Please answer question 11 Part A The human eye contains a molecule called 11-cis-retinal that changes shape when struck with light ofsufficient energy. The change in shape triggers aseries of events that results in an electrical signalbeing sent to the brain that results in vision. Theminimum energy required to change theconformation of 11-cis-retinal within the eye isabout 164 kJ/mol.Part ACalculate the longest wavelength visible to the human eye.Express the wavelength in nanometers to three significant figures.ΑΣφ?nm

From given datas By using energy formula we are calculating longest wavelength visible to human eye…

Answered: The human eye contains a molecule…

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 2QRT

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Give the maximum number of electrons in an atom that can have these quantum numbers: a. n = 4 b. n = 5, ml = + l c. n = 5,ms = +12 d. n = 3, l = 2 e. n = 2, l = 1
Potassium atoms in a flame emit light as they undergo transitions from one energy level to another that is 4.91019J lower in energy. Calculate the wavelength of light emitted and, by referring to Figure 4.3, predict the color visible in the flame.
6.71 Several excited states of the neon atom are important in the operation of a helium-neon laser. In these excited states, one electron of the neon atom is promoted from the 2p level to a higher energy orbital. An excited neon atom with a 1s22s22p55s1 electron configuration can emit a photon with a wavelength of 3391 nm as it makes a transition to a lower energy state with a 1s22s22p54p1 electron configuration. Other transitions are also possible. If an excited neon atom with a 1s22s22p53p1 electron configuration makes a transition to a lower energy state with a 1s22s22p53p1 electron configuration, it emits a photon with a wavelength of 632.8 nm. Find the wavelength of the photon that would be emitted in a transition from the 1s22s22p54p1 electron configuration to the 1s22s22p53p1 electron configuration. (It should help if you start by drawing an energy-level diagram.)
An energy of 3.3 1019 J/atom is required to cause a cesium atom on a metal surface to lose an electron. Calculate the longest possible wavelength of light that can ionize a cesium atom. In what region of the electromagnetic spectrum is that radiation found?
It requires 799 kJ of energy to break one mole of carbon-oxygen double bonds in carbon dioxide. What wavelength of light does this correspond to per bond? Is there any transition in the hydrogen atom that has at least this quantity of energy to one photon?
The root-mean-square speed of an oxygen molecule, O2, at 21C is 479 m/s. Calculate the de Broglie wavelength for an O2 molecule traveling at this speed. How does this wavelength compare with the approximate length of this molecule, which is about 242 pm? (For this comparison, state the wavelength as a percentage of the molecular length.)
One bit of evidence that the quantum mechanical model is correct lies in the magnetic properties of matter. Atoms with unpaired electrons are attracted by magnetic fields and thus are said to exhibit pararamagnetism. The degree to which this effect is observed is directly related to the number of unpaired electrons present in the atom. Consider the ground-state electron configurations for Li, N, Ni, Te, Ba, and Hg. Which of these atoms would be expected to be paramagnetic, and how many unpaired electrons are present in each paramagnetic atom?
Which of the following statements is (are) true? I. The product of wavelength and frequency of light is a constant. II. As the energy of electromagnetic radiation increases, its frequency decreases. III. As the wavelength of light increases, its frequency increases. a I only b II only c III only d I and III only e II and III only
A photon with a wavelength of 93.8 nm strikes a hydrogen atom, and light is emitted by the atom. How many emission lines would be observed? At what wavelengths? Explain briefly (see Figure 6.10).

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