Integrated Science
7th Edition
ISBN: 9780077862602
Author: Tillery, Bill W.
Publisher: Mcgraw-hill,
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Chapter 8, Problem 15CQ
To determine
An analysis to prove that Thomson discovered the electron.
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Consider the statement below that could be made based on Thomson’s cathode ray experiment: “All atoms contain extremely small, negatively-charged particles called electrons.” a) This statement can be broken down into three (3) distinct claims about electrons. What are those claims? b) What evidence (observations) from J.J. Thomson’s cathode ray experiment supports each claim?
Using the Bohr formulas, estimate the average distance from the nucleus for an electron in the innermost (n=1) orbit in uranium (Z = 92). What is its kinetic energy and potential energy? Approximately how much energy would be required to remove it?
PLEASE draw the diagram/situation
Iron has a magnetic moment of 2.22 Bohr
magnetons per atom and a density of
7.87-103 kg.m-3. Calculate the expected
magnetization of iron at 0 K and describe any
assumptions that you have made. How would
you expect this magnetization of iron to vary
as temperature is increased. How does the
number of Bohr magnetons per atom change
from 0 K to 300 K. Why does a piece of iron
typically not exhibit high magnetization at
room temperature (unless it has been
"magnetized")?
Chapter 8 Solutions
Integrated Science
Ch. 8.1 - Prob. 1SCCh. 8.1 - Prob. 2SCCh. 8.1 - Prob. 3SCCh. 8.1 - Prob. 4SCCh. 8.1 - Prob. 5SCCh. 8.1 - Prob. 6SCCh. 8.2 - Prob. 7SCCh. 8.2 - Prob. 8SCCh. 8.2 - Prob. 9SCCh. 8.3 - Prob. 10SC
Ch. 8.3 - Prob. 11SCCh. 8.3 - Prob. 12SCCh. 8.5 - Prob. 13SCCh. 8.5 - Prob. 14SCCh. 8 - Prob. 1CQCh. 8 - Prob. 2CQCh. 8 - Prob. 3CQCh. 8 - Prob. 4CQCh. 8 - Prob. 5CQCh. 8 - Prob. 6CQCh. 8 - Prob. 7CQCh. 8 - Prob. 8CQCh. 8 - Prob. 9CQCh. 8 - Prob. 10CQCh. 8 - Prob. 11CQCh. 8 - Prob. 12CQCh. 8 - Prob. 13CQCh. 8 - Prob. 14CQCh. 8 - Prob. 15CQCh. 8 - Prob. 16CQCh. 8 - Prob. 17CQCh. 8 - Prob. 18CQCh. 8 - Prob. 1PEACh. 8 - Prob. 2PEACh. 8 - Prob. 3PEACh. 8 - Prob. 4PEACh. 8 - Prob. 1PEBCh. 8 - Prob. 2PEBCh. 8 - Prob. 3PEBCh. 8 - If the charge-to-mass ratio of a proton is 9.58 ...
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Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, physics and related others by exploring similar questions and additional content below.Similar questions
- Given that 0.750 mol of a particular atom all release an identical photon, resulting in a total energy change of -176.0 kJ. Answer the following: (Hint: n does not equal 1 here) a. What is the wavelength of the photons released? b. What is the frequency of these photons? c. What region of the electromagnetic spectrum is this emitted photon in?arrow_forwardA doubly ionized lithium atom (Li++) is one that has had two of its three electrons removed. The energy levels of the remaining single-electron ion are closely related to those of the hydrogen atom. The nuclear charge for lithium is +3e instead of just +e. How are the energy levels related to those of hydrogen? How is the radius of the ion in the ground level related to that of the hydrogen atom? Explain.arrow_forwardWhich of the following best describes J.J. Thomson's atomic model? Atoms are composed of negatively charged particles embedded within a positively charged sphere. The mass of an atom and its positive charge is located in the center of the atom. The atoms of solid materials are rough, while the atoms of liquids are smooth. All matter is made up of earth, water, fire, and air.arrow_forward
- Explain the structure and fine structure of an atom in stark and zeman field effect in quantum mechanics?Explain in detail?arrow_forwardThe energy levels for a Bohr atom are shown below. Use this diagram to solve problems 7 and 8. 0 eV -2.5 eV -4.0 eV -7.0 eV -12.5 eV 7. What amount of energy is needed for an electron to jump from n = 1 to n = 4? 8. What is the wavelength of the photon needed to make this happen? Is it emission or absorption?arrow_forwardThe first three energy levels of the fictitious element X are as shown.a. What wavelengths are observed in the absorption spectrum of element X? Give your answers in nm.b. State whether each of your wavelengths in part a corresponds to ultraviolet, visible, or infrared light.c. An electron with a speed of 1.4 × 106 m/s collides with an atom of element X. Shortly afterward, the atom emits a 1240 nm photon. What was the electron’s speed after the collision? Assume that, because the atom is so much more massive than the electron, the recoil of the atom is negligible.arrow_forward
- Why didn't Bohr use the concept of de Broglie waves in his theory? Explain. Please Answer my question Im needed Max 30 minutes please.... Thank uarrow_forwardA Thomson-type experiment with relativistic electrons. One of the earliest experiments to show that p = mv (rather than p = mv) was that of Neumann. [G. Neumann, Ann. Physik 45:529 (1914)]. The apparatus shown in Figure P4.5 is identical to Thomsons except that the source of high-speed electrons is a radioactive radium source and the magnetic field B is arranged to act on the electron over its entire trajectory from source to detector. The combined electric and magnetic fields act as a velocity selector, only passing electrons with speed v, where v = V/Bd (Equation 4.6), while in the region where there is only a magnetic field the electron moves in a circle of radius r, with r given by p = Bre. This latter region (E = 0, B = constant) acts as a momentum selector because electrons with larger momenta have paths with larger radii. (a) Show that the radius of the circle described by the electron is given by r = (l2 + y2)/2y. (b) Typical values for the Neumann experiment were d = 2.51 104 m, B = 0.0177 T, and l = 0.0247 m. For V = 1060 V, y, the most critical value, was measured to be 0.0024 0.0005 m. Show that these values disagree with the y value calculated from p = mv but agree with the y value calculated from p = mv within experimental error. (Hint: Find v from Equation 4.6, use mv = Bre or mv = Bre to find r, and use r to find y.) Figure P4.5 The Neumann apparatus.arrow_forwardDiscuss the way in which Thomson’s model is nonphysical. Support your argument with experimental evidence.arrow_forward
- How do the allowed orbits for electrons in atoms differ from the allowed orbits for planets around the sun?arrow_forwardA physicist is watching a 15-kg orangutan at a zoo swing lazily in a tire at the end of a rope. He (the physicist) notices that each oscillation takes 3.00 s and hypothesizes that the energy is quantized. (a) What is the difference in energy in joules between allowed oscillator states? (b) What is the value of n for a state where the energy is 5.00 J? (c) Can the quantization be observed?arrow_forwarda.) Find the frequency in Hertz of radiation with energy of 2.179 x 10-18 J per photon. b.) What frequency of light would be needed to make an electron in a Hydrogen atom jump from n=1 to n=3? c.) A spectral line is measured to have a wavelenght of 1000nm. Is this within the Balmer series?arrow_forward
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