The Bohr model can be applied to singly ionized helium
He+ (Z = 2). Using this model, consider the
series of lines that is produced when the electron makes a
transition from higher energy levels into the 
= 4 level. Some of
the lines in this series lie in the visible region of the spectrum
(380−750 nm). What are the values of 
for the energy levels
from which the electron makes the transitions corresponding to
these lines?
Homework Answers
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The Bohr model can be applied to singly ionized helium
He+ (Z = 2). Using this...
Chapter 30, Problem 59 The Bohr model can be applied to singly ionized helium He+ (Z=2)....
Chapter 30, Problem 59
The Bohr model can be applied to singly ionized helium He+
(Z=2). Using the model, consider the series of lines that is
produced when the electron makes a transistion from higher energy
levels into the nf = 4 level. Some of the lines in the series lie
in the visible region of the spectrum (380 nm - 750 nm). What are
the (a) minimum value and (b) maximum value of ni for the energy
levels from...
Problem 2: Helium Spectra In helium, there are two electrons, which makes the math in finding...
Problem 2: Helium Spectra In helium, there are two electrons, which makes the math in finding their energy levels much more complicated. As a first approximation to that math, we can use Bohr energy levels with Z = 1.34 for the neutral helium atom (ie when both electrons are present), and Z = 2 for the singly ionized helium atom (ie when only one electron is present). The lower Z value for the neutral helium atom can be thought of...
Use the following information to answer the next question. The following diagram represents the emission lines...
Use the following information to answer the next question. The following diagram represents the emission lines that are produced for the Balmer Series of hydrogen. Each line is produced as an electron makes a transition from a higher Bohr energy level to n-2. Balmer Series Spectral Line Wavelengths IT I 300 nm 400 nm 500 nm 600 mm 700 nm 8. The regions of the electromagnetic spectrum into which the lines of the Balmer Series of hydrogen are classified are...
Prelaboratory Assignment: The Atomic Spectra of Hydrogen 1. The helium ion, He', has energy levels similar...
Prelaboratory Assignment: The Atomic Spectra of Hydrogen 1. The helium ion, He', has energy levels similar to those of hydrogen and are given by the equation: E, (-8.72 x 10-" /n') Joules a) Calculate the energy of the four lowest energy levels of the He ion. E,- Joules EJoules Joules Joules b) What is the energy and wavelength associated with the n2 1 transition in He'? kJ/mol; λ= nm c) The strongest lines of the He spectrum occur at the...
answer is not 122 or 97.2 Review Constants Let's use the Bohr model equations to explore...
answer is not 122 or 97.2
Review Constants Let's use the Bohr model equations to explore some properties of the hydrogen atom. We will determine the kinetic, potential, and total energies of the hydrogen atom in the n=2 state, and find the wavelength of the photon emitted in the transition n = 2 →n=1. En= 1 med 602 8nºh? -13.6 eV 722 These two equations are equal only if the coefficients of 1/n2 are equal: met =hcR= 13.6 eV 8€0h?...
Although the Bohr model was very successful in accounting for the line spectrum of hydrogen, from...
Although the Bohr model was very successful in accounting for the line spectrum of hydrogen, from what limitations did it suffer? It failed to predict the line spectrum for multi-electron atoms. It incorrectly proposed that electrons could reside between orbital's. It only accurately predicted the visible series of lines in the line spectra of atoms, but not the ultraviolet or infrared series. It incorrectly proposed that electrons move in fixed, defined orbits. It did not explain the quantized nature of...
3. For the n=5 to n=2 transition: E = in nm = in Å = Color...
3. For the n=5 to n=2 transition: E = in nm = in Å = Color of corresponding line in the hydrogen spectrum: We were unable to transcribe this image
There is an electron in the Bohr model in orbit 2. n=2. Now using de Brogile...
There is an electron in the Bohr model in orbit 2. n=2. Now using de Brogile standing wave perspective so the electron in this orbit. Calculate the time required for the electron to complete one revolution. Calculate the current in amperes corresponding to the electron motion in orbit 2. What is the magnitude of the magnetic field produced at the nucleus due to electron circulation? Know there is a current now. There is a circular current. There will be a...
When an electron of an excited hydrogen atom descends, from an initial energy level (ni) to...
When an electron of an excited hydrogen atom descends, from an initial energy level (ni) to a lower (nf), characteristic electromagnetic radiation is emitted. The Bohr model of the H-atom allows the calculation of ?E for any pair of energy levels. ?E is related to the wavelength (?) of the radiation according to Einstein's equation ( ?E = [(hc)/?]). Distinct series of spectral lines have been classified according to nf: Lyman series:nf=1 (91<?<123 nm; near-UV). Balmer series:nf=2 (365<?<658 nm; visible)....
4 Item 4 Learning Goal: To calculate the wavelengths of the lines in the hydrogen emission...
4
Item 4 Learning Goal: To calculate the wavelengths of the lines in the hydrogen emission spectrum Atoms give off light when heated or otherwise excited! The light emitted by excited atoms consists of only a few wavelengths, rather than a full rainbow of colors. When this light is passed through a prism, the result is a series of discrete lines separated by blank areas. The visible lines in the series of the hydrogen spectrum are caused by emission of...
Chapter 30, Problem 59
The Bohr model can be applied to singly ionized helium He+
(Z=2). Using the model, consider the series of lines that is
produced when the electron makes a transistion from higher energy
levels into the nf = 4 level. Some of the lines in the series lie
in the visible region of the spectrum (380 nm - 750 nm). What are
the (a) minimum value and (b) maximum value of ni for the energy
levels from...
Problem 2: Helium Spectra In helium, there are two electrons, which makes the math in finding their energy levels much more complicated. As a first approximation to that math, we can use Bohr energy levels with Z = 1.34 for the neutral helium atom (ie when both electrons are present), and Z = 2 for the singly ionized helium atom (ie when only one electron is present). The lower Z value for the neutral helium atom can be thought of...
Use the following information to answer the next question. The following diagram represents the emission lines that are produced for the Balmer Series of hydrogen. Each line is produced as an electron makes a transition from a higher Bohr energy level to n-2. Balmer Series Spectral Line Wavelengths IT I 300 nm 400 nm 500 nm 600 mm 700 nm 8. The regions of the electromagnetic spectrum into which the lines of the Balmer Series of hydrogen are classified are...
Prelaboratory Assignment: The Atomic Spectra of Hydrogen 1. The helium ion, He', has energy levels similar to those of hydrogen and are given by the equation: E, (-8.72 x 10-" /n') Joules a) Calculate the energy of the four lowest energy levels of the He ion. E,- Joules EJoules Joules Joules b) What is the energy and wavelength associated with the n2 1 transition in He'? kJ/mol; λ= nm c) The strongest lines of the He spectrum occur at the...
answer is not 122 or 97.2
Review Constants Let's use the Bohr model equations to explore some properties of the hydrogen atom. We will determine the kinetic, potential, and total energies of the hydrogen atom in the n=2 state, and find the wavelength of the photon emitted in the transition n = 2 →n=1. En= 1 med 602 8nºh? -13.6 eV 722 These two equations are equal only if the coefficients of 1/n2 are equal: met =hcR= 13.6 eV 8€0h?...
Although the Bohr model was very successful in accounting for the line spectrum of hydrogen, from what limitations did it suffer? It failed to predict the line spectrum for multi-electron atoms. It incorrectly proposed that electrons could reside between orbital's. It only accurately predicted the visible series of lines in the line spectra of atoms, but not the ultraviolet or infrared series. It incorrectly proposed that electrons move in fixed, defined orbits. It did not explain the quantized nature of...
3. For the n=5 to n=2 transition: E = in nm = in Å = Color of corresponding line in the hydrogen spectrum: We were unable to transcribe this image
4
Item 4 Learning Goal: To calculate the wavelengths of the lines in the hydrogen emission spectrum Atoms give off light when heated or otherwise excited! The light emitted by excited atoms consists of only a few wavelengths, rather than a full rainbow of colors. When this light is passed through a prism, the result is a series of discrete lines separated by blank areas. The visible lines in the series of the hydrogen spectrum are caused by emission of...
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