Interpretation:
The maximum numbers of electrons in the alternate universe with the principal quantum number 3 in a given atom should be identified using the concept of quantum numbers.
Concept Introduction:
Quantum Numbers
Quantum numbers are explained for the distribution of electron density in an atom. They are derived from the mathematical solution of Schrodinger’s equation for the hydrogen atom. The types of quantum numbers are the principal quantum number (
Principal Quantum Number (
The principal quantum number (
Angular Momentum Quantum Number (
The angular momentum quantum number (
Magnetic Quantum Number (
The magnetic quantum number (
If
If
If
If
The number of
Electron Spin Quantum Number (
It specifies the orientation of the spin axis of an electron. An electron can spin in only one of two directions. There are two possible ways to represent
Pauli exclusion principle
No two electrons in an atom should have the four same quantum numbers. Two electrons are occupied in an atomic orbital because there are two possible values of
To find: Count the maximum number of electrons in the alternate universe with the principal quantum number 3 in a given atom
Want to see the full answer?
Check out a sample textbook solutionChapter 3 Solutions
Chemistry: Atoms First
- • identify an orbital (as 1s, 3p, etc.) from its quantum numbers, or vice versa.arrow_forwardWhich of the following sets of quantum numbers correctly represents a 4p orbital? (a) n = 4, = 0, m = 1 (b) n = 4, = 1, m = 0 (c) n = 4, = 2, m = 1 (d) n = 4, = 1, m =2arrow_forwardWhat are quantum numbers? What information do we get from the quantum numbers n, l, and ml? We define a spin quantum number (ms), but do we know that an electron literally spins?arrow_forward
- What is the maximum number of electrons that can occupy a f subshell (l = 3)?arrow_forwardAccording to a relationship developed by Niels Bohr, for an atom or ion that has a single electron, the total energy, En, of an electron in a stable orbit of quantum number n is En = [Z2/n2] (2.179 1018 J) where Z is the atomic number. Calculate the ionization energy for the electron in a ground-state He+ ion.arrow_forward6.96 When a helium atom absorbs light at 58.44 nm, an electron is promoted from the 1s orbital to a 2p orbital. Given that the ionization energy of (ground state) helium is 2372 kJ/ mol, find the longest wavelength of light that could eject an electron from the excited state helium atom.arrow_forward
- Chemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage LearningChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningChemistry: Matter and ChangeChemistryISBN:9780078746376Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl WistromPublisher:Glencoe/McGraw-Hill School Pub CoChemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning