True statements about the absorption and emission of energy by an atom include which of the...
True statements about the absorption and emission of
energy
by an atom include which of the following?
I. An atom can only absorb photons of light that have certain
specific energies.
II. An atom can emit photons of light of any energy.
III. At low temperature, the lines in the absorption spectrum
of
an atom coincide with the lines in its emission spectrum that
represent transitions to the ground state.
A. I only
B. III only
C. I and III only
D. I, II, and III
full explanation, please!
Homework Answers
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True statements about the absorption and emission of
energy
by an atom include which of the...
please help Part 1: Emission Background Energy level diagram for hydrogen 50mm 121.6 mm 1026m 973...
please help
Part 1: Emission Background Energy level diagram for hydrogen 50mm 121.6 mm 1026m 973 mm UV 410.1 4340 nm 6563 1. On the energy level diagram above, which transitions emit light in visible region of the electromagnetic spectrum? (ii) Label these transitions with the appropriate color. (iii) Which of these emits the highest energy photons? (ix). Which emits the lowest energy photons? 2. On the energy level diagram above, which transitions emit light in ultraviolet (UV) region of...
Hydrogen gas can only absorb EM radiation that has an energy corresponding to a transition in...
Hydrogen gas can only absorb EM radiation that has an energy corresponding to a transition in the atom, just as it can only emit these discrete energies. When a spectrum is taken of the solar corona, in which a broad range of EM wavelengths are passed through very hot hydrogen gas, the absorption spectrum shows all the features of the emission spectrum. But when such EM radiation passes through room-temperature hydrogen gas, only the Lyman series is absorbed. Explain the...
Below is both an energy level diagram for an atom and an emission spectrum for that...
Below is both an energy level diagram for an atom and an emission spectrum for that atom. Match the peak in the emission spectrum to the corresponding transition in the energy level diagram. III Intensity n = 1 (nm) O A Peaki=e, Peak II = f, Peak III = C, Peak IV = b O B Peak I=b, Peak II = c Peak III = f, Peak IV = e O C Peak I = a, Peak II = d...
Which of the following statements about the absorption of light by a molecule is true? Absorption...
Which of the following statements about the absorption of light by a molecule is true? Absorption of visibloe light can cause only vibrational transitions. Absorption of visible light can cause vibrational and electronic transitions. Absorption of visible light can cause only electronic transitions. Electronic transitions occur at smaller wavelengths than vibrational transitions.
How does the energy possessed by an emitted photon compare to the difference in energy levels tha...
Answer all of these, please
How does the energy possessed by an emitted photon compare to the difference in energy levels that gave rise to the emission of the photon? When a tube containing hydrogen atoms is energized by pass- ing several thousand volts of electricity into the tube, the hy- drogen emits light that, when passed through a prism, resolves into the "bright line" spectrum shown in Fig. 11.10. Why do hydrogen atoms emit bright lines of specific wavelengths...
(b) Light oF a certain wavelength is just able to cause the emission of photoelectrons with...
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A certain type of atom (not hydrogen) has three energy levels numbered 1, 2, and 3,...
A certain type of atom
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3, as shown in the upper illustration. There are three possible
transitions between these levels that lead to emission of a photon:
3 ® 1, 3 ® 2, and 2 ® 1.
The lower illustration shows the emission spectrum from a gas of
these atoms. There are three emission lines, A, B, and C.
(a) Rank the photons emitted in the transitions 3 ®...
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42) is the phenomenon whereby the electrons of an atom absorb energy as they transition from...
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the following diagrams are rough depictions of an atom, where the circles represent the different energy...
the following diagrams are rough depictions of an
atom, where the circles represent the different energy levels that
an electron could occupy, with the new keyless at the center.
straight arrows represent the motion of an electron between energy
levels, while squiggly arrows will be used to represent
photons.
A) Bsed on the change in energy that the electron is
undergoing at a squiggly arrow showing the photon associated with
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please help
Part 1: Emission Background Energy level diagram for hydrogen 50mm 121.6 mm 1026m 973 mm UV 410.1 4340 nm 6563 1. On the energy level diagram above, which transitions emit light in visible region of the electromagnetic spectrum? (ii) Label these transitions with the appropriate color. (iii) Which of these emits the highest energy photons? (ix). Which emits the lowest energy photons? 2. On the energy level diagram above, which transitions emit light in ultraviolet (UV) region of...
Below is both an energy level diagram for an atom and an emission spectrum for that atom. Match the peak in the emission spectrum to the corresponding transition in the energy level diagram. III Intensity n = 1 (nm) O A Peaki=e, Peak II = f, Peak III = C, Peak IV = b O B Peak I=b, Peak II = c Peak III = f, Peak IV = e O C Peak I = a, Peak II = d...
Which of the following statements about the absorption of light by a molecule is true? Absorption of visibloe light can cause only vibrational transitions. Absorption of visible light can cause vibrational and electronic transitions. Absorption of visible light can cause only electronic transitions. Electronic transitions occur at smaller wavelengths than vibrational transitions.
Answer all of these, please
How does the energy possessed by an emitted photon compare to the difference in energy levels that gave rise to the emission of the photon? When a tube containing hydrogen atoms is energized by pass- ing several thousand volts of electricity into the tube, the hy- drogen emits light that, when passed through a prism, resolves into the "bright line" spectrum shown in Fig. 11.10. Why do hydrogen atoms emit bright lines of specific wavelengths...
(b) Light oF a certain wavelength is just able to cause the emission of photoelectrons with close to zero velocity from silver whose work-function is 4,73 electron-volts. The same light is now shone on to a sodium surface whose work-function is 2,46 e-V. Calculate the energy of the electrons which are emitted, in electron-volts. [6] (c) The electron in a Bohr hydrogen atom has been excited to the n = 3 state. (I) Sketch on a labelled energy level diagram...
A certain type of atom
(not hydrogen) has three energy levels numbered 1, 2, and
3, as shown in the upper illustration. There are three possible
transitions between these levels that lead to emission of a photon:
3 ® 1, 3 ® 2, and 2 ® 1.
The lower illustration shows the emission spectrum from a gas of
these atoms. There are three emission lines, A, B, and C.
(a) Rank the photons emitted in the transitions 3 ®...
42) is the phenomenon whereby the electrons of an atom absorb energy as they transition from lower energy orbitals to higher energy ones. (1 point) 43) How many 7f orbitals are there? (1 point) 45) For the hydrogen emission spectrum, which of the following would be generated by the return of energetic electrons to the ground state: Paschen lines, Bohr lines, Lyman lines, Einstein lines, Bunsen lines, or Balmer lines? (1 point) 47) Condensed phosphates with three or more units...
the following diagrams are rough depictions of an
atom, where the circles represent the different energy levels that
an electron could occupy, with the new keyless at the center.
straight arrows represent the motion of an electron between energy
levels, while squiggly arrows will be used to represent
photons.
A) Bsed on the change in energy that the electron is
undergoing at a squiggly arrow showing the photon associated with
this process i.e., is it being emitted from or observed...
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