Question

Exercise2 The absorption spectrum of an atom consists of the wavelengths 200nm, 300 nm, and 500nm....

Exercise2

The absorption spectrum of an atom consists of the wavelengths 200nm, 300 nm, and 500nm.

a) Draw the atom's energy level diagram. Label each level with the energy and the principal quantum number.

b) What wavelengths are seen in the atom's emission spectrum?

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
The allowed energies of a simple atom are 0.00 eV, 4.21 eV , and 5.63 eV...
The allowed energies of a simple atom are 0.00 eV, 4.21 eV , and 5.63 eV . Part A What wavelengths appear in the atom's emission spectrum? Enter your answers in ascending order separated by commas. Part B What wavelengths appear in the atom's absorption spectrum? Enter your answers in ascending order separated by commas.
The allowed energies of a simple atom are 0.00 eV, 3.73 eV , and 5.58 eV...
The allowed energies of a simple atom are 0.00 eV, 3.73 eV , and 5.58 eV . Part A What wavelengths appear in the atom's emission spectrum? Enter your answers in ascending order separated by commas. Part B What wavelengths appear in the atom's absorption spectrum? Enter your answers in ascending order separated by commas.
The allowed energies of a simple atom are 0.00 eV, 4.05 eV , and 5.12 eV...
The allowed energies of a simple atom are 0.00 eV, 4.05 eV , and 5.12 eV . Part A What wavelengths appear in the atom's emission spectrum? Enter your answers in ascending order separated by commas. Part B What wavelengths appear in the atom's absorption spectrum? Enter your answers in ascending order separated by comma
The electron in a hydrogen atom falls from an excited energy level to the ground state...
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 electron in a hydrogen atom relaxes to the ground state while emitting a 93.8 nm...
An electron in a hydrogen atom relaxes to the ground state while emitting a 93.8 nm photon. a. Is this light visible? In what region of the electromagnetic spectrum does it lie? b. What was the initial principal quantum number, ni, of the electron undergoing the transition?
A hydrogen atom in the ground state absorbs a 12.75 eV photon. Immediately after the absorption,...
A hydrogen atom in the ground state absorbs a 12.75 eV photon. Immediately after the absorption, the atom undergoes a quantum jump to the next-lowest energy level. What is the wavelength of the photon emitted in this quantum jump? Express your answer using four significant figures. I've seen this question before, but I'm looking the wavelength, not the energy, or n. Thanks!
The microwave spectrum of the 12C16O molecule consists of a series of lines separated by 3.913...
The microwave spectrum of the 12C16O molecule consists of a series of lines separated by 3.913 cm−1. Draw the corresponding energy level diagram for this spectral line spacing for the first 5 energy levels, assuming the rigid rotor model. Give the value for the energy gap between each level.
Light from a laser of wavelength 475 nm is incident upon an atom of hydrogen in...
Light from a laser of wavelength 475 nm is incident upon an atom of hydrogen in the first excited state. (a) What is the highest energy level (value of n) to which the hydrogen atom can be excited by the laser?   (b) What happens if the laser wavelength is 295 nm? Another way to get the energy levels of the Bohr atom is to assume that the stationary states are those for which the circumference of the orbit is an...
Answer the following questions using the Bohr model of the hydrogen atom. a) A hydrogen atom...
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...
A. An electron emits a photon with an energy of 424 nm as it relaxes to...
A. An electron emits a photon with an energy of 424 nm as it relaxes to (n=2) what is the initial energy level of this electron? B. Is energy released or absorbed a result of this transition? Briefly explain. C. Calculate the wavelength (nm) of the electron having the kinetic energy (K.E. = 1/2 mv^2) of the above transition 434 nm. D. If an electron has the following three quantum number, n=2, l= 1, m= 0, and m=-1/2. Briefly explain...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT