Question

Q1)

Calculate the energy of an electron in the n =
**2** level of a hydrogen atom.

Energy = _______Joules

Q2)

What would be the wavelength of radiation emitted from a
hydrogen atom when an electron moves from the *n* =
**2** to *n* = **1**energy level?
In what region of the spectrum does this radiation lie?

Wavelength = ________nm

Region = _________(ultraviolet or visible or infrared)

Answer #1

1)

Energy in eV in nth level is given by:

En = -13.6/n^2

for n=2,

E = -13.6/2^2 eV

E = -13.6/4 eV

E = -3.4 eV

E = -3.4*1.602*10^-19 J

E = 5.45*10^-19 J

Answer: 5.45*10^-19 J

2)

Here photon will be emitted

1/lambda = R* (1/nf^2 - 1/ni^2)

R is Rydberg constant. R = 1.097*10^7

1/lambda = R* (1/nf^2 - 1/ni^2)

1/lambda = 1.097*10^7* (1/1^2 - 1/2^2)

lambda = 1.215*10^-7 m

lambda = 122 nm

Answer: 122 nm

this wavelength is less than wavelength of violet rays

So, this is ultraviolet

A photon is emitted from a hydrogen atom when an electron goes
from the n = 6 to the n = 2 state. What kind of electromagnetic
radiation is this? Select one:
a. Visible Light
b. Ultraviolet Light
c. Infrared Radiation
d. X-Ray Radiation
e. Microwave Radiation

1. The energy of the electron in the lowest level of the
hydrogen atom (n=1) is -2.179×10-18 J. What is the energy of the
electron in level n=5? -8.716×10-20 J 2.The electron in a hydrogen
atom moves from level n=6 to level n=4.
a) Is a photon emitted or absorbed?
b) What is the wavelength of the photon?

Calculate the energy of the emitted photon as well as the
wavelength and frequency of electromagnetic radiation emitted from
the hydrogen atom when the electron undergoes the transition from n
= 5 to n = 1. In what region of the spectrum does this line
occur?

Part B
Using equation E=(hcRH)(1n2)=(−2.18×10−18J)(1n2), calculate the
energy of an electron in the hydrogen atom when n= 5.
Part C
Calculate the wavelength of the radiation released when an
electron moves from n= 5 to n=2.

Light is emitted from a hydrogen atom as an electron in the atom
jump from the n=9 orbit to the n=3 orbit.
What is the energy of the emitted photon in eV?
(b) What are the frequency and wavelength of the photon?
(c) In which frequency range (UV, visible, IR) is the emitted
electromagnetic radiation? Justify your answer.

4. [15] Light is emitted from a hydrogen atom as an electron in
the atom jump from the n=9 orbit
to the n=3 orbit.
(a) [7] What is the energy of the emitted photon in eV?
(b) [4] What are the frequency and wavelength of the photon?
(c) [4] In which frequency range (UV, visible, IR) is the
emitted electromagnetic radiation?
Justify your answer.

2. Planck’s hypothesis (a) was the basis of Wien’s law,
(b) called for the intensity of blackbody radiation to be
proportional to 1 / 4 , (c) quantized the energy of thermal atomic
oscillators, or (d) predicted the ultraviolet
catastrophe.
What is the wavelength of the radiation component of
maximum intensity emitted by our bodies? In what region of the EM
spectrum is this wavelength?
. A metal with a work function of 2.40 eV is illuminated
with a beam...

) Describe the Bohr theory of the hydrogen atom and how it
explains the line spectrum of hydrogen. What is the
energy and wavelength of the
photon of energy that was emitted by hydrogen if one of its
electrons dropped from the n=6 state to the n=2 state. In what
region of the electromagnetic spectrum does this wavelength fall?
Which color line is this in the line spectra of hydrogen?

a. what is the energy of the emitted photon if an electron in
the hydrogen atom makes a transition from the n=7 state to the n=2
state?
b. Now, Imagine there is a photon with the same wavelength. What
is the speed of this photon?

When an
electron moves from level n= 4 to level n =5 in an excited hydrogen
atom, what amount of energy is required for this electronic
transition?
Please show
your full work!! Where you got number from step by step

ADVERTISEMENT

Get Answers For Free

Most questions answered within 1 hours.

ADVERTISEMENT

asked 23 minutes ago

asked 31 minutes ago

asked 33 minutes ago

asked 56 minutes ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago