The only visible spectral lines of hydrogen are the four Balmer series lines (transitions to n=2)....

The only visible spectral lines of hydrogen are the four Balmer series lines (transitions to n=2). We wish to cause hydrogen gas to glow with all its characteristic visible colors.

a) To how high an energy level must the electrons be excited?

b) Energy is absorbed in collisions with other particles. Assume that after absorbing energy in one collision, an electron jumps down through lower levels so rapidly so that it is in the ground state before the collision occurs. If an electron is to be raised to the level found in part (a), how much energy must be available in a single collision?

c) If such energetic collisions are to be effected simply by heating a gas until the average KE equals the desired upward energy jump, what temperature would be required?

Solutions

Expert Solution

genius_generous answered 1 year ago

Next > < Previous

Related Solutions

The Balmer series for the hydrogen atom corresponds to electronic transitions that terminate in the state...

The Balmer series for the hydrogen atom corresponds to electronic transitions that terminate in the state with quantum number n = 2 as shown in the figure below. Consider the photon of longest wavelength corresponding to a transition shown in the figure. (a) Determine its energy (b) Determine its wavelength Consider the spectral line of shortest wavelength corresponding to a transition shown in the figure (c) Find its photon energy (d) Find its wavelength (e) What is the shortest possible wavelength in the Balmer series?

4. The Balmer Series The Balmer series is limited to wavelengths in the visible regions from...

4. The Balmer Series The Balmer series is limited to wavelengths in the visible regions from 250 nm to 700 nm. On the basis of your entries in the above table and the transitions on your energy level diagram what common characteristic do the lines in the Balmer series have? What would be the shortest and longest possible wavelengths for a line in the Balmer series?

Explore the Balmer series of atomic transitions for a hydrogen atom. Assume the shortest wavelength possible...

Explore the Balmer series of atomic transitions for a hydrogen atom. Assume the shortest wavelength possible occurs when the atom is ionized or when n = ∞ . What is the longest and shortest wavelengths possible? What is the frequency, wavelength and energy of the longest wavelength? longest λ = ___________ nm frequency = _________ Hz energy = _________ eV Shortest λ = ___________ nm

The wavelengths in the hydrogen spectrum with m = 1 form a series of spectral lines...

The wavelengths in the hydrogen spectrum with m = 1 form a series of spectral lines called the Lyman series. Part A Calculate the wavelength of the first member of the Lyman series. Express your answer to three significant figures and include the appropriate units. λ1λ 1 = nothing nothing Request Answer Part B Calculate the wavelength of the second member of the Lyman series. Express your answer to three significant figures and include the appropriate units. λ2λ 2 =...

D. The Balmer Series 1. When Balmer found his famous series for hydrogen in 1886, he...

D. The Balmer Series 1. When Balmer found his famous series for hydrogen in 1886, he was limited experimentally to wavelengths in the visible and near ultraviolet regions from 250 nm to 700 nm, so all the lines in his series lie in that region. a) Based on the entries in Table 2 and the transitions on your energy level diagram, what common characteristic do the lines in the Balmer series have? B) What would be the longest possible wavelength...

Calculate the wavelengths (in nm) of the first 5 transitions in the Balmer series using the...

Calculate the wavelengths (in nm) of the first 5 transitions in the Balmer series using the Rydberg equation. Convert the wavelengths calculated into frequencies.

Atomic hydrogen exhibits a series of emission spectral lines that includes the following wavelengths: 1875 nm,...

Atomic hydrogen exhibits a series of emission spectral lines that includes the following wavelengths: 1875 nm, 1282 nm, and 1094 nm. (a) What is the name of the series of emission spectral lines? (b) What is the wavelength of the next line in the series?

Consider only transitions involving the n =1 through n = 4 levels for the hydrogen atom

a Consider only transitions involving the n =1 through n = 4 levels for the hydrogen atom. How emission lines are possible, considering only the four quantum levels? b Consider only transitions involving the n = 1 through n = 4 energy levels for the hydrogen atom.Photons of the lowest energy are emitted in a transition from the level with n = _______ to a level with n = _______ c Consider only transitions involving the n = 1 through n = 4...

1. The lines observed in H-lamp are parts of Balmer Series. All these lines are due...

1. The lines observed in H-lamp are parts of Balmer Series. All these lines are due to a transition from various higher n value to a common n. What is this common lower n value for all these lines? 0 1 2 3 2. The lines on Absorption Atomic Spectra correspond to energies needed for electrons to be excited from a lower energy level to a higher energy level. Assume that the energy needed for an electron in 2p orbital...

Question 1 The lines observed in H-lamp are parts of Balmer Series. All these lines are...

Question 1 The lines observed in H-lamp are parts of Balmer Series. All these lines are due to a transition from various higher n value to a common n. What is this common lower n value for all these lines? 0 1 2 3 ------------------------------------------------------------------------------------------------------ Question 2 The bright violet line of Hg lamp has a wavelength of 435.8 nm. What is the energy of the photon associated with this emission line? 4.56*10^-19 J 4.56*10^-28 J 6.88*10^14 J 2.89*10^-31 J...

Subjects