Mastering Electronic Configurations and Subshells in Chemistry

This video tutorial provides a comprehensive guide to electronic configuration, focusing on subshells and orbitals. It explains how electrons are placed in subshells using principles like the Aufbau principle, and addresses common student mistakes. The tutorial includes examples, such as the electronic configuration of oxygen, to illustrate these concepts.

What is the maximum number of electrons that the 'p' subshell can accommodate?

• 6

• 2

• 10

• 14

Which quantum number represents the main energy level or shell of an atom?

• Spin quantum number

• Magnetic quantum number

• Principal quantum number

• Azimuthal quantum number

According to the Aufbau principle, which subshell is filled first?

• 4d

• 1s

• 3s

• 2p

What is the correct order of filling subshells according to the trick taught in the video?

• 1s, 2s, 2p, 3s

• 2s, 1s, 3p, 3s

• 3s, 2p, 1s, 4s

• 4s, 3d, 2p, 1s

What does Hund's Rule state about filling orbitals?

• Fill orbitals with opposite spins first

• Fill the highest energy orbital first

• Fill each orbital singly before pairing

• Fill each orbital with two electrons first

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

• They must have the same spin

• They must have opposite spins

• They must be in different energy levels

• They must be in different subshells

What is a common mistake students make when applying Hund's Rule?

• Filling the highest energy orbital first

• Filling orbitals doubly before singly

• Filling orbitals with opposite spins first

• Filling orbitals with the same spin

How many electrons does the oxygen atom have in its 2p subshell?

• 2

• 6

• 4

• 8

In the electronic configuration of oxygen, how many orbitals are in the 2p subshell?

• 2

• 1

• 3

• 4

What is the electronic configuration of oxygen in terms of subshells?

• 1s² 2s² 2p²

• 1s² 2s² 2p⁶

• 1s² 2s² 2p⁴

• 1s² 2s¹ 2p⁵