Atomic Orbitals and Electron Configuration

This video by MSJ Chem explores atomic orbitals, focusing on s and p orbitals. It explains that atomic orbitals are regions with a high probability of finding electrons, as per the Heisenberg uncertainty principle. S orbitals are spherical and can hold two electrons with opposite spins, while p orbitals are dumbbell-shaped and consist of three orientations (px, py, pz), each holding two electrons, totaling six in the p sublevel.

What do atomic orbitals represent?

• The exact location of an electron

• The nucleus of an atom

• A region of space with high probability of finding an electron

• The path of an electron around the nucleus

According to the Heisenberg uncertainty principle, what is not possible?

• Measuring the mass of an electron

• Determining the charge of an electron

• Finding an electron within an atomic orbital

• Knowing the exact location of an electron within an atom

What is the shape of an s orbital?

• Dumbbell

• Spherical

• Elliptical

• Tetrahedral

How many electrons can an s orbital hold?

• Four

• Three

• Two

• One

What is the shape of p orbitals?

• Spherical

• Dumbbell

• Elliptical

• Linear

How many p orbitals are there in a p sublevel?

• Four

• Two

• One

• Three