mestions: Quantum Theory, Atomic Structure, and Periodicity e in 26 minutes 9/15 answered HQ7.43 Homework Unanswered Rank the following from highest ionization energy (at top) to lowest ionization energy (at bottom). Drag and drop options into correct order and submit. For keyboard navigation... SHOW MORE V Aluminium Chlorine Sodium Argon Phosphorus Unanswered • 2 attempts left hulu II II II II II

mestions: Quantum Theory, Atomic Structure, and Periodicity e in 26 minutes 9/15 answered HQ7.43 Homework Unanswered Rank the following from highest ionization energy (at top) to lowest ionization energy (at bottom). Drag and drop options into correct order and submit. For keyboard navigation... SHOW MORE V Aluminium Chlorine Sodium Argon Phosphorus Unanswered • 2 attempts left hulu II II II II II

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter5: Electron Configurations And The Periodic Table

Section: Chapter Questions

Problem 139QRT

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Similar questions

Consider the representations of the p and d atomic orbitals in Figs. 2-15 and 2- 17. What do the + and signs indicate?
Spectroscopic studies show that Li can have electrons in its 1s, 2s, and 2p Hartree orbitals, and that Zeff(2s)=1.28 for the 1s22s1 configuration. Estimate the energy of the 2s orbital of Li. Calculate the average distance of the electron from the nucleus in the 2s orbital of Li.
(a) The nitrogen atom has one electron in each of the 2px , 2py , and 2pz orbitals. By using the form of the angular wave functions, show that the total electron density, 2(2px)+2(2py)+2(2pz) , is spherically symmetric (that is, it is independent of the angles and ). The neon atom, which has two electrons in each 2p orbital, is also spherically symmetric. (b) The same result as in part (a) applies to d orbitals, thus a filled or half-filled subshell of d orbitals is spherically symmetric. Identify the spherically symmetric atoms or ions among the following: F , Na, Si, S2,Ar+ , Ni, Cu, Mo, Rh, Sb, W, Au.
Using Table 5.2, write down the mathematical expression for the 2px wave function for an electronically excited H atom. Estimate the probability of finding the 2px electron if you look in a cubical box of volume of 0.8(pm)3 centered at a distance of 0.5001010m in the =/2 , =0 direction. Does this probability change as you change ? At what angles is the probability of finding the electron smallest and at what angles is the probability the largest? (Note that =2 is the same location as =0 , so don’t double count.)
The helium ion He+ is a one-electron system whose wave functions and energy levels are obtained from those for H by changing the atomic number to Z=2 . Calculate the average distance of the electron from the nucleus in the 2s orbital and in the 2p orbital. Compare your results with those in Problem 11 and explain the difference.
When metallic sodium is dissolved in liquid sodium chloride, electrons are released into the liquid. These dissolved electrons absorb light with a wavelength near 800 nm. Suppose we treat the positive ions surrounding an electron crudely as defining a three-dimensional cubic box of edge L, and we assume that the absorbed light excites the electron from its ground state to the first excited state. Calculate the edge length L in this simple model.
Estimate the probability of finding an electron which is excited into the 2s orbital of the H atom, looking in a cubical box of volume 0.751036m3 centered at the nucleus. Then estimate the probability of finding the electron if you move the volume searched to a distance of 105.8 pm from the nucleus in the positive z direction. (Note that since these volumes are small, it does not matter whether the volume searched is cubical or spherical.)
Q.1(a) What were the important advance (s) as a result of which, idea of an electron orbitmovement was swapped by, the notion of probability of finding electron in an orbital?What name was given to the transformed atomic model? Also explain its variouspostulates.(b) Which quantum numbers revel information about the shape, energy, orientation, andsize of the orbitals? How many orbitals are possible for n=4? Which of these may bedescribed as gerade?(c) The signs of the unsquared wave functions are usually shown in plots of the squaredfunctions. Why do you think this practice exists? Give values of angular nodes andplane of 3p, 4d, 2p, 4f, 4s.(d) Predict the trend in values of slater’s constant of the every first element of each groupof p-block elements.
In the experiment shown schematically below, a beam ofneutral atoms is passed through a magnetic field. Atoms thathave unpaired electrons are deflected in different directionsin the magnetic field depending on the value of the electronspin quantum number. In the experiment illustrated,we envision that a beam of hydrogen atoms splits into twobeams. (a) What is the significance of the observation that the single beam splits into two beams? (b) What do you thinkwould happen if the strength of the magnet were increased?(c) What do you think would happen if the beam of hydrogenatoms were replaced with a beam of helium atoms? Why?(d) The relevant experiment was first performed by OttoStern and Walter Gerlach in 1921. They used a beam of Agatoms in the experiment. By considering the electron configurationof a silver atom, explain why the single beam splitsinto two beams.
(a) If the core electrons were totally effective at screeningthe valence electrons and the valence electrons providedno screening for each other, what would be the effectivenuclear charge acting on the 3s and 3p valence electronsin P? (b) Repeat these calculations using Slater’s rules. (c)Detailed calculations indicate that the effective nuclearcharge is 5.6+ for the 3s electrons and 4.9+ for the 3pelectrons. Why are the values for the 3s and 3p electronsdifferent? (d) If you remove a single electron from a P atom,which orbital will it come from?
Use Hund's rules to deduce the term of the lowest level of aTi atom.
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?