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. 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. 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. 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. 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. 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