Modern Periodic Table

Modern Periodic Table

Father of Periodic Table – Mendeleev

Classification of Elements

The arrangement of the known elements in certain groups in such a way so that the elements with similar properties are grouped together is known as classification of elements.

Genesis of Periodic Classification

1. Lavoisier

Classified the elements into metals and non-metals.

2. Dobereiner's Triads

In 1829, Dobereiner, a German chemist arranged certain elements with similar properties in groups of three in such a way that the atomic mass of the middle element was nearly the same as the average atomic masses of the first and third elements.

Atomic mass of sodium =

3. Newland's Law of Octaves

In 1866, John Newlands, an English chemist, proposed the law of octaves by stating that,
“When elements are arranged in order to increasing atomic masses, every eighth element has properties similar to the first, just like musical notes.”

But this generalization was also rejected because it could not be extended to the elements with atomic mass more than 40.

4. Lother–Mayer’s Atomic Volume Curve

In 1869, Lother Mayer plotted a graph between atomic volume of the elements and their atomic mass and he pointed that the elements with similar properties occupy similar position in the curve.

5. Mendeleev’s Periodic Law

The physical and chemical properties of the elements are the periodic function of their atomic masses.

Mendeleev arranged the elements known at that time in increasing order of atomic masses and the arrangement was periodic table.

In the periodic table:

• Horizontal line is called periods.

• Vertical line is called group.

In Mendeleev’s periodic table:

• Period – 7

• Group – 9 (I, II, III, IV, V, VI, VII, VIII, Zero)

6. Modern Periodic Law

Modern periodic law was given by Moseley.

According to Moseley:
“The physical and chemical properties of the elements are the periodic function of their atomic numbers.”

In modern periodic table:

• Period – 7

• Group – 18

Classification of Modern Periodic Table

Modern periodic table is classified as:
(i) s–block
(ii) p–block
(iii) d–block
(iv) f–block

• s–block: Alkali & Alkaline earth metals.

• p–block: Chalcogen, Picogens, Halogens and inert gases.

• d–block: Transition elements.

• f–block: Inner transition elements.

Periodic Properties

(i) Atomic Radii

The distance from the centre of the nucleus of the outermost shell containing electrons called atomic radius.

It is not possible to measure the absolute value of atomic radius of an element. However, it may be expressed in three different forms: covalent radii, metallic radii, van der wall radii.

Van der wall radii > metallic radii > covalent radii

(ii) Ionic Radii

The effective distance from the centre of nucleus of the ion upto which it exerts its influence on the electron cloud is called ionic radii.

Anionic radii > atomic radii > cationic radii

(iii) Ionization Potential (I.P.)

The amount of energy required to remove an electron from isolated gaseous atom is called Ionization Potential (I.P.) or Ionization Energy (I.E.)

A (g) – e + Energy required (I.P.) → A⁺ (g)

(iv) Electron Affinity (En)

The energy released during addition of an extra electron in isolated gaseous atom is called Electron Affinity.

A (g) + e → A⁻ (g) + Energy released

Chlorine (Cl) has highest Ea value.

(v) Electronegativity (Ea)

The relative electron attracting tendency of its atom for a shared pair of electrons in a chemical bond is called electronegativity.

F is the most electronegative atom.

En value > 1.7 → Ionic compound
En value < 1.7 → Polar covalent compound
En value = 0 → Nonpolar compound

(vi) Lattice Energy

The amount of energy released during formation of one mole of ionic compound from its constituent ions is called Lattice energy.

(vii) Hydration Energy

The amount of energy released during dissolution of one mole of compound into water is called hydration energy.

• If hydration energy > lattice energy, then compound is soluble in water.

• If hydration energy < lattice energy, then compound is insoluble in water.

Final Thoughts

The periodic table, developed by Dmitri Mendeleev, organizes elements based on their properties and atomic structure.

Early scientists like Lavoisier, Dobereiner, and Newlands made initial attempts to classify elements, leading to Mendeleev’s periodic law, which stated that the properties of elements are a periodic function of their atomic masses.

Later, Moseley refined it using atomic numbers, giving rise to the modern periodic law. The table is divided into s, p, d, and f blocks, representing different types of elements. Key periodic properties—such as atomic and ionic radii, ionization potential, electron affinity, and electronegativity—help explain the chemical behavior and reactivity of elements.