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Chemistry 11

Introduction     New Microsoft Word Document.docx ,     

Chapter No.  2   3   4   5   6   7   8   9   


Chapter 2

Powerpoints: 1_UnitConversions.ppt ,     2_Significant_Digits.pdf ,     2_significant.ppt ,     2_significant_digits.pdf ,     3_Accuracy Precison.ppt ,     3_Accuracy_Precison.ppt ,     4_readingscales.ppt ,     5_uncertainty.ppt ,     6_Review.pptx ,     PrecisionUncertaintyAccuracy.pdf ,     

Worksheets: Answers to Extra Unit Conversions.doc ,     CH11 Unit 2 Review.doc ,     CH11 Unit 2 Review.pdf ,     CH11 Units1-3Outline.doc ,     Chapter 2 Density Review Questions Chemistry 11 JB.doc ,     HandIn1UnCon.pdf ,     HandIn2SigDigs.doc ,     Sig Figs Worksheets.pdf ,     Significant Digits.pdf ,     Unit 2 Intro to Chemistry S.pdf ,     Unit 2 Review.doc ,     Unit 2 Rewrite D.docx ,     Unit2ReviewKEYp_1.pdf ,     Unit2ReviewKEYp_2.pdf ,     Unit2ReviewKEYp_3.pdf ,     Unit2ReviewKEYp_4.pdf ,     checklist.docx ,     chem 11 worksheet.doc ,     exponentadditionandsubtraction.docx ,     review ideas.docx ,     sigfigcaluclations.pdf ,     sigificatn digits.pdf ,     significant figures rules and worksheet.pdf ,     unit_2_review.doc ,     unit_2_rewrite_d.docx ,     

2 .2 SI Units

1. A “base unit” is the foundational unit of measurement like “m”, it’s more familiar unit.

2. Here is some example of base unit in the international system. (SI)

                            Quantity                     Written Unit                      Symbol

                            Length                      meter                                m

                            Mass                          gram                                   g

                            Time                           second                                s

3. There are also some prefix using before the unit: mega, kilo, deci, centr, milli, micro, as symbol: M, k, d, c, m.

4. There are some equivalences like 1ml= 1cm3 1m3=103L 1t=103kg

5. Lots of re-write question are in this topic. Transferring one unit to another, we should be careful of the prefix and the exponential.

Worksheet:   ws1_2.1-SI-unit.docx ,     ws1_ws12.1-SI-unit.docx ,     ws1key_2.1-SI-unit-answer-key.docx ,     ws1key_ws1key2.1-SI-unit-answer-key.docx ,     

2 .3 Metric Conversion

1. All prefix symbols are directly connected with the base unit, which it becomes a central unit. For example: m for meter has a branch of Mm, km, dm, cm, mm.

2. Metric conversions is basically solving unit conversions question using prefix symbols and exponential equivalent.

3. When we are doing unit conversion question, there are two method which are 3-step method and 1-step method. It's harder to make a mistake when we are using these two methods.

4. A derived quantity is a combination of two or more other values for example: molar concentration.

5. For example: A derived symbol “c” stand for one derived quantity, having derived units, which is the combination of change of H, change of T and m.

Tutorial Videos:    Amazing 9 Layer Density Tower - Sick Science! #012 (1).mp4 ,     

Worksheet:   ws1_Metric-Conservation.docx ,     ws1_ws1Metric-Conservation.docx ,     ws1key_Metric-Conservation-answer-key.docx ,     ws1key_ws1keyMetric-Conservation-answer-key.docx ,     

2 .4 2.4 Density

1. Mass is the quantity of matter in an object. Volume is the amount of space an object occupy. Density is the mass of a particular volume of an object.

2.  The density of an object is measured by its mass per unit of volum, namely the formular of density is mass divided by volume. The unit of density is g/L.

3. We may rearrange the density formular to V = m/d or m = Vd depending on what information the question ask for.

4. The density of water at 4ºC is fixed --- d = 1000.0 g/L (1.0000 g/mL). Therefore, for water at 4ºC, 1g = 1mL.

5. Objects that are less dense (liquid or solid) will float on liquids with greater density.

Tutorial Videos:    24.mp4 ,     242.mp4 ,     

Worksheet:   ws1_Ch-2.4-Density.docx ,     ws1key_Ch-2.4-Density-Answer-key.docx ,     

2 .5 2.5 Significant Figures And Experimental Uncertainty

1. Sig-fig rules are not for exact values that have infinite sig-figs, which include definitions, countings, and abstract numbers.

2. For zeros in decimals, the leading ones are not significant while the ones at the end are. Zeros in whole numbers are not significant unless there's a decimal point. 

3. In a measurement like "28.6 plus or minus 0.1 cm", "28" is the certain digits, ".6" is the uncertain digit, "plus or minus 0.1" is the uncertainity, and finally, "cm" is the unit.

4. Uncertainity is calculated by dividing the range (the difference between the two subdivisions next to the measured value) by the number of subdivisions.

5. No rounding till the last step of the calculation.

6. The difference between accuracy and precisition is: accuracy tells how close a measurement is to the real value, while precision shows how close the measurements are to each other. (Plus, greater precision means more sig-figs.)

Tutorial Videos:    2-5.mp4 ,     252.mp4 ,     

Worksheet:   ws1_Ch-2.5-Significant-Figures-and-Experimental-Uncertainity.docx ,     ws1key_Ch-2.5-Significant-Figures-and-Experimental-Uncertainity-Answer-Key.docx ,     

Chapter 3

Powerpoints: 3.1 basic definitions.pptx ,     3.3 classification of matter.pptx ,     3.4 separation of matter2.pptx ,     3.5 phase changes.pptx ,     3.5_phase_changes.pptx ,     Ch11MatterClassification.pdf ,     Ch11Phys_ChemChanges.pdf ,     Chem Jeoprady.ppt ,     Classification of Matter 2.pdf ,     alloys.ppt ,     scientificmethod.ppt ,     

Worksheets: 3.3_Matter_Flow_Chart.doc ,     3.4 Vocabulary for making flow chart.xlsx ,     Chemistry 11 Chapter 3 Dictionary Assignment - Copy.docx ,     Chemistry 11 Poster Project Outline JB - new.doc ,     Dictionary rubrics.docx ,     Is Gravity a Theory or a Law.docx ,     Physical and Chemical Properties.xlsx ,     Unit 3 Review.doc ,     concept map properties.png ,     dictionaryassignment.docx ,     separation methods.docx ,     

3 .1 Some Basic Definitions In Science

1. We learn that qualitative is non-numerical, descriptive information and quantitative is numeral information. For example, five marbles of 1.5cm diameter each is quantitative and a bunch of beautiful, round and smooth glass marbles is qualitative.

2. Hypothesis is an unproven proposal which attempts to explain certain facts or observation, which is an educated guess based on some evidences.

3. Theory is a tested explanation intended to explain some aspects of the nature world.

4. Laws summarize the results of many experiments and describe recurring facts or events in nature.

5. Hypothesis is an assumption while theory can be used to make a prediction.

Tutorial Videos:    01_The Scientific Method Song.failed-conv.mp4 ,     01_Theory vs Hypothesis - Science Rap Video - Coma Niddy Univer.failed-conv.mp4 ,     01_What is Science and the Scientific Method.failed-conv.mp4 ,     311.mp4 ,     312.mp4 ,     

Worksheet:   ws1_3.1-questions.docx ,     ws1key_3.1-answer-key.docx ,