Valence, Oxidation States and Chemical Reactivity

Introduction

The physical properties of the atoms present in the periodic table are classified with the help of the valence and oxidation state. However, both of these are somehow related to each other. There are numerous elements, which are also considered the icon of chemistry. Still, the three groups of elements are discussed from the periodic table, including Group I, II, and III. The structure of Group I of the periodic table contains the one-electron present in the outer shell. They react with the other chemical while releasing one extra electron from its structure, creating a valence of one. 

Valence 

The Valence of an element is defined as the measure of elements combining capacity. In simple terms, this can be defined as the number of electrons that are gained or lost by an atom to obtain a stable electronic configuration. 

Oxidation State 

Another term that you can hear in chemical reactions, especially in chemistry, is the Oxidation State. The oxidation state of an atom determines the total number of electrons gained and lost by the atom itself. However, both valence and oxidation are the common properties of an element that demands the help of electronic configuration to perform further understanding. 

What are valence and oxidation states for an atom? 

Usually, the electrons present in the outermost shell are commonly called the valence electrons. However, the number of these electrons further defines the valence of an atom. 

• Usually, the valence of elements of p-block and s-block of the primary periodic table are obtained with the help of the calculative method that includes eight minus the number of these electrons or just by calculating the number of valence electrons. 

Examples : Carbon has atomic number 6 and 4 valence electrons  in its outermost shell.

So, its valency is 4. 

 Nitrogen has atomic number 7 and 5 valence electrons. So, valency = 8-5=3

• However, for the d and the f block elements present in the periodic table, the Calculation of valence is not only based on the valence electron but also both d and f orbital electrons. Furthermore, the valencies of the f and d block usually are represented as 2 and 3. Example : Scandium (Z=21) has 2,8,9,2 electrons per shell and its  d and f electrons are 11  so its valency =-(8-11) =3

The oxidation number of all elements further represents the oxidation state of an atom found in a chemical compound. Also, it is considered to be speculative when all atoms bond with each other forming the ionic elements. Oxidation number further represents the sure, negative, and state of zero.

• All elements’ most demanded oxidation number can be denoted with the +8 in the xenon, ruthenium, iridium, osmium, and hassium. However, some complex forms of plutonium can also witness these bonds. 
• The lowest amount of state can be further denoted with the -4 for certain carbon groups. 
• The increments in the oxidation number of all elements with the help of chemical reaction are defined as oxidation, where losses of electrons, including the decrease in the atoms, are also performed with some addition of the electrons. 

What is chemical reactivity? 

In chemistry, chemical reactivity is defined as the state for which a substance performs a chemical reaction. It can take part in two ways, either on its own or with the help of other minerals. It further takes place with an overall release of energy. 

• Reactivity  refers to  either the chemical reaction of a single substance  or two or  more substances that interact with each other
• It also refers to the systematic study of sets of reactions of these two kinds.

Furthermore, the chemical reactivity of a single substance further looks after the behaviors of the reactants where it includes:

• Forming of new substances by adding the atoms from one element to another. 
• Decomposition
• Interacting with two or more reactants to form the same number of products.
  
  

What periodic trends are found in the oxidation state of elements?

The valence periodic tables are availed in the oxidation state of elements with the help of the following grounds:

• Variation of the oxidation number in a single period
• While going from left to right in a valence periodic table, the number of electrons can change with an increment from 1-to 8. However, when mixed with O or H, the number of elements increases from 1-4 and then comes to 0. 
• For instance, consider two compounds with Oxygen Na2O and F2O. In the F2O compound, the electronegativity of F is more than that of Oxygen. Due to this reason, each F atom will bind with one electron from the Oxygen compound.
• Furthermore, the oxidation number of all elements ensures the charge possessed by the atom due to the gain or loss of their electrons present in the molecule. 
• Variation of the oxidation number in a single group
• However, when moving down a group, no change in the number of valence electrons. Due to this, all elements of a single group hold the same valence. 

How to find the valence of an element? 

The easiest method to determine the valence of an element is taking the help of the periodic table. In this table, the elements are arranged in groups, and the elements present in these groups including 1-8,  carry the similar valency as others in their group. For instance, the group 8 elements  contains l 8 electrons with high stability.  

Conclusion

As per the information, it is thus found that the valency of the elements is measured with the ability to bind with the other forms of elements in the form of Chemical reactions. However, no bounding will occur if the amounts of electrons are present in the complete state. To perform the calculation, the numbers of electrons left out in the outer shell determine the valency of the element.