1. Properties Chapter 1  Physical – characteristics Quantitative: measurements using numbers and units.Quantitative: measurements using numbers and units.  Mass (grams)  Volume (liters)  Length (meters)  Temperature (Kelvin or Celsius)  Pressure (kPa, atm, or mmHg)  Density (g/ml) Qualitative: descriptions using the five senses.Qualitative: descriptions using the five senses.  Color  Texture  Smell  Chemical - behaviors ToxicityToxicity FlammabilityFlammability CorrosiveCorrosive RadioactivityRadioactivity

2. Properties of Acids & Bases Chapter 14 AcidsBases Taste Sour H+ > OH- pH below 7 pOH above 7 Conducts Electricity Corrosive Reacts with Base to form Salt H 2 O Turns Indicators Red Taste Bitter OH- > H+ pH above 7 pOH below 7 Conducts Electricity Corrosive Reacts with Acid to form Salt H 2 O Turns Indicators Blue Feels Slippery

3. Nitric Acid  Old fashioned name: Aqua Fortis strong waterstrong water  Only acid that reacts with copper.  The acid in acid rain.  Highly Corrosive  Poisonous

4. Properties: Metals & Nonmetals Chapter 5 MetalsNonMetals Mostly Solids (Hg is only liquid) Hard (Dense) Lustrous (Shiny) Malleable (Bend, Dent, Flatten) Ductile (Stretches into Wires) Great Conductors of Electricity 80% of Periodic Table 7A & 8A Gases (Br is only liquid) All others are Solids (Iodine) Solids are Brittle 7A Gases are diatomic molecules 8A Gases are unreactive (stable) Poor Conductors of Electricity 20% of Periodic Table

5. Phase Labels Chapter 10  Solid (s)  Liquid (l)  Gas (g)  Aqueous (aq) = dissolved in water

6. Types of Chemical Reactions Chapter 8  SynthesisA + B  C  DecompositionC  A + B  Single DisplacementA + BC  B + AC  Double DisplacementAB + CD  AD + CB  CombustionC x H y + O 2  CO 2 + H 2 O  NeutralizationAcid + Base  Salt + H 2 O  Redox ReactionsOxidation and Reduction

7. Nomenclature Chapter 7  Roman Numerals – represents the charge on a B metal.  Common Names – Sodium Hydroxide is lye. Nitric Acid was once known as Aqua Fortis.  Nonmetals – end in “ide”.  Metals – just say the name.  Molecules – Molecular Compounds (NM,NM)  Formula Units – Ionic Compounds (M,NM)  Polyatomic Ions

8. Mole Review Chapter 7  1Mole = Molar MassMolar Mass 6.02x10 23 particles6.02x10 23 particles 22.4L of a gas at STP22.4L of a gas at STP  Standard Temp 0K = 273˚C  Standard Pressure 101.3kPa = 1atm = 760mmHg = 760torr101.3kPa = 1atm = 760mmHg = 760torr

9. More Review  Metric Conversions (1L=1000ml, 1kg=1000g)  Density = Mass/Volume of H2O = 1g/1ml (1ml=1cm 3 )of H2O = 1g/1ml (1ml=1cm 3 )  TemperatureK = ˚C + 273  Conservation of Matter and Energy  Limiting Reactants (Chapter 9)  PV=nRTR=8.31kPa*L/mol*K (Chapter 11)  Molarity= moles solute/liters solution (Chapter 12)  Equilibrium & Keq (Constant) (Chapter 18)

10. Lab Equipment Chapter 2  Polystyrene Bottle (type of plastic)  Scale measures mass in grams.  Graduated Cylinder measures volume in milliliters.  Beaker is best for mixing solutions.  Flask is best for storing solutions.

11. Nitrogen Dioxide  Brown, Highly Corrosive Gas  Lung Irritant, Respiratory Infections  Produced by factories, volcanoes, cars, etc.  Combine with other molecules to produce smog.

12. Parafilm  Wax Paper – Lab Grade  Can Stretch  Bubbles up if gas builds up in bottle.  Relieves pressure so bottle does not expand and potentially break.

13. Fume Hood  Keeps dangerous odors out of the classroom.

14. Safety  Goggles  Acid – rinse graduated cylinder thoroughly.  Rinse paper towels that were used to clean up spilled acid.  Loosen the cap on the bottle containing conversion reaction one.  Use the fume hood.  Wash your hands before leaving.

15. Reaction Indicators Chapter 8  Bubbles, Smoke, Gas, Heat, Light production.  Temperature change not create by equipment.  Color change not created with dyes.  The formation of a precipitate (solid).  Odor change.

16. Energy of the Reaction Chapter 16  Exothermic – reaction produces energy. Reaction feels warm/hot.  Endothermic – reaction absorbs energy. Reaction feels cool/cold.

17. Neutralization Reaction Chapter 15  Acid and Base create salt and water.  Hydrogen ion concentration would equal the hydroxide concentration to make water.H + + OH -  H 2 O  Normality = equivalents/Liter  Equivalents = the number of H + or OH - ions.  Neutralization Formula: N A V A =N B V B

18. Balancing Chapter 8  Conservation of Mass  Use whole number coefficients to balance the atoms on both sides of the equation.  Never change the correct compound formula’s subscripts.

19. Acids Chapter 14  Sour, corrosive, good conductors of electricity.  High Hydrogen Ion Concentration: Arrhenius.  Hydrogen Donor: Bronsted-Lowry.  Electron Acceptor: Lewis.  Neutralized by Bases to form Salt Water  Strong Acid = Weak Bonds, Easily Ionized  Weak Acid = Strong Bonds, Hard to Ionize  Naming: Hydro-----ic (Hydrogen + NM)Hydro-----ic (Hydrogen + NM) -----ic (Hydrogen + Polyatomic ending in “ate”)-----ic (Hydrogen + Polyatomic ending in “ate”) ------ous (Hydrogen + Polyatomic ending in “ite”)------ous (Hydrogen + Polyatomic ending in “ite”)

20. Bases Chapter 14  Bitter, slippery, corrosive, good conductor of electricity.  High Hydroxide Ion Concentration: Arrhenius.  Hydrogen Acceptor: Bronsted-Lowry.  Electron Donor: Lewis.  Neutralized by Acids to form Salt Water  Strong Base = Weak Bonds, Easily Ionized  Weak Base = Strong Bonds, Hard to Ionize  Also called alkali substances. NaOH is commonly known as Lye.NaOH is commonly known as Lye.

21. Litmus Paper Chapter 14  Acid/Base Indicator  Blue Paper is turned Red by Acid  Red Paper is turned Blue by Base  Litmus is a chemical which red in the presence of an acid and blue in the presence of a base.

22. Reaction Rates Chapter 17  Temperature  Pressure (of gas reactions only)  Concentrations of Reactants  Surface Area/Particle Size  Catalyst/Inhibitor

23. Temperature Chapter 17  Temperature changes the rate of a reaction.  Increase temperature and the reaction proceeds faster. (hot water bath)  For every 10°C that the temperature is increased, the reaction rate doubles.  Decrease temperature and the reaction slows down. (ice water bath)  Temperature changes do affect the pH. Therefore, pH must be measured at room temperature (RT).

24. Catalyst  Speeds up a chemical reaction  Does not get used up.  Neither a reactant or a product.  Written above the arrow in a chemical reaction.  Lowers the activation energy.  Biological catalyst is an enzyme. Chapter 17

25. Water Bath  Used for regulating the temperature of substances at lower than 100˚C.  Used to heat substances, which can't be heated directly.

26. Structural Formulas Chapter 6  Ionic Bonds – transfer of electrons from cation to anion. Goal is to have 8 valence electrons to be stable like a noble gas.Goal is to have 8 valence electrons to be stable like a noble gas. No lines connecting the atoms.No lines connecting the atoms. Write the ions charges.Write the ions charges.  Molecular Bonds – share electrons between two nonmetal anions. Line connects the atoms, represents a shared pair of electrons.Line connects the atoms, represents a shared pair of electrons. Do not label charges.Do not label charges. Creates a VSEPR shape: linear, bent, triginal planar, pyramidal, tetrahedral, or complex.Creates a VSEPR shape: linear, bent, triginal planar, pyramidal, tetrahedral, or complex. Can be polar or nonpolar depending on the differences in electronegativity. (Periodic Trends - Chapter 5)Can be polar or nonpolar depending on the differences in electronegativity. (Periodic Trends - Chapter 5)

27. Concentration Chapter 12  Molarity = moles of solute / liters of solution = Molal concentration = M  M 1 V 1 = M 2 V 2 Dilutions Formula. Example: HCl from the factory is 12M. It is diluted with water to create a 6M solution.  When making dilutions always add the acid or base to the water.  Molality = moles of solute / kg of solution = molal concemtration = m

28. pH Calculations Chapter 14  pH = -log[H+]  [H+] = 10 x (-pH)  pOH = -log[OH-]  [OH-] = 10 x (-pOH)  pH + pOH = 14

29. Reactivity Series of Metals Chapter 8  Single Replacement or Displacement  More reactive metals replace less reactive metals.

30. Collision Theory Chapter 17  Particles must collide in order to react.  Particles must… collide with a minimum quantity of energy (activation energy)collide with a minimum quantity of energy (activation energy) and in the correct orientation.and in the correct orientation.

31. Filter Paper  Fold in half once.  Fold in half again.  Open one pocket.

32. Decant  Means to pour the liquid (supernatant) off leaving the solid (precipitate) behind.  In this lab we always want the solid. The liquid is the waste material.  In other labs, the liquid (supernatant) might be what we want to keep. what we want to keep.  The solid is the pellet.

33. Centrifuge  A piece of equipment that spins the solution in extremely fast circles. Ex: 3500rev/min.  Never open the lid while the centrifuge is still spinning.  Useful for separating liquids and solids.  If the solid is more dense than the liquid it forms a pellet at the bottom of the tube.  The liquid above the pellet is known as the supernatant.

34. Vortex  Also called an Agitator.  Used to help mix substances.

35. Drying Oven  Warm oven used to quickly and completely evaporate water off of our product.  When we get our final measurements, we only want copper, not the acetone and excess water.

36. Percent Yield Chapter 9  Actual Yield/Theoretical Yield x 100  Amount of Cu recovered/ the original amount of Cu you started with multiplied by 100.  Percent Error = 100% - % Yield  % Error + % Yield = 100%

37. Homoethermic  Warm-blooded.  Requires lots of food.  Can live in a variety of climates.