• Define mass as the measure of atomic “stuff”; contrast with volume – the amount of space an object occupies.
  • Use a multiple beam or double-pan balance to determine the mass of various objects.
  • Record the value of an object’s mass in a manner consistent with the limit of precision of the balance.
  • Represent class data using a histogram; use the histogram to interpret trends in the data.
  • Develop, from experimental evidence, the law of conservation of system mass.
  • Relate the volume of a container (in cm3) to the volume of liquid it contains (in mL).
  • Recognize that instruments have a limit to their precision; relate the data recorded to the quality of the measurement.
  • Given a graph of mass vs. volume of a various substances, relate the slope to the density of the substances.
  • Recognize that density is a characteristic property of matter (i.e., it can be used to help identify an unknown substance).
  • Use density as a conversion factor between mass and volume; apply this to quantitative problems.
  • Use differences in density of solids, liquids and gases as evidence for differences in the structure of matter in these phases.



Lab Safety
GPB: Scientific Method 
Eureka Mass
Density Calculations
Graphing Guide
Graphing Line of Best Fit in Desmos
Significant Figures
Physical & Chemical Properties & Changes
Scientific Notation
States of Matter
Properties of Matter
Physical vs. Chemical Properties
Physical vs. Chemical Changes
Dimensional Analysis
Metric & Double Conversions
Operations with Scientific Notation
Unit Conversions with Cubed Units



Explore States of Matter at PhET
Explore Density, Mass & Volume at PhET


NFPA Diamond
Practice Identifying Variables
Printable Ruler
Practice: Physical vs. Chemical Changes (Khan Academy)
More Practice: Physical vs. Chemical Changes