Exam

=Second Semester Exam=

2 Hours Friday, 6 June 8:25 -10:25 Be sure to bring Redo and rework old worksheets and quizzes. You will receive a periodic table and a list of common polyatomic ions. Visit student-generated review wiki topics Consult a source when you have a question, need help or need practice Focus your time on your weakest areas
 * Ruler
 * Calculator
 * Pencil/Pen/Eraser
 * Biology Textbook to turn in

Chemical naming and formula writing

 * Binary Ionic ( only 2 elements, metal+nonmetal, -ide)
 * Binary Ionic (with multi-charge cation) Tranistion metals can sometimes have more than one charge: Au. Pb, Fe, Cu, etc)
 * Polyatomic (covalently bonded group that ionically bonds with another ion)
 * Binary Covalent (nonmetal+nonmetal, prefixes)
 * Diatomic (halogens, nonmetal, two of same element)
 * Common Acids (Hydrogen ion + anion)
 * Alkanes (hydrocarbons, ethane, butane, pentane, etc....look to prefixes)

Polar covalent bonding and the behaviour of water

polar vs. nonpolar characteristics polar: slight pos side and slight neg size Electronegativity Hydrogen bonding cohesion adhesion capillary action

Stoichiometry
__**Ch. 7.1**__

The amount of a substance that contains 6.02 x 10^23 particles of that substance Ex: the gram molecular mass of SO3 is: 80.1 (what you do is get the mass of sulfur which is 32.1, then you get the mass of oxygen and times it by three because there are three atoms (48.0) and then just add the two together to get 80.1)
 * What is a Mole????**
 * Avogadro’s number:** 6.02 x 10^23
 * Representative particles:** the species such as atoms, molecules, or ions (formula units) that is present in a certain substance.
 * Gram Atomic Mass:** The atomic mass of an element expressed in grams. For example the gram atomic mass of carbon is 12.0 grams. Gram atomic mass applies o a SINGLE atom!
 * Gram Molecular Mass**: The mass of any molecular compound. It is the mass of 1 mol of that compound.
 * Gram Formula Mass:** The mass of 1 mole of an ionic compound

Practice Problem 1 How many moles of magnesium is 3.45 x 10^23 atoms of magnesium?
 * Practice Problems:**

Practice Problem 2 How many atoms are in 3.45 mol of propane?

Practice Problem 3 What is the gram molecular mass of hydrogen peroxide (H2O2)?

Practice Problem 4 What is the gram formula mass of ammonium carbonate ((NH4)CO3)?

Answers: 1) 5.73 x 10^ -1 mol Mg. 2) 2.28 x 10^2 atoms 3) 34.0 g 4) 96.0 g

relationship between mass, moles, and elementary particles 22.4 g/L (STP 101.3 kPa) Molar mass molarity molality concentration: solute, solvent, solution preparation of solutions and dilutions saturated, unsaturated, supersaturated  **see link-->** http://labscience10ablock.wikispaces.com/stoichiometryreviewpart1

Sample problems for mole-mass and mole volume relationships:

How many grams are in 9.45 mol of dinitrogen trioxide (N2o3) 9.45 mole N2O3 x 76.0 g N2O3/1.00 mol N2O3= 718.2 g N2O3 Basically we're just using a conversion rate to convert moles of a substance the number of grams of a substance. Because 1 mol of N2O3 has a mass of 76.0 g, and there are almost ten moles of the compound, the answer should be about 700. The answer has been rounded to the correct number of significant figures

Biology Topics
Evolution Genetics DNA, DNA replication, and protein synthesis