are all correct.

Question 65

In quantum mechanics, an atomic orbital ________

A) provides the position of an electron at any instant of time in the space around an atomic nucleus.
B) locates all the electrons in an atom.
C) is identical to the orbits Bohr used in his analysis of the hydrogen atom.
D) identifies the most probable position of an atomic nucleus.
E) provides the probability of finding an electron at any point in the space around an atomic nucleus.

Question 66

Which statement A-D about the wave function for a single electron is not correct?

A) A French graduate student named Louis de Broglie first had the idea that an electron should be described as a wave.
B) Since = c, an expression for the wavelength of an electron can be found by combining Einstein's equation that relates mass and energy (E = mc²) with his equation that gives the energy of a photon in terms of its frequency (E = 11ef1a67_6eab_04e9_a3cb_813dba8b61e6_TB3834_11).
C) The square of the wave function's amplitude at a particular point in space gives the probability density of finding the electron at that point.
D) Wave functions can have nodes, which are points where the amplitude is zero.
E) Statements A-D are all correct.

Question 67

Which statement about the quantum numbers that identify an atomic orbital is not correct?

A) The angular momentum quantum number, $\ell$
, identifies the shape of an orbital.
B) The value of the angular momentum quantum number can range from 0 to n, where n is the principal quantum number for the orbital.
C) Orbitals with the same value for the principal quantum number and the angular momentum quantum number are said to be in the same subshell.
D) Orbitals with the same values for the principal quantum number and the angular momentum quantum number have the same energy.
E) The value for the angular momentum quantum number also is designated by a letter:
S = 0, p = 1, d = 2, f = 3, etc.

Question 68

According to de Broglie, if the circumference of the electron's orbit in the hydrogen atom is twice the electron's wavelength, the orbit will ________

A) decay until the electron falls into the nucleus.
B) diverge, allowing the electron to escape.
C) be stable.
D) cause the electron to emit a photon.
E) not be circular.

Question 69

Which statement A-D about the wave function for a single electron is not correct?

A) A French graduate student named Louis de Broglie first had the idea that an electron should be described as a wave.
B) Louis de Broglie postulated that the wavelength of an electron is given in terms of Planck's constant and its momentum, $\lambda$ = h/p.
C) The amplitude of a wave function at a particular point in space equals the probability density of finding the electron at that point.
D) Wave functions can have nodes, which are points where the amplitude is zero.
E) Statements A-D are all correct.

Question 70

De Broglie reasoned that for the electron in the hydrogen atom to behave as a stable circular wave, the circumference of the electron's orbit must be ________

A) equal to the wavelength of the electron.
B) an integer multiple of the electron's wavelength.
C) a half integer multiple of the electron's wavelength.
D) twice the wavelength of the electron.
E) twice the diameter of the orbit.

Question 71

The mathematical description of an electron as a wave was developed by ________

A) Bohr.
B) Heisenberg.
C) Einstein.
D) De Broglie.
E) Schrödinger.

Question 72

Which of the following electrons will have the smallest de Broglie wavelength?

A) an electron moving 220 m/sec
B) an electron moving 20 mi/hr
C) an electron moving 75 km/hr
D) an electron moving at 25% the speed of light
E) an electron at rest with no velocity

Question 73

Recently, buckyballs (C₆₀) became the largest objects with a measured de Broglie wavelength. If the mass of a C₆₀ molecule is 1.20 *10^-24 kg, what will be its de Broglie wavelength if it is moving at a speed of 220 m/sec?

A) 2.52 pm
B) 2.52 fm
C) 2.52 m
D) 1.20 pm
E) 5.22 m

Question 74

A shell consists of all ________

A) electrons with the same $\ell$
Quantum number.
B) orbitals with the same quantum numbers.
C) orbitals with the same principal quantum number.
D) electrons with the same magnetic quantum number.
E) orbitals with the same $\ell$
And m_l quantum numbers.

Question 75

Subshells are ________

A) orbitals with the same principal and angular momentum quantum numbers.
B) orbitals with the same principal quantum numbers.
C) orbitals with the same angular momentum quantum numbers.
D) orbitals with the same angular momentum and magnetic quantum numbers.
E) orbitals with the same spin quantum number.

Question 76

How many orbitals are possible for the n = 2 shell?

A) 1
B) 2
C) 3
D) 4
E) 5

Question 77

A proton in a cyclotron has a velocity of 2 * 10⁸ m/s, which is nearly the speed of light. The uncertainty in the velocity is 1%. What is the minimum uncertainty in the position of the proton in meters? The proton mass is 2 *10^-27 kg.

A) 3 *10^-11 m
B) 1 * 10^-22 m
C) 1 *10^-18 m
D) 3 *10^-41 m
E) 1 *10^-17 m

Question 78

How many orbitals that have the principal quantum number equal to 3 are there in an atom?

A) 2
B) 4
C) 9
D) 16
E) 18

Question 79

Which statement about the quantum numbers that identify an atomic orbital is not correct?

A) The principal quantum number, n, identifies the size of an atomic orbital.
B) The angular momentum quantum number, $\ell$
, identifies the shape of an atomic orbital.
C) The magnetic quantum number, m_l, identifies the orientation of the orbital in space.
D) The magnetic quantum number can have values that range from - $\ell$
To + $\ell$
In integer steps.
E) The principal quantum number alone, n, identifies the energy of an atomic orbital.

Question 80

Which statement about the quantum numbers that identify an atomic orbital is not correct?

A) The principal quantum number, n, identifies the size and energy of an orbital.
B) The value of the principal quantum number can be 0 or a positive or negative integer.
C) Orbitals with the same value for the principal quantum number are said to be in the same shell.
D) Orbitals with larger values of the principal quantum number locate the electron farther from the atomic nucleus.
E) Orbitals with smaller values of the principal quantum number describe electrons with a lower energy.