Practice: What is the wavelength of a photon (in nm) absorbed during a transition from the n = 2 to n = 5 state in the hydrogen atom?

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In the **Bohr Equation**, the energy and wavelength a photon is related to its energy shell transitions.

Example #1: What is the energy of a photon (in Joules) released during a transition from n = 4 to n = 1 state in the hydrogen atom?

Practice: What is the wavelength of a photon (in nm) absorbed during a transition from the n = 2 to n = 5 state in the hydrogen atom?

Practice: Determine the end (final) value of n in a hydrogen atom transition, if the electron starts in n = 5 and the atom releases a photon of light with an energy of 4.5738 × 10^{-19} J.

Practice: An electron releases energy as it moves from the 6^{th} shell to the 3^{rd} shell. If it releases 4.25 x 10^{9} kJ of energy at a wavelength of 915.7 nm, how many photons were released in the process?

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It is possible to determine the ionization energy for hydrogen using the Bohr equation. Calculate the ionization energy (in kJ) for a mole of hydrogen atoms, making the assumption that ionization is the transition from n = 1 to n = ∞.
A. 7.62 x 103 kJ
B. 2.76 x 103 kJ
C. 1.31 x 103 kJ
D. 3.62 x 103 kJ
E. 5.33 x 103 kJ

When an electron of an excited hydrogen atom falls from level n = 3 to level n = 1, what is the frequency (in s-1) of the light emitted?
a. 2.92 x1 0 15
b. 3.43 x 10 -16
c. 1.62 x 10 -15
d. 6.17 x 10 14
e. 4.00 x 10 19

For a hydrogen atom, calculate the energy (in kJ) of a photon in the Balmer series that results from the transition n = 5 to n = 2.
a. 1.09x10 -20 kJ
b. 2.04x10 -21 kJ
c. 2.18x10 -21 kJ
d. 3.03x10 -22 kJ
e. 4.58x10 -22 kJ

How much energy is emitted in kJ/mol when an electron in the H atom transitions from n = 6 to n = 2?
A. 275
B. 292
C. 302
D. 310
E. 321

What is the energy of the light emitted from a hydrogen atom as it relaxes from the
n = 5 to n = 3 excited states?
What is the wavelength of the emitted light?

The Rydberg equation is an empirical equation that describes mathematically
1. the lines in the emission spectrum of hydrogen.
2. the results of the cathode ray experiments.
3. the results of the oil drop experiment.
4. the Bohr model of the atom
5. the possible paths of two isotopes of the same element in a constant magnetic field in a mass spectrometer.

The electron in the n = 5 level of a hydrogen atom emits a photon with a wavelength of 1280 nm. To what energy level does the electron move?
1. 5
2. 9
3. 8
4. 4
5. 6
6. 2
7. 7
8. 3
9. 1

A hydrogen atom initially in the n - 6 state emits a photon of ligiht of wavelength:
λ = 1093 nm
The value for n after emission of the photon is
a. n = 1
b. n = 2
c. n = 3
d. n = 4
e. n = 5

An electron in a hydrogen atom moves from the n = 2 to n = 5 level. What is the wavelength of the photon that corresponds to this transition and is the photon emitted or absorbed during this process?
1. 1875 nm; emitted
2. 434 nm; absorbed
3. 276 nm; emitted
4. 1875 nm; absorbed
5. 276 nm; absorbed
6. 434 nm; emitted

A hydrogen atom emits light in an electronic transition going from n=4 to n=2 lower shell. 1.) What is the frequency of this light? 2.) What wavelength is this and what color will it appear to the eye?(R = 2.18x10 -18 J; h = 6.63 x 10 -34 J•sec; c = 3.00x10 8 m/sec;1 nm = 10 -9 m)

The second line of the Balmer series occurs at wavelength of 486.13 nm. To which transition can we attribute this line?a) n = 6 to n = 2b) n = 5 to n = 2c) n = 4 to n = 2d) n = 3 to n = 2e) it is to the n = 1 level

A red laser pointer emits light with a wavelength of 650 nm. (c) The laser pointer emits light because electrons in the material are excited (by a battery) from their ground state to an upper excited state. When the electrons return to the ground state, they lose the excess energy in the form of 650 nm photons. What is the energy gap between the ground state and excited state in the laser material?

For each of the following electronic transitions in the hydrogen atom, calculate the energy, frequency, and wavelength of the associated radiation, and determine whether the radiation is emitted or absorbed during the transition: (c) from n = 3 to n= 6. Does any of these transitions emit or absorb visible light?

Calculate the wavelength of light associated with the transition from n=1 to n=3 in the hydrogen atom.
A. 103 nm
B. 155 nm
C. 646 nm
D. 971 nm
E. 136 nm

Suppose energy is delivered to atoms of fluorine, chlorine, bromine, and iodine sufficient to cause each atom’s outermost electron to jump to the n=7 state. Now imagine that these electrons return to the ground state, giving off light as they fall. Which gas will emit light of the highest frequency?1. iodine2. chlorine3. fluorine 4. bromine

An excited hydrogen atom emits a photon with a frequency of 1.141 x 10 14 Hz to reach the n = 4 state. From what state did the electron originate?
a) n=2
b) n=3
c) n=5
d) n=6

What is the wavelength of the light emitted from a hydrogen atom when an electron moves from the n = 6 to n = 2 energy level?R = 1.096776 x 107 m-1.A. 2.74 x 10-7 mB. 4.10 x 10-7 mC. 2.22 x 10-1 mD. 2.44 x 106 mE. 3.65 x 106 m

How much energy is emitted in kJ/mol when an electron in the H atom transitions from n=6 to n=2?A. 275B. 292C 302D. 310E. 321

The n = 2 to n = 10 transition in the Bohr hydrogen atom corresponds to the __________ of a photon with a wavelength of __________nm.
a) emission, 380
b) absorption, 380
c) absorption, 657
d) emission, 657
e) emission, 389

An electron in a hydrogen atom relaxes to the n = 4 level, emitting light of 114 THz. What is the value of n for the level in which the electron originated?

Calculate the energy of a photon emitted when an electron in a hydrogen atom undergoes a transition from n = 6 to n = 1.

One of the emission lines of the hydrogen atom has a wavelength of 93.8 nm. (b) Determine the initial and final values of n associated with this emission.

Calculate the energy, in joules, required to excite a hydrogen atom by causing an electronic transition from the n = 1 to the n = 4 principal energy level.a. 2.07 x 10-29 J b. 2.19 x 105 J c. 2.04 x 10-18 J d. 3.27 x 10-17 J e. 2.25 x 10-18 J

A hydrogen atom absorbs a photon with a wavelength of 397.1 nm, which excites the atom’s electron. Determine the electron’s initial quantum level if the transition results in a final quantum level of n = 7.a) n = 4b) n = 3c) n = 1d) n = 2e) n = 5

Calculate the frequency of the light emitted by a hydrogen atom during a transition of its electron from the n = 3 to n = 1 energy level, based on the Bohr theory. Use the equation En = -2.18 x 10 -18 J [(1/nf2)-(1/ni2)]a. 2.92 x 1015 s-1b. 3.56 x 1014 s-1c. 2.92 x 1014 s-1d. 1.17 x 1015 s-1

An atomic emission spectrum of hydrogen shows three wavelengths: 121.5 nm, 102.6 nm, and 97.23 nm. Assign these wavelengths to transitions in the hydrogen atom.1) 2 →1 , 2) 3 → 1 3) 4 → 11) 2 →1 , 2) 2 → 1 3) 4 → 11) 2 →1 , 2) 2 → 1 3) 3 → 11) 2 →1 , 2) 3 → 1 3) 3 → 1

What is the frequency in Hz of the photon released when a hydrogen atom undergoes a transition from the excited state where n = 2 to the state where n = 1?

An electron in the n=7 level of the hydrogen atom relaxes to a lower energy level, emitting light of 397 nm. What is the value of n for the level to which the electron relaxed?

What wavelength of light (in nm) if absorbed by a ground-state hydrogen atom could cause an electron to transition to n=3?

An excited hydrogen atom emits light with a wavelength of 397.2 nm to reach the energy level for which n = 2. In which principal quantum level did the electron begin?

What are the wavelengths, in nanometers, of the bright lines of the hydrogen emission spectrum corresponding to the transition: n = 5 to n = 2?

An electron in a hydrogen atom relaxes to the n = 4 level, emitting light of 138 THz.What is the value of n for the level in which the electron originated? Express your answer as an integer.

Determine the energy change associated with the transition from n = 2 to n = 5 in the hydrogen atom.a. +3.76 x 10 -19 Jb. +6.54 x 10 -19 Jc. -1.53 x 10 -19 Jd. -2.18 x 10 -19 Je. +4.58 x 10 -19 J

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