Electronic configuration in Structure Of Atom – Class 10 Science Experiment

Chapter Name: Structure Of Atom

Activity Name: Electronic configuration in Structure Of Atom

Activity Description:

In this activity, we will complete the electronic configuration of certain elements, understanding how electrons are distributed in different energy levels around the nucleus of an atom.

Required Items:

Periodic table, pen/pencil, paper.

Step by Step Procedure:

  1. Take a periodic table to refer to the atomic numbers and electron configurations of elements.
  2. Choose the elements for which you want to complete the electronic configurations.
  3. Locate the element’s atomic number on the periodic table, which represents the number of protons in its nucleus.
  4. Understand the rules for filling electrons in different energy levels (orbitals) following the Aufbau principle, Pauli exclusion principle, and Hund’s rule.
  5. Begin filling the electrons in the orbitals, starting from the lowest energy level (closest to the nucleus) and moving towards higher energy levels, until you reach the total number of electrons for that element.
  6. Use the notation: 1s² 2s² 2p⁶, and so on, to represent the completed electronic configuration.

Experiment Observations:

  • The electronic configuration of elements can vary, with different numbers of electrons in their energy levels.
  • Electrons are filled in specific orbitals based on their increasing energy levels.

Note down your observations in table format:

Electronic configuration in Structure Of Atom - Class 10 Science Experiment

Precautions:

  1. Double-check the atomic numbers and the corresponding element symbols while referring to the periodic table to avoid errors.
  2. Follow the rules of electron filling strictly to ensure accurate electronic configurations.

Lesson Learnt from Experiment:

The experiment helps to understand how electrons are arranged in different energy levels around the nucleus of an atom, and how the electronic configuration determines an element’s properties and chemical behavior.

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