10.) Hurlimann Universe Problem: Suppose the quantum rules allowed m, 0 in addition to m, -t.. (a) Draw a periodic table for this system (H→ Zn). (b) According to your table, which elements would be inert? Why? (c) What would be the formulas for compounds formed between the following elements. Explain. (1) Na and Cl (2) Al and S

10.) Hurlimann Universe Problem: Suppose the quantum rules allowed m, 0 in addition to m, -t.. (a) Draw a periodic table for this system (H→ Zn). (b) According to your table, which elements would be inert? Why? (c) What would be the formulas for compounds formed between the following elements. Explain. (1) Na and Cl (2) Al and S

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter5: Quantum Mechanics And Atomic Structure

Section: Chapter Questions

Problem 26P: Suppose that the spin quantum number had three allowed values (ms=0,+12,12) . Give the atomic...

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QUESTION 3 (a) Look very carefully at the pictures below: Picture 1 and Picture 2. What does each of the pictures represent? Give FULL EXPLANATIONS for your answer. (1) (2) (b) Look very carefully at the picture below. Give the relevant quantum numbers. Explain your answer. у-аxis (c) (i) What is a wavefunction? (ii) What are the two parts of a wavefunction? (iii) What is the importance of squaring a wavefunction? (iv) Where is a wavefunction obtained from? 4
An atom contains 2 electrons in shell having principal quantum number=1, 8 electronsin shell having principal quantum number=2 and 8 electrons in shell having principalquantum number=3. Determine its (a) symbol and electronic configuration (b) totalnumber of s and p orbitals (c) calculate and draw total number of angular nodes in eachorbitals.(c) If we replace the hydrogen atoms in ammonia with the ethyl moieties (C2H5)3— N),there is no change in the hybridization of central oxygen atom, yet they have differentbond angles, Why? Which molecule has lower bond angle? Give reasons to supportyour answer.(d) What is the simplest justifications for believing that molecular structure is more oftengoverned by BP-BP/BP-LP/LP-LP repulsions than by the van der Walls repulsions ofthe nonbonding electrons on the substituent atoms?
What is the ionization energy (J) of an electron from the n=8 stationary in the hydrogen atom (answer in 3 sig figs)
14. The picture below shows a cross-section of the electron density of an orbital (dark areas represent electron density). a) Which orbital is represented? Identify the features that allow you to identify the orbital unambiguously. (2) b) In the coordinate system to the right, qualitatively draw the corresponding radial wave function. (3) intensity of wave function distance r from nucleus
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QUESTION 3 (a) Look very carefully at the pictures below: Picture 1 and Picture 2. What does each of the pictures represent? Give FULL EXPLANATIONS for your answer. (1) (2) (b) Look very carefully at the picture below. Give the relevant quantum numbers. Explain your answer. у-аxis (c) (1) What is a wavefunction? (ii) What are the two parts of a wavefunction? (ii) What is the importance of squaring a wavefunction? (iv) Where is a wavefunction obtained from? 4
The ground-state electron configuration of calcium is (a) 1s22s22p63s2 (b) 1s22s22p63s23p64s2 (c) 1s22s22p63s2 (d) [Ne]4s2
(1)Draw a ground state energy level diagram for a silicon atom that shows where all of the electrons would be (n, L, ml and show spin up or spin down with an arrow). (2) Determine the values of L and S for the ground state using Hund's rule. (3) For chlorine, repeat steps 1 and 2.
Two possible electron configurationsfor an Li atom are shown here. (a) Doeseither configuration violate the Pauliexclusion principle? (b) Does eitherconfiguration violate Hund’s rule? (c)In the absence of an external magneticfield, can we say that one electron configurationhas a lower energy than theother? If so, which one has the lowestenergy?
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1.45 (a) Sketch the shape of the boundary surfaces corresponding 1s- 2p-, and 3d-orbitals. (b) What is meant by a node? (c) How many radial nodes and angular nodal surfaces does each orbital have? (d) Predict the number of nodal planes expected for a 4f-orbital.
Use the figure below to answer the following: a) Determine the energy difference between the 6s and 5p states, as well as the energy difference between the 4d and 5p states and between the 6s and 4d states. (b) The transitions from (4d to 5p) and (4d to 5s) are allowed, respectively. Why? (c) What are the four selection rules, including the four atomic quantum numbers, in general for an electronic transition involving the emission or absorption of a photon for an atom? (d) What are the energies of the 5p, 6s, and 4d levels now that it is known that the 4s level is really at -4.34 eV rather than 0 eV? -In the following Figure. Potassium transitions with wavelength labels in A' (angstrom). The ground state has been skewed to read zero eV, as you can see. Actually, the ground state is at -4.34 eV.