Electron Orbitals and Energy Levels

The video tutorial explains how electrons are arranged in atoms, focusing on the principle energy levels and sub-levels (s, p, d, f) to achieve the lowest energy state. It describes the energy hierarchy among these sub-levels and the capacity of orbitals to hold electrons. The tutorial uses hydrogen and oxygen as examples to illustrate electron configuration, showing how electrons fill the available orbitals in order of increasing energy.

What is the primary reason electrons fill principal energy levels or shells?

• To maximize energy

• To achieve the lowest possible energy

• To balance the atom

• To create a magnetic field

Which sub-level has the lowest energy?

• d sub-level

• f sub-level

• s sub-level

• p sub-level

How many electrons can each orbital hold?

• Two

• One

• Three

• Four

Where does the single electron of hydrogen reside?

• 2s orbital

• 3d orbital

• 1s orbital

• 2p orbital

In the case of oxygen, how are the remaining four electrons distributed after filling the 2s orbital?

• One in each 2p orbital

• Two in one 2p orbital, one in each of the remaining 2p orbitals

• All in one 2p orbital

• All in the 2s orbital