PhysicsLAB: Atomic Models and Spectra

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Worksheet
Atomic Models and Spectra

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1. Alpha particles were repelled by the atomic nucleus in Rutherford's gold foil experiment cause they are

(A) negatively charged(B) positively charged(C) very large and massive

2. Most of the alpha particles that were fired through the gold foil emerged un-deflected because they

(A) passed through the empty regions of the gold foil
(B) were attracted to the nucleus
(C) were attracted to the electrons

3. A few of the alpha particles bounced backwards because they

(A) struck the centers, nuclei, of the gold atoms head-on and recoiled
(B) collided with the shells of the negatively charged electrons surrounding the gold nuclei and recoiled

4. Rutherford's experiment discovered that

(A) electron clouds surround the nucleus
(B) electrons are negatively charged
(C) the atom is mostly empty space surrounding a small, positively charged, massive nucleus

5. True or False. Classical physicists were correct when they stated that electrons radiate energy as they accelerate around the nucleus within a single orbital.

TrueFalse

6. Atoms are considered to be excited when

(A) their electrons return to their stable states
(B) an electron is raised in any way to a higher energy level
(C) the nucleus is raised in any way to a higher energy state

7. Which has the greatest energy with respect to the atomic nucleus?

(A) electrons in inner electron shells
(B) electrons in outer electron shells

8. Electrons emit light when they transition from a

(A) a lower energy state to a higher energy level
(B) a higher energy level to a lower energy state

9. The energy of the emitted photons is equal to the ____ in the energies between the two energy levels between which it is transitioning.

(A) sum(B) difference(C) product(D) quotient

10. What is the name of the visible series in the hydrogen spectrum?

(A) Balmer(B) Fraunhofer(C) Lyman(D) Paschen(E) Ritz

11. What formula is used to calculate the energy of a photon?

12. Specifically, what does the letter "h" stand for in your answer to question #11?

13. In your answer to question #11, what does "f" stand for?

14. Which has a higher energy per photon?

(A) red light(B) green light(C) blue light

15. When an accelerated electron in an electrified neon sign strikes one of the neon atoms,

(A) each smash boosts orbital electrons in the neon atom to higher energy levels
(B) the kinetic energy lost by the accelerated electron equals the energy difference between two orbitals in an neon atom
(C) the energy lost by the accelerated electron is eventually released as the characteristic red light of neon's emission spectra
(D) ALL of the above are true

16. True or False. The process of excitation and de-excitation described in question #15 can only occur once for each neon atom.

TrueFalse

17. ____ is the idea that physical quantities come in discrete bundles - that is, nature is not continuous. For example, matter is a whole-number multiple of the mass of single atoms, electricity is a whole-number multiple of the charge of a single electron, radiation is a whole-number multiple of discrete bundles of radiant energy, photons.

18. Which scientist first postulated that radiation comes in whole-number multiples of discrete bundles of radiant energy called photons?

(A) Bohr(B) deBroglie(C) Planck(D) Rutherford

19. Which scientist first postulated that light is only emitted by electrons during de-excitation?

(A) Bohr(B) deBroglie(C) Planck(D) Rutherford

20. Which scientist first recognized that stable electron orbitals are based on an integer multiple of the wavelength for an orbiting electron's standing wave.

(A) Bohr(B) deBroglie(C) Planck(D) Rutherford

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