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Classification of Elements & Periodicity of Properties | NEET 2023 | Shimon Sir | V Master Tamil

Vedantu Master Tamil・31 minutes read

The session covers the preparation for the 10th board exam, focusing on atomic weight, atomic number, periodic properties, and trends in atomic radius, ionization energy, electron affinity, and electronegativity among elements, along with their practical applications and exceptions. These concepts are vital for understanding the periodic table, electron configurations, ion formation, and chemical bonding, with specific rules and trends guiding the behavior and characteristics of elements based on their atomic structure and properties.

Insights

  • The Modern Periodic Law states that properties of elements are based on atomic number, not atomic weight, revolutionizing the organization of the periodic table.
  • Electronegativity plays a pivotal role in determining bond characteristics, with factors like atomic size and nuclear charge influencing the strength and polarity of bonds, essential for predicting properties and behaviors of compounds.

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Recent questions

  • How are elements arranged in the Modern Periodic Table?

    By increasing atomic number.

  • What determines the formation of ions in atoms?

    Gaining or losing electrons.

  • How does electron affinity vary across the Periodic Table?

    Increases across a period, decreases down a group.

  • What is the significance of electronegativity in chemical bonding?

    Determines polarity and bond strength.

  • How are atomic radius and properties influenced by factors like shielding effect?

    Shielding effect affects atomic radius and properties.

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Summary

00:00

"Atomic Weight, Periodic Table, Electronic Configuration"

  • The session is focused on preparing for the 10th board exam.
  • The average of the first and third elements' atomic weight determines the middle one's atomic weight.
  • Elements like lithium, potassium, calcium, strontium, and barium are arranged in increasing order of atomic weight.
  • Lothar Meyer plotted Atomic volume against atomic weight to group similar elements.
  • The periodic properties are based on atomic weight according to the Mentally Periodic Law.
  • The Modern Periodic Law states that properties are based on atomic number.
  • The Modern Periodic Table is based on Bohr-Bury electronic configuration.
  • The filling of orbitals follows the Aufbau principle.
  • The electronic configuration of elements follows specific rules for group and period placement.
  • Factors like shielding effect and penetration influence atomic radius and properties of elements.

01:23:34

Ionic Radius Trends and Exceptions in Chemistry

  • Option C is the correct answer for ionic radius comparison.
  • Ions are formed by gaining or losing electrons, with cations losing electrons to gain a positive charge.
  • The atomic number determines the number of protons and electrons in an atom.
  • The trend for ionic radius is that anions are larger than their corresponding atoms, while cations are smaller.
  • Isoelectronic species have the same number of electrons but different nuclear charges.
  • The trend for ionic radius is inversely proportional to effective nuclear charge.
  • The trend for ionization energy is that it increases across a period and decreases down a group.
  • Exceptions to the trend include elements like Boron, Nitrogen, and Oxygen due to their electronic configurations.
  • Electron affinity is the energy released when an electron is added to an isolated gaseous atom.
  • The trend for electron affinity is that it increases across a period and decreases down a group, with exceptions like Fluorine and Oxygen due to their small sizes.

02:26:46

Importance of Electronegativity in Chemical Bonding

  • Electronegativity is crucial in studying the polarity of molecules, with more electronegative atoms attracting electron clouds towards themselves, leading to polar bonds like in HCL where chlorine becomes slightly negative and hydrogen positive due to chlorine's higher electronegativity.
  • The Pauling scale determines electronegativity differences between atoms, aiding in predicting polarity and bond strength, with electronegativity dependent on factors like atomic size, nuclear charge, and hybridization.
  • Understanding electronegativity is vital for predicting bond characteristics, such as ionic character in covalent bonds, with applications like determining oxide types based on electronegativity differences, classifying them as basic, amphoteric, or acidic oxides.
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