Periodic Classification of Elements Class 11 Questions | CBSE Chemistry Half Yearly | Midterm

Vedantu 9,10 &11・2 minutes read

Nikita from Vedanta leads Proton Army in a session on Periodic Classification of Elements, covering topics like ionization enthalpy, electron configurations, and screening effects. The discussion includes identifying actinoid elements, determining ionic radii, and explaining differences in properties like ionization enthalpy and atomic radius.

Insights

  • The session led by Nikita at Vedanta focused on discussing key concepts in Chemistry, such as ionization enthalpy, electron gain enthalpy, and the order of screening effect in orbitals.
  • Understanding the periodic table involves analyzing electronic configurations, identifying trends in properties like first ionization enthalpy, and recognizing similarities and differences between elements, ultimately highlighting the significance of valence electrons in determining chemical behavior.

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Recent questions

  • What is the significance of the order of screening effect in s, p, d, and f orbitals?

    The order of screening effect in orbitals determines how effectively inner electrons shield outer electrons from the attraction of the nucleus. Understanding this order helps in predicting trends in atomic properties like ionization enthalpy and electron gain enthalpy.

  • How are actinoid elements different from lanthanoids?

    Actinoid elements differ from lanthanoids in their electronic configurations and properties. Actinoids have electrons filling the 5f orbital, while lanthanoids fill the 4f orbital. This distinction leads to variations in chemical behavior and physical characteristics between the two groups.

  • Why are Zinc, Cadmium, and Mercury not classified as D block elements?

    Zinc, Cadmium, and Mercury are not classified as D block elements despite having electrons in the d orbital because their last electron enters the s orbital. This entry pattern results in these elements exhibiting properties similar to D block elements while not fitting the traditional classification criteria.

  • How does electronegativity vary in p block elements from groups 13 to 18?

    Electronegativity in p block elements from groups 13 to 18 varies based on the formation of acidic oxides and the resulting compounds. The ability of these elements to form different oxidation states influences their electronegativity, impacting their reactivity and chemical properties.

  • What determines the position of an element in the periodic table?

    The electronic configuration of an element determines its position in the periodic table. By analyzing the arrangement of electrons in the atom, one can identify the group and period to which the element belongs. This information helps in understanding the element's properties and behavior in chemical reactions.

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Summary

00:00

"Master Teacher Guides Proton Army in Chemistry"

  • Nikita, Chemistry master teacher at Vedanta, welcomes the Proton Army for a session on solving 15 questions on Periodic Classification of Elements.
  • The session involves interactions with students, addressing queries, and starting with questions on exceptions, ionization enthalpy, and electron gain enthalpy.
  • The order of screening effect in s, p, d, and f orbitals is discussed, with s having the maximum screening effect.
  • The first ionization enthalpy order of sodium, magnesium, aluminum, and silicon is determined based on their electronic configurations and atomic numbers.
  • The electronic configurations of magnesium, sodium, aluminum, and silicon are analyzed to understand the trend in first ionization enthalpy.
  • The concept of stable and unstable arrangements in elements is explained in relation to ionization enthalpy.
  • Identification of actinoid elements and their differences from lanthanoids is discussed.
  • Determining the electronic configuration of an element with atomic number 64, leading to the correct answer of option C.
  • The order of increasing ionic radii among iso electronic species is determined based on their charges and electron configurations.
  • The reasons behind the differences in first ionization enthalpy and atomic radius of elements like sodium, carbon, and aluminum are explained.

16:41

Chemical Elements and Periodic Table Properties

  • Zinc, Cadmium, and Mercury are not classified as D block elements due to the last electron entering the A orbital, but they exhibit similar properties to D block elements.
  • Transition elements are D block elements, but not all D block elements are transition elements; classification depends on the electron's entry into the D orbital.
  • Nitrogen has positive electron gain enthalpy, while oxygen has lower ionization enthalpy due to its stable half-filled configuration.
  • Electronegativity increases moving left to right in the periodic table, while ionization enthalpy decreases from top to bottom in a group.
  • The position of an element in the periodic table can be determined by its electronic configuration, with n-1 d1 ns2 indicating group 3 and period 4.
  • P block elements from groups 13 to 18 exhibit various oxidation states and acidic oxide formation, with electronegativity varying based on the compound formed.
  • Elements in the same group share similar physical and chemical properties due to having the same number of valence electrons.
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