6.3 Development of Quantum Theory
Matter waves and their wavelengths, orbitals as probability distributions rather than paths, and the four quantum numbers labeling an electron's state.
6 exercises
6.3 Exercise 1
How are the Bohr model and the quantum mechanical model of the hydrogen atom similar? How are they different?
6.3 Exercise 3
Describe the properties of an electron associated with each of the following four quantum numbers: n, l, ml, and ms.
6.3 Exercise 5
Identify the subshell in which electrons with the following quantum numbers are found:
(a) n = 2, l = 1
(b) n = 4, l = 2
(c) n = 6, l = 0
6.3 Exercise 7
Identify the subshell in which electrons with the following quantum numbers are found:
(a) n = 3, l = 2
(b) n = 1, l = 0
(c) n = 4, l = 3
6.3 Exercise 13
How many electrons could be held in the second shell of an atom if the spin quantum number ms could have three values instead of just two? (Hint: Consider the Pauli exclusion principle.)
6.3 Exercise 15
Write a set of quantum numbers for each of the electrons with an n of 4 in a Se atom.
Adapted from General Chemistry © 2019 Rice University. Licensed under CC BY 4.0. Sources: Chemistry 2e, Chemistry: Atoms First 2e. Imported at revision 32c7196.