Question 1920 ptsHarry Moseley's discovered that an element's dominant X-ray spectral lines increase regularly and validates thearrangement and organization of the periodic table. Another implication of this discovery at that time was that there is aconnection betweenO an element's atomic number and its number of protonsO an element's properties and its atomic weightO an element's atomic number and its atomic weightO an element's radioactivity and its number of electronsNext ▸

The correct answer to the question based on Harry Moseley's discovery is "an element's atomic number…

Answered: Question 19 20 pts Harry Moseley's…

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter2: Atoms Molecules And Ions

Section: Chapter Questions

Problem 29PS

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2.42 What is a period in the periodic table? From what does it derive its name?
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?
2.87 What is the heaviest element to have an atomic weight that is roughly twice its atomic number? What does this suggest must he true about the nuclei of atoms with higher atomic numbers?
How does Daltons atomic theory account for the Law of Conservation of Mass?
Where are neutrons found in an atom? Are neutrons positively charged, negatively charged, or electrically uncharged?
2-102 An element consists of 90.51% of an isotope with a mass of 19.992 amu, 0.27% of an isotope with a mass of 20.994 amu, and 9.22% of an isotope with a mass of 21.990 amu. Calculate the average atomic mass and identify the element.
2-29 How many protons and how many neutrons does each of these isotopes of radon contain? (a) Rn-210 (b) Rn-218 (c) Rn-222
How many protons and neutrons are contained in the nucleus of each of the following atoms? For an atom of the element, how many electrons are present? a.2963Cu b.3580Br c.1224Mg
How many electrons, protons, and neutrons are found in isolated atoms having the following atomic symbols? a.817Oe.24He b.92235Uc.50119Sn c.1737Clg.54119Xe d.13Hh.3064Zn
Which of the following are isotopes of element X, the atomic number for which is 9: 919X, 920X, 189X, and 921X?
What refinements had to be made in Daltons atomic theory to account for Gay-Lussacs results on the combining volumes of gases?

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