Weekly Outlines February to March

Latest Update March 12 2005

Course notes may be found by

Opening Day February 17

• Introduction of course topics
• Periodic table; columns, rows families, shells
• Remember the three simple rules you were given:
  1. The period in whcih the atom is found on the periodic table is the number of shells in that particular atom.
  2. Outer shell can achieve a maximum of 8 electrons; no exceptions.
  3. Inner shells will never exceed 18 electrons; this will start to occur when the atomic number is greater than 56 or 57. (Not a worry at this level)
• Introduction to the Periodic Table;
  A discussion on the catagorization of the periodic table was presented.
• Introduction to chemical families:
  1. Halogens
  2. Noble gases
  3. Alkali metals
  4. Alkaline earth metals
  5. Coinage metals
• Representaive elements, transition metals and the two series, lanthanide (rare earth elements) & actinide series.
• States of matter
• What's on the Internet; a quick outline.
• Physical & Chemical changes
• Two videos: i) Physical and Chemical Changes ii) Atoms & Their Electrons

Week Two Feb 21 & 24

• Organization of elements into physical and chemical similarities. A fill in the blank work sheet was used as a guide.
  

• The periodic table ===> how constructed.
• Comparison between cation and atomic size
  Comparison between anion and atomic size
  Factors that effect atomic size
  Size trends on the periodic table both in families and in rows or periods.
• A video on Chemical Families was seen & how these similarities are used in the organization of the periodic table. A more formal video than last day, also much older.
• Quick review of Nomenclature. Binary compounds are be studied first.
  Colouring in a periodic table to differenciate univalent metal ions from multi or divalent metal ions.
  Nonmetal ions, in binary compound, are always negative and have fixed values based on how many electrons they need to fill up thier outer shell.
• Ion valencies based on electrons lost or gained.
• Lesson is presented in class dealing with the following:
  1. Name to Formula
     1. Write elements symbols with valence values; metals or positive valence species always come first.
     2. Use the Criss-cross rule or method.
     3. Reduce were necessary.
  2. Formula to Name
     1. Back criss-cross and look out for reduced values.
     2. Is the metal univalent or divalent?
     3. Write the metal name; insert valence value if needed (all elements that are not univalent must have their valcence stated (two formats possible)).
     4. The nonmetal is named with its name ending in ...IDE
• Try my Nomenclature Quiz Click Here
• Trends in Periodic Table: Graphical analysis of radii, first ionization energy, valency versus atomic number. This is the Internet assignment number C
• Atomic size and ionic sizes (radii). Atomic radii courtesy of Webelements.
• General trends that arise as you go across a period and down a family
  Ionizations Energy; the definition
  Electron Affinity; defined
  Multiple ionizations energies; trends developed.
  
• A summary of periodic table trends is given in the diagram below.
  

  Extra readings or understanding may be found at Trends in Periodic Table which inludes the topics   

  • atomic radius
  • ionization energy
  • electron affinity
  • reactivity of the elements  just click on the pencil
  
• Bonding; first we do ionic then covalent. Properties of each.
  Ionic bonding has already been introduced; based on the octet rule where nonmetals gain electrons to arrive at filled valence shell of eight and metal lose all their valence electrons.
  The number follow nomenclature valence values you already know.
• Lewis dot diagrams; used for representative elements to help track valence shell electrons.
• Chemical family lab: probably a demonstration lab
  • Alkali metals & alkaine earth metals with water
  • Alkaline earth metals with sulfate & carbonate solutions
  • Halogens with plumbous and silver ions
  • Potassium reacting with iodine
• The covalent bond; electron sharing to achive a filled valence shell.

• Nomenclature Part II
  Must memorize valencies, three radicals and the five main oxyacid radicals as listed below. Worksheets handed out
  
• Three polyatomic ions hydroxide (OH)^-1 ammonium NH₄⁺¹ and cyanide (CN)^-1.
  Try this to help you remember & test yourself Click Here
• You must memorise these oxy-acid polyatomic ions
  
  • carbonate CO₃^-2
  • phosphate PO₄^-3
  • nitrate NO₃^-1
  • sulfate SO₄^-2
  • chlorate ClO₃^-1
• Polyatomic ion work sheet: answers to be found
• Practice quiz or test handed out on Monday; for answers Click Here
• Demo lab; nice dramatic example of chemical reactions.
• We will start into the first chapter immediately after the opening day.
• Make sure you tell the difference between the two types of changes, with examples and the various definition terms relating to each, such as sublimation or combustion.
• A small chapter one quiz; give it a try Click Here
• Laws, Theories, Hypthesis & Models:
  Law of Conservation of Mass & Energy
  Law of Constant Composition
• Introduction to chemical calculations: using ratios to solve problems. A test would be in order for next week.

Week Three Feb 28 to March 4

• Use of Electronegativity to help predict bond type.
• Discussion of ionic and covalent bonding using Lewis dot diagrams
  Here's a 3-D graph of electonegativities
  

• Balancing equations, with a worksheet. Make sure you ask questions if problems arise.
• Experimental evidence of nonpolar and polar molecules
• Pure covalent, polar covalent and ionic: the bonding continuium. Test on everything Monday (A touch of nomenclature is always included).
• Five main types of chemical reactions: on which you should know examples of each. Try to remember the Lego examples.
  • synthesis
  • decomposition
  • single replacement or displacement
  • double replacement or displacement (special category = neutralization)
  • combustion, complete and incomplete
• Chemical nomenclature, formula and balancing equations will be done on an ongoing activity. See page 97 and 98 for charts of ions and polyatomic ions.
  or Click Here for my chart.
• Introduction to the mole: Skittle example.
• Intoduction to formula weights, example: What is the formula of iron (III) sulfate Fe₂(SO₄)₃?
  atomic weight of iron X 2 + atomic weight of sulfur X 3 + atomic weight of oxygen X 12

• Internet assignment C due on Monday March 7. Late assignments will NOT be accepted.
  Internet assignment D (Triton Project) due Thursday March 10
• Isotopes ---> Know what are they and examples of isotopes.
  Working with relative abundances; be able to solve both ways: Determining atomic weight from given relative abundances and
  If given atomic weights of isotope and sample determine relative abundances.

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