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Test Review

Test Review. 5.1 Electromagnetic Radiation 5.2 Atomic Spectra and Energy Levels. ANSWER KEY. 1. Which of the following is the correct symbol for wavelength of electromagnetic radiation? . c γ ν λ h.

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Test Review

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  1. Test Review 5.1 Electromagnetic Radiation 5.2 Atomic Spectra and Energy Levels

  2. ANSWER KEY

  3. 1. Which of the following is the correct symbol for wavelength of electromagnetic radiation? • c • γ • ν • λ • h

  4. 2. Which of the following are the correct units forfrequencyof electromagnetic radiation? • joules • hertz • nanometers • wavelength • electron volt

  5. 3. Which principal energy level change by the electron of a hydrogen atom will cause the greatest amount of energy to be absorbed? • n = 5 to n = 2 • n = 2 to n = 5 • n = 4 to n = 2 • n = 2 to n = 4 • n = 3 to n = 4

  6. 4. Which diagram shows a wave with the highest frequency? • A • B • C • D

  7. 5. As an atom in the excited state returns to the ground state, the energy of the atom • remains the same • increases • decreases

  8. 6. What causes the emission of radiant energy that produces characteristic spectral lines? • neutron absorption by the nucleus • movement of electrons to higher energy levels C. return of electrons to lower energy levels • gamma ray emission from the nucleus • electromagnetic radiation in the visible range being released by the nucleus

  9. 7. Which form of electromagnetic radiation travels the fastest through the vacuum of space? • visible light • gamma rays • radio waves of any type • microwaves • all travel at the same speed

  10. 8. Which form of electromagnetic radiation is also known as thermal radiation or “heat”? • ultraviolet • infrared • visible light • microwaves • x-rays

  11. 9. Which form of electromagnetic radiation has the highest frequency? • cosmic rays • long-wave radio • visible light • gamma rays • all have the same frequency

  12. 10. Which form of visible light has the most energy? • red light • yellow light • green light • violet light • all have the same energy

  13. 11. Which form of electromagnetic radiation causes the majority of skin cancers? • visible light • infrared light • ultraviolet light • x-rays • microwaves

  14. 12. Which form of electromagnetic radiation is caused by the energy emissions from the nuclei of radioactive atoms? • radio waves • visible light • ultraviolet light • gamma rays • microwaves

  15. 13. __ is/are mostly stopped by the Earth’s ozone layer while __ is/are mostly deflected by the Earth’s magnetic field. • infrared, ultraviolet • ultraviolet, cosmic rays • microwaves, VHF waves • gamma rays, infrared • microwaves, ultraviolet

  16. 14. __ is/are stopped when they encounter nitrogen molecules in the Earth’s atmosphere • ultraviolet • cosmic rays • microwaves • gamma rays • visible light

  17. 15. Which type of electromagnetic radiation is actually made up of charged particles rather than just waves of energy? • ultraviolet • cosmic rays • microwaves • gamma rays • infrared

  18. 16. Which type of electromagnetic radiation is ionizing radiation? • ultraviolet • X-ray • microwaves • radio • infrared

  19. 17. In an atom, an electron in principal energy level ___ would have the least energy. • n = 1 • n = 2 • n = 3 • n = 4 • n = 5

  20. 18. An electron occupying the lowest energy level is said to be ___. • farthest from the nucleus • neutral • in the ground state • ionized • positively charged

  21. 19. Which of the following is stated correctly? • an photon carries a quantum of energy • a quantum carries a photon of energy

  22. 20. Calculate the frequency of electromagnetic radiation with a wavelength of 560 nm. use the equation: c = λν Step 1:rearrange the formula to solve for ν ν = c /λ Step 2:convert nanometers to meters P T G M k h d – 0 – d c m μ n Å p f a 560 nm = 5.60 x 10−7 m Step 3:plug the known amounts into the formula and solve 3.00 x 108 m/ s v = 5.60 x 10−7 m → 5.36 x 1014 Hz

  23. 21. Calculate the energy of a photon a wave- length of 560 nm. use the equation: Ephoton= hv Step 1:we know from question # 20 that frequency (v) at 560 nm = 5.36 x 1014 Hz Step 2:recall that h = Plank’s constant 6.63 x 10−34 J•s Step 3:plug the known amounts into the formula and solve Ephoton = (6.63 x 10−34 J•s)(5.36 x 1014/s) → 3.56 x 10−19 J

  24. 22. From what portion of the electromagnetic spectrum was the electromagnetic radiation of Questions # 20 and # 21 ? visible light

  25. 23. What color was the light from Questions # 20 and # 21 ? green

  26. 24. Calculate the energy of a photon a wave- length of 310 nm. use the equation: Ephoton= hc/λ Step 1:convert 310 nm to m P T G M k h d – 0 – d c m μ n Å p f a 310 nm = 3.10 x 10−7 m Step 2: plug the known amounts into the formula and solve Ephoton = [(3.00 x 108m/s) (6.63 x 10−34 J•s)] / 3.10 x 10−7 m → 6.42 x 10−19 J

  27. 25. Calculate the wavelength, in nm, of electro- magnetic radiation with a frequency 2.50 x 1016 Hz. use the equation: c = λν Step 1:rearrange the formula to solve for λ λ= c /ν Step 2: plug the known amounts into the formula and solve for λ in meters 3.00 x 108 m/ s λ = 2.50 x 1016 s → 1.20 x 10−8 m Step 3:convert meters to nanometers P T G M k h d – 0 – d c m μ n Å p f a 1.20 x 10−8 m = 12 nm

  28. 26. The characteristic bright-line spectrum of an atom is produced by its • protons emitting quanta • electrons emitting quanta • protons absorbing quanta • electrons absorbing quanta • forming an ionic bond

  29. 27. Which of the following is the correct relationship between wavelength and energy? • as λ↑, E↓ (inverse) • as λ↓,E↓ (direct)

  30. 28. A photon of which of the following forms of electromagnetic radiation would have the largest quantum of energy? • red visible light • infrared light • ultraviolet light • microwaves • violet visible light

  31. 29. Which of the following forms of electro- magnetic radiation would have the smallest frequency? • red visible light • infrared light • ultraviolet light • microwaves • violet visible light

  32. 30. The following show some of the possible transitions of the electron in the hydrogen atom. Which series of transitions would result in a visible atomic spectrum? • Lyman • Balmer • Paschen • Brackett • Pfund FYI: Lyman = UV spectrum Pachen = IR spectrum Backett = IR spectrum Pfund = IR spectrum

  33. 31. Which transition would represent the green line of hydrogen’s visible emission spectrum? • n = 6 to n = 2 • n = 5 to n = 1 • n = 4 to n = 2 • n = 7 to n = 5 • n = 4 to n = 1

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