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According to Mendeleev’s periodic law, the physical and chemical properties of elements are periodic functions of their.
- a)Atomic n umbers
- b)Atomic weights
- c)Number of electrons
- d)Number of protons
Correct answer is option 'B'. Can you explain this answer?
Most Upvoted Answer
According to Mendeleev’s periodic law, the physical and chemical...
Mendeleev’s Periodic Law and Atomic Weights
Mendeleev's Periodic Law states that the properties of elements are periodic functions of their atomic weights. This means that when elements are arranged in order of increasing atomic weight, certain sets of properties recur periodically.
Mendeleev's Periodic Law states that the properties of elements are periodic functions of their atomic weights. This means that when elements are arranged in order of increasing atomic weight, certain sets of properties recur periodically.
- Elements' Properties: Mendeleev noticed that there was a periodic recurrence of elements with similar physical and chemical properties. This led him to formulate the periodic law.
- Atomic Weights: Mendeleev used atomic weights (now we use atomic numbers due to the discovery of isotopes) to arrange elements into the periodic table. He found that elements with similar properties had either similar atomic weights or weights that increased in a regular manner.
- Element Arrangement: Mendeleev arranged elements in order of increasing atomic weight and grouped them by their properties. This resulted in a table where elements with similar properties fell into vertical groups.
- Periodicity: The repetition of properties after certain regular intervals when elements are arranged in increasing order of atomic weight is called periodicity. This is the fundamental concept behind Mendeleev's Periodic Law and the Periodic Table.
However, it's essential to note that the Modern Periodic Law, proposed by Moseley, is based on atomic numbers, not atomic weights. This is because isotopes (atoms of the same element with different numbers of neutrons, hence different atomic weights) possess identical chemical properties.
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According to Mendeleev’s periodic law, the physical and chemical...
Understanding Mendeleev's Periodic Law
Mendeleev's periodic law is foundational to the study of chemistry and the organization of elements. It states that the physical and chemical properties of elements are periodic functions of their atomic weights. Here’s a deeper look into why option 'B' is correct:
Atomic Weights and Properties
- Definition: Atomic weight refers to the weighted average mass of an element's isotopes, measured in atomic mass units (amu).
- Periodic Trends: Mendeleev observed that when elements were arranged in order of increasing atomic weight, elements with similar properties appeared at regular intervals or periods.
Examples of Periodicity
- Group Similarities: Elements in the same group (column) of the periodic table display similar chemical properties due to their comparable atomic weights, which influence electron configurations.
- Physical Properties: Trends such as melting points, boiling points, and reactivity can often be predicted based on the atomic weights of the elements in a given group.
Limitations of Atomic Number
- Historical Context: At the time Mendeleev formulated his periodic law, atomic numbers were not yet defined. Thus, he based his observations on atomic weights.
- Modern Understanding: While modern periodic law emphasizes atomic numbers as the organizing principle, Mendeleev’s work laid the groundwork for this understanding.
Conclusion
Mendeleev's assertion that properties are periodic functions of atomic weights holds true within the context of his time. It highlights the relationship between atomic mass and chemical behavior, providing a foundational framework for the development of the modern periodic table. Understanding this historical perspective enriches our appreciation of elemental chemistry.
Mendeleev's periodic law is foundational to the study of chemistry and the organization of elements. It states that the physical and chemical properties of elements are periodic functions of their atomic weights. Here’s a deeper look into why option 'B' is correct:
Atomic Weights and Properties
- Definition: Atomic weight refers to the weighted average mass of an element's isotopes, measured in atomic mass units (amu).
- Periodic Trends: Mendeleev observed that when elements were arranged in order of increasing atomic weight, elements with similar properties appeared at regular intervals or periods.
Examples of Periodicity
- Group Similarities: Elements in the same group (column) of the periodic table display similar chemical properties due to their comparable atomic weights, which influence electron configurations.
- Physical Properties: Trends such as melting points, boiling points, and reactivity can often be predicted based on the atomic weights of the elements in a given group.
Limitations of Atomic Number
- Historical Context: At the time Mendeleev formulated his periodic law, atomic numbers were not yet defined. Thus, he based his observations on atomic weights.
- Modern Understanding: While modern periodic law emphasizes atomic numbers as the organizing principle, Mendeleev’s work laid the groundwork for this understanding.
Conclusion
Mendeleev's assertion that properties are periodic functions of atomic weights holds true within the context of his time. It highlights the relationship between atomic mass and chemical behavior, providing a foundational framework for the development of the modern periodic table. Understanding this historical perspective enriches our appreciation of elemental chemistry.
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