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Ch.1 Matter and MeasurementsWorksheetSee all chapters
All Chapters
Ch.1 Matter and Measurements
Ch.2 Atoms and the Periodic Table
Ch.3 Ionic Compounds
Ch.4 Molecular Compounds
Ch.5 Classification & Balancing of Chemical Reactions
Ch.6 Chemical Reactions & Quantities
Ch.7 Energy, Rate and Equilibrium
Ch.8 Gases, Liquids and Solids
Ch.9 Solutions
Ch.10 Acids and Bases
Ch.11 Nuclear Chemistry
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
What is Chemistry?
The Scientific Method
Classification of Matter
States of Matter
Physical & Chemical Changes
Chemical Properties
Physical Properties
Intensive vs. Extensive Properties
Temperature (Simplified)
Scientific Notation
SI Units (Simplified)
Metric Prefixes
Significant Figures (Simplified)
Significant Figures: Precision in Measurements
Significant Figures: In Calculations
Conversion Factors (Simplified)
Dimensional Analysis
Specific Gravity
Density of Geometric Objects
Density of Non-Geometric Objects

The number of Significant Figures for a value affects its precision. 

Exact Numbers, Inexact Numbers, & Sig Figs

Concept #1: Exact vs Inexact Numbers

Example #1: Determine if the following statement deals with an exact or inexact number: The combined mass of all doses of a bronchodilator administered to a patient measure 10.0 mg.

Concept #2: Rules for Significant Figures

Example #2: Determine the number of significant figures in the following value: 0.003840

Practice: How many sig figs does each number contain?

a) 100. min                                                          

b) 17.3 x 103 mL

c) 10 apples

Practice: Indicate the number of significant figures in the following: 

A liter is equivalent to 1.059 qt.