Petrucci • Harwood • Herring • Madura GENERAL CHEMISTRY Ninth Edition Principles and Modern Applications Chapter 1: Matter—Its Properties and Measurement Philip Dutton University of Windsor, Canada Prentice-Hall © 2007 Slide 1 of 28 General Chemistry: Chapter 1 Prentice-Hall © 2007 Contents 1-1 1-2 1-3 1-4 1-5 1-6 1-7 The Scientific Method Properties of Matter Classification of Matter Measurement of Matter: SI (Metric) System Density and Percent Composition: Their Use in Problem Solving Uncertainties in Scientific Measurements Significant Figures Focus On The Scientific Method at Work: Polywater Slide 2 of 28 General Chemistry: Chapter 1 Prentice-Hall © 2007 1-1 The Scientific Method • Louis Pasteur (1822-1895) – Developer of Germ Theory – Pasteurization – Rabies Vaccination • Called the greatest physician of all time by some. • He was a chemist by training and profession. Slide 3 of 28 General Chemistry: Chapter 1 Prentice-Hall © 2007 Figure 1-1 The Scientific Method Illustrated Slide 4 of 28 General Chemistry: Chapter 1 Prentice-Hall © 2007 1-2 Properties of Matter Matter: Occupies space, has mass and inertia Composition: Parts or components ex. H2O, 11.19% H and 88.81% O Properties: Slide 5 of 28 Distinguishing features physical and chemical properties General Chemistry: Chapter 1 Prentice-Hall © 2007 1-2 Classification of Matter • • • • • Matter is made of atoms. 114 elements. About 90% available from natural sources Compounds are comprised of two or more elements. Molecules are the smallest units of compounds. Slide 6 of 28 General Chemistry: Chapter 1 Prentice-Hall © 2007 Separating Mixtures Slide 7 of 28 General Chemistry: Chapter 1 Prentice-Hall © 2007 Separating Mixtures Slide 8 of 28 General Chemistry:Chapter Chapter General Chemistry: 1 1 Prentice-Hall © 2007 Decomposing Compounds Slide 9 of 28 General Chemistry:Chapter Chapter General Chemistry: 1 1 Prentice-Hall © 2007 States of Matter Slide 10 of 28 General Chemistry:Chapter Chapter General Chemistry: 1 1 Prentice-Hall © 2007 1-4 The Measurement of Matter Slide 11 of 28 General Chemistry: Chapter 1 Prentice-Hall © 2007 Slide Slide 12 of 28 12 of 19 General Chemistry:Chapter Chapter General Chemistry: 1 1 Prentice-Hall © 2007© 2007 Prentice-Hall Mass • Mass is the quantity of matter in an object. • Weight is the force of gravity on an object Wm Slide 13 of 28 W=gm General Chemistry: Chapter 1 Prentice-Hall © 2007 Temperature Slide 14 Slide of 28 14 of 28 General Chemistry: 1 1 General Chemistry:Chapter Chapter Prentice-Hall © 2007 Prentice-Hall © 2007 Volume Slide 15 of 28 General Chemistry: Chapter 1 Prentice-Hall © 2007 SI and non-SI Units Compared 1 Imperial qt 1.136 L 1 US qt 0.936 L 1 kg Slide 16 of 28 1 lb 1 in General Chemistry: Chapter 1 1L 1 cm Prentice-Hall © 2007 Units S.I. Units Other Common Units Length meter, m Length Angstrom, Å, 10-8 cm Mass Kilogram, kg Volume Liter, L, 10-3 m3 Time second, s Energy Calorie, cal, 4.184 J Temperature Kelvin, K Quantity Pressure Mole, 6.0221023 mol-1 1 Atm = 1.064 102 kPa 1 Atm = 760 mm Hg Derived Quantities Force Newton, kg m s-2 Pressure Pascal, kg m-1 s-2 Energy Joule, kg m2 s-2 Slide 17 of 28 General Chemistry: Chapter 1 Prentice-Hall © 2007 1-5 Density and Percent Composition = m/V m=V V=m/ g/mL Mass and volume are extensive properties Density is an intensive property Slide 18 of 28 General Chemistry: Chapter 1 Prentice-Hall © 2007 Density in Conversion Pathways What is the mass of a cube of osmium that is 1.25 inches on each side? Have volume, need density Slide 19 of 28 = 22.48g/cm3 General Chemistry: Chapter 1 Prentice-Hall © 2007 EXAMPLE 1-2 Relating Mass, Volume and Density The stainless steel in the solid cylindrical rod pictured below has a density of 7.75 g/cm3. If we want a 1.00 kg mass of this rod, how long a section must we cut off? Calculate the Volume needed Calculate the Length Slide 20 of 28 1 m = m V= d d V = h r2 h = V2 r General Chemistry: Chapter 1 Prentice-Hall © 2007 EXAMPLE 1-2 Calculate the Volume needed V= m d = m 1 d 1 cm3 V = = (1.00kg)(1000g/kg) 7.75 g = 129 cm3 Calculate the Length V = h r2 h= V r2 3 V 129 cm h= = = 25.5 cm 2 2 (3.1415){(0.5)(1.000 in)(2.54 cm/in)} r Slide 21 of 28 General Chemistry: Chapter 1 Prentice-Hall © 2007 Measuring Volume of an Irregular Object Slide 22 of 28 General Chemistry: Chapter 1 Prentice-Hall © 2007 1-6 Uncertainties in Scientific Measurements • Systematic errors. – Thermometer constantly 2°C too low. • Random errors – Limitation in reading a scale. • Precision – Reproducibility of a measurement. • Accuracy – How close to the real value. Slide 23 of 28 General Chemistry: Chapter 1 Prentice-Hall © 2007 Precision Reproducibility 0.1 g Precision Slide 24 of 28 0.0001 g low high General Chemistry: Chapter 1 Prentice-Hall © 2007 1-7 Significant Figures Slide 25 of 28 General Chemistry: Chapter 1 Prentice-Hall © 2007 Significant Figures The calculators show the effect of the change in a low precision number in a calculation 14.79 12.11 5.05 5.04 Slide 26 of 28 5.05 General Chemistry: Chapter 1 5.06 Prentice-Hall © 2007 End of Chapter Questions Instructors may provide lists of questions that reinforce topics they feel are particularly pertinent in the chapter. If no list is given students should attempt questions from each section of the chapter. Build from the easier questions where the topic is identified, to the more difficult integrative examples where the approach to the question must be identified. Slide 27 of 28 General Chemistry: Chapter 1 Prentice-Hall © 2007