In order to attract oxygen"s molecular orbital diagram, you need to start by taking a look in ~ what atomic orbitals you have actually for an oxygen atom, #"O"#.

As you know, oxygen is located in period 2, group 16 of the regular table and also has an atomic number equal to #8#. This method that the electron construction of a neutral oxygen atom have to account for #8# electrons.

More specifically, the electron configuration of an oxygen atom will certainly be

#"O: " 1s^2 2s^2 2p^4#

So, how numerous atomic orbitals are lived in in one oxygen atom?

the 1s-orbitalthe 2s-orbitalall three of the 2p-orbitals

Now, each equivalent pair of atomic orbitals will create two molecular orbitals, a bonding molecular orbital, which is lower in energy when compared with the atom orbitals, and also an anti-bonding molecule orbital, i m sorry is higher in energy when contrasted with the atomic orbitals.

Since you have a complete of five atomic orbitals, you have the right to expect to have actually a full of ten molecule orbitals because that the #"O"_2# molecule.

For simplicity, I"ll usage a diagram that doesn"t display the 1s-orbitals and also their corresponding #sigma_(1s)# and also #sigma_(1s)^"*"# molecule orbitals (MO"s).

So, here"s how should draw the diagram

The 1s-orbitals and also their matching molecular orbitals look exactly like the 2s-orbitals, so you can attract them below the 2s-orbitals if friend want.

Now, because we"re not included the 1s-orbitals, the total number of electrons easily accessible for this diagram will certainly be equal to #12#, #6# from each oxygen atom.

Start filling the molecular orbitals through suing the Aufbau Principle, Hund"s Rule, and Pauli"s exclusion Principle.

Start from the molecular orbit that"s lowest in energy, i m sorry in this chart is the #sigma_(2s)# MO, and also make your method up.

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Your diagram should end up looking favor this

Now, the bond order, which tells you how numerous bonds you deserve to expect come find in between two atoms, is calculated using the formula

#color(blue)("B.O." = 1/2 * ("no. The bonding e"^(-) - "no. That anti-bonding e"^(-))#

The bonding electrons space those electrons situated in bonding MO"s. They are displayed in #color(green)("green")# in the over diagram.

So, let"s count these electrons - the ones located in the #sigma_(1s)# and also #sigma_(1s)^"*"# MO"s count together well!

#2# in the #sigma_(1s)# MO#2# in the #sigma_(2s)# MO#2# in the #pi_(2px)# MO#2# in the #pi_(2py)# MO#2# in the #pi_(2pz)# MO

This offers you a complete of #10# bonding electrons.

Now emphasis on finding the variety of anti-bonding electrons, which are located in anti-bonding MO"s. Castle are presented in #color(red)("red")# in the over diagram.

#2# in the #sigma_(1s)^"*"# MO#2# in the #sigma_(2s)^"*"# MO#1# in the #pi_(2py)^"*"# MO#1# in the #pi_(2pz)^"*"# MO

This provides you a complete of #6# anti-bonding electrons.

The bond order for the oxygen molecule will therefore be

#"B.O." = 1/2 * (10 - 6)#

#"B.O." = 1/2 * 4 = color(green)(2)#

This tells you that the two oxygen atoms room bonded with each other via a double bond, i beg your pardon of course is composed of a sigma and also a pi bond.

Finally, the magnetic behavior is identified by the visibility of unpaired electrons.

More specifics if a molecule has unpaired electrons, it will certainly be paramagnetic, i.e. It will be attractive by an outside magnetic field.

If that does not have unpaired electrons, it will certainly be diamagnetic, i.e.

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It will be repelled by an outside magnetic field.

As you deserve to see, the oxygen molecule has actually two unpaired electrons in 2 anti-bonding MO"s, #pi_(2py)^"*"# and #pi_(2pz)^"*"#.