2s 1an8 1s Questions: 1. set of four Write the principle's or rules below: Pauli exclusion principle: no two electrons in an atom may hova ha soa Aufbau principle: electrons fi atomiC orbitals from lowest enar sy to Hund's rule: when Rlectrons fill degenerate orbitals, they tirst Fill them singy w Parallel spins 2. Calculate the de Broglie wavelength of a hydrogen atom traveling at 1.00 x 104 m/s. (1 highest . = 1.66 x 10-27 kg) =A- mv .020 X 1034 J.S (dox102 .0oxiO ms) 3. Compare the calculated de Broglie wavelength above with the radius of a hydrogen atom is approximately 0.040 nm. Are wave properties important for the hydrogen atom? 4. Calculate the uncertainty in the position of a hydrogen atom when its velocity is known to within 50.0 m/s (Av). How does the uncertainty in position compare to the radius of the hydrogen atom at approximately 0.040 nm? (1 amu= 1.66 x 1027 kg) AX mAV h

2s 1an8 1s Questions: 1. set of four Write the principle's or rules below: Pauli exclusion principle: no two electrons in an atom may hova ha soa Aufbau principle: electrons fi atomiC orbitals from lowest enar sy to Hund's rule: when Rlectrons fill degenerate orbitals, they tirst Fill them singy w Parallel spins 2. Calculate the de Broglie wavelength of a hydrogen atom traveling at 1.00 x 104 m/s. (1 highest . = 1.66 x 10-27 kg) =A- mv .020 X 1034 J.S (dox102 .0oxiO ms) 3. Compare the calculated de Broglie wavelength above with the radius of a hydrogen atom is approximately 0.040 nm. Are wave properties important for the hydrogen atom? 4. Calculate the uncertainty in the position of a hydrogen atom when its velocity is known to within 50.0 m/s (Av). How does the uncertainty in position compare to the radius of the hydrogen atom at approximately 0.040 nm? (1 amu= 1.66 x 1027 kg) AX mAV h

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

Chapter4: Introduction To Quantum Mechanics

Section: Chapter Questions

Problem 59AP

See similar textbooks

Similar questions

Use the mathematical expression for the 2pz wave function of a one-electron atom (see Table 5.2) to show that the probability of finding an electron in that orbital anywhere in the x-y plane is 0. What are the nodal planes for a dxz orbital and for a dx2y2 orbital?
What type of relationship (direct or inverse) e xists between wavelength, frequency, and photon energy? What does a photon energy unit of a joule equal?
The figure below represents part of the emission spectrum for a one-electron ion in lhe gas phase. All the lines result from electronic transitions from excited states to the n = 3 state. (See Exercise 160.) a. What electronic transitions correspond to lines A and B? b. If the wavelength of line B is 142.5 nm, calculate the wavelength of line A.
State which of the following orbitals cannot exist according to the quantum theory: 2s, 2d, 3p, 3f, 4f, and 5s. Briefly explain your answers.
In a FranckHertz experiment on sodium atoms, the first excitation threshold occurs at 2.103 eV. Calculate the wavelength of emitted light expected just above this threshold. (Note: Sodium vapor lamps used in street lighting emit spectral lines with wavelengths 5891.8 and 5889.9 Å.)
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.
(a) Use the radial wave function for the 3p orbital of a hydrogen atom (see Table 5.2) to calculate the value of r for which a node exists. (b) Find the values of r for which nodes exist for the 3s wave function of the hydrogen atom.
Consider an electron for a hydrogen atom in an excited state. The maximum wavelength of electromagnetic radiation that can completely remove (ionize) the electron from the H atom is 1460 nm. What is the initial excited state for the electron (n = ?)?
How do 2p orbitals differ from each other? How do 2p and 3p orbitals differ from each other? What is a nodal surface in an atomic orbital? What is wrong with lp, ld, 2d, lf, 2f, and 3f orbitals? Explain what we mean when we say that a 4s electron is more penetrating than a 3d electron.
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.)
Potassium atoms in a flame emit light as they undergo transitions from one energy level to another that is 4.91019J lower in energy. Calculate the wavelength of light emitted and, by referring to Figure 4.3, predict the color visible in the flame.
6.27 Refer w the data and energy-Ievel diagram shown in Problem 6.26, and find the wavelength of light that would be emitted when a hydrogen atom undergoes the transition from the state labeled as n = 4 to the state labeled as n = 2. Express your answer in nm.