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

Vedantu Master Tamil・2 minutes read

The text covers various topics related to atomic weight, electronic configuration, ionic radius, and electronegativity, discussing trends, principles, and comparisons between different elements based on these properties. Key points include the relationship between atomic weight and atomic properties, the formation of ions through gaining or losing electrons, and the impact of electronegativity on bond polarity and properties of molecules.

Insights

  • The Modern Periodic Law states that properties of elements are based on atomic number, not atomic weight, revolutionizing the understanding of the periodic table.
  • Electronegativity plays a crucial role in determining the polarity of molecules, with atoms attracting electron clouds based on their electronegativity values, influencing bond strength and oxide properties.

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Recent questions

  • How are elements arranged in the periodic table?

    Elements are arranged by increasing atomic weight.

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Summary

00:00

"Atomic Weight, Periodic Law, 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.
  • The atomic radius decreases along a period and increases along a group, with exceptions like gallium being smaller than aluminum.

01:23:34

"Ionic Radius Trends and Isoelectronic Species"

  • 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.
  • Phosphorus 3- has the largest ionic radius among isoelectronic species.
  • The ionic radius trend follows the nuclear charge, with larger nuclear charges leading to smaller radii.
  • The ionic radius trend is evident in the comparison of Ar, K+, and Ca2+.
  • The decreasing ionic radii order among isoelectronic species is S2-, Cl-, K+, and Ca2+.
  • The electron configuration stability affects ionization energy, with half-filled or fully filled orbitals being more stable.

02:26:46

Understanding Electronegativity and Predicting Molecular Polarity

  • 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 based on values for elements, influenced by factors like atomic size, nuclear charge, and s character percentage in hybridized atoms.
  • Applications of electronegativity include predicting bond strength, ionic character in covalent bonds, and oxide properties, where differences above 2.3 indicate basic oxides, equal to 2.3 are amphoteric, and below 2.3 are acidic, with examples like lead oxide and aluminum oxide.
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