مكتبة الباوربوينت للثانوية العامة ( رياضيات - كيمياء - فيزياء - أحياء )عربي - لغات

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. مكتبة الباوربوينت للثانوية العامة ( رياضيات - كيمياء - فيزياء - أحياء )عربي - لغات




مكتبة الباوربوينت للثانوية العامة ( رياضيات - كيمياء - فيزياء - أحياء )عربي - لغات
Crossword puzzle and periodic table activity.


4
Atomic model
Historical overview of the atom from Democritus to Bohr.

5
Alkali Metals Lab
Combining alkali metals with water – what could be more fun than explosions?

6
Periodic Trends
Examining how ionization energy and electron affinity change with an element's position on the periodic table.

8
Ionic Bonding
Lewis dot diagrams and chemical bonding between metals and nonmetals.


9
Covalent Bonding
Chemical bonding between two nonmetals (a continuation of yesterday's worksheet).

10
Physical Properties Lab
Comparing the physical properties of two solids. (This is a good time to teach students how to light and use Bunsen burners.)


11
Electronegativity
Using electronegativity to predict bond strength and solubility. The
second half of today's class is spent learning element names and
symbols.


12
Naming
Rules for naming ionic and covalent compounds.


13
...
Continuing yesterday's work. Rules for naming acids, bases, and hydrates.


14
Naming Review
It is difficult to name all types of compounds. Today's assignment is a
good way for students to gauge their understanding of this topic.


15
Types of chemical reactions
Reaction types include synthesis, decomposition, single displacement,
and double displacement. Part 1 is set up as a lab but is better as a
demonstration. Students should do part 2 themselves - it's fun.


16
The Activity Series
Predicting chemical reactions using the activity series. (Note: brief lab activity.)


17
Review
Review of unit 1: matter and chemical bonding.



Unit 2: Quantities in Chemical Reactions
#
Topic
Description
Links
20
Proportions
Proportions and percentage composition – lab and calculations.


21
Significant Digits
Significant digits and isotopic abundance.


22
The Mole
Introducing the mole concept. Today's lesson is brief, which leaves time to return and discuss the tests from Unit 1.


23
Molar Mass
Molar mass and simplest formula calculations (see yesterday's lesson for files).
24
Molecular Formula
Empirical (i.e. simplest) and molecular formula calculations.


25
Hydrates Lab
Applying the molecular calculations from yesterday to determine the number of moles in a hydrate.


26
Balancing Equations
Balancing chemical equations and balancing nuclear equations.


27
Calcium Lab
The reaction of calcium with water.


28
Factor Label Method
Introducing the factor label method, which will be used for all subsequent lessons in this unit.


29
Stoichiometry
Introducing stoichiometry - used to calculate the relative quantities of two chemicals in a reaction.


30
...
Continuing the calculations from yesterday.
31
Limiting Reagents
Limiting reagents adds another layer of complexity to stoichiometry.


32
Limiting Reagents Lab
Using the concepts from yesterday's lesson to predict the limiting reagent in a reaction.


33
...
Completing yesterday's lab and the calculations from the first "Limiting Reagents" class.
34
Percentage Yield
Comparing theoretical and actual yields to determine percentage yield. Builds on stoichiometry and limiting reagents.


35
...
Continuing the percentage yield calculations from yesterday.
36
Review
Review of unit 2: quantities in chemical reactions.


Unit 3: Solutions and Solubility
#
Topic
Description
Links
38
Solubility
Introduction to solubility, including a discussion of intermolecular forces.


39
Concentration
Concentration = quantity of solute ÷ quantity of solution. This lesson
focuses on concentration calculations (V/V, W/W, W/V, ppm, ppb, mol/L).


41
Molar Solutions
Making molar solutions from solids – procedure and calculations. (Note: brief lab activity.)


42
...
Making molar solutions from liquids – similar to molar solutions from
solids except pipettes are used to measure moles (via volume). (Note:
brief lab activity.)


43
Net Ionic Equations
Writing net ionic equations by breaking salts into ions: e.g. MgCl2(aq) really means Mg2+(aq) + 2Cl–(aq).


44
Solubility Rules
Today's lab involves a series of double displacement reactions that
yield precipitates. Results are summarized as a series of solubility
rules.


45
...
Finishing the questions from yesterday's lesson.
47
Solubility Curves
Students investigate the solubility of a chemical at different
temperatures. Class data is plotted to create a "solubility curve".


48
Water Treatment
Water treatment crossword puzzle.


49
Solutions Stoichiometry
Extending the stoichiometry calculations from Unit 2 to include solutions.


50
Conductivity Lab
Students investigate why some solutions conduct electricity but others do not.


51
Acids & Bases
Looking at acid/base properties, pH, the Arrhenius definition of acids
and bases, and the Bronsted-Lowry concept. (Note: brief lab activity.)


52
Neutralization
Writing and balancing neutralization reactions.


53
Titration
Titration: the quantitative analysis of neutralization reactions. Note:
teachers should spend time before the lab showing students how to set up
and use equipment.


54
...
Finishing yesterday's work. Students compete in a competition to see who is "best with a burette".

55
Review
Review of unit 3: solutions and solubility.



Unit 4: Gases & Atmospheric Chemistry
#
Topic
Description
Links
58
KMT
Introduction to gases, starting with a discussion of the Kinetic Molecular Theory. Students complete questions 1-10.


59
Pressure
Finishing yesterday's lesson, including demonstrations. The last
demonstration is more dramatic with a balloon rabbit. This lesson is
short to give time to return tests from Unit 3.
60
Boyle's Law
Students investigate the mathematical relationship between pressure and volume (i.e. Boyle's Law).


62
Charles's Law
Finishing the Boyles' Law questions from last class. The second half of today's lesson is spent on Charles's Law.


63
Combined Gas Law
Combining Boyle's Law and Charles's Law to get the "combined gas law".


64
Weighing Gases Lab
How do you weigh a gas? In today's lab, students find out.


65
Partial Pressures
Dalton's law of partial pressures: the total pressure of a mixture of
gases is equal to the sum of the pressure of individual gases.


66
Molar Volume Lab
In today's lab, students determining the "molar volume" of hydrogen gas.


67
Ideal Gas Law
The ideal gas law (PV=nRT), like the other gas laws, is used to
calculate one unknown variable when all other variables are known.
(Note: brief lab activity.)


68
Gas Stoichiometry
Extending the stoichiometry calculations from Unit 2 to include gases.


69
Review
Review of unit 4: gases & atmospheric chemistry.


Unit 5: Hydrocarbons and Energy
#
Topic
Description
Links
71
Foods Lab
Introduction to organic chemistry.


72
Hydrocarbon Models
Students build models and draw diagrams of hydrocarbons: alkanes, alkenes, alkynes, and aromatics.


73
Combustion
Students investigate the products of complete and incomplete combustion.


74
Hydrocarbon Naming
Organic nomenclature follows a different set of rules than inorganic
nomenclature. Students learn these rules and try several examples.


75
...
This period is spent entirely on practice problems. Students apply the rules they learned yesterday.


76
Chemsketch
Students learn to use ChemSketch - a program for drawing organic molecules. A computer lab with ChemSketch installed is needed.

77
Isomers & Polymers
Students build models of isomers (compounds with the same chemical
formula but different structures) and polymers (long chains of
carbon-containing monomers).


78
Alkanes and alkenes Lab
Comparing the chemical properties of alkanes and alkenes to illustrate
the reactivity of a double bond. This is a lab, but it may be better as a
demonstration.


79
Thermochemistry
Concepts related to thermochemistry are introduced, including calorimetry, heat capacity, molar heat of reaction, etc.


80
Candle Lab
Students determine the molar heat of combustion for paraffin wax, applying the concepts learned in yesterday's lesson.


81
Bond Energies
Using bond energies to predict the energy change when atoms rearrange themselves in chemical reactions.


82
Review
Review of unit 5: hydrocarbons and energy.


85
Exam Review
Review of the course, mainly focusing on calculations.


86

Atomic Structure
An overview of the model of the atom, stopping at Bohr and introducing EM radiation.




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