science

• All substances are made of tiny particles called "ATOM"
• Electrons


  Negatively charge subatomic particles
• Electrons


  • J. J. Thomson was the first person to accurately calculate the mass and the charge of an electron
• Protons


  Positively charge subatomic particles
• Protons


  • Discovery of protons is credited to Earnest Rutherford
• Neutrons


  Neutrally charged subatomic particles
• Neutrons


  • Discovered by James Chadwick in 1932
• Quantum Mechanical Model


  Louie de Broglie (1924) proposed that the electron could also be thought of as a wave
• Quantum Mechanical Model


  Erwin Schrodinger used the wave idea to develop a mathematical equation to describe the hydrogen atom
• Quantum Mechanical Model


  Werner Karl Heisenberg discovered that for a very small particle like the electron, its location cannot be exactly known and how it is moving
• Uncertainty Principle


  It is impossible to locate the exact position of an electron at any given time (too small, too fast)
• Atomic orbital


  The volume or region of space around the nucleus where the electron is most likely to be found
• Electron Orbit Model


  Electrons were thought to orbit around the nucleus in defined paths
• Electron Cloud Model


  Discovered that electrons move in waves in a defined space called an electron cloud
• Quantum Numbers


  • Principal quantum number
  • Angular momentum quantum number
  • Magnetic Quantum Number
• Electron Configuration


  The electron configuration of a certain element consists of three Quantum Numbers
• Octet Rule | Valence Electron | Lewis Dot Structure (LDS)
• Chemical Bonding


  Chemical bonding refers to the formation of a chemical bond between two or more atoms, molecules, or ions to give rise to a chemical compound
• Ionic Bonding


  Formed between Metal and a Nonmetal
• Covalent Bonding


  Bonding is common between two nonmetals
• Ions


  Uneven numbers of protons and electrons which results in an overall positive or negative charge
• Types of Ions


  • Cation (positive charge)
  • Anion (negative charge)
• Octet Rule


  It refers to the tendency of atoms to prefer to have eight electrons in the valence shell
• Valence Electron


  Electrons in the outermost (valence) principal energy level of an atom that can participate in the formation of chemical bonds with other atoms
• Periodic Table Groups


  • Group 1 (I) -alkali metals
  • Group 2 (II) - alkaline earth metals & He
  • Group 3-12 (transition metals)
  • Group 13 (III) - boron group
  • Group 14 (IV) - carbon group
  • Group 15 (V) - nitrogen group
  • Group 16 (VI) - oxygen group
  • Group 17 (VII) - halogen
  • Group 18 (VIII) - noble gases except Helium
• Lewis Dot Structure (LDS)


  Lewis dot structures (LDS) are diagrams that show the bonding between atoms of a molecule and the lone pairs of electrons that may exist in the molecule
• Covalent Bonding


  The formation of compound also involves sharing of electrons, thus resulting in a covalent bonding
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• Atom


  Tiny particles that all substances are made of
• Electrons


  • Negatively charged subatomic particles
  • J.J. Thomson was the first to accurately calculate the mass and charge of an electron
• Protons


  • Positively charged subatomic particles
  • Discovery of protons is credited to Ernest Rutherford
• Neutrons


  • Neutrally charged subatomic particles
  • Discovered by James Chadwick in 1932
• Quantum Mechanical Model


  • Model of the atom where the electron can be thought of as a wave (proposed by Louis de Broglie)
  • Erwin Schrodinger developed a mathematical equation to describe the hydrogen atom
  • Werner Heisenberg discovered the Uncertainty Principle - the exact position and motion of an electron cannot be known
• Atomic Orbital


  The volume or region of space around the nucleus where the electron is most likely to be found
• Electron Orbit Model


  Electrons were thought to orbit around the nucleus in defined paths
• Electron Cloud Model


  Electrons move in waves in a defined space called an electron cloud
• Quantum Numbers


  • Principal quantum number
  • Angular momentum quantum number
  • Magnetic quantum number
• Electron Configuration


  The arrangement of electrons in an atom's orbitals
• Chemical Bonding


  The formation of a chemical bond between two or more atoms, molecules, or ions to give rise to a chemical compound
• Octet Rule


  The tendency of atoms to prefer to have eight electrons in the valence shell