Classification of Element & Periodicity in Properties Class 11 Full Chapter in 60 Minutes ⌛
Vedantu JEE Made Ejee・2 minutes read
The session will cover exceptions, a surprise DP, the Periodic Classification of Elements, and the importance of arranging elements by atomic number. Attendees are urged to listen attentively, take notes, and engage with the material while focusing on atomic numbers, periods, and electron configurations.
Insights
- The study session must be completed within 60 minutes due to traffic constraints, focusing on revising an important class 11th chapter. Attendees are urged to listen attentively, take notes, and engage with the material, which covers the history of the Periodic Classification of Elements, including Sir Dobereiner's grouping based on atomic mass, the New Land classification method, and the significance of arranging elements by atomic number for the modern periodic table structure.
- Understanding the period of an element based on its atomic number is crucial, with the sequence of filling electrons in D elements following a specific order. Factors like effective nuclear charge, shielding by inner electrons, and trends in ionization energy and electron affinity play a significant role in determining atomic properties and bonding characteristics, impacting the nature of elements and their interactions in chemical reactions.
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Recent questions
What is the importance of arranging elements by atomic number?
Arranging elements by atomic number is crucial as it leads to the modern periodic table structure. This organization allows for a clear understanding of an element's properties, trends, and behavior based on its atomic number. By following this order, elements with similar chemical properties are grouped together, aiding in the prediction of an element's characteristics and behavior.
How does effective nuclear charge impact atomic radius?
Effective nuclear charge influences atomic radius by affecting the attraction of valence electrons to the nucleus. As the effective nuclear charge increases, the pull on valence electrons becomes stronger, causing the atomic radius to decrease. However, noble gases in group 17 are exceptions to this trend, as their atomic radius remains larger despite an increase in effective nuclear charge.
What is the relationship between ionization energy and atomic size?
Ionization energy is inversely related to atomic size, meaning that larger atoms require more energy to remove electrons compared to smaller atoms. This is because the electrons in larger atoms are farther from the nucleus, experiencing weaker attraction, making them easier to remove. Exceptions to this trend can be observed in certain groups like group 13 and 14, where anomalies in ionization energy values occur.
How does electron affinity vary across the periodic table?
Electron affinity, the tendency of an element to attract electrons, varies across the periodic table due to factors like atomic radius, nuclear charge, and penetration power. Second period elements have lower electron affinity due to their small size, leading to repulsion of incoming electrons. This property influences the nature of bonding and the stability of elements in different groups and periods.
What factors influence the polarity of covalent bonds?
The polarity of covalent bonds is influenced by the electronegativity difference between atoms involved in the bond. Greater differences in electronegativity lead to higher polarity and a greater percentage of ionic character in the bond. The Polling Make formula is used to calculate the polarity of covalent bonds based on these differences, determining the nature of the bond and the sharing of electrons between atoms.
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