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6. What is the frequency of a light source that has a wavelength of 620 nm? What is the energy this wave? of

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter7: Atomic Structure And Periodicity

Section: Chapter Questions

Problem 9RQ

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Concept explainers

Quantum Chemistry

Quantum chemistry deals with the properties of chemical systems and their reactions. The branch of chemistry which is more concerned with quantum chemistry is physical chemistry. It is a more sophisticated field of theoretical physics which is concerned towards the application of physical concepts towards various chemical aspects such as, formation of atoms, chemical structure descriptions, chemical bond strength, hybridization, conjugation etc. Quantum chemistry mainly studies the various states i.e., ground state, excited state, transition states of the individual atoms or molecules taking place during any chemical reaction. The laws of motion explained by various scientists, which are termed as “classical mechanics” were not acceptable in terms of electrons, protons, atoms, light etc. Thus, a new theory named “quantum mechanics” emerged to understand the basic framework of various atomic and subatomic particles.

Question

Number 6 please

5. A new element, element Jn, is discovered on a separate planet. The energy requires to ionize one
mole of Jn atoms is about 4750 kJ/mol. What is the frequency of light necessary to ionize one atom of
this element?
6. What is the frequency of a light source that has a wavelength of 620 nm? What is the energy of
this wave?
7. Find the frequency of flasher that has a wavelength of 476 nm. What is the energy of a photon in
this light?
8. A Chlorine atom has a first ionization energy of 1251.2 kJ/mol. Light of what frequency is required
to ionize one mole of chlorine atoms?

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r Questions 11—13, you will need to consider ionizations beyond the first ionization energy. For example, the second ionization energy is the energy to remove a second electron from an element. Compare the first ionization energy of helium to its second ionization energy, remembering that both electrons come from the 1s orbital. l> X Y First 170 200 second 350 400 Third 1800 3500 fouth 2500 5000 entify the elements X and Y. There may be more than one answer. so explain completely.
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?
A metallic element reacts vigorously with water, evolving hydrogen gas. An excited atom of this element has its outer electron in the 3p orbital. When this electron drops to its ground state in the 3s orbital, light is emitted of wavelength 589 nm What is the identity of the element? Explain how you arrived at your answer. What is the color of the emitted light?
On which quantum numbers does the energy of an electron depend in each of the following? a. a one-electron atom or ion b. an atom or ion with more than one electron
Consider the eight most abundant elements in the human body, as outlined in Exercise 156. Excluding hydrogen, which of these elements would have the smallest size? largest size? smallest first ionization energy? largest first ionization energy?
It takes 7.21 1019 J of energy to remove an electron from an iron atom. What is the maximum wavelength of light that can do this?
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?
Photogray lenses incorporate small amounts of silver chloride in the glass of the lens. When light hits the AgCl particles, me following reaction occurs: AgClhvAg+Cl The silver metal that is formed causes the lenses to darken. The energy change for this reaction is 3.10 102 kJ/mol. Assuming all this energy must be supplied by light, what is the maximum wavelength of light that can cause this reaction?
From what you know in a general way about electron affinities, state which member of each of the following pairs has the greater value: a As, Br b F, Li.
Describe briefly why the study of electromagnetic radiation has been important to our understanding of the arrangement of electrons in atoms.
Which atom would be expected to have a half-filled 6p subshell?
The following shapes each represent an orbital of an atom in a hypothetical universe. The small circle is the location of the nucleus in each orbital. a If you placed an electron in each orbital, which one would be higher in energy? b When an electron makes a transition from the orbital represented on the right to the orbital on the left, would you expect energy to be absorbed or released? c Draw a sketch of an orbital of the same type that would be higher in energy than either of the two pictured orbitals.

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