Order the following molecules from least to most oxidized, based on the marked carbon atom:

The loss of electrons by an atom during a reaction is known as oxidation.

When the oxidation state of a molecule, atom, or ion is enhanced, it is called oxidation. When an atom, molecule, or ion gains electrons or the oxidation states of an atom, molecule, or ion drop, the process is termed reduction.

a) 2-propanol

This chemical has a carbon atom that is designated and has the OH group linked to it.

Let's take a look at the atoms it has attached.

There are two carbon atoms, one oxygen atom, and one H atom.

If the X atom is connected to its identical atom, it does not affect the oxidation state - it has no change.

This means that only the H and O atoms are affected in this case.

If the O atom is more electronegative, the charge of the C atom will increase by one, resulting in +1

If the H atom is less electronegative, the carbon atom will have a smaller charge, -1

This means that when all of the oxidation states are combined, the oxidation state of this carbon atom is zero.

b) Propane.

Two single bonds with C atoms and two single bonds with H atoms exist on the highlighted carbon atom.

Only those with H atoms are counted.

Because H is more electropositive, its oxidation state will be -2 if the oxidation state of C decreases by -1 for every C-H bond.

This is due to the presence of two C-H bonds.

c) 2-propanone.

One double bond exists between the designated carbon atom and the oxygen atom, while two single bonds exist between the marked carbon atom and other C atoms.

This double bond with the O atom is the equivalent of two single bonds with the O atom.

Because oxygen is more electronegative than carbon, its formal charge increases by +1 for every C-O bond.

This suggests that this carbon atom's oxidation state will be +2