This document provides an agenda for a Chemistry II class. It includes completing chapter reviews, presentations, a molecule simulation lab, learning about chemical naming and composition, working on a final project, and covering content in Chapter 7 including chemical formulas, binary compounds, acids and salts, oxidation numbers, and calculating molecular formulas. Homework includes reviewing Chapter 7 and advancing work on a final project.

1. Welcome to Chemistry II – Day III
Portland Evening Scholars
Mr. Treothe Bullock – Instructor
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Complete - Chapter Review
Presentations
 Last chance to present for full
credit
Build a Molecule Simulation Lab
 Debrief & Questions
Chemical Naming and
Composition - The Language of
Chemistry
 Formulae & Naming
Systems
 Practice reading and writing
names

Final Project Work time
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Be ready to share what you think
you will research
It is an option to work with a
partner – you will double the
components you research on your
object
Today’s Goal – Research and
build slides I-III
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Identify Your specific Object
Develop a list of
components / ingredients
Choose a component to
focus on
Research raw materials
sourcing

2. Chapter 7

Chemical Formula’s

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Are single charged atoms
Binary Ionic Compounds
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Naming Binary Molecular
Compounds
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Monatomic Ions
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Be able to read elements
and number of atoms

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
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2 elements in these
compounds
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Nomenclature or naming
systems rely on both
elements.
The prefix system of
naming describes the
number of atoms (Table 73 & 4)
Some elements have more
than one ionic form
requiring stock system ID
Polyatomic ions exist and
have unique names
(Table 7-2)

3. Chapter 7

Covalent Network Compounds
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These compounds are written
in the simplest ratio of
elements despite large
networks
Using Oxidation Numbers for
Formulas and Names
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Acids and Salts
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Most are either binary
(2 elements H & a halogen)
or
oxyacids (H, O & 3rd nonmetal
element)
Table 7-5
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Formula Masses
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Oxidation Numbers
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Indicates general distribution
of electrons in molecular
compound or ion
Rules on p 216
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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)
Is the sum of the average
atomic masses of all atoms
represented in its formula.
Molar Masses

Mass if one mole of a
substance

4. Chapter 7

Molar Mass as a
Conversion Factor
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Moles x molar mass =
mass in grams
Percentage
Composition

Calculation of empirical
formulas
Mass of element in
sample of compound /
mass of compound x
100 = % element in
compound

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Consists of the symbols for
the elements combined in a
compound, with subscripts
showing the smallest wholenumber ratio of the different
atoms in the compound.
Use % composition and
determine mass of individual
elements – establish a molar
ratio
Calculation of Molecular
formulas
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X (empirical formula) =
molecular formula
X (empirical formula mass) =
molecular formula mass

5. Welcome to Chemistry II – Week II
Homework for next week


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Complete Chapter 7 review sheets –
sections 1 & 2
Remember lab safety sign off if needed.
Progress on Final Project far enough to
know you can commit on your object.

6. Welcome to Chemistry II – Week II
Homework for next week



Complete Chapter 7 review sheets –
sections 1 & 2
Remember lab safety sign off if needed.
Progress on Final Project far enough to
know you can commit on your object.