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Classification of Element & Periodicity in Properties Class 11 Full Chapter in 60 Minutes ⌛

Vedantu JEE Made Ejee・54 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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Summary

00:00

"60-Minute Study Session: Class 11 Chemistry Recap"

  • The study session must be completed within 60 minutes due to traffic constraints.
  • The focus is on revising an important class 11th chapter within the hour.
  • The session will cover exceptions, a surprise DP, and the entire chapter.
  • Attendees are urged to listen attentively, take notes, and engage with the material.
  • The history of the Periodic Classification of Elements is discussed.
  • The classification proposed by Sir Dobereiner is explained, emphasizing atomic mass and groupings of three elements.
  • Similar chemical properties are observed in elements grouped together.
  • The New Land classification method is introduced, arranging elements based on atomic mass.
  • The Mental's periodic table classification is detailed, focusing on oxides and hydrides formulas.
  • The importance of arranging elements by atomic number is highlighted, leading to the modern periodic table structure.

12:54

Understanding Periodic Table: Noble Gases & Electrons

  • Remember the Group 18 elements, noble gases, and zero gas are real gases.
  • Focus on their atomic numbers and the periods they belong to.
  • Understanding the period of an element based on its atomic number is crucial.
  • Knowing the next noble gas after a specific atomic number helps determine the period.
  • The sequence of filling electrons in D elements follows a specific order.
  • The energy sequence of elements in different periods is based on the configuration.
  • The general electron filling order in different periods involves S, D, and P orbitals.
  • Exceptions exist in electron configurations, especially in the 3d series.
  • The general configuration for F block elements involves filling the D orbitals first.
  • Predicting the period, group, and atomic number of an element based on given information is possible using specific rules.

26:27

Atomic Structure and Periodic Trends Explained

  • The group number determines the block type: S block for group one, two blocks from three to 12, and P block for groups 13 to 18.
  • The F block is identified by the topic number, guiding the grouping process.
  • Adding 32 to 18 when a number turns negative aids in predictions.
  • Electron configuration and atomic number can be determined by adding up electrons, aiding in question-solving.
  • The nucleus attracts valence electrons, affecting the effective nuclear charge.
  • Shielding by inner electrons reduces the nucleus's attraction on valence electrons.
  • Effective nuclear charge increases with more shielding, impacting electron removal difficulty.
  • Atomic radius decreases as effective nuclear charge increases, except for noble gases in group 17.
  • Transition elements show exceptions in atomic size variations due to screening effects.
  • Lanthanide contraction and transition contraction affect atomic size irregularities in specific elements.

39:41

Ionization Energy and Electron Affinity Relationships

  • To extract an additional electron from an atom, more energy is required, leading to successive ionization energy.
  • The effective nuclear charge increases as electrons are removed, making it harder to extract subsequent electrons.
  • The size of an atom impacts ionization energy, with larger atoms requiring more energy to remove electrons.
  • Exceptions to the general trend of increasing ionization energy are seen in certain groups, like group 13 and 14.
  • Electron affinity is the tendency of an element to attract electrons, measured by electron gain enthalpy.
  • Electron affinity is influenced by 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.
  • The electronegativity of elements determines the nature of their bonding, with greater differences leading to more polar covalent bonds.
  • The greater the difference in electronegativity, the higher the polarity and percentage of characters in a covalent bond.
  • The Polling Make formula is used to calculate the polarity of covalent bonds based on electronegativity differences.

53:18

Electronegativity and Oxidation State Trends in Chemistry

  • The electronic fluorine of some elements has a maximum value of 4, while chlorine in the same period has a value of 0.5.
  • Factors affecting closed energy include an increase in size with higher electronegativity, leading to a decrease in attraction due to shared electrons moving away from the nucleus.
  • Cationic species with more cations exhibit higher electronegativity, effective nuclear charge, and oxidation state.
  • Hybridization influences electronegativity, with sp having higher values than sp2 and sp3, following the general trend of increasing electronegativity from left to right.
  • Metal oxides tend to be basic and increase in basic nature from top to bottom due to increasing metallic character, while non-metallic acidic oxides decrease in acidic nature as size increases.
  • Isoelectronic species comparison reveals trends in properties based on electron and proton counts, affecting effective nuclear charge, acidic nature, and oxide formation.
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