Mnemonics & Short tricks: Structure of Atom - NEET PDF Download

In this EduRev document, you will find creative ways to remember critical topics such as subatomic particles, electronic configurations, and the experiments that shaped our understanding of the atom. These mnemonic devices and memory aids are not only meaningful but also easy to grasp, making the learning process more engaging and accessible for students. So, let's embark on this atom-sized adventure, armed with memory hacks that turn intricate chemistry concepts into memorable and enjoyable learning experiences.

1. Subatomic Particles:

   • PEN: Protons, Electrons, Neutrons. This acronym helps remember the three fundamental subatomic particles.

2. Atomic Number and Mass Number:

   • Atomic Number = Proton Number: The atomic number tells you the number of protons in an atom.
   • Mass Number = Protons + Neutrons: Mass number is the sum of protons and neutrons in the nucleus.

3. Electronic Configuration:

   • SPDF: S, P, D, and F blocks represent the different energy levels or orbitals. "Silly Penguins Dance Funny" is a fun way to remember the sequence.
   • 2-8-18-32 Rule: The maximum number of electrons that can be accommodated in each energy level is 2, 8, 18, and 32 (for S, P, D, and F orbitals, respectively).

4. Aufbau Principle:

   • Aufbau sounds like "off-bow." Think of electrons getting on a bow, starting from the lowest energy level.

5. Pauli Exclusion Principle:

   • PEP: Pauli Exclusion Principle. Remember it as "People don't like to share the same seat in a bus." Electrons in the same orbital have opposite spins.

6. Hund's Rule:

   • Hund's Hopping Rule: Electrons fill orbitals of the same energy level one at a time before pairing up. Think of electrons hopping into empty seats on a bus before sitting together.

7. Valence Electrons:

   • Valence Veggies: Valence electrons are the electrons in the outermost energy level. Remember them as "Valence Veggies" because they are on the outermost shelf (like vegetables in a grocery store).

8. Isotopes and Isobars:

   • Isotopes have the same number of protons but different numbers of neutrons.
   • Isobars have the same mass number but different atomic numbers.

9. Bohr's Model:

   • Bohr's Bullseye: Imagine electrons orbiting like a bullseye target around the nucleus in specific energy levels, just as Bohr proposed.

10. Quantum Numbers:

    • n, l, m, s: Remember them as "Nerdy Little Monkeys Skipping." Each quantum number specifies an electron's position and spin.

11. Rutherford's Gold Foil Experiment:

    • Golden Arrows Experiment: Think of shooting arrows (alpha particles) at a golden foil (gold foil) to discover the nucleus.

12. Heisenberg Uncertainty Principle:

    • Heisenberg Hides: You can't simultaneously know the exact position and momentum of a tiny Heisenberg hiding in your hand. This represents the uncertainty principle.

13. Schrodinger's Equation:

    • Schrödinger's Cat Equation: Imagine a cat (electron) in a box (atom) that is both alive and dead until you open the box (make a measurement).