Answered: Calculate the energy change when an…

Calculate the energy change when an electron moves from energy level 4 to energy level 1 in the hydrogen atom. 3.49 × 10-17 -2.04 x 10-18 2.04 x 10-18 -1.63 x 10-18 1.36 × 10-19

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 5.CCP

See similar textbooks

Similar questions

The electron configuration of the isotope 16O is 1s22s22p4. What is the electron configuration of the isotope 18O?
Of the five elements Sn, Si, Sb, O, Te, which has the most endothermic reaction? (E represents an atom.) What name is given to the energy for the reaction? E(g)E+(g)+e
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
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.
A hydrogen atom absorbs a photon of ultraviolet light, exciting an electron from energy level 1 to energy electron drops back down in three steps, as shown. Using the table, identify the energy released in each tr visible, or infrared. 7 Transition from 7→5: 6. E = 4.23 x 10-20 J 2 = 4,668 nm 4 Transition from 5→ 2: E = 4.58 × 10-19 J 1 = 434 nm 2 Transition from 2→ 1: E = 1.63 x 10-18 J 1 = 122 nm Transition Wavelength Region 7 → 5 4,668 nm 5 → 2 434 nm 2 → 1 122 nm Answer Bank ultraviolet infrared visible Energy
need it fast!! In a hydrogen atom, an electron loses energy from n = 5 to n = 2, a process that leads to some kind of “interaction” with electromagnetic radiation. What is the wavelength of this light in nanometers? Do NOT include a sign with this answer. Rydberg's constant is equal to -2.179 x 10-18 J. Planck's constant is equal to 6.626 x 10-34 Joule-seconds. The speed of light is 3.00 x 108 meters per second. Express exponents as number followed by E followed by the power (e.g., 7.34E-12).
Which of the following reactions represents an electron gain energy that would be positive (i.e. endothermic). S(g) → S+(g) + e- Cl(g) → Cl+(g) + e- Kr(g) + e- → Kr-(g) S(g) + e- → S-(g) Kr(g) → Kr+(g)+ e- Cl(g) + e- →Cl-(g)
Consider the following approximate visible light spectrum: (insert image) Barium emits light in the visible region of the spectrum. If each photon of light emitted from barium has an energy of 3.59 x 10^-19 J, what color of visible light is emitted?
need it fast! In a hydrogen atom, an electron loses energy from n = 5 to n = 2, a process that leads to some kind of “interaction” with electromagnetic radiation. What is the frequency of this light in Hertz? Do NOT include a sign with this answer. Rydberg's constant is equal to -2.179 x 10-18 J. Planck's constant is equal to 6.626 x 10-34 Joule-seconds. Express exponents as number followed by E followed by the power (e.g., 7.34E-12).
When a red light with a wavelength of 670 nm shines on a piece of metal, an electron is ejected. What is the energy of the photon absorbed by the electron to overcome the attractive forces? O 4.7 x 10-35 J O 4.3 x 10-37 J O O O 3.3 x 10-¹⁹J 3.0 x 10-¹9 J 2.9 x 10-37 J
Answer question 9 and please make it short and let your handwriting clear
This energy diagram shows the allowed energy levels of an electron in a certain atom. (Note: the SI prefix 'zepto' means 10-21. You can find the meaning of any SI prefix in the ALEKS Data tab.) energy (zJ) 1400 1200 1000 800 600 400 200 0 I B -A Use this diagram to complete the table below. What is the energy of the electron in the ground state? What is the energy of the electron in the first excited state? If the electron makes the transition shown by the red arrow, from A to C, will a photon be absorbed or emitted? Calculate the wavelength of the photon that would be absorbed or emitted. Round your answer to 3 significant digits. 250 ZJ 400 ZJ absorbed emitted nm x10 X S