Understanding Paramagnetism and Diamagnetism

The video tutorial explains how to identify substances as paramagnetic or diamagnetic based on their electron configurations. It provides examples using magnesium, manganese, nickel, and zinc, detailing the process of writing electron configurations and drawing orbital diagrams. The video also covers Hund's rule and the Aufbau principle, emphasizing the importance of unpaired electrons in determining magnetic properties.

What is the key characteristic of a paramagnetic substance?

• It is strongly attracted to a magnetic field.

• It contains unpaired electrons.

• It has no electrons.

• It has a full outer shell of electrons.

What is the electron configuration of magnesium?

• 1s2 2s2 2p6 3s2

• 1s2 2s2 2p6 3s1

• 1s2 2s2 2p5 3s2

• 1s2 2s2 2p6 3p1

Why is magnesium considered diamagnetic?

• It has a half-filled d sublevel.

• All its electrons are paired.

• It has a full f sublevel.

• It has unpaired electrons.

What is the atomic number of manganese?

• 12

• 28

• 25

• 30

According to Hund's rule, how should electrons be added to degenerate orbitals?

• All at once with parallel spins.

• One at a time with parallel spins.

• All at once with opposite spins.

• One at a time with opposite spins.

How many unpaired electrons does nickel have?

• 2

• 3

• 1

• 0

What is the total number of electrons in a neutral atom of nickel?

• 32

• 30

• 28

• 26

What is the electron configuration of zinc using noble gas notation?

• [Kr] 5s2 4d10

• [Ne] 3s2 3p6

• [Ar] 4s2 3d10

• [Xe] 6s2 4f14

Why is zinc considered diamagnetic?

• It has a full f sublevel.

• It has a half-filled p sublevel.

• It has a full d sublevel.

• It has unpaired electrons.

Which of the following elements is an exception when writing electron configurations?

• Copper

• Zinc

• Nickel

• Magnesium