[References] Which of the following statements is false? An orbital can accommodate at most two electrons. A 2p orbital is more penetrating than a 2s; i.e., it has a higher electron density near the nucleus and inside the charge cloud of a Is orbital. In the usual order of filling, the 6s orbital is filled before the 4f orbital. The spin quantum number of an electron must be either +% or -%: The electron density at a point is proportional to y at that point. Submit Answer Try Another Version 5 item attempts remaining

[References] Which of the following statements is false? An orbital can accommodate at most two electrons. A 2p orbital is more penetrating than a 2s; i.e., it has a higher electron density near the nucleus and inside the charge cloud of a Is orbital. In the usual order of filling, the 6s orbital is filled before the 4f orbital. The spin quantum number of an electron must be either +% or -%: The electron density at a point is proportional to y at that point. Submit Answer Try Another Version 5 item attempts remaining

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 30QAP: Consider the following representation of a set of p orbitals for an atom: mg...

See similar textbooks

Similar questions

What does wave-particle duality mean? What are its implications in our modem view of atomic structure?
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?
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.
Using vertical lines, indicate the transitions from Exercise 58 on an energy-level diagram for the hydrogen atom (see Fig. 2-9).
Consider the representations of the p and d atomic orbitals in Figs. 2-15 and 2- 17. What do the + and signs indicate?
Tbe relative orbital levels for the hydrogen atom can be represented as Draw the relative orbital energy levels for atoms with more than one electron and explain your answer. Also explain bow the following radial probability distributions support your answer.
Identify the element that corresponds to each of the simplified photoelectron spectral data given below. (Energy data taken from D. A. Shirley, R. L Martin, S. P. Kowalczyk. F. R. McFeely, and L. Ley: Core-electron binding energies of the first thirty elements, Physical Review B, Vol. 15, pp. 544-552, 1977.) (a) There are peaks at energies of 64.8 and 5.4 eV, corresponding to 2 and 1 electrons, respectively. (b) There are peaks at energies of 3614, 384, 301, 40.9, 24.7, and 4.34 eV, corresponding to 2, 2, 6, 2, 6, and 1 electrons, respectively. (c) There are peaks at energies of 4494, 503, 404, 56.4, 33.6, 8.01, and 6.65 eV, corresponding to 2, 2, 6, 2, 6, 1, and 2 electrons, respectively.
How far from the nucleus in angstroms (1 angstrom =11010 m) is the electron in a hydrogen atom if it has an energy of 8.721020 J?
Answer the following questions. (a) What characteristic of an atomic orbital does the quantum number ms describe? (b) Does a photon with a frequency of 35.8 Hz have more or less energy than one with a frequency of 125 Hz? (c) How many orbitals can be associated with the following set of quantum numbers:n=3, l=2? (d) Is a sample of ZnCl2 containing the Zn2+ ion diamagnetic?
Consider the orbitals shown here in outline. (a) What is the maximum number of electrons contained in an orbital of type (x)? Of type (y)? Of type (z)? (b) How many orbitals of type (x) are found in a shell with n=2? How many of type (y)? How many of type (z)? (c) Write a set of quantum numbers for an electron in an orbital of type (x) in a shell with n=4, of an orbital of type (y) in a shell with n=2. Of an orbital of type (z) in a shell with n=3. (d) What is the smallest possible n value for an orbital of type (x)? Of type (y)? Of type (z)? (e) What are the possible I and ml values for an orbital of type (x)? Of type (y)? Of type (z)?
State which of the following orbitals cannot exist according to the quantum theory: 2s, 2d, 3p, 3f, 4f, and 5s. Briefly explain your answers.
Sketch a picture of the 90% boundary surface of an s orbital and the px orbital. Be sure the latter drawing shows why the p orbital is labeled px and not py, for example.