Step 1: Identify the atoms in the molecule. He2 consists of two helium (He) atoms.
Step 2: Determine the number of electrons in each helium atom. Each helium atom has 2 electrons.
Step 3: Calculate the total number of electrons in He2. Since there are 2 helium atoms, the total is 2 + 2 = 4 electrons.
Step 4: Understand the molecular orbital theory. In this theory, electrons fill molecular orbitals starting from the lowest energy level.
Step 5: Fill the molecular orbitals for He2. The first 2 electrons fill the bonding orbital (σ1s), and the next 2 electrons fill the antibonding orbital (σ*1s).
Step 6: Count the number of bonding and antibonding electrons. There are 2 bonding electrons and 2 antibonding electrons.
Step 7: Calculate the bond order using the formula: Bond Order = (Number of bonding electrons - Number of antibonding electrons) / 2.
Step 8: Substitute the values into the formula: Bond Order = (2 - 2) / 2 = 0.
Step 9: Conclude that the bond order of He2 is 0, indicating that there is no net bonding and the molecule is unstable.
