Electronegativity - Overview, Factors, Elements, Applications, FAQs

Electronegativity is another important concept within chemistry that provides insight into how the atomic structures of the different elements manage to attract some electrons when both of them are involved in a chemical bond. This idea was earlier formulated by Linus Pauling; electronegativity reflects how many electrons an element attracts toward its nucleus during the performance of a chemical bond. This property determines the characteristics of the bonding— it can be ionic, covalent, or polar covalent, and describes the distribution of charge within the atoms of the molecule. Since fluorine or oxygen has a higher electronegativity than the other elements, it attracts the electrons more sharply creating a strong polar covalent bond in which the electron is found more in the vicinity of fluorine or oxygen atom.

This Story also Contains

1. Unveiling the Power of Electronegativity
2. Some Solved Examples
3. Conclusion

Also read -

• NCERT Solutions for Class 11 Chemistry
• NCERT Solutions for Class 12 Chemistry
• NCERT Solutions for All Subjects

This article delves into the concept of electronegativity, a crucial topic in the Class 11 Chemistry curriculum under the chapter "Classification of Elements and Periodic Table." Understanding electronegativity is essential not only for academic assessments but also for competitive examinations such as JEE Main, NEET, SRMJEE, BITSAT, WBJEE, BCECE, and others. Electronegativity plays a significant role in determining the nature of chemical bonds, influencing molecular polarity, and predicting the reactivity of substances. Given its importance, a thorough grasp of this concept is beneficial for students aiming to excel in these examinations.

Related Topics Link

• Electronic Configuration of First 30 Elements
• Electron Gain Enthalpy
  
• Homologous Series
  
• Atomic radius in periodic table in basic chemistry
  
• Classification of Elements in Modern Periodic Table
• 118 elements, their symbols and their atomic number

Unveiling the Power of Electronegativity

Electronegativity

The tendency of an atom to attract the shared pair of electrons towards itself is called electronegativity. It is a relative quantity. This concept was introduced in 1932 by Pauling. It has no units. Fluorine is the most electronegative element known so far and its value is arbitrarily assigned as 4.0. In moving from left to right in a period, the electronegativity increases while in moving from the top to bottom in a group, the electronegativity decreases.

Factors affecting Electronegativity

Several key influences determine an atom’s electronegativity:

First, as atomic size increases, electronegativity declines because outer electrons are farther from the nucleus and less strongly attracted .

Next, a higher effective nuclear charge—due to more protons or reduced shielding—boosts electronegativity by increasing the nucleus’s pull on valence electrons.

Lastly, an element’s oxidation state affects its electronegativity. Atoms in higher oxidation states have fewer electrons shielding the nucleus and a smaller radius, so they attract bonding electrons more strongly—as seen, for instance, with Fe³⁺ being more electronegative than Fe²⁺ .

Read more :

• NCERT notes Class 11 Chemistry Chapter 3 Classification of Elements and Periodicity in Properties
• NCERT solutions for Class 11 Chemistry Chapter 3 Classification of Elements and Periodicity in Properties
• NCERT Exemplar Class 11 Chemistry Solutions Chapter 3 Classification of Elements and Periodicity in Properties

Recommended topic video on (Electronegativity)

Some Solved Examples

Example 1: The correct option concerning the Pauling electronegativity values of the elements is :

1) Ga < Ge

2) P > S

3) Si < Al

4) Te > Se

Solution: Electronegativity -A qualitative measure of the ability of an atom in a chemical compound to attract shared electrons is electronegativity.- wherein It is not a measurable quantity.

Electronegativity and non-metallic character -

Non-metallic elements have a strong tendency to gain electrons. Therefore electronegativity is directly related to non-metallic properties of elements.

- wherein

Electronegativity ∝ non-metallic property
Correct order
(1) Ga<Ge
(2) Si<Al
(3) P<S
(4) Te<Se

Hence, the answer is the option (1).

Example 2: The electronegativity of an element is related to ionization energy and

1) Atomic radii

2) Electron affinity

3) Ionic radii

4) Nucleus

Solution: The electronegativity depends upon the sum of Ionisation and Electron Affinity.

The electronegativity of any given element is not constant. It varies depending on the elements to which it is bound.

Though it is not measurable, it does provide a means to predict the nature of the force that holds atoms.

More electronegative elements will have positive Electron affinity due to electron attraction as well as more Ionisation Energy.

Hence, the answer is the option (2).

Example 3: Which of the following is the most electronegative?

1) Be

2) B

3) C

4) N

Solution: Electronegativity generally increases across a period from left to right.

e.g. from lithium to fluorine.

N is the most electronegative element among the given elements as we move from left to right in a period, the electronegativity increases.

Hence, the answer is the option (4).

Example 4: Which one of the following elements is most electronegative?

1) Fluorine

2) Sulphur

3) Oxygen

4) Bromine

Solution: As we learned, Variation of electronegativity along group

Electronegativity generally decreases down a group in the periodic table.

- wherein

e.g. from fluorine to astatine.

Electronegativity decreases as we move down the group and increases as we move from left to right in a period.

Hence, the answer is the option (1).

Example 5: Which of the following is most electronegative?

1) Carbon

2) Silicon

3) Lead

4) Tin

Solution: Electronegativity - The electronegativity of any element decreases down the group. Thus carbon is the most electronegative element.

Hence, the answer is the option (1).

Variation of Electronegativity

• In moving from top to bottom in a group the atomic size increases thus the force of attraction decreases and hence the electronegativity decreases.

• In moving from left to right in a period, the atomic size decreases and effective nuclear charge increases, thus the electronegativity increases.

• Halogens are the most electronegative elements and fluorine has the highest electronegativity.

• For transition elements, the electronegativity values vary between 1.1 to 1.3.

• Metals have lower electronegativity values while non-metals have higher electronegativity values.

Example 6: Two elements with electronegativities are 1.2 and 3.2 respectively, the bond formed between them will be:

1) Covalent

2) Metallic

3) Ionic

4) None

Solution: Electronegativity - Nature of Bond: The nature of the bond can be estimated from the electronegativity values of respective atoms.

(i) When the electronegativity difference between two atoms, i.e., M_A—M_B = 0, then the bond is purely covalent.

(ii) When M_A - M_B is small, the bond is polar but covalent.

(iii) When M_A - M_B is 1.9, the bond is 50% ionic and 50% covalent.

(iv) When M_A—M_B is greater than 1.9, the bond is more ionic and less covalent.

The percentage of ionic character is given by the following formula:

Percentage of ionic character = 16(M_A - M_B) + 3.5(MA - MB)2

M_A and M_B are the electronegativities of two bonded atoms, i.e., A and B.

The electronegativity difference between the constituent atoms must be greater than 1.9 to form the ionic bond.

Hence, the answer is the option (3).

Example 7: On going from right to left in a period in the periodic table the electronegativity of the elements
1) Increases

2) Decreases

3) Remain unchanged

4)Decreases first then increases

Solution: As we learned, Electronegativity is the ability of any atom to attract a bonded pair of electrons towards itself. It increases on moving from left to right along a period as the size of the atom decreases.

Hence, the answer is the option (1).

Practice more Questions from the link given below:

Importance of Electronegativity

The following predictions can be made out of the information on the electronegativities of atoms.

• Nature of Element: The elements with lower electronegativity values are metals while the elements with higher electronegativity values are non-metals. The elements with intermediate electronegativity values are metalloids. Fluorine has the highest electronegativity value, thus it is the most non-metallic element. Similarly, cesium has the lowest electronegativity value, thus it is the most metallic element.

• Nature of Oxides: The nature of the oxides formed by the elements can also be predicted by electronegativity. When the MO - MA difference is lower, then the oxide is acidic but when this difference MO - MA is large, then the oxide is basic. MO here is the electronegativity of oxygen.

Also check-

• NCERT Exemplar Class 11th Chemistry Solutions
• NCERT Exemplar Class 12th Chemistry Solutions
• NCERT Exemplar Solutions for All Subjects

Conclusion

Electronegativity measures how strongly an atom attracts electrons in a chemical bond, directly influencing whether the bond is nonpolar, polar covalent, or ionic. Differences in electronegativity between atoms create charge separation—larger differences result in greater polarity and may even form ions . This polarity governs key chemical behaviors: polar molecules tend to dissolve in polar solvents (“like dissolves like”), exhibit higher boiling and melting points, and often engage in stronger intermolecular forces. Moreover, electronegativity affects acidity—atoms that strongly attract electrons stabilize negative charges in conjugate bases, enhancing acid strength. In short, electronegativity not only defines bond type and molecular polarity but also underpins solubility, thermal properties, and acid–base behavior.