Sublevel Shapes and Electron Capacity in the Periodic Table

The video tutorial covers the SPDF sublevels, their shapes, and how they relate to energy levels. It explains quantum numbers and their role in identifying electron positions. The video also demonstrates how to determine the electron configuration and orbital notation for elements like phosphorus, using principles like the Aufbau principle and Hund's rule.

What shape is associated with the s sublevel?

• Unusual

• Spherical

• Clover leaf

• Dumbbell

How many electrons can the p sublevel hold?

• 2

• 14

• 6

• 10

Which group in the periodic table corresponds to the s block?

• Group 13 to 18

• Group 1 and 2

• Group 17 and 18

• Group 3 to 12

What does the quantum number 'l' represent?

• Specific orbital

• Spin of the electron

• Type of sublevel

• Principal energy level

For a d sublevel, what is the range of possible ml values?

• -1 to 1

• 0 to 4

• -2 to 2

• -3 to 3

According to the Pauli Exclusion Principle, what is true about electrons in the same orbital?

• They must have the same spin

• They cannot have the same set of four quantum numbers

• They must be in different energy levels

• They must have opposite charges

What is the electron configuration for phosphorus?

• 1s2 2s2 2p6 3s2 3p3

• 1s2 2s2 2p6 3s1 3p4

• 1s2 2s2 2p6 3s2 3p6

• 1s2 2s2 2p4 3s2 3p3

What principle states that electrons fill the lowest energy orbitals first?

• Hund's Rule

• Pauli Exclusion Principle

• Aufbau Principle

• Heisenberg Uncertainty Principle

How many s electrons are present in phosphorus?

• 6

• 4

• 8

• 2

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

• In reverse order

• In pairs

• One at a time

• All at once