Anand Classes provides comprehensive study material on Electronegativity and its relation to Metallic and Non-Metallic Character for Class 11, NEET, and JEE preparation. Understanding electronegativity trends across the periodic table is essential to predict the chemical behavior of elements, bond formation, and the distinction between metals, non-metals, and metalloids. This concept also helps students in mastering important topics like periodic properties, bond polarity, and the classification of elements. Click the print button to download study material and notes.
Electronegativity and Metallic / Non-Metallic Character
Electronegativity is one of the most important periodic properties of elements because it is closely related to the nature of bonding and to the metallic or non-metallic character of elements.
🔹 Relation Between Electronegativity and Metallic / Non-Metallic Properties
- Non-Metallic Character
- Non-metals have a strong tendency to gain electrons in order to complete their octet.
- A higher electronegativity means a stronger ability to attract electrons.
- Thus, electronegativity is directly proportional to non-metallic character.
- Example: Fluorine (EN = 4.0) is the most non-metallic element.
- Metallic Character
- Metals have a strong tendency to lose electrons to form cations.
- A lower electronegativity means a weaker pull on electrons.
- Thus, electronegativity is inversely proportional to metallic character.
- Example: Cesium (EN = 0.7) is one of the most metallic elements.
🔹 Periodic Trends
- Across a Period (Left → Right):
- Electronegativity increases because:
- Atomic size decreases.
- Effective nuclear charge increases.
- As a result:
- Non-metallic character increases.
- Metallic character decreases.
- Example:
- Sodium (Na, EN = 0.9) → Metallic
- Chlorine (Cl, EN = 3.0) → Non-metallic
- Electronegativity increases because:
- Down a Group (Top → Bottom):
- Electronegativity decreases because:
- Atomic size increases.
- Shielding effect reduces nuclear pull on bonding electrons.
- As a result:
- Non-metallic character decreases.
- Metallic character increases.
- Example:
- Fluorine (EN = 4.0) → Strongly non-metallic
- Iodine (EN = 2.4) → Less non-metallic
- Electronegativity decreases because:
🔹 General Rule of Classification
- Elements with Electronegativity ≥ 2.0 → Generally Non-metals
- Elements with Electronegativity < 2.0 → Generally Metals
- Elements with intermediate values (~2.0) → Metalloids (showing both metallic and non-metallic properties).
🔹 Importance in Bond Formation
Electronegativity is not only linked with metallic and non-metallic character but also predicts the type of chemical bond:
- Large difference in EN (≥ 1.7) → Ionic bond
- Example: NaCl (Na = 0.9, Cl = 3.0 → ΔEN = 2.1)
- Moderate difference in EN (0.4 – 1.7) → Polar covalent bond
- Example: HCl (H = 2.1, Cl = 3.0 → ΔEN = 0.9)
- Small or negligible difference in EN (≤ 0.4) → Non-polar covalent bond
- Example: Cl₂ (both atoms have same EN = 3.0 → ΔEN = 0)
🔹 Key Examples
- Fluorine (EN = 4.0) → Highest EN, most non-metallic.
- Oxygen (EN = 3.5) → Strong non-metallic nature.
- Cesium (EN = 0.7) → Lowest EN, highly metallic.
- Metalloids (e.g., Si, As, Sb) → Intermediate EN values, showing both properties.
Metallic vs Non-Metallic Character and Electronegativity
| Property | Metals | Non-Metals |
|---|---|---|
| Electronegativity | Low (usually < 2.0) | High (usually ≥ 2.0) |
| Tendency | Lose electrons (form cations) | Gain electrons (form anions) |
| Relation with EN | Inversely proportional (low EN = more metallic) | Directly proportional (high EN = more non-metallic) |
| Across a Period (→) | Metallic character decreases as EN increases | Non-metallic character increases as EN increases |
| Down a Group (↓) | Metallic character increases as EN decreases | Non-metallic character decreases as EN decreases |
| Bonding Nature | Form ionic bonds (with non-metals) | Form covalent bonds (with other non-metals) |
| Examples | Na (0.9), K (0.8), Cs (0.7) | O (3.5), F (4.0), Cl (3.0) |
✅ Quick Points:
- Fluorine (EN = 4.0) → Most non-metallic element.
- Cesium (EN = 0.7) → Most metallic element.
- Elements with intermediate EN (~2.0) → Often metalloids (e.g., Si, As, Sb).
✅ In summary:
- High EN → Non-metallic nature.
- Low EN → Metallic nature.
- EN trends across the periodic table directly explain the distribution of metals, non-metals, and metalloids.
FAQs on Electronegativity and Metallic / Non-Metallic Character
Q1. How is electronegativity related to metallic and non-metallic character?
Electronegativity is directly proportional to non-metallic character and inversely proportional to metallic character.
Q2. Why do non-metals have higher electronegativities?
Non-metals have a strong tendency to gain electrons to complete their octet. This requires a strong attraction for electrons, so their electronegativity is high.
Q3. Why do metals have low electronegativities?
Metals prefer to lose electrons and form cations. Since they do not attract electrons strongly, their electronegativity values are low.
Q4. How does electronegativity vary across a period?
Electronegativity increases across a period (left → right) due to decreasing atomic size and increasing nuclear charge. As a result, non-metallic character increases and metallic character decreases.
Q5. How does electronegativity vary down a group?
Electronegativity decreases down a group due to increasing atomic size and shielding effect. Hence, metallic character increases and non-metallic character decreases.
Q6. Which element is the most non-metallic? Why?
Fluorine (EN = 4.0) is the most non-metallic element because it has the highest electronegativity in the periodic table.
Q7. Which element is the most metallic? Why?
Cesium (EN = 0.7) is one of the most metallic elements because it has the lowest electronegativity and loses electrons very easily.
Q8. How can electronegativity values classify elements as metals or non-metals?
- Elements with EN ≥ 2.0 → Non-metals
- Elements with EN < 2.0 → Metals
- Elements with values around 2.0 → Metalloids
Q9. How does electronegativity help in predicting bond type?
- Large EN difference (≥ 1.7): Ionic bond (e.g., NaCl)
- Moderate EN difference (0.4 – 1.7): Polar covalent bond (e.g., HCl)
- Small or zero EN difference (≤ 0.4): Non-polar covalent bond (e.g., Cl₂)
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