Purchase Solution

Calculating Wavelength of Light that is Absorbed in a Electron Level Transition

Not what you're looking for?

Ask Custom Question

Calculate the wavelength of the light that is absorbed for the electron's transition from n = 5 to n = 6 in Be3+ ion. (ans in nm.)

c:3.00E8 m/s
h:6.63E-34 Js
R:2.18E-18 J

I am not sure is Be Z = 4 or Z = 3.
Could you show me the steps of how you solve this problem please?
Thank you.

Purchase this Solution
Solution Summary

The solution shows step-by-step calculations of wavelength of light absorbed when an electron jumps to a higher atomic shell level.

Solution Preview

Please see attachment for solution.

Solution:

First of all ...

Purchase this Solution
Free BrainMass Quizzes
Match Elements with their Symbols

Elements are provided: choose the matching one- or two-letter symbol for each element.

Thermochemistry

The quiz helps in revising basic concepts about thermochemistry.

Functional groups in Organic Chemistry

You will be tested on the names of functional groups in Organic Chemistry. It is very important to know the functional groups to understand Organic reactions.

Organic Chemistry Naming: Alkanes

This is a quiz which is designed to assist students with learning the nomenclature used to identify organic compounds. This quiz focuses on the organic compounds called Alkanes.

General Chemistry - Classification of Matter

This test will assess your knowledge on the classification of matter which includes elements, compounds and mixtures.

View More Free Quizzes
Related BrainMass Solutions

  • Calculate the wavelength of light that is absorbed in a transition from n=5 to n=6 in Be3+?

    8880 Calculate wavelength of light that is absorbed in a transition from n=5 to n=6 in Be3+? How do you calculate the wavelength of the light that is absorbed for the electron's transition from n=5 to n=6 in Be3+ ion?

  • Atoms, Energy, and the Periodic Table

    A hydrogen atom with an electron in its ground state interacts with a photon of light with a wavelength of 1.22 × 10−6m. Could the electron make a transition from the ground state to a higher energy level?

  • Atomic States

    a) What is the energy of the excited state referred to in the passage? b) What is the wavelength of light corresponding to this transition? --- Please see the attached file.

  • E of Light, Electron Transitions, The Photoelectric Effect

    237899 Energy of Light, Electronic Transitions, The Photoelectric Effect and Quantum Numbers 1. Energy is ____ when an n = 4 to n = 2 transition occurs when an electron adds to the H+ ion and ends up in the n = 3 shell.

  • Electron configuration, orbitals, deBroglie wavelength

    If we did it backwards, we'd only be calculating the wavelength of light required to make the energy change were a photon absorbed.) Since E=hc/wavelength, wavelength=hc/E, where h is Plank's constant and c is the speed of light.

  • Hydrogen Spectrum

    x 1013 Hz Wave length λ = c/υ = 3 x 108/11.4 x 1013 = 2.63 x 10-6 m As the transition is from a lower energy level to a higher energy level, the radiation equal to the energy level difference is absorbed.

  • Wavelength questions

    IF the electron absorbed the photon, it would "jump" from a low level (like n=1) to a high level (like n=10). If the electron went from 10---> 1 it would emit a photon of the same energy.

  • Na atom and configuration

    Using the table, give the energy (in cm-1) and wavelength of absorbed light (in nm) for each transition. From this example you can see that tables such as the one above allow one to predict/explain atomic spectra.

  • Frequency and hydrogen atom transition

    12363 Frequency and hydrogen atom transition Find the frequency of the light that corresponds to a transition in the hydrogen atom from the n=7 state to the n=2 state. The energy of an electron in an atom is negative.

View More Related Solutions