Chapters 1 & 2 Study Guide Measurements, Atomic History & Moles

Chapters 1 & 2 Study Guide Measurements, Atomic History & Moles

Chapter 1 Learning Goals

1. Describe the Kinetic Molecular Theory and be able to describe how it helps to explain the properties of gases, liquids and solids.

2. Know the common units for temperature, mass, length and volume.

3. Convert from one measure to another using the factor label method and solve problems using dimensional analysis.

4. Express measurements using the correct number of significant figures indicating the uncertain digit. Use significant figures correctly in mathematical operations.

5. Differentiate between accuracy and precision and explain the conditions under which a measuring instrument can be deemed "accurate.'' Explain how random error differs from systematic error.

6. Be able to determine the density of a substance using laboratory techniques or mathematical operations.

7. Diagram a flow chart illustrating the separation of homogeneous and/or heterogeneous mixtures. Be able to identify the mixture type, pure substances, compounds and elements. Identify the physical and chemical changes used in the separation process.

AP Chemistry

Chapter 2 Study Guide

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Chapter 2 Learning Goals

1. Be able to summarize and recognize applications of the following laws: Conservation of Mass, Law of Definite Proportions, Law of Multiple Proportions, Dalton's Atomic Theory, and Avogadro's Hypothesis.

2. Outline the development of the modern atomic model including the work of Thomson, Millikan, and Rutherford.

3. Identify the number of subatomic particles using information from the nuclear symbol for atoms, ions and isotopes.

4. Define the term atomic mass and explain why a mass spectrometer can be used to determine the atomic mass of an element. Use data from the mass spectrometer to determine the atomic mass.

5. For a given sample of an element be able to determine a) the number of moles b) the number of individual atoms c) the mass of the sample. Be able to explain the significance of using mole measurements in the chemical laboratory.

6. For a given sample of a compound you should be able to determine a) the number of moles of the compound b) the number of moles of individual ions or atoms and c) the molar mass

7. Using the Periodic Chart predict the properties of a substance from its position in the chart.

8. Describe the difference between an ionic and a molecular compound.

9. Identify the information given in a chemical and a structural formula for a molecular compound. Be able to write the formula and name from the sturctural formula.

10. Explain how cations and anions are formed and determine the ionic charge from given data.

11. Describe the difference between the ionic and the covalent bond. Predict the properties of both molecular and ionic compounds

12. Know the name of polyatomic ions.

13. Name type I, II and III binary ionic compounds; compounds composed of polyatomic ions; and common acids.

14. Given the systematic names of compounds, write the correct chemical formulas.

15. Determine the percent by mass of an element in a given compound and the percentage composition of a given compound. Predict the mass of a particular element found in a given sample of a compound.

16. Determine the empirical formula and molecular formula for a given compound from provided data and from the laboratory setting.

AP Chemistry

Chapter 2 Study Guide

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SIGNIFICANT FIGURES

NOTES CHAPTER 1

USE IN THE LAB - use all digits on electronic devices

use all marked lines and 1 estimate on instruments with gradations.

PROBLEM SOLVING - USE OF SIGNIFICANT FIGURES

How many significant figures?

40.150 g

1 m = 1000 mm 4050 mL 4000 km

RULES : 1. 2. 3. 4. 5.

AP Chemistry Chapters 1 & 2 Study Guide ? Measurements, Atomic History & Moles

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MATHEMATICAL OPERATIONS ADDITION/SUBTRACTION:

MULTIPLICATION/DIVISION

What is the volume of 14.25 g of alcohol if the density of alcohol is 0.70 g/mL. Express the volume in both milliliters and cubic centimeters.

CONVERSIONS - USE DIMENSIONAL ANALYSIS. SHOW ALL UNITS AND CANCEL

100 base L, g, m

Convert 0.0537 cm to meters

to nanometers

to kilometers

Convert a density of 4.85 g/ cm3 to kg/L Convert 25.0 cm3 to m3 and dL

AP Chemistry Chapters 1 & 2 Study Guide ? Measurements, Atomic History & Moles

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The aluminum in a package containing 75.0 ft2 of kitchen foil weighs approximately 12.0 oz. Aluminum has a density of 2.70 g/cm3. What is the approximate thickness of the aluminum foil in millimeters? ( 1 oz = 28.4 g)

PERCENT PROBLEMS

The density of a solution of sulfuric acid is 1.285 g/ cm3 and it is 38.08 % acid by mass. What volume of the acid solution ( in mL) do you need to supply 125 g of sulfuric acid?

ACCURACY AND PRECISION

Three student lab groups measured the mass of five aluminum bars, each labeled "one mole'.

Al bar 1 2 3 4 5

Group A 28.01 28.38 28.38 28.67 28.40

Group B 27.00 26.90 25.70 28.51 25.41

Group C 26.78 26.93 27.00 26.96 27.21

What is the mass of 1 mole of aluminum exactly?

How would you describe the accuracy and precision of each group's measurements?

Propose explanations for the patterns you see in each group's data.

Determine the % Error for Group A's Bar 1.

AP Chemistry Chapters 1 & 2 Study Guide ? Measurements, Atomic History & Moles

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