Memorizing the Periodic Table of Elements

• Group I-A: The Alkali Metals (Soluble group)

  Mnemonic: HaLiNa Kayo, Ruby, Ces & Friends

  Hydrogen, Lithium, Sodium, Potassium, Rubidium, Cesium, Francium
• Group II-A: The Alkaline Earth Metals

  Mnemonic: Be MagCano StroBaRa?

  Beryllium, Magnesium, Calcium, Strontium, Barium, Radium
• Group III-A: The Boron Group (The Icosagens)

  Mnemonic: BoAlGaInTal

  Boron, Aluminum, Gallium, Indium, Thallium
• Group IV-A: The Carbon Group (The Crystallogens)

  Mnemonic: “C-SiGe, Sn Pb?”

  Carbon, Silicon, Germanium, Tin, Lead
• Group V-A: The Nitrogen Group (The Pnictogens)

  Mnemonic: NaPASabBi


  Nitrogen, Phosphorus, Arsenic, Antimony, Bismuth
• Group VI-A: The Oxygen Group (The Chalcogens)

  Mnemonic: OsuSeTePo


  Oxygen, Sulfur, Selenium, Tellurium, Polonium
• Group VII-A The Halogens (Salt-forming)

  Mnemonic: Florence Claire BIAs

  Fluorine, Chlorine, Bromine, Iodine, Astatine
• Group VIII-A The Noble Gases (Group O)

  Mnemonic: Hel NeAr KryXeRa

  Helium, Neon, Argon, Krypton, Xenon, Radon
• Group I-B: The Coinage Metals

  Mnemonic: CoSiGo


  Copper, Silver, Gold
• Group II-B: The Volatile Metals

  Mnemonic: ZiCadMer

  Zinc, Cadmium, Mercury
• Nihonium (Nh)

  Kosuke Morita
• Flerovium (Fl)

  Georgy Nikolayevich Flyorov
• Oganesson


  Yuri Tsolakovich Oganessian
• Principal Quantum Number (n)


  Energy level; Determines the size of the particle
• Azimuthal Quantum Number/Angular Quantum Number (ℓ)


  Sub-shell or sub-level; Determines the shape
• Magnetic Quantum Number (m or ml)


  Orbitals; Determines the orientation
• Spin Quantum Number (s or ms)


  Direction of the spin or rotation of electron
• Paramagnetic Elements


  Elements that have unpaired electrons. They are attracted to external magnetic field.
• Diamagnetic Elements


  Elements that have completely paired electrons. They are weakly repelled by a magnetic field.
• Ferromagnetic Elements


  Fe, Co, Ni
• Ferromagnetism arises when the unpaired electrons of the atoms or ions in a solid are influenced by the orientations of the electrons in neighboring atoms or ions.
• Pauli’s Exclusion Principle


  No two electrons can have the same set of 4 quantum numbers. Each atomic orbital can only accommodate 2 electrons.
• Heisenberg’s Uncertainty Principle


  It is impossible to determine simultaneously the electron momentum and position.
• Aufbau Building Up Principle


  Lower energy level are filled up first
• Hund’s Rule of Max Multiplicity

  Orbitals are filled up singly before pairing up.