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1 | | Calculate the wavelength, in nanometers, of visible light having a frequency of 4.37 x 1014s-1. |
| | A) | 12.0 nm |
| | B) | 343 nm |
| | C) | 686 nm |
| | D) | 674 nm |
| | E) | None of the above |
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2 | | For the hydrogen atom, En = -(1/n2)RH, where RH = 2.18 x 10-18 J. The wavelength of the transition from the ground state to the n = 3 state is: |
| | A) | 1.03 x 10-7 m |
| | B) | 6.56 x 10-8 m |
| | C) | -1.03 x 10-7 m |
| | D) | -6.76 x 10-8 m |
| | E) | 4.27 x 10-8 m |
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3 | | Which of the following is not a possible value of ml for an electron with l = 2? |
| | A) | -1 |
| | B) | 0 |
| | C) | +1 |
| | D) | +2 |
| | E) | +3 |
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4 | | The set of quantum numbers that correctly describes an electron in a 3p orbital is: |
| | A) | n = 3; l = 0; ml = 0; ms = 0 |
| | B) | n = 3; l = 2; ml = -2, -1, 0, 1, or 2; ms = +1/2 or -1/2 |
| | C) | n = 3; l = 1; ml = -1, 0, or 1; ms = +1/2 or - 1/2 |
| | D) | n = 4; l = 0; ml = -1, 0, or 1; ms = +1/2 or -1/2 |
| | E) | None of the above |
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5 | | What is the total number of orbitals associated with the principal quantum number n = 2? |
| | A) | 1 |
| | B) | 2 |
| | C) | 3 |
| | D) | 4 |
| | E) | None of the above |
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6 | | What is the maximum number of electrons that can be accommodated in the shell with n = 4? |
| | A) | 32 |
| | B) | 18 |
| | C) | 24 |
| | D) | 10 |
| | E) | None of the above |
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7 | | An atom of chromium has ___ unpaired electrons and is ___. |
| | A) | 3, diamagnetic |
| | B) | 5, diamagnetic |
| | C) | 3, paramagnetic |
| | D) | 5, paramagnetic |
| | E) | 6, paramagnetic |
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8 | | The electronic configuration and filling order of the element whose atomic number is 26 is: |
| | A) | 1s22s22p63s23p64s03d8 |
| | B) | 1s22s22p63s23p63d64s2 |
| | C) | 1s22s22p63s23p64s23d6 |
| | D) | 1s22s22p63s23p64s23d44p2 |
| | E) | None of the above |
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9 | | An atom in its ground state contains 33 electrons. How many of these electrons are in p orbitals? |
| | A) | 15 |
| | B) | 12 |
| | C) | 3 |
| | D) | 33 |
| | E) | None of the above |
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10 | | Using the noble gas core designation, which of the configurations below correctly describes the ground state electron configuration of Cu? |
| | A) | [Ne]4s23d9 |
| | B) | [Ar]4s23d9 |
| | C) | [Kr]4s13d10 |
| | D) | [Ar]4s13d10 |
| | E) | None of the above |
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11 | | The Heisenberg uncertainty principle states that: |
| | A) | it is not possible to know either the momentum or position of an electron with precision |
| | B) | it is not possible to know the momentum of an electron without knowing the position |
| | C) | it is possible to know either the momentum or the position of an electron but not both simultaneously |
| | D) | none of the above |
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12 | | Emission spectra: |
| | A) | cannot be used to identify an unknown atom |
| | B) | can be used to identify unknown atoms |
| | C) | can be explained by the movement of protons colliding with electrons |
| | D) | none of the above |
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13 | | Bohr's Theory of the hydrogen atom was important because: |
| | A) | It gave a fixed value or quantized the energy levels of electrons. |
| | B) | It gave a fixed or quantized value to the nucleus of the atom. |
| | C) | It identified the ground level energies of several atoms. |
| | D) | None of the above |
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14 | | Energy emission by an electron is an energy releasing process, while energy absorption requires an input of energy. |
| | A) | True |
| | B) | False |
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15 | | De Broglie explained electron movements by relating them to: |
| | A) | waves only |
| | B) | particles only |
| | C) | waves and particles |
| | D) | none of the above |
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