Work in groups on these problems. You should try to answer the questions without referring to your textbook. If you get stuck, try asking another group for help.
For \(n = 4\), what are the possible values of \(l\)? For \(l = 2\), what are the possible values of \(m_l\)?
How many possible values for l and ml are there when a) n=3 and b) n=5?
Give the numerical values of \(n\) and \(l\) corresponding to each of the following designations:
Give the values for n, l, and ml for:
- Each orbital in the 2p subshell
- each orbital in the 5d subshell
Which of the following represent impossible combinations of n and l:
Which of the following are permissible sets of quantum numbers for an electron in a hydrogen atom. For those combinations that are permissible, write the appropriate designation for the subshell to which the orbital belongs (ex. 1s)
- [2, 1, 1, +1/2]
- [1, 0, ‐1, ‐1/2]
- [4, 2, ‐2, +1/2]
- [3, 3, 0, ‐1/2]
What is the maximum number of electrons in an atom that can have the following quantum numbers:
- \(n = 2\), \(m_s = ‐1/2\)
- \(n=5\), \(l=3\)
- \(n= 4\), \(l=3\), \(m_l = ‐3\)
- \(n=4\), \(l=1\), \(m_l=1\)
Write the condensed electron configurations for the following atoms, using the appropriate noble‐gas core abbreviations:
Write the full electron configuration for the following atoms.
What is wrong with the following electron configurations for atoms in their ground states?