Question

Singly ionized helium (He+) atom/ion has a single remaining electron and a nuclear charge of +2? (twice that of a proton). Using the Bohr model with appropriate modifications, estimate a) the radius and b) the total energy (in electron volts) of such an atom in its first excited level. c) When the state of this atom changes from the first excited level to the ground level, a photon is emitted in the process. Estimate the energy (in electron volts) of this photon.

Answer #1

The ionized helium atom can be treated with a Bohr model with
nuclear charge Z=2. The resulting energy levels are four times
those of the hydrogen atom:
Ehelium=4Ehydrogen= -(54.4eV)/n^2
From those energy levels, calculate the wavelengths of spectral
lines from ionized helium for transitions that end on nf=1. Do any
of these lie in the visible range? Would any spectral lines of
ionized helium lie in the visible range?

The electronic energy levels for a Helium ion He+ (ie a nuclear
charge of +2e and a single bound electron of –e) are similar to
that of the hydrogen atom (ie a nuclear charge of +e and a single
bound electron of charge –e), except for an extra factor of 4
corresponding to the square of the nuclear charge changing from
(+e)2 for hydrogen to (+2e)2 for Helium. Thus, the electronic
energy levels for Helium are 4 times the electronic...

why are the electrons of the helium atom not all in the 1s
state.
Which of the following
choices best explains this observation?
Coulomb's law
the Pauli exclusion principle
the Einstein quantum entanglement principle
Rutherford's explanation of atomic structure
the Heisenberg uncertainty principle
2.)There is a singly-ionized helium atom, which has 2 protons
with its remaining electron in the ground state.
Using the Bohr model calculation, determine the maximum
wavelength in nanometers for a photon that could remove the
remaining...

Hydrogen, deuterium, and singly ionized helium are all examples
of one-electron atoms.
The deuterium nucleus has the same charge as the hydrogen
nucleus, and almost exactly
twice the mass. The helium nucleus has twice the charge of the
hydrogen nucleus, and
almost exactly four times the mass. Make an accurate prediction
of the ratios of the
ground state energies of these atoms. (Hint: Remember the
variation in the reduced
mass.)

Consider an atom of singly- ionized helium (Z=2)
a. calculate its ground-state energy in eV
b. work out an expression for the wavelengths of photons needed
to raise the ion from its ground state to the state n. compute
values (in nm) of the largest and samllest such wavelengths
c. compute the circumference (in nm) of the orbit for the
particular value of n in part b that gives the largest wavelength
and its orbital speed as a fraction of...

(a) (5 pts.) What are the three lowest energies of the singly
ionized He-atom according to the Bohr model? (b) (5 pts.) Calculate
the energies of the photons emitted when electronic transitions
take place between all possible states.
The excited levels of Hydrogen have lifetimes of order 10^-8 s.
In very highly excited states (large n), the states get closer and
closer together. At what value of n do the spacings of
the energy levels become comparable to the energy...

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.
Find the wavelength for the transition n=3 ?
n=2 for singly ionized helium, which has one electron and
a nuclear charge of 2e. (Note that the value of the
Rydberg constant is four times as great as...

Consider a hydrogen atom: a single electron that orbit the
proton, the electron circular orbit has radius Bohr ground state
.529 angstrom.
a. Calculate the magnitude of the Coulomb's force between the
proton and electron
b. Write this force in vector form.
c. Calculate the velocity and acceleration of the electron.
d. Calculate the electron's electric potential energy in
electron volt.

The electron in a hydrogen atom falls from an excited energy
level to the ground state in two steps, causing the emission of
photons with wavelengths of 656.5 nm and 121.6 nm (So the in the
first step the 656.5 nm photon is emitted and in the second step
the 121.6 nm photon is emitted). What is the principal quantum
number (ni) of the initial excited energy level from which the
electron falls?

An ionized atom has only a single electron. The n = 6
state of this atom has an energy of -9.444 eV. Find the radius of
the n = 3 state.
Group of answer choices
0.233 nm
0.182 nm
0.0952 nm
0.204 nm
0.0317 nm

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