Electron Configuration and Stability

This video tutorial explains how to find the electron configurations of chromium and copper, which are exceptions to the typical rules. It covers the sublevels and electron distribution for each element, highlighting the stability achieved by unpaired electrons in higher energy levels. The video emphasizes the importance of understanding these exceptions for chemistry tests.

Why is it important to understand electron configuration exceptions?

• They are commonly tested on chemistry tests.

• They help in understanding chemical reactions.

• They are rarely tested in chemistry exams.

• They are not relevant to real-world applications.

What is the maximum number of electrons that the s sublevel can hold?

• 14

• 10

• 2

• 6

In the electron configuration of chromium, why does one electron move from the 4s to the 3d sublevel?

• To decrease the energy level.

• To fill the 4s sublevel completely.

• To achieve a more stable configuration.

• To increase the total number of electrons.

What is the final electron configuration of chromium?

• 1s2 2s2 2p6 3s2 3p6 4s2 3d4

• 1s2 2s2 2p6 3s2 3p6 4s2 3d5

• 1s2 2s2 2p6 3s2 3p6 4s1 3d4

• 1s2 2s2 2p6 3s2 3p6 4s1 3d5

Where is copper located in the periodic table?

• Second row

• Third row

• Fourth row

• Fifth row

What is the initial electron configuration of copper before any rearrangement?

• 1s2 2s2 2p6 3s2 3p6 4s1 3d10

• 1s2 2s2 2p6 3s2 3p6 4s2 3d10

• 1s2 2s2 2p6 3s2 3p6 4s2 3d9

• 1s2 2s2 2p6 3s2 3p6 4s1 3d9

Why does one electron move from the 4s to the 3d sublevel in copper?

• To fill the 4s sublevel completely.

• To decrease the energy level.

• To achieve a more stable configuration.

• To increase the total number of electrons.

What is the final electron configuration of copper?

• 1s2 2s2 2p6 3s2 3p6 4s2 3d9

• 1s2 2s2 2p6 3s2 3p6 4s1 3d10

• 1s2 2s2 2p6 3s2 3p6 4s2 3d10

• 1s2 2s2 2p6 3s2 3p6 4s1 3d9

How many electrons does copper have in total?

• 24

• 29

• 30

• 28

Which sublevel can hold a maximum of 10 electrons?

• s

• p

• d

• f