- Chapter 1: Matter, Measurement, and Problem Solving o Chemistry – The science that seeks to understand the behavior of matter by studying the behavior or atoms and molecules- Atoms and Molecules o Atoms – Submicroscopic particles and the fundamental building blocks of lifeo Molecules - Two or more atoms attached together in a specific geometrical arrangement- Scientific Approach to Knowledge o Types of Observations Qualitive – Observations that are descriptions of the characteristics or behaviorsof nature Quantitive – Compare a characteristic to a standard numerical scaleo The result of observation is a Hypothesis – a tentative interpretation or explanation for an observationo Validate or invalidate hypothesizes with an Experiment – A set of highly controlled procedures designed to test whether an idea about nature is valid- From Specific to General Observationso Scientific Law – A statement that summarizes all past observations and predicts future observations Law of Conservation of Mass – “In a chemical reaction, matter is neither created nor destroyed Scientific Laws allow you to predict future observations (ex. Periodic Law)- From Specific to General Understandingo Scientific Theory – A general explanation for WHY things in nature are the way they are and behave the way they do- Relationships Between Pieces of theScientific Method - Classification of Matter - Matter – anything that occupies space and has masso Matter is separated into two types of classifications- State- Compositiono Classifying Matter by Physical State- Solids may be eithero Crystalline (Salt, Diamonds, Sugar)o Amorphous (Plastic, Glass, Charcoal)oo Pure Substances – Matter whose composition doesn’t change from one sample to another Made of a single type of atom or moleculeo Mixture – Matter whose composition may vary from one sample to another Two or more types of atoms or molecules combined in variable proportions- Pure Substances – Possible to be elements OR compoundso Elements – Pure substances that cannot be decomposed into simpler substances by chemical reactions are called elements Composed of single type of atom- Atoms may or may not be combined into moleculeso Compounds – Pure Substances that can be decomposed Chemical Combination of elements Composed of molecules that contain two or more separate atoms- Mixtureso Homogeneous Mixture – Mixtures that have uniform composition throughout Every piece of a sample has identical Characteristics Atoms or molecules mixed uniformly (Tea with Sugar) o Heterogeneous Mixture – Mixture that does not have uniform composition throughout Regions within the sample can have different characteristics Atoms or molecule not mixed uniformly (Wet Sand)- Changes in Mattero Physical changes in matter occur without any changes in composition of matter The state of the matter changes generally- Boiling: Condensing, Melting: Freezing, Subliming: Dissolvingo Chemical changes in matter occur with changes in matter composition Rusting, Burning, etc.- Properties of Mattero Physical Properties – Characteristics of matter that can be changed without changing itscomposition Characteristics that describe the behavior of mattero Chemical Properties - Characteristics that determine how the composition of matter changes as a result of contact with other matter or the influence of energy- Energy - Energy Changes in Mattero Changes in matter, both physical and chemical, result in the matter either gaining or releasing energyo Energy – The capacity to do work Work – The action of a force applied across a distance All matter possesses energyo Energy is classified as: Kinetic Potential- Energy of Mattero Kinetic Energy – The energy of motion Thermal (heat) energy is a form of kinetic energy because it is caused by molecular motiono Potential Energy – Energy that is stored in the matter Due to the composition of the matter and its position relative to other thingso Law of Conservation of Energy - Energy can be converted from one form to another, butthe total amount of energy remains the same- Standard Units of Measure- The Standard Unitso SI Units – A set of international standard units for comparing all our measurements Length – distance traveled in a specific period of time- SI Unit – Meter [m] (about 3.37 inches longer than a yard) Mass – Measure of the amount of matter present in an object- SI Unit – Kilogram [kg] (about 2 lbs. 3 oz) Time - SI Unit – Second [s]- Derivatives of length and mass unitso 1 M = 100 cmo 1 cm = .01 m = 10mmo 1 inch = 2.54 cmo 1 kg = 2.2046 pounds, 1 lb. = 453.59go 1 kg = 1000g = 10^3go 1 g = 1000 mg = 10^3 mgo 1 g - .001 kg = 10^-3 kgo 1 mg = .001 g = 10^-3- Temperatureo Temperature – Measure of the Average amount of kineticenergy caused by motion of the particles- Temperature Scaleso Fahrenheit Scale °F  Used in the U.S.o Celsius Scale °C  Used in all other countrieso Kelvin Scale  Absolute Scale- No negative Numbers Directly proportional to average amount of kinetic energy 0 K = absolute zero- Common Prefix Multipliers in the SI System- Volume – Derived Unito 1 mL = 1 cm³o 1 m³ = 10^-6 m³ = .00001m³o Commonly measure liquid or gas volume in milliliters 1 L is slightly larger than 1 quart 1 L = 1 dm³ = 1000 mL = 10³ mL 1 mL = .001 L = 10^-3- Common Units and their Equivalentso Length 1 kilometer (km) = 0.6214 mile (mi) 1 meter (m) = 39.37 inches (in.) 1 meter (m) = 1.094 yards (yd) 1 foot (ft.) = 30.48 centimeters (cm) 1 inch (in.) = 2.54 centimeters (cm)o Mass 1 kilogram (km) = 2.205 pounds (lbs.) 1 pounds (lb.) = 453.59 grams (g) 1 ounce (oz) = 28.35 grams (g)o Volume 1 liter (L) = 1000 milliliters (mL) 1 liter (L) = 1000 cubic centimeters (cm³) 1 liter (L) = 1.057 quarts (qt) 1 U.S. gallon (gal) = 3.785 liters (L)- Intensive and Extensive Propertieso Extensive Properties – properties whose value depends on the quantity of matter Extensive properties cannot be used to identify what type of matter something is Mass and Volume are extensive propertieso Intensive Properties – Properties whose values are independent of the quantity of mattero Density – ratio of mass to volume Intensive Property- Densityo Solids = g/cm³ = g/mLo