Which statement is true regarding Slater's rules and the calculation of effectivenuclear charge?In the calculation of S, the total number of valence electrons should be multiplied by0.35Zeff is greater than Z for all atoms.Core electrons are less effective at shielding valence electrons than are other valenceelectrons.Valence electrons do not contribute at all to the value of S.The value of S (shielding) is greater for the last electron of O than for the last electron ofN.

Slater's rule is used to calculate the effective nuclear charge of an atom

Answered: Which statement is true regarding…

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter2: Atomic Structure And Periodicity

Section: Chapter Questions

Problem 158CWP

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Name and give the symbol of the element that has the characteristic given below. (a) Its electron configuration in the excited state can be 1s22s22p63s1 3p3. (b) It is the least electronegative element in period 3. (c) Its +3 ion has the configuration [36Kr]. (d) It is the halogen with the largest atomic radius. (e) It has the largest ionization energy in Group 16.
The electron affinity of the lutetium atom (element 71) was measured using the technique of photoelectron spectroscopy with an infrared laser (the essay on p. 310 describes this instrumental method, using X rays). In this experiment, a beam of lutetium negative ions, Lu, was prepared and irradiated with a laser beam having a wavelength at 1064 nm. The energy supplied by a photon in this laser beam removes an electron from a negative ion, leaving the neutral atom. The energy needed to remove the electron from the negative ion to give the neutral atom (both in their ground states) is the electron affinity of lutetium. Any excess energy of the photon shows up as kinetic energy of the emitted electron. If the emitted electron in this experiment has a kinetic energy of 0.825 eV, what is the electron affinity of lutetium?
Which of the following ions are unlikely to be found in a chemical compound: Cs+, ln4+, Fe6+, Te2, Sn5+, and I? Explain briefly.
Write electron configurations for the following elements. a. The Group III A element in the same period as 4Be b. The Period 3 element in the same group as 5B c. The lowest-atomic-numbered metal in Group IIA d. The two Period 3 elements that have no unpaired electrons
Write the electron configurations far each of the following elements: (a) Sc. (b) Ti. (c) Cr. (d) Fe. (e) Ru
An ion having a 4+ charge and a mass of 49.9 u has 2 electrons with principal quantum number n = 1.8 electrons with n = 2. and 10 electrons with n = 3. Supply as many of the properties for the ion as possible from the information given. (Hint: In forming ions for this species, the 4j electrons are lost before the 3d elections.) a. the atomic number b. total number of s electrons c. total number of p electrons d. total number of d electrons e. the number of neutrons in the nucleus f. the ground-state electron configuration of the neutral atom
Two elements are in the same group, one following the other. One is a metalloid; the other is a metal. Both form oxides of the formula RO2. The first is acidic; the next is amphoteric. Identify the two elements.

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