Slide 15:Put in 4 x 6 index card. Then attach a 1x1 photo on the upper right portion Bring another 1x1 photo then pass it to your secretary


Slide 16:cpesison.multiply.com


Slide 18:Chapter 01 Introduction: Matter and Measurement


Slide 19:Surgery with Anesthesia


Slide 20:Can you imagine it without anesthesia?


Slide 22:Vaccines and Antibiotics


Slide 23:Gasoline


Slide 24:Solar Energy


Slide 25:Size of Electronics


Slide 27:Chemistry is the study of matter and the changes it undergoes Matter is anything that has mass and occupies space


Slide 28:Major Areas of Chemistry Inorganic Chemistry Organic Chemistry Biochemistry Analytical Chemistry Physical Chemistry


Slide 29:Scientific Method is a systematic approach to research Hypothesis is a tentative explanation of a set of observations Theory is a well substantiated explanation of some aspect of the natural world. Law is a generalization that describes recurring facts or events in nature


Slide 31:A physical change does not alter the composition or identity of a substance.


Slide 32:A chemical change alters the composition or identity of the substance(s) involved.


Slide 33:Intensive Property does not depend on the amount of the sample Extensive Property depend on the amount of the sample Density Temperature Color Mass Length Volume


Slide 34:A mixture is a combination of two or more substances in which the substances retain their distinct identities. Homogenous mixture – composition of the mixture is the same throughout. Heterogeneous mixture – composition is not uniform throughout.


Slide 35:Physical means can be used to separate a mixture into its pure components.


Slide 36:An element is a substance that cannot be separated into simpler substances by chemical means. 114 elements have been identified 82 elements occur naturally on Earth gold, aluminum, lead, oxygen, carbon 32 elements have been created by scientists technetium, americium, seaborgium


Slide 38:A compound is a substance composed of atoms of two or more elements chemically united in fixed proportions. Water (H2O) Ammonia (NH3) Glucose (C6H12O6)


Slide 40:International System of Units (SI Units)


Slide 41:Metric Prefixes


Slide 42:Mass: English and Metric


Slide 43:Mass: Metric


Slide 44:Volume: Metric


Slide 45:Derived Units Volume Density


Slide 46:Which is more dense? a b Density is the ratio of mass to volume


Slide 47:Unit English Metric SI Mass pound (lb) gram (g) kilogram (kg) Length yard (yd) meter (m) meter (m) Volume gallon (gal) liter (l) cubic meter (m3) English, Metric and SI Units


Slide 48:Practice on Density Problems A piece of platinum metal with a density of 21.5 g/cm3 has a volume of 4.49 cm3. What is its mass? 96.5 g


Slide 49:Practice on Density Problems The density of sulfuric acid in a certain car battery is 1.41 g/mL. Calculate the mass of 242 mL of the liquid. 341 g


Slide 51:Practice on Temperature Conversions Convert (a) 327.5 °C (the melting point of lead) to degrees Fahrenheit; (b) 172.9 °F (the boiling point of ethanol) to degrees Celsius; and (c) 77 K, the boiling point of liquid nitrogen, to degrees Celsius 621.5 °F 78.3 °C -196 °C


Slide 52:Accuracy tells us how close a measurement is to the true value of the quantity that was measured. Precision refers to how closely two or measurements of the same quantity agree with one another.