The contour representation zof one of the orbitals for then = 3 shell of a hydrogen atomis shown here. (a) What is thequantum number l for thisorbital? (b) How do we label thisorbital? (c) In which of the followingways would you modifythis sketch if the value of themagnetic quantum number, ml,were to change? (i) It would bedrawn larger, (ii) the number of lobes would change, (iii) thelobes of the orbital would point in a different direction, (iv)there would be no change in the sketch. [Section 6.6]

The contour representation zof one of the orbitals for then = 3 shell of a hydrogen atomis shown here. (a) What is thequantum number l for thisorbital? (b) How do we label thisorbital? (c) In which of the followingways would you modifythis sketch if the value of themagnetic quantum number, ml,were to change? (i) It would bedrawn larger, (ii) the number of lobes would change, (iii) thelobes of the orbital would point in a different direction, (iv)there would be no change in the sketch. [Section 6.6]

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 5P: Estimate the probability of finding an electron which is excited into the 2s orbital of the H atom,...

See similar textbooks

Similar questions

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.)
For the Li atom, the energy difference between the ground state and the first excited state, in which the outermost electron is in a 2p orbital, is 2.961019J . In the Li2+ ion, the energy difference between the 2s and 2p levels is less than 0.00002 of this value. Explain this observation.
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.
Which of the following sets of quantum numbers refers to a 4porbital?
If the transition of an electron fromthe n = 3 state to the n = 2 stateresults in emission of visible light, isthe transition from the n = 2 stateto the n = 1 state more likely toresult in the emission of infrared orultraviolet radiation?
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.
The accompanying drawingshows a contour plot for a dyzorbital. Consider the quantumnumbers that could potentiallycorrespond to this orbital. (a)What is the smallest possiblevalue of the principal quantumnumber, n? (b) What is the valueof the angular momentumquantum number, l? (c) What isthe largest possible value of themagnetic quantum number, ml?(d) The probability density goes to zero along which of thefollowing planes: xy, xz, or yz?
Would youexpect it to require more or less energy to remove a 3s electronfrom the chlorine atom, as compared with a 2p electron?
6.113 When an electron makes a transition between energylevels of a hydrogen atom, there are no restrictions onthe initial and final values of the principal quantumnumber n. However, there is a quantum mechanicalrule that restricts the initial and final values of theorbital angular momentum l. This is the selectionrule, which states that Δl = ±1; that is, in atransition, the value of l can only increase or decreaseby 1. According to this rule, which of the followingtransitions are allowed:
Describe and account for the variation of first ionizationenergies along Period 2 of the periodic table . Would you expect the same variation in Period 3?
Imagin a world in which the Puli principle is " No more than one electron can occupy an atomic orbitals , irrespective of it's spin ". How many elements would there be in the second row of periodic table , assuming that nothing else is different about this world?
What is the probability of find ing the electron in a volume of 6.5 pm3 centred on the nucleus in (a) a hydrogen atom, (b) a He+ ion?