Question

An excited hydrogen atom could, in principle, have a radius of 1.50 mm .

A - What would be the value of

*n* for a Bohr orbit of this size? n= ?

B - What would its energy be?

e = ? eV

Answer #1

A hydrogen atom is in its first excited state
(n = 2).
Using Bohr's atomic model, calculate the following.
(a)
the radius of the electron's orbit (in nm)
nm
(b)
the potential energy (in eV) of the electron
eV
(c)
the total energy (in eV) of the electron
eV

Answer the following questions using the Bohr model of the
hydrogen atom.
a) A hydrogen atom is the n = 3 excited state when its electron
absorbs a photon of energy 4.40 eV. Draw a diagram roughly to
scale, of relevant energy levels for this situation. Make sure to
show and label the initial energy of the H atom in the n=3 state,
the energy level at which this atom loses its electron, and kinetic
energy of the electron.
b)What...

The Bohr Model of the hydrogen atom proposed that there were
very specific energy states that the electron could be in. These
states were called stationary orbits or stationary states. Higher
energy states were further from the nucleus. These orbits were
thought to be essentially spherical shells in which the electrons
orbited at a fixed radius or distance from the nucleus. The
smallest orbit is represented by n=1, the next smallest n=2, and so
on, where n is a positive...

1). The Bohr Model of the hydrogen atom proposed that there were
very specific energy states that the electron could be in. These
states were called stationary orbits or stationary states. Higher
energy states were further from the nucleus. These orbits were
thought to be essentially spherical shells in which the electrons
orbited at a fixed radius or distance from the nucleus. The
smallest orbit is represented by n=1, the next smallest n=2, and so
on, where n is a...

In the hydrogen atom the radius of orbit B is nine times greater
than the radius of orbit A. The total energy of the electron in
orbit A is -3.40 eV. What is the total energy of the electron in
orbit B?

A hydrogen atom is initially at n=2 excited state and then
absorbs energy 2.55 eV. The excited state is unstable, and it tends
to finally return to its ground state.
(a) How many possible wavelengths will be emitted as the atom
returns to its ground state? draw a diagram of energy levels to
illustrate answer
Answer: (number) ________
(b) Calculate the shortest wavelength emitted.
Answer: ________

A hydrogen atom has an angular momentum 5.275 x 10 ^ -34 kg *
m^2/s According to the Bohr model, determine:
A) The number of the orbit (main quantum number)
B) The energy (eV) associated with this state.
C) The radius of this orbit.
D) The speed of the electron associated with this orbit.
e) If a transition occurs from this state to the base state (n =
1), what is the energy that the photon has during the
transition?
f))....

A hydrogen atom is initially at n=2 excited state and then
absorbs energy 2.86 eV. The excited state is unstable, and it tends
to finally return to its ground state. 8%
(a) How many possible wavelengths will be emitted as the atom
returns to its ground state? (also draw a diagram of energy levels
to illustrate your answer)
Calculate the second shortest wavelength emitted.

a) If the 3rd energy level of a hypothetical
hydrogen-like atom is −1.50×10−18 J, what is the energy
of the 2nd energy level?
b) If a photon whose frequency is 2.50×1016 Hz
collides with an electron at rest and loses 25.0% of its energy,
what is the speed of this electron after collision?
c) An electron of a hydrogen atom is on its 4th energy orbit.
How many possible photons it could emit?
a)3
b)4
c)5
...

Take the potential energy of a hydrogen atom to be zero for
infinite separation of the electron and proton. Then the ground
state energy of a hydrogen atom is –13.6 eV. The energy of the
first excited state is:
A) 0eV
B) –3.4 eV
C) –6.8 eV
D) –10.2 eV
E) –27 eV

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