Question

**Calculate the energy difference
(Δ***E***) for the electron transition
of** *n* **= 5 to** *n* **=
1 for 1.00 mol of hydrogen atoms. Enter your answer in scientific
notation.**

Answer #1

1.) Calculate the energy difference (?E) for the electron
transition of n = 3 to n = 2 for 1.00 mol of hydrogen atoms. Enter
your answer in scientific notation.
2.) A lithium flame has a characteristic red color due to
emissions of wavelength 671 nm. What is the mass equivalence of 1.0
mol of photons of this wavelength
(1 J = 1 kg·m2/s2)?
------ × 10^------- kg (Enter your answer in scientific
notation.) -> the dotted lines are the...

Calculate the energy of a photon produced when an electron in
hydrogen makes a transition from an excited state in the 5th n=5
level, back to the ground state, n=1. Would you expect to see
radiation from this photon? Explain.

The Balmer lines are from
a) The transition of hydrogen atoms into the lowest energy
level
b) The transition of hydrogen atoms into the n=2 level.
c) The transition of helium atoms into the lowest energy
level.
d) The transition of oxygen atoms to the lowest energy
level.
Emission lines are caused when an electron moves ____ energy;
Absorption lines are caused when an electron moves ______
energy
a) to higher; to lower
b) to a higher n; to a...

An electron in a hydrogen atom makes a transition from the n = 7
to the n = 2 energy state. Determine the wavelength of the emitted
photon (in nm). Enter an integer.

An electron in a hydrogen atom undergoes a transition from the n
= 6 level to some lower energy level. In doing so, energy is
released in the form of light. a) Calculate the frequency in s-1
(to 3 significant figures) of a photon of light associated with the
highest frequency transition (i.e. largest difference in frequency)
possible from the n = 6 to a lower level. (HINT: Try drawing a
picture first…) b) Calculate the wavelength (in nm) of...

calculate delta e for the n= 4 to the n=2 transition of an electron
in a hydrogen atom. Where on the electromagnetic spectrum would
this appear? what does the sign of this value mean?

4.). An excited electron falls from n=4 to n=2.
a.) Calculate the energy change in Joules associated
with this transition
b.) what Is the wavelength in nm of the emmitted
electromagnetic radiation? what color Is it?
c.) calculate the energy change in Kj mol -1.

Calculate the difference in energy (in joules) between a
photon with
λ
= 719 nm and a photon with
λ
= 339 nm. Enter your answer in scientific
notation.

1. Calculate the energy (in kJ/mol) of the Lyman series line for
hydrogen that is, the transition from n=2 to n=1 (1 kJ/mol= 8.6
cm^-1)
2. Would you expect the energy of the same transition as in the
first problem to be greater or less for the helium ion, He^+? Why?
Make a sketch to relative scale the energy levels that give rise to
the Lyman bands in H-atoms and He^+.

An electron in a hydrogen atom makes a transition from the n =
68 to the n = 4 energy state. Determine the wavelength of the
emitted photon (in nm).

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