# Quantum Numbers (Worksheet)

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Section: _____________________________

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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:

1. 3p
2. 2s
3. 4f
4. 5d

## Q4.

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

1. Each orbital in the 2p subshell
2. each orbital in the 5d subshell

## Q5.

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

1. 1p
2. 4s
3. 5f
4. 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)

1. [2, 1, 1, +1/2]
2. [1, 0, ‐1, ‐1/2]
3. [4, 2, ‐2, +1/2]
4. [3, 3, 0, ‐1/2]

## Q7.

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

1. $$n = 2$$, $$m_s = ‐1/2$$
2. $$n=5$$, $$l=3$$
3. $$n= 4$$, $$l=3$$, $$m_l = ‐3$$
4. $$n=4$$, $$l=1$$, $$m_l=1$$

## Q8.

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

1. $$Cs$$
2. $$Ni$$
3. $$Se$$
4. $$Cd$$
5. $$Ac$$
6. $$Pb$$

## Q9.

Write the full electron configuration for the following atoms.

1. $$Ga$$
2. $$Ca$$
3. $$V$$
4. $$I$$
5. $$Y$$
6. $$Pt$$
7. $$Lu$$

## Q10.

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

1. $$1s^22s^23s^1$$
2. $$[Ne]2s^22p^3$$
3. $$[Ne]3s^23d^5$$