Properties Chapter 1

1. Properties Chapter 1 • Physical – characteristics • 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. • Color • Texture • Smell • Chemical - behaviors • Toxicity • Flammability • Corrosive • Radioactivity

2. Properties of Acids & Bases Chapter 14

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

4. Properties: Metals & Nonmetals Chapter 5

5. 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.

6. Types of Chemical ReactionsChapter 8 Synthesis A + B  C Decomposition C  A + B Single Displacement A + BC  B + AC Double Displacement AB + CD  AD + CB Combustion CxHy + O2  CO2 + H2O Neutralization Acid + Base  Salt + H2O Redox Reactions Oxidation and Reduction

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

8. 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. • No lines connecting the atoms. • Write the ions charges. • Molecular Bonds – share electrons between two nonmetal anions. • Line connects the atoms, represents a shared pair of electrons. • Do not label charges. • 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)

9. 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

10. Mole Review Chapter 7 • 1Mole = • Molar Mass • 6.02x1023 particles • 22.4L of a gas at STP • Standard Temp 0K = 273˚C • Standard Pressure • 101.3kPa = 1atm = 760mmHg = 760torr

11. More Review • Metric Conversions (1L=100ml, 1kg=1000g) • Density = Mass/Volume • of H2O = 1g/1ml (1ml=1cm3) • Temperature K = C + 273 • Conservation of Matter and Energy • Limiting Reactants (Chapter 9) • PV=nRT R=8.31kPa*L/mol*K (Chapter 11) • Molarity= moles solute/liters solution (Chapter 12) • Equilibrium & Keq (Constant) (Chapter 18)

12. Fume Hood • Keeps dangerous odors out of the classroom.

13. 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.

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

15. 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.

16. 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.

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- H2O • Neutralization Formula: NAVA=NBVB

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) • -----ic (Hydrogen + Polyatomic ending in “ate”) • ------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.

21. Concentration Chapter 12 • Molarity = moles of solute / liters of solution = Molal concentration = M • M1V1 = M2V2 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 = molalconcemtration = m

22. 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.

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

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

25. 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).

26. Catalyst Chapter 17 • 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.

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

28. Filter Paper Fold in half once. Fold in half again. Open one pocket.

29. 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. • The solid is the pellet.

30. 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.

31. Vortex Also called an Agitator. Used to help mix substances.

32. 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.

33. 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%

34. Homoethermic • Warm-blooded. • Requires lots of food. • Can live in a variety of climates.