Extra Practice Week 7 PDF

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Week 7 Practices with Answers Answers are posted at the end on the last page. 1 1 ∆  2.18  10 󰇧  󰇨          1  1  v  h = 6.626  10−34 J  s



 

  ∆v 

 4

1 m = 109 nm

c = 3.00  108 m/s (a)

1. In the following diagram of a wave A) (a) is amplitude and (b) is wavelength B) (a) is frequency and (b) is amplitude C) (a) is wavelength and (b) is frequency D) (a) is amplitude and (b) is frequency E) (a) is wavelength and (b) is amplitude

(b)

2. A(n) _________ is a point at which a standing wave has zero amplitude. A) crevice B) node C) pit D) burrow

E) orbital

3. What is the frequency of light having a wavelength of 360 nm? A) 8.3  1014 s‒1

B) 1.2  10‒6 s‒1

C) 8.3  105 s‒1

D) 108 s‒1

E) 1.2  10‒15 s‒1

4. Select the arrangement of electromagnetic radiation which starts with the shortest wavelength and increases to longest 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 5. Which of the following wavelengths of electromagnetic radiation has the highest energy? A) 450. nm C) 3.50  10‒9 m D) 8.40  10‒7 m ‒5 B) 225 nm E) 2.50  10 m 6. What is the energy in joules of one photon of microwave radiation with a wavelength 0.122 m? A) 2.70  10–43 J B) 5.43  10–33 J

C) 1.63  10–24 J D) 4.07  10–10 J

E) 2.46  109 J

7. What is the energy in joules of one mole of photons associated with red light of wavelength 7.00  102 nm? A) 256 kJ B) 1.71  105 J C) 4.72  10–43 J D) 12.4 kJ E) 2.12  1042 J 8. Electrons in an orbital with l = 3 are in a/an _____________. A) d orbital B) f orbital C) g orbital D) p orbital

E) s orbital

9. What is the wavelength of light having a frequency of 4.8  1014 s‒1? A) 0.0016 nm B) 1600 m C) 630 nm D) 1600 nm E) 6.3  10‒7 nm

10. Calculate the wavelength associated with a 20Ne+ ion moving at a velocity of 2.0  105 m/s. The atomic mass of a 20Ne is 3.32  10‒26 kg. A) 1.7  10‒40 m C) 1.0  10–16 m E) 9.7  1012 m –18 –13 B) 1.0  10 m D) 1.0  10 m 11. 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 is at least what? (electron mass = 9.11  10‒31 kg). C) 17 m E) None of these choices is correct A) 1.7  10‒8 m D) 66 m B) 6.6  10‒8 m 12. 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 (ml). D) the spin quantum number (ms). E) the magnetic and spin quantum numbers, together. 13. 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. 14. Which of the following statements regarding the Bohr model of the hydrogen atom is incorrect? A) Bohr's model shows the electron circling the nucleus in fixed orbits. B) In Bohr's model, electrons could exist between orbits. C) In Bohr's model, when an electron absorbs energy, it can move to a higher-energy orbit. D) In Bohr's model, when an electron emits energy, it can move to a lower-energy orbit. E) In Bohr's model, n = 1 is the lowest energy orbit. 15. The wavelength of the blue light given off by a mercury vapor street lamp is 436 nm. What is the frequency of this light in hertz (s–1)? A) 6.88  105 s–1 C) 1.45  10–6 s–1 E) 1.31  102 s–1 14 –1 –13 –1 B) 6.88  10 s D) 1.45  10 s 16. What is the energy of a photon of yellow light whose wavelength is 589 nm? A) 3.37  10–19 J C) 1.77  102 J E) 3.38  10–28 J –10 5 B) 3.37  10 J D) 5.09  10 J 17. Calculate the energy, in joules, required to excite a hydrogen atom by causing an electronic transition from the n = 1 to the n = 4 principal energy level. A) 2.07  10–29 J C) 2.04  10–18 J E) 2.19  105 J –19 –17 B) 2.25  10 J D) 3.27  10 J 18. Calculate the wavelength, in nanometers, of the light emitted by a hydrogen atom when its electron falls from the n = 7 to the n = 4 principal energy level. A) 9.18  10–20 nm C) 2.16  10–6 nm E) 1.38  1014 nm –20 3 B) 4.45  10 nm D) 2.16  10 nm 19. Calculate the frequency of the light emitted by a hydrogen atom during a transition of its electron from the n = 6 to the n = 3 principal energy level. A) 1.82  10–19 /s C) 2.74  1014/s E) 1.64  1015 /s 13 14 B) 9.13  10 /s D) 3.65  10 /s Answers: 1E, 2B, 3A, 4E, 5C, 6C, 7B, 8B, 9C, 10D, 11A, 12B, 13A, 14B, 15B, 16A, 17C, 18D, 19C...