|
Chemistry Syllabus 2002 |
|
|
Chemistry 4th Edition by Addison-Wesley |
|
|
|
|
Gary Eatherton - Instructor Montgomery Co R-2 |
|
| |
|
|
1997 Wilbraham/Staley/Matta |
|
|
|
|
|
|
|
Chapter |
Description |
Duration |
Student Objectives |
MAP performaqnce Goal |
MAP SC Standard |
Frameworks |
A+ objectives |
Assessments and Assignments |
Activities & Labs |
|
|
|
|
|
|
|
|
|
|
|
|
2 |
Scientific Measure |
2-1/2 weeks |
Determine the number of significant figures in a measured quantity. |
1.6, 1.8 |
SC7 |
III A |
|
work sheets - scientific notation, metric conversions and measurements,
density page34-36 7,9,10,38,41,44,47,53,57 teacher
generated assessment |
intro math quiz, density lab with pennies, lab safety |
| |
|
|
Express the result of a calculation with the proper number of significant
figures |
|
|
|
|
|
Convert temperatures |
|
|
|
|
|
Perform density calculations |
|
|
1 |
Introduction - Matter and Change |
1-1/2 weeks |
Distinguish between physical and chemical properties and between chemical
and physical changes |
1.6, 1.8 |
SC 1,2 |
II B, |
Distinguish between physical and chemical properties and between chemical
and physical changes |
Peroidic elements - symbols and names worksheets page 22 -29,
31,35,38,43,47,56,57,58; element quiz; teacher generated assessment |
element quiz, Lab-evidence for Chemical Change, Lab-paper chromatography |
| |
|
|
Differentiate between the three states of matter |
|
|
|
| |
|
|
Distinguish between elements, compounds, and mixtures - Give the symbols and
names for assigned elements |
|
|
|
|
3 |
Problems Solving |
2 weeks |
Use unit analysis to solve problems |
1.6, 1.7, 1.8 |
SC 7 |
III A |
|
page 78 - 33, 36, 38, 40, 42, 45, 46, 48, 51; worksheets; teacher generated
assessment |
Unit analysis aproach to problem solving |
| |
|
|
Interconvert metric and SAE measurements and values |
|
| |
|
|
Perfect techniques to set up and solve multistep problems |
|
|
4 |
Atomic Structure |
2 weeks |
Describe the composition of an atom in terms of protons, neutrons, and
electrons. |
1.6, 1.8 |
SC 1 |
III A |
Describe the composition of an atom and its subatomic particles |
p 105-108 1,3,7,21,29,43,47,51 worksheets; electron. Proton, neutron quiz;
teacher generated assessment |
detect radiation with GM tube |
| |
|
|
Give the approximate size, relative mass, and charge of an atom, proton,
neutron, and electron |
|
|
|
| |
|
|
Write the chemical symbol for an element, if you have been given its mass
number, atomic number, and perform the reverse operation |
|
|
|
| |
|
|
Write the symbol, atomic number, charge, mass, and charge for an atom or ion |
Use the periodic table to predict physical properties of elements |
|
|
| |
|
|
Use the periodic table to predict the charges of monatomic ions |
|
|
| |
|
|
Use the periodic table to predict whether an element is a metal, metalloid,
or non-metal |
|
|
|
5 |
Chemical Names and Formulas |
2 weeks |
Write the simplest formula for a compound |
1.6, 1.8 |
SC 1 |
III A |
|
worksheets, page 137 47,50,52,56,59,62; teacher generated assessment |
Demo- hydrogen peroxide and magnesium dioxide Demo-hydrogen production
from zinc and HCl |
| |
|
|
Write the name of a simple inorganic compound from its chemical formula and
vise versa |
|
|
6 |
Chemical Quantities |
2 weeks |
Determine the number of moles from grams or volume of a chemical |
1.6, 1.8 |
SC 1 |
III A |
|
page 170 - 41,42,43.44.45a,b,47b,c, 48a,c,e, 50,51.52a,c,e,
53b,d,56a,c,59a,c; teacher generated assessment |
|
| |
|
|
Perform mole, mass, volume conversions |
|
|
|
| |
|
|
Calculate the empirical and molecular formula of a compound, having been
given appropriate analytical data such as elemental percentages or the
quantity of carbon dioxide and water produced by combustion |
Use the periodic table to predict chemical reactivity , Balance chemical
equations and use the equation to calculate quantities of chemicals involved
in the reaction |
|
Lab-Silver Nitrate and Copper lab |
|
|
|
|
Balance chemical reactions |
|
|
|
7 |
Chemical Reactions |
2 weeks |
Predict the products of a chemical reaction |
1.6, 1.7, 1.8 |
SC 1 |
III A |
|
204-205 56d,58a,b,c 60c, 62a-e ; teacher generated assessment |
|
| |
|
|
Classify the types of chemical reactions |
Predict the products of a chemical reaction |
Lab-Silver and Nitric Acid |
| |
|
|
Determine the limiting reactant in a reaction |
|
|
|
8 |
Stoichiometry |
2 weeks |
Determine the moles of reactants and products involved in chemical reactions |
1.6, 1.7, 1.8 |
SC 1 |
III A |
|
p 233-235 1,3,5,7,13,17,19,23,29,33,37; teacher generated assessment |
|
| |
|
|
Determine the volume of gaseous reactants and products involved in chemical
reactions |
|
|
|
| |
|
|
Determine the percent and actual yield for a reaction |
|
|
|
| |
2nd Semester |
|
|
|
|
|
|
|
|
|
9 |
The States of Matter |
1-1/2 weeks |
Employ the kinetic-molecular model to explain the differences in motion of
particles in gases, liquids, and solids and how these relate to their states |
1.6, 1.7, 1.8 |
SC 1 |
III A |
|
|
|
| |
|
|
Explain the meaning of the terms: viscosity, surface tension, critical
temperature, and critical pressure, and account for the variations in these
properties in terms of intermolecular forces and temperature |
|
|
|
|
|
|
|
|
|
|
|
| |
|
|
Explain the way in which the vapor pressure of a substance changes with
intermolecular forces and temperature |
|
page231, 28,29,31,35,36,37,48,49,50; teacher generated assessment |
Demo-butane phase change Lab-melting of ice in fresh and salt water |
| |
|
|
Describe the relationship between the pressure on the surface of a liquid
and the boiling point of the liquid |
|
|
|
|
Ch 9 continued |
The States of Matter |
|
Given the needed heat capacities and enthalpies for phase changes, calculate
the heat absorbed or evolved when a given quantity of a substance changes
from one condition to another |
|
|
|
| |
|
|
Distinguish between crystalline and amorphous solids |
|
|
|
|
|
|
| |
|
|
List the important units in which energy is expressed and convert from one
to another |
|
|
|
|
|
|
|
10 |
Thermochemistry |
1-1/2 weeks |
Define the first law of thermodynamics |
1.6, 1.8 |
SC 1, 5, 8 |
IIIB |
Apply the laws of Thermodynamics to chemical reactions and physical change |
p 286-288 35,38,41,46,48,49,51,52,56,59,68,70,74; teacher generated
assessment |
Lab-thermodynamics of NaOH and HCl |
| |
|
|
Define enthalpy, and relate the enthalpy change in a process occurring at
constant pressure to the heat added to or lost by the system during the
process |
|
|
|
|
|
|
|
Sketch an energy diagram |
|
