CBSE Class 10 Chapter 5 Periodic Classification of Elements Notes

According to the CBSE Syllabus 2023-24, this chapter has been removed from NCERT Class 10 Science textbook.

CBSE Class 10 Science Notes Chapter 5 Periodic Classification of Elements

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Periodic element classification is the process of categorising elements into various classes. This strategy involves grouping like things together and separating those that are unrelated by comparing the characteristics of several elements. It aids in our comprehension of how various compounds combine to form various elements.

For a complete chapter summary on Periodic Classification of Elements, watch the below video

Introduction to Periodic Classification of Elements

Why Classification?

Without the classification of elements, it would be extremely difficult and time-consuming to individually study the chemistry of all the elements. Hence, to simplify and systematize the study of elements and their compounds, they are classified into groups and periods.

Early Attempts of Classification

The chemical and physical characteristics that scientists had noticed served as the foundation for the early attempts to classify elements. We compared a few reactions using well-known substances and elements.

They were arranged according to their atomic weights. They tried to study the periodicity of the properties as the atomic weight increased in order to categorise them into groups.

The law of octaves was then put forth after the law of triads. These laws were proposed by Doberneiner, Chancourtois, and Newlands, who also created several tables.

Early Models of Periodic Table

Dobereiner’s Triads

Dobereiner arranged a group of three elements with similar properties in the order of increasing atomic masses and called it a triad. He showed that the atomic mass of the middle element is approximately the arithmetic mean of the other two. But, Dobereiner could identify only the following three triads from the elements known at that time.

Newlands’ Law of Octaves

When the elements are arranged according to increasing atomic masses, the physical and chemical properties of every eighth element are similar to that of the first.
Newlands compared these octaves to the series of eight notes of a musical scale.

Assumptions and Limitations:

1. The law was applicable for elements with atomic masses up to 40.
2. Properties of new elements discovered did not fit into the law of octaves.
3. In a few cases, Newlands placed two elements in the same slot to fit elements in the table.
4. He also grouped unlike elements under the same slot.

Mendeleev’s Periodic Table and Law

The physical and chemical characteristics of elements are a periodic function of their atomic masses, in accordance with Mendeleev’s Periodic Law. Mendeleev organised the elements in ascending order of their atomic masses after classifying them according to their atomic masses.

The physical and chemical properties of elements are periodic functions of their atomic weights.

Features of Mendeleev’s Periodic Table

● Twelve horizontal rows, which were condensed to 7, known as periods.
● Eight vertical columns known as groups.
● Groups I to VII are subdivided into A and B subgroups.
● Group VIII doesn’t have any subgroups and contains three elements in each row.
● Elements in the same group exhibit similar properties.

Achievements of Mendeleev’s Periodic Table

1. A systematic study of elements: Elements with similar properties were grouped together, which made the study of their chemical and physical properties easier.
2. Correction of atomic masses: The placement of elements in Mendeleev’s periodic table helped in correcting the atomic masses of certain elements. For example, the atomic mass of beryllium was corrected from 13.5 to 9. Similarly, atomic masses of indium, gold, platinum etc., were also corrected.
3. Prediction of properties of yet-to-be-discovered elements: Eka-boron, eka-aluminium and eka-silicon were the names given to yet-to-be-discovered elements. The properties of these elements could be predicted accurately from the elements that belonged to the same group. These elements, when discovered, were named scandium, gallium, and germanium, respectively.
4. Placement of noble gases: When discovered, they were placed easily in a new group called the zero group of Mendeleev’s table without disturbing the existing order.

Limitations of Mendeleev’s Periodic Table

1. Position of hydrogen: Hydrogen resembles both the alkali metals (IA) and the halogens (VIIA) in properties, so Mendeleev could not justify its position.
2. Position of isotopes: Atomic weights of isotopes differ, but they were not placed in different positions in Mendeleev’s periodic table.
3. Anomalous pairs of elements: Cobalt (Co) has higher atomic weights but was placed before Nickel (Ni) in the periodic table.
4. Placement of like elements in different groups: Platinum (Pt) and Gold (Au) has similar properties but were placed in different groups.
5. Cause of periodicity: He could not explain the cause of periodicity among the elements.

For more information on the Introduction to Periodic Table, watch the below video

To know more about Mendeleev’s Periodic Table, visit here.

The Modern Periodic Table

In the past, scientists believed that an element’s qualities were periodic functions of its atomic mass. Mendeleev arranged 63 elements in a vertical column named groups and horizontal rows called periods based on this idea.

This approach was disregarded since it was unable to account for the locations of several elements, rare earth metals, and isotopes. Henry Moseley, a scientist, corrected these flaws and proposed the modern periodic table and periodic rule.

Modern Periodic Law

The physical and chemical properties of elements are the periodic function of their atomic numbers.
Cause of periodicity – It is due to the repetition of the same outer shell electronic configuration at a certain regular interval.

For more information on The Modern Periodic Table, watch the below video

To know more about Modern Periodic Table, visit here.

Features of Modern Periodic Table

The vertical columns and horizontal rows that make up the long version of the periodic table are called groups and periods, respectively.

• According to their increasing atomic numbers, elements are organised.
• The contemporary periodic table divides the elements into 7 periods and 18 groups.
• Vertical columns are known as groups and horizontal rows are known as periods.
• Depending on how many atomic shells each element has, it is classified into periods.
• The first period, which only has two elements—hydrogen and helium—is the shortest.
• The sixth period in the periodic table is regarded as the longest period. It contains substances ranging from Radon to Cesium.
• The seventh period is a blank period.
• Actinides and Lanthanides are included at the bottom of the periodic table.

Periods in Modern Periodic Table

Elements present in the same period have the same number of shells which is equal to the period number. A period is a row of the periodic table that is horizontal. The periodic table contains seven periods, each of which starts at the left.

On moving from left to right in a given period, the number of electrons in the valence shell increases from one to eight while the number of shells remains the same.

Number of Elements in a Period

The first period contains only two elements, 1H and 2He, and is known as the shortest period.

The second period (₃Li to ₁₀Ne) and the third period (₁₁Na to ₁₈Ar) contain 8 elements each and are known as short periods.

The fourth period (₁₉K to ₃₆Kr) and the fifth period (₃₇Rb to ₅₄Xe) contain 18 elements each and are called long periods.

The sixth period contains 32 elements (₅₅Cs and ₈₆Rn) and is also known as the longest period.

The seventh period is an incomplete period.

(After the recent discoveries of the new elements and their addition to the periodic table, the seventh period is officially complete)

For more information on Periodic Table of Elements, watch the below video

Groups in Modern Periodic Table

The modern periodic table contains 18 vertical columns known as groups.

Group 1 elements are known as alkali metals.
Group 2 elements are known as alkaline earth metals.
Group 15 elements are known as pnicogens.
Group 16 elements are known as chalcogens.
Group 17 elements are known as halogens.
Group 18  elements are known as noble gases.

Alkali Metals

The elements in the first group, lithium (Li), sodium (Na), potassium (K), rubidium (Rb), caesium (Cs), and francium (Fr) are called alkali metals.
They were given the name because they all react with water to form alkalis.
The alkali metals are all shiny, soft, highly reactive solids at standard temperature and pressure and readily lose their outermost electron to form cations with charge +1.
Number of valence electrons = 1

Alkali Earth Metals

Halogens

Noble Gases

Classification of Modern Periodic Table

Metals

Non-Metals

Metalloids

Trends in the Modern Periodic Table

Trends in the Modern Periodic Table

Variation of Valency

Variation of Atomic Size

Atomic size or radii: It is defined as the distance from the centre of the nucleus to the valence shell of the atom.

Along the period – Atomic radius decreases because effective nuclear charge increases by one unit, and it pulls valence electrons or the electron cloud closer to the nucleus.
Down the group – Atomic radius increases because new shells are added; hence, the distance between the nucleus and valence electrons or the electron cloud increases.

Variation of Metallic Properties

Along the period – The metallic character decreases because the tendency to lose valence electrons decreases due to increasing nuclear charge.
Down the group – As the distance between the nucleus and the outermost electron increases, nuclear pull decreases. This increases the tendency of an atom to lose valence electron/s; hence metallic character increases.

Variation of Non-Metallic Properties

Along the period – Non-metallic character increases as the tendency to gain electrons in the valence shell increases due to increasing nuclear charge.
Down the group – As the distance between the nucleus and valence shell increases, nuclear pull decreases. This decreases the tendency of an atom to gain an electron in its valence shell; hence non-metallic character decreases.

Variation of Electronegativity

Along the period – Electronegativity increases as the tendency to gain electrons in the valence shell increases due to increasing nuclear charge.
Down the group – As the distance between the nucleus and valence shell increases, nuclear pull decreases. This decreases the tendency of an atom to gain an electron; hence electronegativity decreases.

Know more on Periodic Table by watching the below video

To know more about Trends in the Modern Periodic Table, visit here.

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