How would the d,2_2 orbital in the n = 5 shell compare to the d,2 12 orbital in the n 3 shell? 1. The orbital in the n = 5 shell is bigger than the orbital in the n = 3 shell. 2. The value of / would increase by 2 for the n = 5 shell. 3. The value of / for both orbitals would be the same. 4. The orientation of the n = 5 orbital would be rotated 45° along the xy plane. 5. The me value for both orbitals would be the same. %3D Drag the appropriate items to their respective bins. View Available Hint(s) Reset Help P Pearson r Copyright O2020 Pearson Education Inc. All rights reserved. I Terms of Use I P

How would the d,2_2 orbital in the n = 5 shell compare to the d,2 12 orbital in the n 3 shell? 1. The orbital in the n = 5 shell is bigger than the orbital in the n = 3 shell. 2. The value of / would increase by 2 for the n = 5 shell. 3. The value of / for both orbitals would be the same. 4. The orientation of the n = 5 orbital would be rotated 45° along the xy plane. 5. The me value for both orbitals would be the same. %3D Drag the appropriate items to their respective bins. View Available Hint(s) Reset Help P Pearson r Copyright O2020 Pearson Education Inc. All rights reserved. I Terms of Use I P

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

15
All orbitals (of any type) can only hold 2 e- each. But some of the subshells have more than 1 orbital. Match the total electrons that can possibly be held by the following subshells: s choose from 2, 10,6,8,4 p d
Which one of the following statements best explains the relative size of the atomic radius of F and F? O The outermost electron of F is in an orbital withn%3D electron in F is in an orbital with n = 2. Since orbital size increases as n increases, 3 while the outermost F has a larger atomic radius than F. O Since both F and F have the same nuclear charge of 9+, and both F and F have their outermost electrons in the 2s and 2p orbitals, both F and F have the same atomic radius. O Since each electron takes up the same volume in an atom or ion, F has the same atomic radius as F. The valence electrons of F are more shielded from the nucleus than the valence electrons of F, which results in F having a larger atomic radius than F. OF has more electrons than F, which can penetrate the region near the nucleus more frequently, which results in F having a smaller atomic radius than F.
9. An electron in the hydrogen atom relaxes to the n =2 orbit and 434 nm light is emitted. What was the initial orbit of the electron? A: 5 Me g ou counoe
The quantum numbers n = 2, l = 0 describe how many orbitals?
4. Calculate the maximum number of electrons that can occupy a shell with (a) n = 2, (b) n = 5, and (c) n as a variable. Note you are only looking at the orbitals with the specified n value, not those at lower energies. %3D
Bohr's model of the atom is a system consisting of a small, dense nucleus surrounded by orbiting electrons. How does Bohr's model explain spectral emission lines? Bohr developed a formula (shown below) that predicted the wavelength of a photon given off when an electron moves from one orbit to another orbit. His formula worked well to explain spectral emission lines in the hydrogen atom. Calculate the wavelength of light that would be emitted for the orbital transition of n = 2 to n = 1. Submit an answer to four significant figures ninitial Mfinal = R Rm = 1.09678 x 107 m-'
Which of the following statements is false? a. If an electron has n= 2, it possesses only s and p orbitals b. Each orbital within a given atom can hold up 2 electrons c. The second shell of an atom possesses d orbitals d. A set of f orbitals can hold a maximum of 14 electrons e. The first energy level contains only s orbitals Determine the number of sub levels,number of orbitals,and maximum number electrons in the n=4 level
Bohr’s model of the atom is a system consisting of a small, dense nucleus surrounded by orbiting electrons. How does Bohr’s model explain spectral emission lines? Bohr developed a formula (shown below) that predicted the wavelength of a photon given off when an electron moves from one orbit to another orbit. His formula worked well to explain spectral emission lines in the hydrogen atom. Calculate the wavelength of light that would be emitted for the orbital transition of n = 7 to n = 1. Submit an answer to four significant figures,