5.

Which scientist first proposed that the electron in the hydrogen atom can have only certain energies?

A) Planck B) Einstein C) Bohr D) Rydberg E) Heisenberg

C

6.

Which scientist first proposed that particles of matter could have wave properties?

A) Einstein B) Planck C) de Broglie D) Compton E) Heisenberg

C

7.

Which scientist demonstrated that photons transferred momentum during collisions with matter?

A) Bohr B) de Broglie C) Planck D) Compton E) Billiard

D

8.

Who proposed the principle which states that one cannot simultaneously know the exact position and velocity of a particle?

A) Einstein B) Planck C) Heisenberg D) Compton E) de Broglie

C

9.

Which word best describes the phenomenon which gives rise to a rainbow?

A) reflection

B) dispersion

C) diffraction

D) interference

E) deflection

B

10.

Contact lenses can focus light due to the ____________ of the waves.

A) diffraction

B) reflection

C) refraction

D) dispersion

E) interference

C

11.

The interference pattern seen when light passes through narrow, closely spaced slits, is due to

A) diffraction.

B) reflection.

C) refraction.

D) dispersion.

E) deflection.

A

12.

Interference of light waves

A)

separates light into its component colors.

B)

creates a pattern of light and dark regions.

C)

focuses a broad beam of light into a point.

D)

bends light as it passes the edge of an object.

E)

creates a laser beam.

B

13.

Select the arrangement of electromagnetic radiation which starts with the lowest energy and increases to greatest energy.

A)

radio, visible, infrared, ultraviolet

B)

infrared, visible, ultraviolet, microwave

C)

visible, ultraviolet, infrared, gamma rays

D)

X-radiation, visible, infrared, microwave

E)

microwave, infrared, visible, ultraviolet

E

14.

Select the arrangement of electromagnetic radiation which starts with the lowest energy and increases to greatest energy.

A)

radio, infrared, ultraviolet, gamma rays

B)

radio, ultraviolet, infrared, gamma rays

C)

gamma rays, infrared, radio, ultraviolet

D)

gamma rays, ultraviolet, infrared, radio

E)

infrared, ultraviolet, radio, gamma rays

A

15.

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

A) 1 kilohertz

B) 1 terahertz

C) 1 dekahertz

D) 1 gigahertz

E) 1 megahertz

D

16.

Select the arrangement of electromagnetic radiation which starts with the lowest wavelength and increases greatest wavelength.

A)

radio, infrared, ultraviolet, gamma rays

B)

radio, ultraviolet, infrared, gamma rays

C)

gamma rays, radio, ultraviolet, infrared

D)

gamma rays, infrared, radio, ultraviolet

E)

gamma rays, ultraviolet, infrared, radio

E

17.

Electromagnetic radiation can be specified by its wavelength (l), its frequency (n) or its period (t). The period t is the time it takes one complete wavelength to pass a point in space. Based on this information, what is the mathematical relationship between n and t?

A) n = 1/t B) n = t C) t = n/c D) c = t x n E) t = c/n

A

18.

Electromagnetic radiation of 500 nm wavelength lies in the __________ region of the spectrum.

A) infrared B) visible C) ultraviolet D) X-ray E) g-ray

B

19.

The FM station KDUL broadcasts music at 99.1 MHz. Find the wavelength of these waves.

A) 1.88 × 10^–2 m B) 0.330 m C) 3.03 m D) 5.33 × 10² m E) > 10³ m

C

20.

The AM station KBOR plays your favorite music from the 20's and 30's at 1290 kHz. Find the wavelength of these waves.

A) 4.30 × 10^–2 m B) 0.144 m C) 6.94 m D) 232 m E) > 10³ m

D

21.

An infrared wave has a wavelength of 6.5 × 10^–4 cm. What is this distance in angstroms, Å?

A) 6.5 × 10^–4 Å

D) 6.5 × 10⁴ Å

B) 2.2 × 10^–4 Å

E) 6.5 × 10⁶ Å

C) 4.6 × 10³ Å

D

22.

A radio wave has a frequency of 8.6 × 10⁸ Hz. What is the energy of one photon of this radiation?

A) 7.7 × 10^–43 J

D) 1.7 × 10^–16 J

B) 2.3 × 10^–34 J

E) > 10^–15 J

C) 5.7 × 10^–25 J

C

23.

Infrared radiation from the sun has a wavelength of 6200 nm. Calculate the energy of one photon of that radiation.

A) 4.l × 10^–39 J

D) 3.2 × 10^–26 J

B) 4.l × 10^–30 J

E) between 10^–20 and 10^–19 J

C) 3.2 × 10^–29 J

E

24.

Green light has a wavelength of 5200 Å. Calculate the energy of one photon of green light.

A) 3.4 × 10^–40 J

D) 3.4 × 10^–27 J

B) 3.4 × 10^–30 J

E) 3.8 × 10^–19 J

C) 3.8 × 10^–29 J

E

25.

If the energy of a photon is 1.32 × 10^–18 J, what is its wavelength in nm?

A) 1.50 × 10^–7 nm

D) 1.99 × 10²⁴ nm

B) 150. nm

E) none of the above

C) 1.99 × 10¹⁵ nm

B

26.

A photon has an energy of 5.53 × 10^–17 J. What is its frequency in s^–1?

A) 3.66 × 10^–50 s^–1

D) 2.78 × 10⁸ s^–1

B) 1.20 × 10^–17 s^–1

E) 8.35 × 10¹⁶ s^–1

C) 3.59 × 10^–9 s^–1

E

27.

A modern compact fluorescent lamp contains 1.4 mg of mercury. If each mercury atom in the lamp were to emit a single photon of wavelength 254 nm, how many joules of energy would be emitted?

A) 7.8 × 10^-19 J B) 3.3 J C) 6.6 × 10² J D) 3.3 × 10³ J E) 4.2 × 10¹⁸ J

B

28.

For potassium metal, the work function f (the minimum energy needed to eject an electron from the metal surface) is 3.68 × 10^–19 J. Which is the longest wavelength of the following which could excite photoelectrons?

A) 550. nm B) 500. nm C) 450. nm D) 400. nm E) 350. nm

B

29.

Platinum, which is widely used as a catalyst, has a work function f (the minimum energy needed to eject an electron from the metal surface) of 9.05 × 10^–19 J. What is the longest wavelength of light which will cause electrons to be emitted?

A) 2.196 × 10^–7 m

D) 1.370 × 10¹⁵ m

B) 4.553 × 10^–6 m

E) > 10⁶ m

C) 5.654 × 10² m

A

30.

In the photoelectric effect, a photon with an energy of 5.3 × 10^-19 J strikes an electron in a metal. Of this energy, 3.6 × 10^-19 J is the minimum energy required for the electron to escape from the metal. The remaining energy appears as kinetic energy of the photoelectron. What is the velocity of the photoelectron, assuming it was initially at rest?

A) 3.7 × 10¹⁴ m/s

D) 6.1 × 10⁵ m/s

B) 3.7 × 10¹¹ m/s

E) 1.7 × 10^-19 m/s

C) 1.9 × 10⁶ m/s

D

31.

Consider the following adjectives used to describe types of spectrum:

continuous line atomic emission absorption

How many of them are appropriate to describe the spectrum of radiation given off by a black body?

A) none B) one C) two D) three E) four

C

32.

Consider the following adjectives used to describe types of spectrum:

continuous line atomic emission absorption

How many of them are appropriate to describe the spectrum of radiation absorbed by a sample of mercury vapor?

A) one B) two C) three D) four E) five

C

33.

What type of spectrum, if any, would be produced if the light radiated by a heated atomic gas were to be dispersed through a prism?

A)

a continuous band of color

B)

a continuous band of color with some dark lines (missing wavelengths)

C)

only blue light

D)

only red light

E)

discrete lines of different colors

E

34.

Use the Rydberg equation to calculate the frequency of a photon absorbed when the hydrogen atom undergoes a transition from n₁ = 2 to n ₂ = 4. (R = 1.096776 × 10⁷ m^–1)

A) 2.056 × 10⁶ s^–1

D) 8.226 × 10¹⁴ s^–1

B) 2.742 × 10⁶ s^–1

E) > 10¹⁵ s^–1

C) 6.165 × 10¹⁴ s^–1

C

35.

Line spectra from all regions of the electromagnetic spectrum, including the Paschen series of infrared lines for hydrogen, are used by astronomers to identify elements present in the atmospheres of stars. Calculate the wavelength of the photon emitted when the hydrogen atom undergoes a transition from n = 5 to n = 3. (R = 1.096776 × 10⁷ m^–1)

A) 205.1 nm B) 384.6 nm C) 683.8 nm D) 1282 nm E) > 1500 nm

D

36.

According to the Rydberg equation, the line with the shortest wavelength in the emission spectrum of atomic hydrogen is predicted to lie at a wavelength (in nm) of

A) 91.2 nm.

D) 1.10 × 10¹⁶ nm.

B) 1.10 × 10^–2 nm.

E) none of the above.

C) 1.10 × 10² nm.

A

37.

According to the Rydberg equation, the longest wavelength (in nm) in the series of H-atom lines with n₁ = 3 is

A) 1875 nm. B) 1458 nm. C) 820. nm. D) 656 nm. E) 365 nm.

A

38.

An electron in the n = 6 level emits a photon with a wavelength of 410.2 nm. To what energy level does the electron move?

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

B

39.

The Bohr theory of the hydrogen atom predicts the energy difference (in J) between the n = 3 and the n = 5 state to be

A) 8.72 × 10^–20 J.

D) 1.55 × 10^–19 J.

B) 1.36 × 10^–19 J.

E) 1.09 × 10^–18 J.

C) 2.42 × 10^–19 J.

D

40.

Excited hydrogen atoms radiate energy in the

A)

infrared region only.

B)

visible region only.

C)

ultraviolet region only.

D)

visible and ultraviolet regions only.

E)

infrared, visible, and ultraviolet regions.

E

41.

According to the Bohr theory of the hydrogen atom, the minimum energy (in J) needed to ionize a hydrogen atom from the n = 2 state is

A) 2.18 × 10^–18 J.

D) 3.03 × 10^–19 J.

B) 1.64 × 10^–18 J.

E) none of the above.

C) 5.45 × 10^–19 J.

C

42.

The ionization energy is the energy needed to remove an electron from an atom. In the Bohr model of the hydrogen atom, this means exciting the electron to the n = ¥ state. What is the ionization energy in kJ/mol, for hydrogen atoms initially in the n = 2 energy level?

A) 290 kJ/mol

D) 983 kJ/mol

B) 328 kJ/mol

E) 1311 kJ/mol

C) 656 kJ/mol

B

43.

For all the allowed vibration(s) (wavelength(s)) of a plucked guitar string, what is the correct relationship between the length of the string, L, and the wavelength, l?

A) L = l/2

D) L = nl where n is a positive integer

B) L = l

E) L = 1/l

C) L = nl/2 where n is a positive integer

C

44.

A sprinter must average 24.0 mi/h to win a 100-m dash in 9.30 s. What is his wavelength at this speed if his mass is 84.5 kg?

A) 7.29 × 10^–37 m

D) 1.34 × 10^–30 m

B) 3.26 × 10^–37 m

E) none of the above

C) 5.08 × 10^–30 m

A

45.

The de Broglie equation predicts that the wavelength (in m) of a proton moving at 1000. m/s is

A) 3.96 × 10^–10 m.

D) 2.52 × 10⁹ m.

B) 3.96 × 10^–7 m.

E) > 10¹⁰ m.

C) 2.52 × 10⁶ m.

A

46.

According to the Heisenberg uncertainty principle, if the uncertainty in the speed of an electron is 3.5 × 10³ m/s, the uncertainty in its position (in m) is at least

A) 1.7 × 10^–8 m.

D) 66 m.

B) 6.6 × 10^–8 m.

E) none of the above.

C) 17 m.

A

47.

The size of an atomic orbital is associated with

A)

the principal quantum number (n).

B)

the angular momentum quantum number (l).

C)

the magnetic quantum number (m_l).

D)

the spin quantum number (m_s).

E)

the angular momentum and magnetic quantum numbers, together.

A

48.

The shape of an atomic orbital is associated with

A)

the principal quantum number (n).

B)

the angular momentum quantum number (l).

C)

the magnetic quantum number (m_l).

D)

the spin quantum number (m_s).

E)

the magnetic and spin quantum numbers, together.

B

49.

The orientation in space of an atomic orbital is associated with

A)

the principal quantum number (n).

B)

the angular momentum quantum number (l).

C)

the magnetic quantum number (m_l).

D)

the spin quantum number (m_s).

E)

none of the above.

C

50.

Atomic orbitals developed using quantum mechanics

A)

describe regions of space in which one is most likely to find an electron.

B)

describe exact paths for electron motion.

C)

give a description of the atomic structure which is essentially the same as the Bohr model.

D)

allow scientists to calculate an exact volume for the hydrogen atom.

E)

are in conflict with the Heisenberg Uncertainty Principle.

A

51.

In an atom, the square of an electron's wave function

A)

becomes zero at the nucleus.

B)

is smallest near the nucleus.

C)

is largest near the nucleus.

D)

may be zero at more than one point.

E)

tends to infinity at large distances from the nucleus.

D

52.

The energy of an electron in the hydrogen atom is determined by

A)

the principal quantum number (n) only.

B)

the angular momentum quantum number (l ) only.

C)

the principal and angular momentum quantum numbers (n & l ).

D)

the principal and magnetic quantum numbers (n & m_l).

E)

the principal, angular momentum and magnetic quantum numbers.

A

53.

Which of the following is a correct set of quantum numbers for an electron in a 3d orbital?

A) n = 3, l = 0, m_l = –1

D) n = 3, l = 3, m_l = +2

B) n = 3, l = 1, m_l = +3

E) n = 3, l = 2, m_l = –2

C) n = 3, l = 2, m_l = 3

E

54.

Which of the following is a correct set of quantum numbers for an electron in a 5f orbital?

A) n = 5, l = 3, m_l = +1

D) n = 4, l = 2, m_l = +1

B) n = 5, l = 2, m_l = +3

E) n = 5, l = 4, m_l = 3

C) n = 4, l = 3, m_l = 0

A

55.

In the quantum mechanical treatment of the hydrogen atom, which one of the following combinations of quantum numbers is not allowed?

E

56.

Which one of the following sets of quantum numbers can correctly represent a 3p orbital?

A) n = 3 l = 1 m_l = 2

D) n = 3 l = 1 m_l = –1

B) n = 1 l = 3 m_l = 3

E) n = 3 l = 0 m_l = 1

C) n = 3 l = 2 m_l = 1

D