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6/27/2014 HOW TO PREPARE FOR EXAMS HOW TO LEARN People “learn” in different ways BUT 1. Students must be self motivated 1. 2. 3. 4. UNDERSTAND examples in chapter(s) WORK practice exercises in chapter(s) Work problems at end of chapter Use web sites such as: 2. Students must be actively involved http://wps.prenhall.com/esm_brown_chemistry_9/1,4647,169060,.html 3. Knowledge is understanding 5. Finally test yourself with old exam from my web page 4. Knowledge results ONLY through Active Participation Use “Blank” area on top of Back of Scantron to write nomenclature Exam 27 Multiple Choice Questions and a 10 Point Bonus Question --------------------------------------------------------------------------------- Bonus Question on back of Scantron (# 882) As Shown ONLY Write Names here Write Formulas here 1. 1. 2. NAME ____________ 2._ 3. 3. 4. 4. 5. 5. Example of using “Blank” area on top of Back of Scantron to write nomenclature Write Names here Write Formulas here 1. Silver 1. AgCl 2. Oxygen 2. H2SO4(aq) 3. Elemental Oxygen 3. CaO 4. Carbon 4. CCl4 5. Alpha particle 5. 11H+1 Chapter 1 • • • • • Classification of Matter Properties of Matter SI Units Uncertainty in Measurement Dimensional Analysis 1 6/27/2014 What Elements & Compounds are you expected to know ? Properties of Matter Intensive Properties do not depend on amount • Elements ………Table 1.2 + ones I introduced • Compounds ……Table 1.1 + ones I introduced What Units of Measurement are you expected to know ? • SI Base Units …………..Table 1.4 • Prefixes ………………….Table 1.5 • Conversion Factors …….. Back of Book ACCURACY & PRECISION • ACCURACY refers to how closely a measured value agrees with the correct value • PRECISION refers to how closely individual measurements agree with one another. Such as density and temperature Density Kelvin (K) weight volume ↔ Celsius (°C) Celsius (°C) ↔ Fahrenheit (°F) Extensive Properties do depend on amount such as weight, volume, etc The Scientific Method • Defining a Problem • Designing an Experiment • Collecting Data • Interpreting Results Exponential Notation In Scientific Notation, Numbers Are Written in The EXPONENTIAL Format A x 10 n 5687.62 meters = 5.68762 x 10 3 meters = 5.68762 Kilo meters = 5.68762 km Dimensional–Analysis method for SOLVING PROBLEMS makes use of conversion factors Use UNITS To Solve Problems !!!!!! 2 6/27/2014 Convert some number of pm to meters Let UNITS SOLVE the problem !!!!! m pm x meters pm Units FIRST then numbers some number pm x 1x 10-12 m answer in meters 1 pm TYPES OF NUMBERS EXACT & APPROXIMATE (MEASURED) SAMPLE EXERCISE 1.5 What difference exists between 4.0 g and 4.00 g? A mass of 4.0 g indicates that the uncertainty is in the first decimal place of the measurement. Thus, the mass might be anything between 3.9 and 4.1 Density • Density relates the mass of an object to its volume. weight Density volume Convert 1.000 inches to cm Let the UNITS solve the problem inches x ( number ) ? cm cm ? in Units FIRST then numbers !! 1.000 inches x 2.54 cm 2.540 cm 1 in SIGNIFICANT FIGURES 1. Digits of a measured number that have uncertainty only in the last digit 2. The NUMBER Of Digits That Are KNOWN With CERTAINTY 3. Digits that indicate the precision of measurements Temperature Conversions Kelvin (K) ↔ Celsius (°C) Kelvin (K) = °C + 273.15 Celsius (°C) ↔ Fahrenheit (°F) 5 C ( F 32) and 9 9 F C 32 5 3 6/27/2014 Predicting Ionic Charge How do I know what the formula for Magnesium sulfate is Magnesium ion: Mg 2+ & sulfate ion SO 2+2 = -2 Mg SO4 How do I know that the sulfate ion is -2? Because I know the formula for sulfuric acid +2 = -2 H2 SO4 (aq) Why is Calcium Phosphate’s formula Ca3(PO4)2 Calcium ion Ca 2+ & Chapter 2 Phosphate ion PO4 3– +6 = -6 Ca3 (PO4)2 How do I know the Phosphate ion is -3 ? Because I know the formula for Phosphoric acid • Atomic Theory of Matter by Dalton • Atomic Structure by Rutherford – atomic numbers, mass numbers, and isotopes – notation +3 = -3 H3 PO4 Periodic Table of the ELEMENTS Atoms , Elements & Compounds • ATOMS : The smallest representative particle of an Element • ELEMENTS Are Fundamental Substances That Can Not Be Broken Down Chemically • A COMPOUND Is A PURE Substance Formed When TWO or More ELEMENTS Combine 4 6/27/2014 Experiments and Observations of Atomic Structure Types of Radiation alpha() beta() gamma() and radiation are both affected by an electric field while radiation is unaffected 1. 2. 3. 4. 5. Dalton Thomson Millikan Becquerel Rutherford Explained by ATOMS The Rutherford Model of Atomic Structure The Modern View of Atomic Structure The Nucleus, containing __________ (protons an neutrons) is surrounded by __________ Notation For Atoms Relative Weight of ATOMIC PARTICLES Name Charge Proton +1 Neutron 0 Electron -1 Mass (amu) 1 1 0 Mass Number Symbol A X Atomic Number Z Mass Number = Protons + Neutrons Atomic Number = Number of Protons 5 6/27/2014 Isotopes What is an ALPHA particle? An Particle is the Helium nucleus 4 2+ He 2 • Element with the same number of protons but different numbers of neutrons Isotopes of Atomic Carbon 612C 6 13 C 6 14C WHICH ONE IS RADIOACTIVE ? Number of Protons ? Number of Neutrons ? Number of Electrons ? 2 2 0 • Average Isotopic Mass: A weighted average of the isotopic masses of an element’s naturally occurring isotopes. The chemical symbol for an element with 22 protons, 26 neutrons, and 19 electrons is • The number of protons (22) is the atomic number so the element is titanium • The mass number of this isotope is the sum of the protons and neutrons • The ion has three more protons than electrons Ti 22 + 26 = 48 48Ti3+ Anatomy of a Chemical Equation CH4(g) + 2O2(g) Reactants appear on the left side of the equation CO2(g) + 2H2O(g) Products appear on the right side of the equation. The states of the reactants and products are written in parentheses to the right of each compound Coefficients are inserted to balance the equation Chapter 3 STOICHIOMETRY Stoichiometry: The chemical arithmetic used to relate the amount of products and reactants to each other in Chemical Reactions CHEMICAL REACTIONS 1st Write Chemical Reaction 2nd Balance Reaction 3rd Interpret Reaction A Couple of Important Reactions 1. Ammonia reacts with nitric acid to produce the fertilizer ammonium nitrate. Write the reaction NH3 (g) + HNO3 (aq) NH4NO3 (s) Is the reaction balanced? 2. When nitroglycerin C3H5N3O9 explodes, water, nitrogen, carbon dioxide, and oxygen form Write the reaction C3H5N3O9(liq) N2(g) + O2(g) + H2O(g) + CO2(g) Is the reaction balanced? © 2012 Pearson Education, Inc. 6 6/27/2014 CHEMICAL REACTIONS (YOU SHOULD KNOW) Chemical Reaction (you should know) COMBUSTION of a HYDROCARBON Reaction of a hydrocarbon with oxygen 1. COMBUSTION (Of a Hydrocarbon) 2. NEUTRALIZATION (Acid + Base) 3. ACID + ACTIVE METAL 4. FORMATION Reaction ACIDS You Should Know 1. 2. 3. 4. 5. 6. 7. 8. HCl (g) HCl (aq) HNO3 (aq) HC2H3O2 (aq) H2CO3 (aq) H2SO4 (aq) H3PO4 (aq) H3BO3 (aq) Hydrogen Chloride Hydro Chloric Acid Nitric Acid Acetic Acid Carbonic Acid Sulfuric Acid Phosphoric Acid Boric Acid Types of Formulas Methane Ethane Ethylene Propane Propylene Butane Some Simple Hydrocarbons CH4 Methanol CH3OH Ethanol C2H5OH C2H6 C2H4 C3H8 Propanol C3H7OH C3H6 C4H10 Butanol C4H9OH Chemical Formulas & Formula Weights Formula Weight is a conversion factor between moles and grams Formula Weight grams mole Formula Weight = the sum of the atomic weight of each atom in its chemical formula. Therefore MUST know chemical formula before formula weight can be calculated What is molecular mass of aspartame, C14H18N 2O5 the artificial sweetener marketed as NutraSweet ? • Empirical formulas give the lowest 14 x 12.0 + 18 x 1.0 + 2 x 14.0 + 5 x 16.0 = 294.3 g/mol whole-number ratio of atoms of each element in a compound. How many moles in 1.00 mg of aspartame ? • Molecular formulas give the exact number of atoms of each element in a compound. (1.00 mg = 1.00 x 10-3 g) 1 .00 x10 g x 2941 .3 mol g -3 3 .398 x10 6 3.40 x 10-6 mol 7 6/27/2014 Avogadro’s number is chosen so that 1 mole of 12C atoms has a mass of exactly 12 grams. 6 protons x 1.66 x 10-24 grams = 9.96 x 10-24 6 neutrons x 1.66 x 10-24 grams = 9.96 x 10-24 So 12 C weighs 19.92 x 10 -24 grams (19.92 x 10 -24) x (X ) = 12 grams Solve for X X = 6.0249638 x 1023 From khanacademy.org on Youtube • The mole and avogadro's number http://www.youtube.com/watch?v=AsqEkF7h cII&feature=related • Balancing Chemical Equations http://www.youtube.com/watch?v=RnGu3xO 2h74&NR=1 8