COLUMN A 6. Atomic model proposed by J.J. Thomso 7. Atomic theory that describes atom as a solid, indestructible sphere with a mass 8. Negative-charged particles in an atom 9. Neutral-charged particles in an atom 10. Positive-charged particles in an atom 11. Proponent of Electron Cloud model 12. Region around the nucleus of an atom with the greatest probability of finding electrons 13. Shorthand representation of how each electron is arranged among the orbitals, levels, and sublevels based on the stated principles. 14. Theory describing atom having positively charged nucleus and negatively-charged particles circulates around it 15. This atomic model says that electrons orbit the nucleus in orbits that have a specific size and energy. COLUMN B A. Electron configuration B. Electrons C. Erwin Schrodinger D. John Dalton E. Neutrons F. Nuclear Model of an Atom G. Orbitals H. Planetary Model of Atom I. Plum-pudding Model of Atom J. Protons K. Solid Sphere Model

COLUMN A 6. Atomic model proposed by J.J. Thomso 7. Atomic theory that describes atom as a solid, indestructible sphere with a mass 8. Negative-charged particles in an atom 9. Neutral-charged particles in an atom 10. Positive-charged particles in an atom 11. Proponent of Electron Cloud model 12. Region around the nucleus of an atom with the greatest probability of finding electrons 13. Shorthand representation of how each electron is arranged among the orbitals, levels, and sublevels based on the stated principles. 14. Theory describing atom having positively charged nucleus and negatively-charged particles circulates around it 15. This atomic model says that electrons orbit the nucleus in orbits that have a specific size and energy. COLUMN B A. Electron configuration B. Electrons C. Erwin Schrodinger D. John Dalton E. Neutrons F. Nuclear Model of an Atom G. Orbitals H. Planetary Model of Atom I. Plum-pudding Model of Atom J. Protons K. Solid Sphere Model

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter11: Modern Atomic Theory

Section: Chapter Questions

Problem 102AP

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What is meant by anuclear atom? Describe the points of Ruth erford’s model for the nuclear atom and how he tested this model. Based on his experiments, how did Rutherford envision the structure of the atom? How did Rutherford’s model of the atom’s structure differ from Kelvin’s “plum pudding” model?
How are the Bohr model and the Rutherford model of the atom similar? How are they different?
Predict and test the behavior of a particles fired at a plum pudding model atom. Predict the paths taken by a particles that are fired at atoms with a Thomson’s plum pudding model structure. Explain why you expect the particles to take these paths. If a particles of higher energy than those in (a) are fired at plum pudding atoms, predict how their paths will differ from the lower-energy a particle paths. Explain your reasoning. Now test your predictions from (a) and (b). Open the Rutherford Scattering simulation (http://openstaxcollege.org/I/16PhetScatter) and select the Plum Pudding Atom tab. Set Alpha Particles Energy to mm, and select show traces. Click on the gun to start firing a particles. Does this match your prediction from (a)? If not, explain why the actual path would be that shown in the simulation. Hit the pause button, or Reset All. Set Alpha Particles Energy to max, and start firing a particles. Does this match your prediction from (b)? If not, explain the effect of increased energy on the actual paths as shown in the simulation.
How does probability fit into the description of the atom?
Defend and criticize Bohrs model. Why was it reasonable that such a model was proposed, and what evidence was there that it "works"? Why do we no longer "believe" in it?
How are the Bohr model and the quantum mechanical model of the hydrogen atom similar? How are they different?
Characterize the Bohr model of the atom. In the Bohr model, what do we mean when we say something is quantized? How does the Bohr model of the hydrogen atom explain the hydrogen emission spectrum? Why is the Bohr model fundamentally incorrect?
Are mathematical expressions for the following potential energies positive or negative? Explain why in each case. a The attraction between an electron and a helium nucleus b The repulsion between two protons in a nucleus c The attraction between a north and a south magnetic pole d The force of gravity between the Sun and Earth e A rock perched on the edge of a cliff with respect to the base of the cliff
How can we account for the fact that most of the alpha particles in the Rutherford scattering experiment passed directly through a solid sheet of gold?
One of the best indications of a useful theory is that it raises more questions for further experimentation than it originally answered. Does this apply to Daltons atomic theory? Give examples.
Give electron configurations according to the Bohr model for each of the following elements. Try to not use Figure 3.11, but instead determine the configuration based on your knowledge of the number of electrons in each atom and the maximum number of electrons in each Bohr orbit. Indicate which of these elements you expect to be the most reactive and the least reactive. a. B b. Si c. Ca d. F e. Ar
In J. J. Thompson’s experiment depicted in Figures 1.10 and 1.11, assume that the electrons are initially traveling at a speed of 8.00106ms1 in the +x direction and the electrostatic plates have a length of l=0.10m , between which the electrons are deflected toward the -y direction (downward) by an electric field of magnitude 200Vm1 . (Note that 1volt=1V=1JC1 .) Calculate S, the magnitude of the downward displacement, if the fluorescent screen is located 0.90 m beyond the exit of the region between the two electrostatic plates. No magnetic field is applied to counteract the electrostatic force. (Caution: L is not 1.0 m nor 0.9 m; see Figure 1.11.)