Really confused on some multiple choice questions. Please Help!
Posted: Mon Oct 16, 2017 8:28 pm
15. In the above spectroscopic experiment what is the most unique characteristic of the observed results? Hint: What does a typical spectrum look like?
A. All wavelengths of light are absorbed or emitted. Spectrum consists of lines.
B. No wavelengths of light are absorbed or emitted. Spectrum consists of waves.
C. Only specific wavelengths of light are absorbed or emitted. Spectrum consists of lines.
D. Only specific wavelengths of light are absorbed or emitted. Spectrum consists of waves.
16. In atomic absorption (or emission) spectroscopy are all wavelengths of light absorbed (or emitted)?
Yes
No
19. When we say hydrogen atoms absorb a specific wavelength of light what do we mean? Use energy in your detailed explanation of what is being excited.
A. We mean that a photon with a specific energy lowers the energy of the electron in the hydrogen atom to its ground state. That is, the photon's energy matches the energy difference between two electronic energy levels.
B. We mean that a photon with a specific energy absorbs the energy of the electron in the hydrogen atom to a higher energy level. That is, the photon's energy matches the energy product of the two electronic energy levels.
C. We mean that a photon with a specific energy excites the electron in the hydrogen atom to a lower energy level. That is, the photon's energy matches the energy sum of two electronic energy levels.
D. We mean that a photon with a specific energy excites the electron in the hydrogen atom to a higher energy level. That is, the photon's energy matches the energy difference between two electronic energy levels.
20. If 1 million photons in the UV region are absorbed by a hydrogen gas sample how many electrons are excited to a higher energy level?
A. zero
B. 500,000
C. 1
D. 1 million
22. In ultraviolet and visible spectroscopy what condition must occur for a photon to be absorbed?
A. The photon must be at its lowest energy state.
B. Energy of the photon must be within the energy difference between two energies that an electron can have.
C. The photon must be at its highest energy state.
D. Energy of the photon must match the energy difference between two energies that an electron can have.
For the hydrogen atom which statement is true?
A. The transition from n = 5 to n = 3 involves greater energy than one from n = 4 to n = 2.
B. The transition from n = 4 to n = 2 emits radiation of longer wavelength than the transition from n = 5 to n = 1.
C. All transitions from states for which n > 1 to the n = 1 state involve the absorption of energy by the atom.
D. A transition from n = 2 to some large value of n corresponds to the ionization energy of the H atom.
OH AND LAST QUESTION, can wavelengths be noted in negative values?!?!?!?!
A. All wavelengths of light are absorbed or emitted. Spectrum consists of lines.
B. No wavelengths of light are absorbed or emitted. Spectrum consists of waves.
C. Only specific wavelengths of light are absorbed or emitted. Spectrum consists of lines.
D. Only specific wavelengths of light are absorbed or emitted. Spectrum consists of waves.
16. In atomic absorption (or emission) spectroscopy are all wavelengths of light absorbed (or emitted)?
Yes
No
19. When we say hydrogen atoms absorb a specific wavelength of light what do we mean? Use energy in your detailed explanation of what is being excited.
A. We mean that a photon with a specific energy lowers the energy of the electron in the hydrogen atom to its ground state. That is, the photon's energy matches the energy difference between two electronic energy levels.
B. We mean that a photon with a specific energy absorbs the energy of the electron in the hydrogen atom to a higher energy level. That is, the photon's energy matches the energy product of the two electronic energy levels.
C. We mean that a photon with a specific energy excites the electron in the hydrogen atom to a lower energy level. That is, the photon's energy matches the energy sum of two electronic energy levels.
D. We mean that a photon with a specific energy excites the electron in the hydrogen atom to a higher energy level. That is, the photon's energy matches the energy difference between two electronic energy levels.
20. If 1 million photons in the UV region are absorbed by a hydrogen gas sample how many electrons are excited to a higher energy level?
A. zero
B. 500,000
C. 1
D. 1 million
22. In ultraviolet and visible spectroscopy what condition must occur for a photon to be absorbed?
A. The photon must be at its lowest energy state.
B. Energy of the photon must be within the energy difference between two energies that an electron can have.
C. The photon must be at its highest energy state.
D. Energy of the photon must match the energy difference between two energies that an electron can have.
For the hydrogen atom which statement is true?
A. The transition from n = 5 to n = 3 involves greater energy than one from n = 4 to n = 2.
B. The transition from n = 4 to n = 2 emits radiation of longer wavelength than the transition from n = 5 to n = 1.
C. All transitions from states for which n > 1 to the n = 1 state involve the absorption of energy by the atom.
D. A transition from n = 2 to some large value of n corresponds to the ionization energy of the H atom.
OH AND LAST QUESTION, can wavelengths be noted in negative values?!?!?!?!