Distinguish between shell and sub-shell.

  • Shell: A shell refers to a group of atomic orbitals with the same principal quantum number, denoted by the letter n (e.g., K shell, L shell, M shell). It represents a specific energy level in an atom where electrons are likely to be found. Each shell can hold a specific number of electrons and is associated with a particular energy level.

  • Sub-shell: A sub-shell is a subdivision of a shell and is characterized by the azimuthal quantum number l. Sub-shells are denoted as s, p, d, and f, where each letter represents a different shape and energy level of orbitals within that shell. The number of sub-shells in a shell depends on the value of n (the shell’s principal quantum number). For example, the first shell (n=1) has one sub-shell (1s), the second shell (n=2) has two sub-shells (2s, 2p), and so on.

Related Questions:

  1. Why is an atom electrically neutral?
  2. How many sub-shells are there in the N shell?
  3. Give notation for sub-shells of the M shell.
  4. List the sub-shells of the M shell in order of increasing energy.
  5. The electronic configurations listed below are incorrect. Explain the mistakes in each and write the correct electronic configurations.
  6. Which orbital in each of the following pairs is lower in energy?
  7. Draw Bohr’s Model for the following atoms, indicating the locations of electrons, protons, and neutrons:
  8. Write the electronic configuration for the following elements:
  9. State the importance and uses of isotopes in various fields of life.
  10. The atomic number of an element is 23, and its mass number is 56.
  11. The atomic symbol of aluminum is written as Al. What information do you get from it?
  12. Describe the principles of green chemistry and how they help in environmental protection.
  13. Can you write the formula of the carbon dioxide gas that we exhale?
  14. Define element, compound, and mixture.
  15. Differentiate between a compound and a mixture.
  16. Differentiate between a concentrated and a dilute solution.
  17. Define the term allotropes and explain the allotropes of carbon.
  18. What is the difference between a homogeneous and a heterogeneous solution?
  19. Differentiate between colloids and suspensions.
  20. How can you identify a solvent and a solute?