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Merits and Demerits of Mendeleev's Periodic Table Video Lecture - Class 10

Q: 1. What are the merits of Mendeleev's Periodic Table?

Ans. The merits of Mendeleev's Periodic Table include:- Systematic arrangement: Mendeleev arranged the elements in a systematic order based on their atomic masses, allowing for easy identification and classification of elements.- Prediction of new elements: Gaps were left in the periodic table for undiscovered elements, and Mendeleev successfully predicted the properties of these elements before they were even discovered.- Grouping of elements: Elements with similar properties were grouped together, which helped in understanding the similarities and trends in chemical behavior.- Basis for periodic trends: Mendeleev's table laid the foundation for understanding periodic trends like atomic size, valency, and electronegativity.- Practical applications: The periodic table provided a comprehensive framework for organizing and studying elements, leading to advancements in chemistry and various practical applications.

Q: 2. What are the demerits of Mendeleev's Periodic Table?

Ans. The demerits of Mendeleev's Periodic Table include:- Placement of isotopes: Mendeleev's table did not consider the existence of isotopes, which are atoms of the same element with different atomic masses. As a result, isotopes were placed separately in the periodic table, disrupting the pattern.- Inaccurate atomic masses: The atomic masses of some elements listed in Mendeleev's table were not accurately known at that time, leading to discrepancies in the arrangement.- Incomplete ordering of elements: Some elements did not fit into Mendeleev's periodic table as they did not follow the pattern of increasing atomic masses. This led to inconsistencies and gaps in the table.- No explanation for periodic trends: Although Mendeleev's table identified periodic trends, it did not provide a theoretical explanation for these trends, leaving them unexplained.- Neglect of noble gases: Mendeleev's table did not include noble gases as they were not discovered during his time. This omission hindered the understanding of their unique properties.

FAQs on Merits and Demerits of Mendeleev's Periodic Table Video Lecture - Class 10

1. What are the merits of Mendeleev's Periodic Table?

Ans. The merits of Mendeleev's Periodic Table include: - Systematic arrangement: Mendeleev arranged the elements in a systematic order based on their atomic masses, allowing for easy identification and classification of elements. - Prediction of new elements: Gaps were left in the periodic table for undiscovered elements, and Mendeleev successfully predicted the properties of these elements before they were even discovered. - Grouping of elements: Elements with similar properties were grouped together, which helped in understanding the similarities and trends in chemical behavior. - Basis for periodic trends: Mendeleev's table laid the foundation for understanding periodic trends like atomic size, valency, and electronegativity. - Practical applications: The periodic table provided a comprehensive framework for organizing and studying elements, leading to advancements in chemistry and various practical applications.

2. What are the demerits of Mendeleev's Periodic Table?

Ans. The demerits of Mendeleev's Periodic Table include: - Placement of isotopes: Mendeleev's table did not consider the existence of isotopes, which are atoms of the same element with different atomic masses. As a result, isotopes were placed separately in the periodic table, disrupting the pattern. - Inaccurate atomic masses: The atomic masses of some elements listed in Mendeleev's table were not accurately known at that time, leading to discrepancies in the arrangement. - Incomplete ordering of elements: Some elements did not fit into Mendeleev's periodic table as they did not follow the pattern of increasing atomic masses. This led to inconsistencies and gaps in the table. - No explanation for periodic trends: Although Mendeleev's table identified periodic trends, it did not provide a theoretical explanation for these trends, leaving them unexplained. - Neglect of noble gases: Mendeleev's table did not include noble gases as they were not discovered during his time. This omission hindered the understanding of their unique properties.

3. How did Mendeleev predict the properties of undiscovered elements?

Ans. Mendeleev predicted the properties of undiscovered elements by leaving gaps in his periodic table for these elements. He noticed that certain patterns and trends in the properties of known elements repeated periodically. Based on these patterns, he made predictions about the properties of elements that were yet to be discovered. Mendeleev used the properties of elements in the same group or period to estimate the properties of the missing elements. His predictions were remarkably accurate, and when these elements were discovered later, their properties matched the ones predicted by Mendeleev.

4. What is the significance of grouping elements in the periodic table?

Ans. Grouping elements in the periodic table is significant because it helps in understanding the similarities and trends in the chemical behavior of elements. Elements within the same group often have similar chemical properties due to the same number of valence electrons. This similarity allows for the prediction of similar reactions, reactions with other elements, and the formation of compounds. Grouping also helps in identifying the physical properties and trends within a group, such as atomic radius, ionization energy, and electronegativity. The periodic table's arrangement based on groups facilitates the study and organization of elements, aiding in the understanding of their properties and behavior.

5. How did Mendeleev's periodic table contribute to practical applications?

Ans. Mendeleev's periodic table contributed to numerous practical applications in the field of chemistry. The systematic arrangement of elements helped in the discovery and development of new elements with specific properties. This, in turn, led to the synthesis and production of various useful materials, such as alloys, polymers, and compounds. The periodic table also facilitated the understanding of the reactivity and behavior of different elements. This knowledge allowed scientists to design and optimize chemical reactions, leading to the development of efficient industrial processes. Additionally, the periodic table aided in the identification and analysis of elements in various samples, supporting fields like forensic science, environmental analysis, and pharmaceutical research.

Text Transcript from Video

[Music]
measured and demerit of Mendeleev
periodic table merit of Mendeleev
periodic table mainly was the first
scientist so successfully classified all
known elements he anticipated the
discovery of more elements and made
provision to accommodate them by leaving
blank spaces manganese periodic tables
could be successfully used to predict
the properties of undiscovered animals
for example Mendeleev predicted the
discovery and properties of ten
undiscovered gallium and named it as
acre aluminum the values of atomic
weight density
melting point valency method of
discovery and formula of oxide predicted
by mentally for eco aluminium are found
to be very close to that of gallium it
was so well structured that when noble
gases were discovered later every one of
them could be accommodated in many
leaves periodic table in a separate
group without causing any immediate
changes in the tables demerit of
Mendeleev periodic tables Mendeleev
could not assign a correct position to
hydrogen in the periodic table as
hydrogen resembles alkali as well as
halogen
isotopes of the same element have
different atomic muscle tense
each of them should have been placed at
a different position in the periodic
table but the isotope being chemically
similar had to be placed at the same
position in the periodic table at
certain places and element of higher
atomic mass was placed before an element
of lower mass so that elements with
similar properties fell in the same
group this tube goes against mainly
periodic law example cobalt with atomic
mass fifty eight point nine is placed
before nickel with atomic mass fifty
eight point seven in the fourth period
till two goes against Mendeleev periodic
law some elements placed in the same
group had different properties example
manganese which is a metal is placed
with halogen which are nonmetals having
entirely different properties
[Music]

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