Effective Nuclear Charge and Electron Shielding Fundamentals

The video tutorial introduces the concept of effective nuclear charge, explaining how it is influenced by the presence of multiple electrons in an atom. The instructor details the formula Z-sigma, where Z is the atomic number and sigma is the screening constant, to calculate the effective nuclear charge. Examples are provided for elements like Lithium, Boron, and Titanium, demonstrating the calculation process. The video concludes with a call to action for viewers to like and subscribe for more content.

What is the main reason an electron in a multi-electron atom experiences less nuclear charge?

• Higher atomic number

• Presence of more electrons in the same or other orbits

• Larger atomic radius

• Presence of more protons in the nucleus

Which formula is used to calculate the effective nuclear charge?

• Z / sigma

• Z * sigma

• Z - sigma

• Z + sigma

What is the contribution of an electron in the n-shell for s and p orbitals?

• 0.85

• 1.00

• 0.35

• 0.50

For d and f orbitals, what is the contribution of an electron in the n-1 shell?

• 0.35

• 0.85

• 1.00

• 0.50

In the example of Lithium, what is the effective nuclear charge calculated?

• 1.7

• 3.0

• 2.6

• 1.3

What is the electronic configuration of Boron used in the example?

• 1s2 2s2 2p1

• 1s2 2s1

• 1s2 2s2

• 1s2 2p1

What is the effective nuclear charge for Boron as calculated in the example?

• 2.6

• 3.5

• 2.4

• 1.3

In the example of Titanium, what is the contribution of the d electron in the n-shell?

• 0.50

• 0.35

• 0.85

• 1.00

What is the effective nuclear charge for Titanium as calculated in the example?

• 4.0

• 1.3

• 2.6

• 3.65

What is the atomic number of Titanium used in the example?

• 23

• 21

• 22

• 20