I Electron Orbitals and Configurations

Open Ended

Why is understanding electron orbitals and their configurations important in chemistry?

Multiple Choice

What is an orbital in terms of electron probability?

• A fixed path for electrons around the nucleus

• A region in space where there is 90% probability of finding an electron

• A solid sphere surrounding the nucleus

• A point where electrons are always found

Multiple Choice

How does the energy of principal energy levels change as the distance from the nucleus increases?

• Energy decreases

• Energy remains the same

• Energy increases

• Energy fluctuates randomly

Multiple Choice

Which of the following statements about the s orbital is correct?

• It has three shapes and can hold up to 6 electrons

• It has one shape and can hold up to 2 electrons

• It has five shapes and can hold up to 10 electrons

• It has seven shapes and can hold up to 14 electrons

Multiple Choice

Which type of orbital is associated with Groups 1 and 2 on the periodic table?

• s orbital

• p orbital

• d orbital

• f orbital

Multiple Choice

Which type of orbital is shaped like a sphere?

• s orbital
• p orbital
• d orbital
• f orbital

Multiple Choice

How many electrons are in 1s² 2s² 2p⁴?

• 5

• 6

• 8

• 13

Open Ended

Explain how the orientation of the 2p orbitals differs from the s orbitals, based on the diagrams provided.

Multiple Choice

Which of the following statements best describes the difference between the 1s, 2s, and 2p orbitals as shown in the diagrams?

• 1s and 2s are spherical, while 2p consists of three dumbbell-shaped orbitals.

• 1s is dumbbell-shaped, 2s is spherical, and 2p is spherical.

• 1s and 2p are spherical, while 2s is dumbbell-shaped.

• All three orbitals are dumbbell-shaped.

Open Ended

What is one concept about electron orbitals or electron configuration that you would like to understand better after this lesson?