CHEMISTRY

• Billiard ball model or Solid’s Fear model by John Dalton

  • every particle has an atom (atoms can be solid or invisible)
• Plum pudding model by J.J Thompson

  • the negative electrons in the positive framework
• Planetary model

  • electrons move around the nucleus
• Nuclear model by ernest rutherford

  • negative electrons in positive framework
• Quantum mechanical model by erwin schrodinger

  • electrons don’t move in fix position. It has no orbit
• Isotope means same atoms number but different mass number
• Isobars- different atoms or different elements but has the same mass number
• Isotones - same neutrons but different number of protons/ electrons
• Isodiaphers - different atoms or elements but same neutron excess
• Neutron excess - difference of protons and neutrons
• Quantum theory - theoretical basis of quantum
• Black body radiation

  • Absorbs all energy and no light is reflected
• Stefan - Boltzman Law

  • brighter radiation but shorter wavelength
• founder of quantum theory

  • max planck
  • albert einstein (3rd founder)
  • Neils bohr
• Max planck

  • quantum particles
  • energy is limited to specific values
  • E=hv
• Albert einstein

  • quantum theory of light
  • photon electric
• Neils bohr

  • planetary model of atom
  • electrons move in waves no specific time and features
• Quantum number & electrons orbits

  • positive (n)
  • high energy if farther to nucleus
• ground state

  • 1st orbital
  • has lowest energy and stationary
• Excited state

  • 2nd orbital is the 1st in this state
  • highe energy than ground state
• Absorption

  • moves to outer
• Emission energy level

  • Higher energy level return to lower
• Quantum mechanical model

  • Erwin schrodinger
  • louis de broglie
  • werner karl heisenberg
• schrodinger named quantum model
• De broglie - wave particle duality
• Heisenberg - uncertainty principle wherein electrons move in cloud of probability (quantum model)
• Quantum mechanical model

  • explains existence and behavior of atoms
  • understanding and predicting properties of atoms based on behavior
• Atomic orbital

  • where electron foun
  • (quantum number- helps to describe atoms)
• 4 quantum numbers

  • principal (n)
  • azimuthal (I)
  • magnetic (me)
  • electrons quantum number (ms)
• Principal quantum number

  • describe relative size of atoms (size)
  • farther = higher energy larger it is
• Azimuthal / angular quantum number

  • size (shape) type of subshell of an electron
• Magnetic quantum number

  • define orientation in space / orbital with sublevel (orientation)
• Electrons spin quantum number

  • direction of the spin
• Pauli exclusion

  • all electrons have different quantum number
• Hunds’ rule - fill all orbitals with same spin
• Aufbau principle

  • “building block”
  • start at lowest energy before filling up the next orbit (GERMANY)
• Quantum mechanical model

  • explain why some elements are stable and some are not
• Oxidation state - electrical charge of an atom
• General properties

  • exist in all materials
  • inertia, mass, weight, volume, density, impermeability
• Specific properties

  • exist in particular materials
  • hardness, brittleness, miscibility, luster, malleability, viscosity, elasticity, ductility, flex, solubility