This energy diagram shows the allowed energy levels of an electron in a certain atom. (Note: the SI prefix 'zepto' means 10 can find the meaning of any SI prefix in the ALEKS Data tab.) -21 energy (z]) 1400- 1200 1000- 800- 600 400- 200- 0 C B E A Use this diagram to complete the table below. If the electron makes the transition shown by the red arrow, from A to C, calculate the wavelength of the photon that would be absorbed or emitted. Round your answer to 3 significant digits. nm X Yo

This energy diagram shows the allowed energy levels of an electron in a certain atom. (Note: the SI prefix 'zepto' means 10 can find the meaning of any SI prefix in the ALEKS Data tab.) -21 energy (z]) 1400- 1200 1000- 800- 600 400- 200- 0 C B E A Use this diagram to complete the table below. If the electron makes the transition shown by the red arrow, from A to C, calculate the wavelength of the photon that would be absorbed or emitted. Round your answer to 3 significant digits. nm X Yo

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Excited H atoms have many emission lines. One series of lines, called the Brackett series, occurs in the infrared region. It results when an electron changes from higher energy levels to a level with n = 4. Calculate the wavelength and frequency of the lowest energy line of this series. Wavelength Frequency = = S m -1
nt BACK PRINTER VERSION FULL SCREEN CALCULATOR SPECTROSCOPY AND REACTIVITY TO4/S06 The energy levels the electron can occupy in the Bet ion can be calculated using the energy level equation. A Be emitted a photon with a frequency of 9.86 x 105 Hz. What is the value of the level n for the new energy? ion with an electron in the n 4.00 level Speed of Light c 3.00x108 m/s Planck's Constant h 6.63x1034 J S Rydberg's Constant RH=2.18x1o-18J Avogadro's No. NA 6.02x1023mol1 Energy Level Eqn En(J)-RH(Z2/n2) Z=nuclear charge =quantum number exact number, no tolerance
Aktiv Chemistry M Gmail C What is the waveleng X app.101edu.co Aktiv Chemistry Bb Courses - Blackb.... Spotify - Advertis 4 X Orbitals S An electron changes 1 X Question 11 of 27 What is the energy (in J) of a photon required to excite an electron from n = 2 to n = 8 in a He* ion? Submit an answer to three significant figures. G
How many electrons can the subshell with n = 5 and ℓ = 3 accommodate? [The answer is a whole number.] *
Two pls
If photons have a frequency of 1.203x1015 s", what wavelength, in nm, does this correspond to? Note: Do not use scientific notation or units in your response. Sig figs will not be graded in this question, enter your response to four decimal places. Carmen may add or remove digits from your response, your submission will still be graded correctly if this happens.
The following is a diagram of energy states and transitions in the hydrogen atom. T ENERGY -A B C D E R: Infinity n=3 n = 2 n=1 Match each of the responses below with the correct arrow from the figure. 1. The emission line with the longest wavelength. 2. The absorption line with the longest wavelength. 3. The emission line with the lowest energy. 4. The absorption line with the lowest energy. 5. The emission line with the lowest frequency. 6. The line corresponding to the ionization energy of hydrogen.
The minimum frequency of light needed to eject electrons from a metal is called the threshold frequency, vo. Find the minimum energy needed to eject electrons from a metal with a threshold frequency of 3.09 x 1014 s-. Eo = J With what maximum kinetic energy will electrons be ejected when this metal is exposed to light with a wavelength of 285 nm? KEelectron J %3D 1 A étv W MacBook Air 80 DO0 D00 DI DD F3 F4 F5 F6 F7 F8 F9 F10 F11 F12 %24 & 25
Complete this chart. I (numeral) 1 3 4 I (letter) What n values are impossible for this value of l? What m¡ values are possible for this value of l? Total number of nl orbitals for this value of I and any possible value of n? Lightest element to use orbitals with this H В I value in the ground state. Lightest element to use orbitals with this I value in an excited state.
Part A: Redand greenlight have wavelengths of about 650 nm and 490 nm, respectively. Which light, red or green, has the higher frequency (must show with calculations)? Part B: Which light has the highest energy (again, must show with calculations)?
In a discharge tube, neon atoms emit light as they undergo transitions from one energy level to another that is 3.396*10-19 J lower in energy. Calculate the wavelength of the light emitted and by referring to the figure to the right, predict the color of the line in the discharge spectrum. Wavelength = ------m color --------.
List these electron subshells in order of increasing energy. 4d, 5s, 6s, 5p Note for advanced students: you may assume these subshells are all in an atom with many electrons, not a hydrogen atom. 0 X 0,0,... Ś