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…

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter4: Introduction To Quantum Mechanics

Section: Chapter Questions

Problem 50AP

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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?
Ozone in the stratosphere absorbs ultraviolet light of wavelengths shorter than 320 nm, thus filtering out the most energetic radiation from sunlight. During this absorption, an ozone molecule absorbs a photon, which breaks an oxygen-oxygen bond, yielding an oxygen molecule and an oxygen atom: O3(g)+hvO2(g)+O(g) (Here, hv denotes a photon.) Suppose a flask of ozone is irradiated with a pulse of UV light of wavelength 275 nm. Assuming that each photon of this pulse that is absorbed breaks up one ozone molecule, calculate the energy absorbed per mole of O2 produced, giving the answer in kJ/mol.
What does it mean to say that the hydrogen atom has discrete energy levels? How is this fact reflected in the radiation that excited hydrogen atoms emit?
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When a tube containing hydrogen atoms is energized by passing several thousand volts of electricity into the tube, the hydrogen emits light than when passed through a prism, resolves into the "bright line" spectrum shown in Fig. 11.10. Why do hydrogen atoms emit bright lines of specific wavelengths rather than a continuous spectrum?
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?
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.
The colors of the visible spectrum and the wavelengths corresponding to the colors are given in Figure 5.2. (a) Which colors of light involve photons with less energy per photon than yellow light? (b) Which color of visible light has photons of greater energy, green or violet? (c) Which color of light has the greater frequency, blue or green?
Give a brief wave description of light. What are two characteristics of light waves?
Light Energy, and the Hydrogen Atom a Which has the greater wavelength, blue light or red light? b How do the frequencies of blue light and red light compare? c How does the energy of blue light compare with that of red light? d Does blue light have a greater speed than red light? e How does the energy of three photons from a blue light source compare with the energy of one photon of blue light from the same source? How does the energy of two photons corresponding to a wavelength of 451 nm (blue light) compare with the energy of three photons corresponding to a wavelength of 704 nm (red light)? f A hydrogen atom with an electron in its ground state interacts with a photon of light with a wavelength of 1.22 106 m. Could the electron make a transition from the ground state to a higher energy level? If it does make a transition, indicate which one. If no transition can occur, explain. g If you have one mole of hydrogen atoms with their electrons in the n = 1 level, what is the minimum number of photons you would need to interact with these atoms in order to have all of their electrons promoted to the n = 3 level? What wavelength of light would you need to perform this experiment?
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.)
6.96 When a helium atom absorbs light at 58.44 nm, an electron is promoted from the 1s orbital to a 2p orbital. Given that the ionization energy of (ground state) helium is 2372 kJ/ mol, find the longest wavelength of light that could eject an electron from the excited state helium atom.

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