1. AP Chemistry Exam Question of the Week Lab safety glasses are NOT needed for which of the following? a). Weighing samples b). Boiling water c). Distilling alcohol d). Pre-lab write-ups e). Titrations

2. Matter Does it really matter?

3. Physical And Chemical Properties Physical Properties Physical Properties Density Density Malleability Malleability Ductility Ductility Conductivity Conductivity Chemical Properties Chemical Properties Kind of chemical changes that material can undergo Kind of chemical changes that material can undergo

4. Physical And Chemical Changes Physical Changes Physical Changes Shape Shape Size Size Color Color Boiling water or freezing water Boiling water or freezing water Chemical Changes Chemical Changes Change in the identity of the material Change in the identity of the material Rust Rust

5. Pure Substances vs. Mixtures Pure Substance Pure Substance One type of matter One type of matter Can be separated into more than one pure substance but only by chemical change Can be separated into more than one pure substance but only by chemical change Mixtures Mixtures Can be separated into 2 or more pure substances by physical change Can be separated into 2 or more pure substances by physical change 2 types 2 types Heterogeneous Heterogeneous Homogenous Homogenous

6. Elements and Symbols Element Element Pure substance that consists of only one kind of atom Pure substance that consists of only one kind of atom Examples Examples Atoms Atoms Basic particles that make up elements Basic particles that make up elements Consists of positive particles called protons, negative particles called electrons and neutral particles called neutrons Consists of positive particles called protons, negative particles called electrons and neutral particles called neutrons Ions Ions Protons and electrons = each other in the atom the atom has a neutral charge Protons and electrons = each other in the atom the atom has a neutral charge When protons and electrons are unbalanced atom is charged and is considered an ion When protons and electrons are unbalanced atom is charged and is considered an ion Molecules Molecules Atoms by themselves in their natural state are called monatomic elements. These are rare. Examples Atoms by themselves in their natural state are called monatomic elements. These are rare. Examples Elements whose atoms naturally bond into 2 atom units are called diatomic elements. Examples Elements whose atoms naturally bond into 2 atom units are called diatomic elements. Examples Distinct groups of atoms bonded together are called molecules. Distinct groups of atoms bonded together are called molecules. Chemical Symbol Chemical Symbol Each element has its own unique chemical symbol and name Each element has its own unique chemical symbol and name Usually the symbol is based on the name but it might be its Latin or Greek name Usually the symbol is based on the name but it might be its Latin or Greek name Colors- Iridium (Latin for rainbow) Colors- Iridium (Latin for rainbow) People- Curium (for Pierre and Marie Curie) People- Curium (for Pierre and Marie Curie) Places- Californium Places- Californium Heavenly bodies- Helium (Helios which is the Greek word for sun) Heavenly bodies- Helium (Helios which is the Greek word for sun) Miscellaneous- Bromine from the Greek word for stench Miscellaneous- Bromine from the Greek word for stench

7. Compounds and Their Formulas Compounds Compounds 2 or more elements chemically combined 2 or more elements chemically combined Some form distinct particles called molecules Some form distinct particles called molecules Other form vast crystalline arrays that repeat called formula units Other form vast crystalline arrays that repeat called formula units Chemical Formulas Chemical Formulas Used to represent the millions of kinds of molecules or formula units that make up compounds Used to represent the millions of kinds of molecules or formula units that make up compounds Molecule or formula unit has a definite number of atoms Molecule or formula unit has a definite number of atoms Chemical formulas indicate the number of atoms in each molecule or formula unit Chemical formulas indicate the number of atoms in each molecule or formula unit Chemical Subscripts Chemical Subscripts Small number written at the lower right of a chemical symbol Small number written at the lower right of a chemical symbol Tells the number of atoms or moles (groups of atoms) in a chemical formula Tells the number of atoms or moles (groups of atoms) in a chemical formula Subscript outside of parenthesis- number of molecules of that entire group Subscript outside of parenthesis- number of molecules of that entire group Coefficient- in front of the entire chemical formula in a chemical equation. This number applies to the entire chemical formula and it is the number of molecules of the formula Coefficient- in front of the entire chemical formula in a chemical equation. This number applies to the entire chemical formula and it is the number of molecules of the formula

8. Energy and Matter Energy Energy Ability to do work Ability to do work Correlation between energy expended and work done (Physics) Correlation between energy expended and work done (Physics) Types of Energy Types of Energy Potential energy Potential energy Kinetic energy Kinetic energy Thermal energy Thermal energy Energy of atoms as they move around Energy of atoms as they move around Sound energy Sound energy Energy of periodic waves Energy of periodic waves Electrical energy Electrical energy Forces that mover electrically charged particles Forces that mover electrically charged particles Electromagnetic energy Electromagnetic energy Electric energy that makes magnetic fields Electric energy that makes magnetic fields Chemical energy Chemical energy Energy when atoms bond into new compounds Energy when atoms bond into new compounds Nuclear energy Nuclear energy Split the atom or removing particles from the nucleus Split the atom or removing particles from the nucleus Conservation of Energy Conservation of Energy Thermodynamics- we will study in greater detail in Chapter 13 Thermodynamics- we will study in greater detail in Chapter 13 Temperature, Heat, Thermal Energy Temperature, Heat, Thermal Energy Kinetic energy= 1/2mv 2 Kinetic energy= 1/2mv 2 Internal energy = KE + PE Internal energy = KE + PE Temperature = average KE of its particles Temperature = average KE of its particles

9. Temperature A measure of the average kinetic energy A measure of the average kinetic energy Different temperature scales, all are talking about the same height of mercury Different temperature scales, all are talking about the same height of mercury Derive a equation for converting ºF to ºC Derive a equation for converting ºF to ºC

10. 0ºC 32ºF 0ºC = 32ºF

11. 100ºC212ºF 100ºC = 212ºF 0ºC 32ºF 0ºC = 32ºF

12. 100ºC212ºF 0ºC 32ºF 100ºC = 212ºF 0ºC = 32ºF 100ºC = 180ºF

13. 100ºC212ºF 0ºC 32ºF 100ºC = 212ºF 0ºC = 32ºF 100ºC = 180ºF 1ºC = (180/100)ºF 1ºC = 9/5ºF

14. 100ºC212ºF 0ºC 32ºF 100ºC = 212ºF 0ºC = 32ºF 100ºC = 180ºF 1ºC = (180/100)ºF 1ºC = 9/5ºF For every °C there is 9/5 (or 1.8) °F, but the Fahrenheit scale starts out 32° higher than the Celsius scale, so you must add 32 to any Celsius reading and subtracted from any Fahrenheit reading to correct for the starting point differences. The final formulas for converting from F to C or C to F: (5/9 X °C) + 32 = F or 9/5(°F-32) = C 5/9 °C = 1°F

15. State of Matter 4 States of Matter 4 States of Matter Solid Solid Liquid Liquid Gas Gas Plasma Plasma Changes in the Common States of Matter Changes in the Common States of Matter Condensation Condensation Vaporization Vaporization Freeze Freeze Melt Melt Sublimation Sublimation Deposition Deposition

16. Measurement and Metrics How we measure in science class

17. TERMS of MEASUREMENT Dimension Dimension Quantities such as length, mass, volume, etc. Quantities such as length, mass, volume, etc. Unit of measure Unit of measure Either in English or Metric Either in English or Metric Scale Scale Calibrated Calibrated Scales are calibrated to make sure they are accurate Scales are calibrated to make sure they are accurate Instrument Instrument Artificial device made for the purpose of refining, extending, or substituting for human senses when measuring. Artificial device made for the purpose of refining, extending, or substituting for human senses when measuring.

18. Metric Vs. English Units English Units Based on Divisions of 8 or 12 Based on Divisions of 8 or 12 Have multiple units for the same measurement Have multiple units for the same measurement Length Length Weight or mass Weight or mass Volume Volume Speed Speed Metric Units Based on division of 10 Based on division of 10 Have one unit with prefixes for the same measurement Have one unit with prefixes for the same measurement Length Length Weight or mass Weight or mass Volume Volume Speed Speed

19. Metric Prefixes in Chemistry PrefixSymbolMeansNumberForm TeraTTrillion1,000,000,000,000 10 12 GigaGBillion1,000,000,000 10 9 MegaMMillion1,000,000 10 6 KilokThousand1,000 10 3 HectohHundred100 10 2 DekadaTen1010 DecidTenth0.1 10 -1 CenticHundredth0.01 10 -2 MillimThousandth0.001 10 -3 MicroµMillionth0.000001 10 -6 NanonBillionth0.000000001 10 -9 PicoPTrillionth0.000000000001 10 -12

20. SI Base Units SI Base Units Dimension Dimension Symbol Si Unit Unit Symbol Length l Meterm MassmKilogramkg TimetSeconds TemperatureTKelvinK Number of particles nMolemol Electrical currentIAmpereA Light intensityILIL Candelacd

21. Conversion Factors Unit conversion Unit conversion Converting from one unit to another with the aid of a… Converting from one unit to another with the aid of a… Conversion factor Conversion factor Fraction that contains the original unit and its equivalent value in a new unit Fraction that contains the original unit and its equivalent value in a new unit 1L = 1000 mL the conversion factor for converting Liters into mL is 1000mL/1L and the conversion factor for converting mL into L is 1L/1000mL 1L = 1000 mL the conversion factor for converting Liters into mL is 1000mL/1L and the conversion factor for converting mL into L is 1L/1000mL Bridge Notation Bridge Notation Special notation for multiplying and dividing several measurements together at the same time Special notation for multiplying and dividing several measurements together at the same time Can (and will) be used to do any calculations but most often is used when converting units. Can (and will) be used to do any calculations but most often is used when converting units. Examples of bridge notation Examples of bridge notation