# Quantum Numbers (Worksheet)

- Page ID
- 20041

Name: ______________________________

Section: _____________________________

Student ID#:__________________________

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.

## Q1.

**For \(n = 4\), what are the possible values of \(l\)? For \(l = 2\), what are the possible values of \(m_l\)?**

## Q2.

**How many possible values for l and ml are there when a) n=3 and b) n=5?**

## Q3.

**Give the numerical values of \(n\) and \(l\) corresponding to each of the following designations: **

- 3p
- 2s
- 4f
- 5d

## Q4.

Give the values for n, l, and ml for:

- Each orbital in the 2p subshell
- each orbital in the 5d subshell

## Q5.

**Which of the following represent impossible combinations of n and l:**

- 1p
- 4s
- 5f
- 2d

## Q6.

**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]

## Q7.

**What is the maximum number of electrons in an atom that can have the following quantum numbers:**

- \(n = 2\), \(m_s = ‐1/2\)
- \(n=5\), \(l=3\)
- \(n= 4\), \(l=3\), \(m_l = ‐3\)
- \(n=4\), \(l=1\), \(m_l=1\)

## Q8.

**Write the condensed electron configurations for the following atoms, using the appropriate noble‐gas core abbreviations:**

- \(Cs\)
- \(Ni\)
- \(Se\)
- \(Cd\)
- \(Ac\)
- \(Pb\)

## Q9.

**Write the full electron configuration for the following atoms.**

- \(Ga\)
- \(Ca\)
- \(V\)
- \(I\)
- \(Y\)
- \(Pt\)
- \(Lu\)

## Q10.

**What is wrong with the following electron configurations for atoms in their ground states?**

- \(1s^22s^23s^1\)
- \([Ne]2s^22p^3\)
- \([Ne]3s^23d^5\)