Welcome to Chemistry II – Week II
Portland Evening Scholars
Mr. Treothe Bullock – Instructor
 Syllabus Revision
 Noteboo...
Chemistry II – Week II
Homework for next week
 Complete Chapter 7 review sheets – 7-1
 Complete Build a Molecule Lab
 R...
Chapter 7
 Chemical Formula’s
 Be able to read elements
and number of atoms
 Monatomic Ions
 Are single charged atoms
...
Chapter 7
 Covalent Network Compounds
 These compounds are written
in the simplest ratio of
elements despite large
netwo...
Chapter 7
 Molar Mass as a
Conversion Factor
 Moles x molar mass =
mass in grams
 Percentage
Composition
 Mass of elem...
Chapter 7
 Molar Mass as a
Conversion Factor
 Moles x molar mass =
mass in grams
 Percentage
Composition
 Mass of elem...
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Chem II Day II

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Chem II Day II

  1. 1. Welcome to Chemistry II – Week II Portland Evening Scholars Mr. Treothe Bullock – Instructor  Syllabus Revision  Notebook set up and notes  Levels of Questioning  Cornell Notes  4 pages of notes on review required with questions from each level  Chapter Review Presentations : Oral with Paper examples – 5 /10 minutes each  Documents will be posted in sequence  Take Cornell notes  After each presentation summarize and/or write a question you still have  Unit 7 – Pre – Assessment and Overview  Building a Molecule pHet Lab –  Course website is bullockchem.wordpress.com  Go to Virtual Lab Page and open the Lab  Lab Safety Agreements Due  Turn in Academic Bio’s
  2. 2. Chemistry II – Week II Homework for next week  Complete Chapter 7 review sheets – 7-1  Complete Build a Molecule Lab  Remember lab safety sign off if needed.  Get a folder for class work if you don’t have one yet.
  3. 3. Chapter 7  Chemical Formula’s  Be able to read elements and number of atoms  Monatomic Ions  Are single charged atoms  Binary Ionic Compounds  Use ide at the end of the element name (Main group elements or Stock system Roman numerals (d block)  (Table 7-1)  Naming Binary Ionic Compounds  2 elements in these compounds  Naming Binary Molecular Compounds  Nomenclature or naming systems rely on both elements.  The prefix system of naming describes the number of atoms (Table 7- 3 & 4)  Some elements have more than one ionic form requiring stock system ID  Polyatomic ions exist and have unique names  (Table 7-2)
  4. 4. Chapter 7  Covalent Network Compounds  These compounds are written in the simplest ratio of elements despite large networks  Acids and Salts  Most are either binary (2 elements H & a halogen)  or  oxyacids (H, O & 3rd nonmetal element)  Table 7-5  Oxidation Numbers  Indicates general distribution of electrons in molecular compound or ion  Rules on p 216  Using Oxidation Numbers for Formulas and Names  Many nonmetals have more than one oxidation state  Table 7-6 and Appendix Table A-15 list common oxidation numbers  2 naming systems exist – prefix and Stock (stock is the oxidation number)  Formula Masses  Is the sum of the average atomic masses of all atoms represented in its formula.  Molar Masses  Mass if one mole of a substance
  5. 5. Chapter 7  Molar Mass as a Conversion Factor  Moles x molar mass = mass in grams  Percentage Composition  Mass of element in sample of compound / mass of compound x 100 = % element in compound  Calculation of empirical formulas  Consists of the symbols for the elements combined in a compound, with subscripts showing the smallest whole- number ratio of the different atoms in the compound.  Use % composition and determine mass of individual elements – establish a molar ratio  Calculation of Molecular formulas  X (empirical formula) = molecular formula  X (empirical formula mass) = molecular formula mass
  6. 6. Chapter 7  Molar Mass as a Conversion Factor  Moles x molar mass = mass in grams  Percentage Composition  Mass of element in sample of compound / mass of compound x 100 = % element in compound  Calculation of empirical formulas  Consists of the symbols for the elements combined in a compound, with subscripts showing the smallest whole- number ratio of the different atoms in the compound.  Use % composition and determine mass of individual elements – establish a molar ratio  Calculation of Molecular formulas  X (empirical formula) = molecular formula  X (empirical formula mass) = molecular formula mass
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