All About Oxidation States

Oxidation and reduction are two important concepts in chemical reactions. During a reaction, the bonds are formed either by losing, gaining, or sharing electrons. Oxidation states are the degree of oxidation occurring for an atom within a compound. In a chemical reaction, the lowest and highest oxidation states calculate the total gain or loss of electrons. The elements with the lowest oxidation state mean it has the lowest degree of loss of an electron. However, the elements with a high oxidation state mean it loses maximum electrons to form a stable bond. 

Importance of Oxidation State 

The oxidation state of elements in a chemical reaction helps find the nomenclature and calculate electrons gained or lost. The definition of oxidation states is crucial for a better understanding of chemical reactions. It is an important concept in organic chemistry and helps understand how the bonds are formed between two atoms in a compound. 

• The definition of oxidation states is not limited to just calculating the loss or gain of electrons. Oxidation states are essential for balancing the redox chemical equations. Hence, it helps in balancing the oxidised atoms with reduced atoms. 

• The oxidation state explains various bonds in a compound. It helps in calculating the oxidation number of each atom in a compound. 

• It helps analyse the algorithm used for assigning the bond. The algorithm is based on Lewis’s structure which shows the total valence electrons. According to Lewis’s structure, the oxidation state equals the charge of an atom when heteronuclear bonds are assigned to the electronegative partner of the bond. However, there is an equal division of the homonuclear bonds.  

What Are the Lowest and the Highest Oxidation States?

The oxidation states of elements are categorised into the highest and lowest states, depending on the loss or gain of an electron. 

The atoms or elements which consist of the highest oxidation states lose maximum electrons to form a stable bond. However, there is a minimum loss of electrons to form a bond with another atom in elements with the lowest oxidation state.

• However, an oxidation state of +12 for uranium is likely when it is presented in the form of UO6
• The value of the highest oxidation state is always positive. 
• In a compound with the lowest oxidation state, the atoms of elements lose the least number of electrons to form a stable bond with another atom in a molecule. 
• The lowest oxidation state of any element is for boron in the compound Al3BC, with an oxidation state of -5. 
• The low oxidation state is always negative.  

The lowest and highest oxidation states depend on the elements and how they are present in a particular compound. The oxidation states are calculated for the elements in a chemical-based reaction on certain rules for the oxidation state.

Calculation of the Oxidation State of Elements  

The calculation of the oxidation state is based on a few rules. However, one of the best, quickest, and most effective ways is to use an oxidation state calculator. The chemical calculator gives the accurate answer but requires that all the number of atoms in the compound be used accurately.  

Here are some examples of oxidation state calculation in chemical reactions:

1. Calculate the oxidation number of P in H3PO4.

Let’s assume the oxidation number of phosphorus is X.

Oxidation number of hydrogen = +1 

Oxidation number of oxygen = – 2

Hence, after implementing the values,

3 X (+1) + (X) + 4 X (-2) = 0

X = 8 -3 = 5

Hence, the oxidation number of P is 5

Here is another example of oxidation state calculation:

2. Calculate the oxidation number of Mn (Manganese) in MnO4-2.

Let’s assume the oxidation number of manganese = X.

Oxidation number for oxygen = -2 

Putting the values,

X + 4 (-2) = – 2

X = – 2 + 8 = 6

Hence, the oxidation number of manganese is +6

The calculation of the atom’s oxidation number helps determine the loss or gain of an electron. The higher the positive value for the oxidation state, the more the loss of electrons to form a stable bond. When the oxidation state is negative, it loses a minimum number of electrons to form a bond with another atom. 

Conclusion

In summary, the oxidation state is a determining factor in understanding how redox reactions occur. It tells us how the oxidation and reduction in a chemical reaction are balanced. 

The definition of oxidation states precisely means the total number of electrons lost, gained, or acquired by an atom to form a bond with another atom within a reaction. The element with the highest oxidation number means it loses all its electrons or maximum electrons to another atom to form a stable bond. The element with the lowest oxidation number means it loses minimum electron numbers to form a stable bond with another atom.