Name for each of the three (3) Atomic Models in the cartoon below: ➤ Who discovered/developed the model and when? Name the main statement/characteristic of the model. ➤What are the assumptions the model is based on and what are the model's limitations? History of Atomic Models: Nucleus (1) Electrons i Late 1800s Electrons Energy Levels 1913 Negatively Charged Cloud 1920s

Name for each of the three (3) Atomic Models in the cartoon below: ➤ Who discovered/developed the model and when? Name the main statement/characteristic of the model. ➤What are the assumptions the model is based on and what are the model's limitations? History of Atomic Models: Nucleus (1) Electrons i Late 1800s Electrons Energy Levels 1913 Negatively Charged Cloud 1920s

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter4: Chemical Foundations: Elements, Atoms, And Ions

Section: Chapter Questions

Problem 25QAP: Do the proton and the neutron have exactly the same mass? How do the masses of the proton and the...

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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.
It is good practice to actively read the textbook and to try to verify claims that are made when you can. The following claim is made in your textbook: “. . . if the nucleus were the size of a grape, the electrons would be about 1 mile away on average.” Provide mathematical support for this statement.
Do the proton and the neutron have exactly the same mass? How do the masses of the proton and the neutron compare to the mass of the electron? Which particles make the greatest contribution W the mass of an atom? Which particles make the greatest contribution to the chemical properties of an atom?
How many Ag atoms are present in a piece of pure silver jewelry weighing 21.3 g?
How would you expect the chemical properties of isotopes of the same element to compare to each other? Explain your answer.
For each of the isotopes in Exercise 21.1, determine the numbers of protons, neutrons, and electrons in a neutral atom of the isotope.
The existence of isotopes violates one of the original ideas of Dalton’s atomic theory. Which one?
What advantage does the atomic mass unit have over grams when speaking of the mass of an atom or a subatomic particle?
Slaters rules are a way to estimate the effective nuclear charge experienced by an electron. In this approach, the shielding constant, S, is calculated. The effective nuclear charge is then the difference between S and the atomic number, Z. (Note that the results in Table 7.2 and Figure 7.2 were calculated in a slightly different way.) Z = Z S The shielding constant, S, is calculated using the following rules: (1) The electrons of an atom are grouped as follows: (1s) (2s, 2p) (3s, 3p) (3d) (4s, 4p) (4d), and so on. (2) Electrons in higher groups (to the right) do not shield those in the lower groups. (3) For ns and np valence electrons a) Electrons in the same ns, np group contribute 0.35 (for 1s 0.30 works better). b) Electrons in n 1 groups contribute 0.85. c) Electrons in n 2 groups (and lower) contribute 1.00. (4) For nd and nf electrons, electrons in the same nd or nf group contribute 0.35, and those in groups to the left contribute 1.00. As an example, let us calculate Z for the outermost electron of oxygen: S = (2 0.85) + (5 0.35) = 3.45 Z = 8 3.45 = 4.55 Here is a calculation for a d electron in Ni: Z = 28 [18 1.00] [7 0.35] = 7.55 and for an s electron in Ni: Z = 28 [10 1.00] [16 0.85] [1 0.35] = 4.05 (Here 3s, 3p, and 3d electrons are in the (n 1) groups.) a) Calculate Z for F and Ne. Relate the Z values for O, F, and Ne to their relative atomic radii and ionization energies. b) Calculate Z for one of the 3d electrons of Mn, and compare this with Z for one of the 4s electrons of the element. Do the Z values give us some insight into the ionization of Mn to give the cation?