Give the noble gas shortened electron configuration for Ga]44Give the noble gas shortened electron configuration for the only Ga ion, Ga*3Remember that ion formation usually results in completely full or completely empty subshells.[]434а. Неb. NeС. Ard. Krе. Хеf. Rng. Uuoh. s°i. s'j. s2k. s3I. p°m. p'n. p2o. p3р. р4q. p5r. p6S. dºt. d'u. d2V. d3w. d4X. d5z. d7ii. j. f6 kk. f7 II. f3 mm. f° nn. f10 oo. f11y. d6aa. d bb. dºСС. d10dd. fº ee. flff. f2gg. fhh. f4pp. f1299. f13rr. f14

Answered: Give the noble gas shortened electron…

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter8: The Periodic Table: Structure And Trends

Section: Chapter Questions

Problem 8.90QE

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Similar questions

The outermost electron in an alkali-metal atom is sometimes described as resembling an electron in the corresponding state of a one-electron atom. Compare the first ionization energy of lithium with the binding energy of a 2s electron in a one-electron atom that has nuclear charge Zeff , and determine the value of Zeff that is necessary for the two energies to agree. Repeat the calculation for the 3s electron of sodium and the 4s electron of potassium.
Using the periodic table and without looking at Table 7.3, write electron configurations for the following elements: (a) P (b) Zn (c) Zr (d) In (e) Pb (f) U Use the spdf and noble gas notations. When you have finished, check your answers with Table 7.3.
Answer the following questions, assuming that ms, could have three values rather than two and that the rules for n, l, and ml are the normal ones. a. How many electrons would an orbital be able to hold? b. How many elements would the first and second periods in the periodic table contain? c. How many elements would be contained in the first transition metal series? d. How many electrons would the set of 4f orbitals be able to bold?
Consider the representations of the p and d atomic orbitals in Figs. 2-15 and 2- 17. What do the + and signs indicate?
State which of the following orbitals cannot exist according to the quantum theory: 2s, 2d, 3p, 3f, 4f, and 5s. Briefly explain your answers.
The work function is the energy required to remove an electron from an atom on the surface of a metal. How does this definition differ from that for ionization energy?
Answer the questions below concerning ground state electron configurations. (a) What element has the electron configuration [Ar]3d64s2? (b) What element has a 2+ ion with the configuration [Ar]3d5? Is the ion paramagnetic or diamagnetic? (c) Mow many unpaired electrons are in a Ni2+ ion? (d) The configuration for an element is given here. What is the identity of the element? Is a sample of the element paramagnetic or diamagnetic? How many unpaired electrons does a 3 ion of this element have? (e) What element has the following electron configuration? Write a complete set of quantum numbers for electrons 1-3.
Consider the following representation of a set of p orbitals for an atom: mg src=Images/HTML_99425-11-30QAP_image001.jpg alt="" align="top"/> ich of the following statements is(are) true? The areas represented by the p orbitals are positively charged clouds with negatively charged electrons embedded within these clouds. The nucleus is located at the center point of each axis. The electrons move along the elliptical paths as indicated by the p orbitals above. The atom could not be hydrogen because its electron is found in the 1s orbital.
Section 11.6 uses a "firefly" analogy to illustrate how the wave mechanical modal for the atom differs from Bohr’s. model. Explain this analogy.
The first ionization energies of As and Se are 0.947 and 0.941 MJ/mol, respectively. Rationalize these values in terms of electron configurations.
The ionization of the hydrogen atom can be calculated from Bohr's equation for the electron energy. E = (NARhc)(Z2/n2) where NARhc =1312 kJ/mol and Z is the atomic number. Let us use this approach to calculate a possible ionization energy for helium. First, assume the electrons of the He experience the full 2+ nuclear charge. This gives us the upper limit for the ionization energy. Next, assume one electron of He completely screens the nuclear charge from the other electrons, so Z = 1. This gives us a lower limit to the ionization energy. Compare these calculated values for the upper and lower limits to the experimental value of 2372.3 kJ/mol. What does this tell us about the ability of one electron to screen the nuclear charge?
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?

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