Chapter 9 Practice Questions
16. Electromagnetic radiation of 500 nm wavelength lies in the ________ region of the spectrum. A) infrared B) visible C) ultraviolet D) X-ray E) -ray
B) visible
25) The energy of each Bohr orbit increases with increasing value of "n," but levels become more closely spaced as "n" increases.
true
30) The subshells of the orbital are represented by the possible letters: s, p, d, or f
true
34) The correct electron configuration for fluorine is: 1s22s22p5.
true
35) Transition metal elements always contain at least one "d" block electron.
true
37) The orbital diagram for fluorine shows 1 unpaired electron in a p orbital.
true
4) Light travels through space at a speed of 3.00 × 10^8 m/s.
true
41) Bromine has 28 core electrons.
true
42) The elements will lose or gain electrons as needed to have an electron configuration that matches a noble gas.
true
44) The atomic size of lithium is larger than the atomic size of nitrogen.
true
46) Based on relative location on the periodic table, vanadium (symbol = V) is expected to have more metallic character than selenium (symbol = Se).
true
63. Line spectra are characteristic of atoms in the gas phase.
true
64. Continuous spectra are characteristic of heated solids.
true
67. The Rydberg equation is an example of an empirical equation.
true
72. In the quantum mechanical treatment of the hydrogen atom, the energy depends on the principal quantum number n but not on the values of l or ml.
true
24) The energy of an electron orbit is quantized.
true
55. What is the speed of an electron in m/s if its wavelength is 0.155 nm?
4.69 x 10^6 m/s
50. Use the Rydberg equation to calculate the wavelength, in nm, of the least energetic (longest wavelength) line in the visible series (n1 = 2) of the spectrum of atomic hydrogen.
656 nm
32. 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) 1875 nm
35) Which orbital would the electron of a ground state hydrogen atom occupy? A) 1s B) 2p C) 0s D) 1p E) none of the above
A) 1s
26. Platinum, which is widely used as a catalyst, has a work function O (the minimum energy needed to eject an electron from the metal surface) of 9.05 x 10^-19 J. What is the longest wavelength of light which will cause electrons to be emitted? A) 2.196 x 10^-7 m B) 4.553 x 10^-6 m C) 5.654 x 10^2 m D) 1.370 x 10^15 m E) >10^6 m
A) 2.196 x 10^-7 m
37. The de Broglie equation predicts that the wavelength (in m) of a proton moving at 1000. m/s is A) 3.96 x 10^-10 m B) 3.96 x 10^-7 m C) 2.52 x 10^6m D) 2.52 x 10^9 m E) >10^10 m
A) 3.96 x 10^-10 m
36. 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 x 10^-37 m B) 3.26 x 10^-37 m C) 5.08 x 10^-30 m D) 1.34 x 10^-30 m E) None of these choices is correct.
A) 7.29 x 10^-37 m
31. 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 B) 1.10 x 10^-2 nm C) 1.10 x 10^2 nm D) 1.10 x 10^16 nm E) None of these choices is correct.
A) 91.2 nm
51) Consider the electron configuration of the ion to determine which ion shown below has an incorrect ionic charge? A) Al^3- B) Se^2- C) Rb+ D) Ba^2+ E) none of the above
A) Al^3-
39) Which element is represented by the electron configuration 1s22s22p2? A) C B) He C) Be D) O E) none of the above
A) C
61) Which of the following atoms has the greatest metallic character? A) Cs B) Be C) Cu D) Ti E) Au
A) Cs
9) What is the correct order of the electromagnetic spectrum from shortest wavelength to longest? A) Gamma Rays→X-rays→Ultraviolet Radiation→Visible Light→Infrared Radiation→Microwaves→Radio Waves B) Visible Light→Infrared Radiation→Microwaves→Radio Waves→Gamma Rays→Xrays→Ultraviolet Radiation C) Radio Waves→X-rays→Ultraviolet Radiation→Visible Light→Infrared Radiation→Microwaves→Gamma Rays D) Gamma Rays→X-rays→Visible Light→Ultraviolet Radiation→Infrared Radiation→Microwaves→Radio Waves E) Gamma Rays→X-rays→Infrared Radiation→Visible Light→Ultraviolet Radiation→Microwaves→Radio Waves
A) Gamma Rays→X-rays→Ultraviolet Radiation→Visible Light→Infrared Radiation→Microwaves→Radio Waves
32) "When filling orbitals of equal energy, electrons fill them singly first with parallel spins." This is known as: A) Hund's rule. B) Pauli exclusion principle. C) Bohr's model. D) Ground state. E) none of the above
A) Hund's rule.
60) Which of the following atoms has the least metallic character? A) Li B) Na C) K D) Rb E) Cs
A) Li
2. Who was the first scientist to propose that an object could emit only certain amounts of energy? A) Planck B) Einstein C) Bohr D) Rydberg E) de Broglie
A) Planck
11) Which form of electromagnetic radiation has the longest wavelength? A) Radio Waves B) Microwaves C) X-rays D) Gamma Rays E) Infrared Radiation
A) Radio Waves
13) Which form of electromagnetic radiation has the lowest frequency? A) Radio Waves B) Microwaves C) X-rays D) Gamma Rays E) Infrared Radiation
A) Radio Waves
15) Which form of electromagnetic radiation has photons with the lowest energy? A) Radio Waves B) Microwaves C) X-rays D) Gamma Rays E) Infrared Radiation
A) Radio Waves
56) Which of the following elements has the lowest ionization energy? A) Rb B) Na C) C D) F E) He
A) Rb
4) Which among the following statements is TRUE? A) The wavelength of light is inversely related to its energy. B) As the energy increases, the frequency of radiation decreases. C) As the wavelength increases, the frequency also increases. D) Red light has a shorter wavelength than violet light. E) none of the above
A) The wavelength of light is inversely related to its energy.
17) When sunlight is passed through a prism, what is observed? A) continuous spectrum B) nothing C) bright spots and lines D) white light E) none of the above
A) continuous spectrum
34) The subshell that has five orbitals and can hold up to ten electrons is the: A) d subshell B) f subshell C) s subshell D) p subshell E) none of the above
A) d subshell
41. 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) describe regions of space in which one is most likely to find an electron.
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) diffraction.
55) The size of an atom generally increases: A) down a group and from right to left across a period. B) up a group and from left to right across a period. C) down a group and from left to right across a period. D) up a group and from right to left across a period. E) up a group and diagonally across the Periodic Table.
A) down a group and from right to left across a period.
44. Which of the following is a correct set of quantum numbers for an electron in a 5f orbital? A) n=5, l=3, ml =+1 B) n=5, l=2, ml =+3 C) n=4, l=3, ml =0 D) n=4, l=2, ml =+1 E) n=5, l=4, ml =3
A) n=5, l=3, ml =+1
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) radio, infrared, ultraviolet, gamma rays
7) Which color of the visible spectrum has the longest wavelength (750 nm)? A) red B) orange C) green D) violet E) yellow
A) red
26) Which subshell letter corresponds to a spherical orbital? A) s B) p C) d D) f E) not enough information
A) s
22) The subshell letter: A) specifies the 3-D shape of the orbital. B) specifies the principal quantum number of the orbital. C) specifies the maximum number of electrons. D) specifies the principal shell of the orbital. E) none of the above
A) specifies the 3-D shape of the orbital.
42. 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 & ml). E) the principal, angular momentum and magnetic quantum numbers.
A) the principal quantum number (n) only.
38. 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 (ml). D) the spin quantum number (ms). E) the angular momentum and magnetic quantum numbers, together.
A) the principal quantum number (n).
2) The distance between adjacent wave crests is called: A) wavelength. B) frequency. C) trough. D) nu. E) none of the above
A) wavelength.
23. If the energy of a photon is 1.32 x 10^-18 J, what is its wavelength in nm? A) 1.50 x 10^-7 nm B) 150. nm C) 1.99 x 10^15 nm D) 1.99 x 10^24 nm E) None of these choices is correct.
B) 150. nm
53) If the electron configuration of a ground state potassium atom is 1s22s22p63s1, the electron configuration of the potassium cation (K+) would be: A) 1s22s22p63s2 B) 1s22s22p6 C) 1s22s22p63s1 D) 1s12s22p63s1 E) none of the above
B) 1s22s22p6
41) What is the electron configuration for Ga? A) 1s22s22p63s23p63d104s24p6 B) 1s22s22p63s23p64s23d104p1 C) 1s22s22p63s23p53d104s24p1 D) 1s22s22p63s23p64s24d104p1 E) none of the above
B) 1s22s22p63s23p64s23d104p1
24) How many subshells are there in the n = 2 principal shell? A) 1 B) 2 C) 3 D) 4 E) not enough information
B) 2
30) How many electrons can exist in an orbital? A) 1 B) 2 C) 3 D) 4 E) none of the above
B) 2
25. For potassium metal, the work function O (the minimum energy needed to eject an electron from the metal surface) is 3.68 x 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) 500. nm
3. Who proposed a model that successfully explained the photoelectric effect? A) Planck B) Einstein C) Compton D) Rydberg E) Bohr
B) Einstein
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) creates a pattern of light and dark regions.
9. Which word best describes the phenomenon which gives rise to a rainbow? A) reflection B) dispersion C) diffraction D) interference E) deflection
B) dispersion
3) The number of cycles of a wave that passes a stationary point in one second is called its: A) wavelength. B) frequency. C) crest. D) trough. E) none of the above
B) frequency.
33. 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) n=2
33) The subshell that has three orbitals and can hold up to six electrons is the: A) s subshell B) p subshell C) d subshell D) f subshell E) none of the above
B) p subshell
39. 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.
B) the angular momentum quantum number (l).
54) Choose the answer that best completes the following statement: When an aluminum atom reacts so as to attain a noble gas electron configuration, A) the atom gains five electrons. B) the result is a configuration of 1s22s22p6. C) a 3- ion forms. D) the noble gas configuration of argon is achieved. E) none of the above
B) the result is a configuration of 1s22s22p6.
2) Which one of the following types of electromagnetic radiation has a higher energy per photon than visible radiation? A) microwave B) ultraviolet C) radio D) infrared E) none of the above
B) ultraviolet
35. 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 x 10^-18 J B) 1.64 x 10^-18 J C) 5.45 x 10^-19 J D) 3.03 x 10^-19 J E) None of these choices is correct.
C) 5.45 x 10^-19 J
46) How many core electrons are in a chlorine atom? A) 1 B) 17 C) 10 D) 7 E) none of the above
C) 10
40) What is the electron configuration for Kr? A) 1s22s22p63s23p43d104s24p6 B) 1s22s22p63s23p64s23d24p6 C) 1s22s22p63s23p64s23d104p6 D) 1s22s22p63s23p24s23d104p6 E) none of the above
C) 1s22s22p63s23p64s23d104p6
3) How many core electrons are in a ground state atom of arsenic? A) 15 B) 33 C) 28 D) 5 E) none of the above
C) 28
25) The n = ________ principal shell is the lowest that may contain a d-subshell. A) 1 B) 2 C) 3 D) 4 E) not enough information
C) 3
17. The FM station KDUL broadcasts music at 99.1 MHz. Find the wavelength of these waves. A) 1.88 x 10^-2 m B) 0.330 m C) 3.03 m D) 5.33 x 10^2 m E) > 10^3 m
C) 3.03 m
20. A radio wave has a frequency of 8.6 x 10^8 Hz. What is the energy of one photon of this radiation? A) 7.7 x 10^-43 J B) 2.3 x 10^-34 J C) 5.7 x 10^-25 J D) 1.7 x 10^-16 J E) >10^-15 J
C) 5.7 x 10^-25 J
29. Use the Rydberg equation to calculate the frequency of a photon absorbed when the hydrogen atom undergoes a transition from n1 = 2 to n2 = 4. (R = 1.096776 x 10^7 m^-1) A) 2.056 x 10^6 s^-1 B) 2.742 x 10^6 s^-1 C) 6.165 x 10^14 s^-1 D) 8.226 x 10^14 s^-1 E) > 10^15 s-1
C) 6.165 x 10^14 s^-1
38) An accepted abbreviation format is to write an electron configuration that includes a noble gas symbol in brackets. If you were writing an electron configuration for a bromine atom, which elemental symbol would you place in the bracket? A) He B) Ne C) Ar D) Kr E) Xe
C) Ar
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) Bohr
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) Heisenberg
20) Which of the following statements about the quantum-mechanical model is FALSE? A) Orbitals are a probability map of finding electrons. B) Electrons do not behave as particles. C) Orbitals are specific paths electrons follow. D) Electron paths cannot be described exactly E) All of the above are correct statements.
C) Orbitals are specific paths electrons follow.
49) Which of the following elements has the electron configuration of 3s23p4 in its outermost shell? A) Al B) Si C) S D) Cl E) none of the above
C) S
19) Which statement below does NOT follow the Bohr Model? A) When energy is absorbed by atoms, the electrons are promoted to higher-energy orbits. B) When an atom emits light, electrons fall from a higher orbit into a lower orbit. C) The energy emitted from a relaxing electron can have any wavelength. D) Electrons exist in specific, quantized orbits. E) none of the above
C) The energy emitted from a relaxing electron can have any wavelength.
42) What is the electron configuration for P? A) [Ar]3s23p64s23d104p3 B) [Ne]1s21p62s22p3 C) [Ne]3s23p3 D) [Ar]3s23p3 E) none of the above
C) [Ne]3s23p3
18) When neon light is passed through a prism, what is observed? A) continuous spectrum B) nothing C) bright spots or lines D) white light E) none of the above
C) bright spots or lines
27) Which subshell letter corresponds to a 4-leaf clover orbital pattern? A) s B) p C) d D) f E) not enough information
C) d
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) de Broglie
50) Chlorine and bromine have very similar chemical properties. This is best explained by the fact that both elements: A) are gases. B) are in period 3 of the Periodic Table. C) have the same number of valence electrons. D) have equal number of protons and electrons. E) none of the above
C) have the same number of valence electrons.
10. Contact lenses can focus light due to the ___________ of the waves. A) diffraction B) reflection C) refraction D) dispersion E) interference
C) refraction
40. 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 (ml). D) the spin quantum number (ms). E) None of these choices is correct.
C) the magnetic quantum number (ml).
28. 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) three
27. 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) two
16) What happens to an atom when it absorbs energy? A) The atom stores the energy for later use. B) The extra energy increases the speed of the electrons in their orbitals. C) The atom re-emits the energy as heat. D) The atom re-emits the energy as light. E) none of the above
D) The atom re-emits the energy as light.
5) How are wavelength and frequency of light related? A) Wavelength is one-half of the frequency. B) Wavelength is double the frequency. C) Wavelength increases as frequency increases. D) Wavelength increases as the frequency decreases. E) Wavelength is independent of frequency.
D) Wavelength increases as the frequency decreases.
1) Which color of visible light has a wavelength in between that of blue and violet light? A) green B) yellow C) red D) indigo E) none of the above
D) indigo
21) The principal quantum number (n): A) specifies the 3-D shape of the orbital. B) specifies the subshell of the orbital. C) specifies the maximum number of electrons. D) specifies the principal shell of the orbital. E) none of the above
D) specifies the principal shell of the orbital.
6) Which color of the visible spectrum has the shortest wavelength (400 nm)? A) red B) orange C) green D) violet E) yellow
D) violet
8) Which color of the visible spectrum has photons with the most energy? A) red B) orange C) green D) violet E) yellow
D) violet
43) Which one of the following is the correct orbital diagram for nitrogen? A) ↑↓ ↑↓ ↓ ↓ ↑ B) ↑↓ ↓↓ ↓ ↑ ↑ C) ↑↓ ↓↓ ↑ ↑ ↑ D) ↑↓ ↑↓ ↑ ↑ ↑ E) none of the above
D) ↑↓ ↑↓ ↑ ↑ ↑
34. 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 x 10^-20 J B) 1.36 x 10^-19 J C) 2.42 x 10^-19 J D) 1.55 x 10^-19 J E) 1.09 x 10^-18 J
D) 1.55 x 10^-19 J
29) The "d" subshell can hold a maximum of ________ electrons. A) 2 B) 5 C) 6 D) 10 E) none of the above
D) 10
30. 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 x 10^7 m-1) A) 205.1 nm B) 384.6 nm C) 683.8 nm D) 1282 nm E) > 1500 nm
D) 1282 nm
31) The lowest energy orbital in the quantum-mechanical model is the: A) zero orbital. B) 1a orbital. C) 1p orbital. D) 1s orbital. E) none of the above
D) 1s orbital.
36) How many electrons are unpaired in the orbitals of carbon? A) 12 B) 6 C) 4 D) 2 E) none of the above
D) 2
18. The AM station KBOR plays your favorite music from the 20s and 30s at 1290 kHz. Find the wavelength of these waves. A) 4.30 x 10^-2 m B) 0.144 m C) 6.94 m D) 232 m E) > 10^3 m
D) 232 m
37) How many electrons are unpaired in the orbitals of nitrogen? A) 14 B) 5 C) 9 D) 3 E) none of the above
D) 3
23) How many subshells are there in the n = 4 principal shell? A) 1 B) 2 C) 3 D) 4 E) not enough information
D) 4
19. An infrared wave has a wavelength of 6.5 x 10^-4 cm. What is this distance in angstroms, Å? A) 6.5 x 10^-4 Å B) 2.2 x 10^-4 Å C) 4.6 x 10^3 Å D) 6.5 x 10^4 Å E) 6.5 x 10^6 Å
D) 6.5 x 10^4 Å
47) How many valence electrons are in a chlorine atom? A) 1 B) 17 C) 10 D) 7 E) none of the above
D) 7
52) Which one of the following species has the electron configuration of 1s22s22p6? 1. Na+ 2. O^2- 3. F- A) 1 and 2 only B) 1 and 3 only C) 2 and 3 only D) All of 1, 2, and 3 E) Neither 1, 2, or 3
D) All of 1, 2, and 3
28) Which statement is NOT true about "p" orbitals? A) A subshell contains three "p" orbitals. B) These orbitals are shaped like dumbbells. C) A 3p orbital has a higher energy than a 2p orbital. D) All three of these statements are true. E) none of the above
D) All three of these statements are true.
44) The element with a completely filled p-subshell is: A) Na. B) Al. C) P. D) Ar. E) none of the above
D) Ar.
4) Which of the atoms represented below is the largest in size? A) N B) As C) Sb D) Bi E) P
D) Bi
7. Which scientist demonstrated that photons transferred momentum during collisions with matter? A) Bohr B) de Broglie C) Planck D) Compton E) Billiard
D) Compton
10) Which form of electromagnetic radiation has the shortest wavelength? A) Radio Waves B) Microwaves C) X-rays D) Gamma Rays E) Infrared Radiation
D) Gamma Rays
12) Which form of electromagnetic radiation has the highest frequency? A) Radio Waves B) Microwaves C) X-rays D) Gamma Rays E) Infrared Radiation
D) Gamma Rays
14) Which form of electromagnetic radiation has photons with the highest energy? A) Radio Waves B) Microwaves C) X-rays D) Gamma Rays E) Infrared Radiation
D) Gamma Rays
1. Who was the first scientist to propose that the atom had a dense nucleus which occupied only a small fraction of the volume of the atom? A) Planck B) Bohr C) Rydberg D) Rutherford E) Thomson
D) Rutherford
45) What is the element in which at least one electron is in the d-orbital? A) Ar B) K C) Ca D) Sc E) none of the above
D) Sc
46. Which one of the following sets of quantum numbers can correctly represent a 3p orbital? a. n=3 l=1 ml=2 b.n=1 l=3 ml=3 c. n=3 l=2 ml=1 d. n=3 l=1 ml=-1 e. n=3 l=0 ml=1 A)a B)b C)c D)d E)e
D)d
22. Green light has a wavelength of 5200 Å. Calculate the energy of one photon of green light. A) 3.4 x 10^-40 J B) 3.4 x 10^-30 J C) 3.8 x 10^-29 J D) 3.4 x 10^-27 J E) 3.8 x 10^-19 J
E) 3.8 x 10^-19 J
24. A photon has an energy of 5.53 x 10^-17 J. What is its frequency in s-1? A) 3.66 x 10^-50 s^-1 B) 1.20 x 10^-17 s^-1 C) 3.59 x 10^-9 s^-1 D) 2.78 x 10^8 s^-1 E) 8.35 x 10^16 s^-1
E) 8.35 x 10^16 s^-1
1) Which of the statements about light is FALSE? A) Light travels through space at a speed of 3.00 × 10^8 m/s. B) Light travels much faster than sound. C) A packet of light energy is called a photon. D) A characteristic feature of light that determines its color is its wavelength. E) All of the above statements are true.
E) All of the above statements are true.
58) Which of the following atoms is the largest? A) Li B) Na C) K D) Rb E) Cs
E) Cs
57) Which of the following elements has the highest ionization energy? A) Ba B) Ca C) Al D) Cl E) Ne
E) Ne
59) Which of the following atoms is the smallest? A) Li B) Be C) B D) O E) Ne
E) Ne
4. Who developed an empirical equation from which the wavelengths of lines in the spectrum of hydrogen atoms can be calculated? A) Planck B) de Broglie C) Bohr D) Rutherford E) Rydberg
E) Rydberg
48) What do the alkali metals all have in common? A) They all undergo similar reactions. B) They all have similar physical properties. C) They all form +1 ions. D) They all have the same number of valence electrons. E) all of the above
E) all of the above
21. Infrared radiation from the sun has a wavelength of 6200 nm. Calculate the energy of one photon of that radiation. A) 4.l x 10^-39 J B) 4.l x 10^-30 J C) 3.2 x 10^-29 J D) 3.2 x 10^-26 J E) between 10^-20 and 10^-19 J
E) between 10^-20 and 10^-19 J
15. Select the arrangement of electromagnetic radiation which starts with the lowest wavelength and increases to 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) gamma rays, ultraviolet, infrared, radio
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) microwave, infrared, visible, ultraviolet
43. Which of the following is a correct set of quantum numbers for an electron in a 3d orbital? A) n=3, l=0, ml =-1 B) n=3, l=1, ml =+3 C) n=3, l=2, ml =3 D) n=3, l=3, ml =+2 E) n=3, l=2, ml =-2
E) n=3, l=2, ml =-2
45. In the quantum mechanical treatment of the hydrogen atom, which one of the following combinations of quantum numbers is not allowed? n l ml a 3 0 0 b 3 1 -1 c 3 2 2 d 3 2 -1 e 3 3 2 A)a B)b C)c D)d E)e
E)e
Explain the context and meanings of the terms "orbit" and "orbital", making a clear distinction between them.
Orbit is a term from the Bohr theory, and refers to an exact, circular path followed by an electron. It has been superseded by the concept of an orbital, which arises from the Schrodinger equation. An orbital is a wave function, or, more loosely, a region of space close to the nucleus where an electron is likely to be found.
47. For the following equations, a. name the scientist to whom the equation is attributed. b. in not more than three lines, explain clearly what the equation means or represents. 1) E=nh 2) = h/mu 3) H = E 4) x·mu h/4 5) Ephoton = h
READ ON PAPER
57. In the quantum mechanical treatment of the hydrogen atom, the functions and 2 both feature prominently. Briefly explain (in principle) how they are obtained and what, if anything, their physical meanings are.
The wave function, , is a solution to the Schrodinger equation. It describes a wave, but has no physical meaning of its own. The square of the wave function, 2, represents the probability of finding the electron at any point in the atom.
56. a. Calculate the momentum of a photon of green light, wavelength 515 nm. b. If this photon is traveling in a vacuum, what is its "mass"?
a. 1.29 x 10^-27 kg·m/s b. 4.29 x 10^-36 kg
54. Use the Bohr equation to calculate the energy of a. the largest energy absorption or emission process involving the n = 2 state of the hydrogen atom. b. the smallest energy absorption or emission process involving the n = 2 state of the hydrogen atom.
a. 1.64 x 10^-18 J (n = 1 to n = 2) b. 3.03 x 10^-19 J (n = 3 to n = 2)
52. a. Use Bohr's equation to calculate how much energy (in J) is needed to promote an electron from the H-atom ground state to the n = 4 level. b. If a photon provides the energy in (a), what is its wavelength in nm?
a. 2.04 x 10^-18 J b. 97.2 nm
53. a. Use the Bohr equation to calculate the energy needed to ionize a hydrogen atom from its ground state. b. What is the minimum wavelength of a photon needed for it to have the energy needed in (a)?
a. 2.18 x 10^-18 J b. 91.2 nm
49. a. What is the frequency of microwave radiation which has a wavelength of 10.7 cm? b. What is the energy of one photon of this radiation?
a. 2.80 x 10^9 s^-1 b. 1.86 x 10^-24 J
51.a. Calculate the wavelength in nm of a photon whose energy is 6.00 x 10^-19 J. b. Would the photon in (a) have enough energy to ionize a hydrogen atom in its ground state (i.e., to separate the proton and electron completely)? Use the Bohr equation to explain your answer.
a. 331 nm b. No. 2.18 x 10^-18 J is needed, the difference between the n = 1 and n = infinity levels.
61. For the following orbitals, state the values of n, l and ml which apply, and draw a sketch showing the shape and orientation of the orbital. a. 3s b. 2px
a. 3s n = 3, l = 0, ml = 0 b. 2px n = 2, l = 1, ml = 1 (or 0 or -1)
48. In not more than three lines for each answer, briefly outline one important scientific contribution of each of the following. a. Planck b. de Broglie c. Heisenberg
a. Planck is responsible for first proposing that energy is quantized. He proposed that a black body can emit or absorb electromagnetic energy E only in exact multiples of hv, giving rise to the equation E = nhv where n is a positive integer. b. de Broglie proposed that particles can have some wavelike properties, and developed a relationship which allows the wavelength (a wave property) to be calculated from the momentum of a particle. c. Heisenberg is responsible for the uncertainty principle which states that we cannot simultaneously know both the position (x) and the momentum (mu) of a particle exactly. There is a minimum uncertainty, h/4(pie), in their product, which is a fundamental property of matter, not an instrumental limitation.
60. What are the possible values for the following quantum numbers in an atom? a. n b. l c. ml
a. n = 1, 2, 3, ... b. l = 0, 1, ...., n-1 c. ml = -l, -l+1, ........, +l
The following combinations of quantum numbers are not allowed. Correct each set by changing only one quantum number, and write in an appropriate corrected value. a. n = 2 l = 2 ml = 2 Corrected: _____ = _____ b. n = 4 l = -2 ml = 0 Corrected: _____ = _____
a.n=3 b. l = 0 (or 1, 2 or 3)
13) Visible light makes up the largest portion of the electromagnetic spectrum.
false
17) The heat you feel when you place your hand near a hot object is ultraviolet radiation.
false
19) The great success of the Bohr model of the atom is that it predicted the emission spectrum lines of multi-electronic elements like helium.
false
20) Bohr showed that the emission spectrum of hydrogen was continuous with no interruption across the entire visible wavelength range.
false
23) When an atom absorbs energy, it often re-emits that energy as heat
false
26) Electrons behave like particles and we can describe their exact paths.
false
27) An orbital is a probability map showing exactly where an electron can be found in an atom.
false
28) The higher the principal quantum number, the lower the orbital energy.
false
29) The possible values for the principal quantum numbers are: n= 0,1,2,3,4
false
3) Light is a type of matter
false
31) A principal shell with a value of n=3 would contain s, p, d, and f orbitals.
false
32) The subshells s, p, d, and f all have the same energy as long as they are in the same principal shell.
false
33) The ground state is when an electron in an atom is excited into the lowest possible vacant orbital.
false
36) The Pauli exclusion principle states that orbitals may hold no more than two electrons of identical spins.
false
38) The correct electron configuration for magnesium is: 1s22s22p63s3.
false
39) The element manganese (symbol = Mn) has five valence electrons.
false
40) Bromine has 17 valence electrons.
false
43) The ionization energy of lithium is higher than that of fluorine.
false
45) Based on relative location on the periodic table, a carbon atom is larger in atomic size than a phosphorous atom.
false
5) A red shirt appears red to our eyes because the shirt absorbs the red wavelengths of visible light.
false
6) A particle of light is called a packet.
false
62. The energy of a photon is directly proportional to the wavelength of the radiation.
false
65. Continuous spectra are characteristic of molecules in the gas phase.
false
66. In the Rydberg equation, for a fixed value of n1, the longest wavelength line has n2 = infinity
false
68. The Rydberg equation, giving the wavelengths of lines in the spectrum of the hydrogen atom, was obtained by assuming that energy is quantized.
false
69. In the Bohr model of the hydrogen atom, the electron moves in a circular path which Bohr referred to as an orbital.
false
7) A photon represents the mass of a single particle of light.
false
70. Other factors being constant, a heavy object will have a longer de Broglie wavelength than a light object.
false
71. In the quantum mechanical treatment of the hydrogen atom, the probability of finding an electron at any point is proportional to the wave function .
false
8) Blue light travels at a faster speed than red light.
false
9) A photon of red light contains the same amount of energy as a photon of blue light.
false
21) Each element produces its own unique and distinctive emission spectrum.
true
22) An emission spectrum results when light emitted by glowing gas is passed through a prism
true
1) When the elements are arranged in order of increasing number of protons, certain sets of properties recur periodically.
true
10) The shorter the wavelength of light, the more energy it has.
true
11) Wavelength of visible light determines color.
true
12) The most energetic photons are gamma rays.
true
14) Photons of ultraviolet radiation contain more energy than do photons of violet visible light.
true
15) X-rays damage biological molecules.
true
16) Ultraviolet light produces suntans and sunburns.
true
18) In order for a substance to be heated in a microwave, it must contain water.
true
2) The early scientists who developed the quantum-mechanical model were bewildered by the model and it altered our fundamental view of matter.
true
