Chemistry

• H3O +1

  Hydronium Ion
• NH4 +1

  Ammonium Ion
• NO3 -1

  Nitrate Ion
• OH -1

  Hydroxide Ion
• CH3COO -1 or CH3CO2 -1

  Acetate Ion
• MnO4 -1


  Permanganate Ion
• SO4 -2

  Sulfate Ion
• CO3 -2

  Carbonate Ion
• CrO3 -2


  Chromate Ion
• Cr2O7 -2 


  dichromate ion
• PO4 -3

  Phosphate Ion
• What does WHMIS stand for?

  Workplace Hazardous Materials Information System
• What does SDS stand for?

  Safety Data sheets
• What is WHMIS?

  A plan that involves education, communication and labels for chemical safety
• What are Safety data sheets?

  Sheets that provide all relevant chemical information including name, storage, handling, first-aid and disposal.
• Flame symbol


  Prone to easy ignition and can burn rapidly
• Flame over circle

  Supports combustion or flammability. Oxidizing hazard. Commonly has a yellow label.
• Corrosion


  material or product chemically reacts with or in reaction to contact with skin and other materials, thus destroying them in the process.
• Health Hazard


  May cause chronic health issues (long-term)
• Exclamation Mark


  less severe health issues such as inflammation and coughing. Generally treatable and less risk of becoming long-term.
• Gas cylinder


  there are gases stored under high pressure. Following a puncture or leak , there is a risk of the product exploding or becoming a makeshift projectile.
• Exploding Bomb


  the material is explosive and risks combusting when handled poorly.
• Environment


  May cause harm to aquatic life and the environment
• Biohazardous, infectious materials


  the product contains organisms harmful to human health by causing disease and/or other serious illnesses. Organisms include: parisites, bacteria, viruses and fungi.
• Skull and crossbones

  may cause death or toxicity with short exposure to small amounts.
• Aristotle/Democratus proposed that all earthly matter is composed of only four possible "elements" (Earth, Wind, Fire, Water). Stars are the exception and made of Aether. This was around 400 BC.
• In the early 1800s, Sir John Dalton proposed fire postulates. He claimed that all matter is made of tiny particles known as atoms. These particles cannot be destroyed, created or divided. All atoms of the same element are identical to eachother and atoms of different elements are different from one another. Atoms combine in whole number ratios.

  Model: Billiard Ball (ex; same colour same element, different colour different elements).
• Around the 1900s, Sir John James Tomson claimed that atoms contain both protons and electrons, protons have a positive charge and electrons have an equal negative charge. protons are heavy and electrons are light.

  Model: Plum Pudding or Raisin Bun, the dough is the protons and the fruit is the electrons.

  Experiment: Cathode Ray Tube (CRT), where the shadow presented itself told him which was heavier, and that they were there.
• Around the 1920s Sir Ernest Rutherford provided the idea of the nucleus. A small dense and positively charged core of the atom. Surrounded by a cloud of electrons.

  Model: Nuclear Cloud. (Positive nucleus in the center, electron cloud surrounding).

  Experiment: Gold Foil, the alpha particles defracted once they passed through the gold sheet and landed at the fluorescent screen.
• (~1930s) Neils Bohr, student of Rutherford, created the spectrophotometry experiment, which provided evidence for the concept that electrons are found on rings at specific distances.

  Model: Solar system, Planetary

  Experiment: Hydrogen connected to line which targeted a prism and hit a screen in four places.
• (~1930s) Sir James Chadwick solved the issues of the relationship between atomic # and atomic mass with the neutron.
• Our current model is the quantum mechanics theory. This theory builds on Bohr's ideas, most importantly that if "n" is the ring #, then the maximum number of electrons is 2n^2
• Atomic radius is the total distance between the nucleus and the outermost orbital of the electron. It decreases across and increases top to bottom. The attraction of the electrons the the increasingly positive nucleus causes the atom to shrink. (The # of protons vs. # of electrons)
• Ionization Energy

  • the amount of energy required by an atom to lose an electron is called 'ionization energy'
  • As new valence shells are added, the distance from the nucleus grows, so they are more easily removed. (If they have more valence shells and more electrons + shells, they have less of a need for them)
  • Increases across, decreases as you go down
• Electron Affinity

  • atoms have the desire to add more electrons to their valence shells. As new valence shells are added this affinity will decrease since the electrons are further from the positive nucleus.
• Electronegativity

  • the amount of valence electrons compared to the size of the atom create what we call 'Electronegativity'
  • a small atom with lots of charge is highly electronegative, and a large one can disperse its charge.
• Intermolecular Forces - Forces that occur between molecules

  • Weaker forces than those within molecules, so when the temp. rises then those forces are broken
  • Example: Boiling water causes molecules to separate, but the molecules stay as H2O
  • Types: 1. VanderWaal's Forces, 2. London Dispension Forces, 3. Dipole-Dipole Forces
• Intramolecular forces - occurs within molecules
• Ionic bonding - metal atoms with low ionization energy easily give one or more valence electrons (e-) to a non-metal with high electron affinity.

  • This creates a cation and an anion
  • The difference in electronegativity in greater than 1.7
• Pure covalent bonding - two or more atoms with high electron affinity will overlap their valence shells.

  • the difference in electronegativity is less than 0.5