IIT/JEE Chemistry Practice #14: Ionization Energy

The video tutorial explores questions related to ionization energy, focusing on second, first, and third ionization energies. It discusses the periodic trends and exceptions, using orbital diagrams to explain the stability of certain electron configurations. The tutorial emphasizes the importance of understanding orbital symmetry and its impact on ionization energy, providing detailed analyses for elements like carbon, nitrogen, oxygen, fluorine, boron, and silicon.

Which element has the highest first ionization energy among the given options?

• Nitrogen

• Carbon

• Oxygen

• Boron

In the context of second ionization energy, which element is harder to ionize than expected due to its orbital configuration?

• Fluorine

• Oxygen

• Nitrogen

• Carbon

What is the correct order of second ionization energies for carbon, nitrogen, oxygen, and fluorine?

• Fluorine > Oxygen > Nitrogen > Carbon

• Carbon > Nitrogen > Oxygen > Fluorine

• Oxygen > Fluorine > Nitrogen > Carbon

• Nitrogen > Oxygen > Fluorine > Carbon

Why does nitrogen have a higher first ionization energy than oxygen?

• Nitrogen has a full P subshell.

• Nitrogen has a half-full P subshell.

• Oxygen has a half-full P subshell.

• Oxygen has a full P subshell.

Which element is the easiest to ionize for the third ionization energy?

• Aluminum

• Silicon

• Magnesium

• Sodium

In the context of third ionization energy, which element is more difficult to ionize than expected due to orbital symmetry?

• Aluminum

• Sodium

• Silicon

• Magnesium

What is the correct order of third ionization energies for sodium, magnesium, aluminum, and silicon?

• Sodium < Silicon < Magnesium < Aluminum

• Sodium < Magnesium < Silicon < Aluminum

• Sodium < Aluminum < Magnesium < Silicon

• Sodium < Magnesium < Aluminum < Silicon