The picture that has table might help you, answer the question using the hand writing,please write clearly on your ans I. Give an example of an application that involves the absorption of X-rays.II. Describe what happens on a molecular level when an X-ray photon is absorbed? What is the nature of the change in energy thatoccurs? Table T01-7-1. The types of changes that occur at a molecular level when photons are absorbed.RadiationgammaX-rayultravioletA< 0.01 nm1 - 10 nm10 - 400 nmvisible 400 - 750 nminfrared 750 nm 1 mmmicrowave 1 mm - 1 mradio> 1mInteraction with matterIonizes atoms and moleculesBreaks chemical bondsIonizes atoms and moleculesBreaks chemical bondslonizes atoms and moleculesBreaks chemical bondsPromotes electrons to higher energy (electronic transitions)Promotes electrons to higher energy (electronic transitions)Increases amplitudes of vibrations (kinetic energy increases)Increases speed of molecular rotations (kinetic energy increases)Flips the nuclear spin-----------………………………………………………………..

Solutions- There are many applications of X-ray. The most applications of X- rays is in medical and…

I. Give an example of an application that involves the absorption of X-rays. II. Describe what happens on a molecular level when an X-ray photon is absorbed? What is the nature of the change in energy that occurs?

I. Give an example of an application that involves the absorption of X-rays. II. Describe what happens on a molecular level when an X-ray photon is absorbed? What is the nature of the change in energy that occurs?

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter5: Electron Configurations And The Periodic Table

Section: Chapter Questions

Problem 30QRT

See similar textbooks

Similar questions

Sunburn is caused by ultraviolet UV radiation. Why does red light not cause sunburn?
6.103 Atomic absorption spectroscopy is based on the atomic spectra of the elements being studied. It can be used to determine the impurities in a metal sample. If an element is present, light at the appropriate wavelength is absorbed. You are working with a metal stamping company and the rolled steel you use to form panels for automobile doors is failing at an alarming rate. There is some chance that the problem is unacceptably high levels of manganese in the steel. Given that the atomic spectrum of manganese has three lines near 403 nm, how could you use a spectrometer to determine the amount of manganese in the steel?
Do atoms in excited states emit radiation randomly, at any wavelength? Why? What does it mean to say that the hydrogen atom has only certain discrete energy levels available? How do we know this? Why was the quantization of energy levels surprising to scientists when it was first discovered?
Are mathematical expressions for the following potential energies positive or negative? Explain why in each case. a The attraction between an electron and a helium nucleus b The repulsion between two protons in a nucleus c The attraction between a north and a south magnetic pole d The force of gravity between the Sun and Earth e A rock perched on the edge of a cliff with respect to the base of the cliff
Assuming HCl and DC1 have the same force constant (k) or potential energy, V(x) = kx², what is the vibrational frequency of DC1 if the vibrational frequency for HCl is 3000 cm ¹? (the atomic masses for H atom, D, atom and Cl atom are 1, 2, and 35, respectively) A. 516 cm-¹ B. 1250 cm-¹ C. 2150 cm-¹ D. 3000 cm-¹ E. 4190 cm-¹
4. How are X-Rays generated, what are characteristic X-Rays and Bremsstrahlung.
Please answer question 18 Part A
"Photosynthesis is a process in which light energy is captured and stored by an organism, and the stored energy is used to drive cellular processes," (Blankenship, p. 1). Photosynthesis doesn't just happen in green plants; it can occur in bacteria, as well. It occurs when light- harvesting molecules absorb energy in the form of light and transfer it to a reaction center, where light energy is converted to chemical energy. Most of us know about chlorophyll as the light-harvesting molecule, but there are many forms of chlorophyll found in different organisms. However, they all have similar properties when interacting with light. PHOTOSYNTHETIC PIGMENTS 1.6 C 0.7 1.4 0.6 1.2- Soret 0.5 A 0.4 0.8 H COOCH, phytyl bacteriochlorophyll a 0.3 0.6 0.2 0.4 0.1 0.2 01 700 750 800 850 900 300 400 500 600 700 800 2 (nm) 2 (nm) Figure 4.7 Absorption (left) and fluorescence (right) spectra of bacteriochlorophyll a in diethyl ether. 5. Look at this figure from Blankenship's book, Molecular Mechanisms…
If a single C-C bond has a bond energy of 346 kJ/mol, could a single photon in the visible range with a wavelength of 550 nm break this bond? O it cannot be calculated or determined. O no. O yes. O only if the C-C bond is part of a large biomolecule. + Post a new auestion hulu stv MacBook Pro + 2$ & %3D 4 5 7 8. { Y U F G J. .. .-
Analysis: What is an ion? Describe what happens to the electrons in an atom when they absorb energy (from the flame)? Why does this produce a bright-line emission spectrum (rather than a continuous spectrum)? In terms of atomic structure, why does each metal ion produce a different color flame? What difficulties are there in identifying metal ions with a flame test? How could you improve the specific identification of the metal ions during a flame test? If it can be determined from the flame test results, what are the identities of the two unknown liquids? What might be some practical (and exciting) applications of metal containing compounds that create different colors of light while burning? Explain.
10.a. A photon has an energy of 3.65 × 10–19 J. What's the wavelength of this photon?A. 727.4 nmB. 481.3 nmC. 851.1 nmD. 544.6 nm 10.2. Calculate the energy of a 730 nm photon.A. 1.88 × 10–19 JB. 5.31 × 10–19 JC. 4.19 × 10–19 JD. 2.72 × 10–19 J
In the energy diagram below: -8.72 x 10-20 -1.36 x 10-19 -2.42 x 10-19 Energy -5.45 x 10-19 J -2.18 x 10-18 ) Has the electron absorbed or emitted a photon and what is the energy change for the electron? Oa. The electron emitted a photon and the change in energy of the electron was - 1.64 x 1018 J. Ob. The electron absorbed a photon and the change in energy of the electron was 1.64 x 10-18 J. c. The electron absorbed a photon and the change in energy of the electron was -1.64 x 10-18 J. Od. The electron emitted a photon and the change in energy of the electron was 1.64 x 1018 J.