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Review Chapter 2: Scientific and Standard Notation Units and conversions - convert 200 cm to meters Sig Figs: how many sig figs in: 0.0031050 pounds 25010 meters Multiply/Divide: 3x4 = ? 3.0 x 4.0 = ? Add/Subtract: + 3.1 45 48.1 +/- .1 +/- 1 = ? Chapter 3: States of matter: solid, liquid, gas Physical Property - property of matter that can be determined without changing the compound. i.e. Color, smell, density, … Chemical Property – property of matter that is determined by changing the substance. i.e. Flammability, corrosiveness,.. Physical Change – Change in state of matter i.e. melt water Chemical Change – Change a substance to a different substance i.e. burn something Element – 1 type of atom Compound – 2 or more different elements that make up a molecule Homogenous Solution – solution that is the same throughout. i.e. Salt and water Heterogenous Solution – solution that is different throughout. i.e. Dirt and water. Examples of Energy: heat, light, motion, nuclear,.. measured in units of: joules, calories, Calories Specific Heat – The amount of energy needed to raise 1 gram of a substance 1 oC. Problem: Determine the Calories needed to warm 27 g of iron by 4 oC. q = ms∆t q = (27 g) ( .45 J g oC = 48.6 J x ) (4 oC) 1 calorie x 1 Calorie = 4.184 J 1000 calories 0.0116 Calories 1 Chapter 4: Proton, Neutron, Electron characteristics: Relative mass, and charge Isotopes: 7 How many protons, neutrons and electrons are in: Names of group 1, 2, 17, 18, 3 Li + 3-12 , 1-2 and 13-18 and charges of each group. Metals, metalloids and non-metals cation vs anion Chapter 5: Nomenclature Polyatomic ions: Type 1 metal & non-metal naming rules ClO3- Cr2O7-2 OH- NO3- NH4+ Type 2 metal & non-metal rules Name the following: Non-metal & non-metal rules FeSO4 Name the following: Ca(OH)2 MgCl2 KH2PO4 Cu 2O P2O5 Write formulas for the following: Write formulas for the following: Manganese (II) nitrate Sodium oxide Zinc phosphate Iron (III) sulfide Ammonium phosphate Nitrogen dioxide Naming acids: Without oxygen: hydro ______________ ic acid HCl? HBr? With oxygen: ic acid if anion ends with ate H NO3? Root + ous acid Root + if anion ends with ite H NO2? 2 Chapter 6: Chemical Reactions: Write a balanced equation for the following reaction: Methane gas reacts with oxygen gas to produce carbon dioxide and water. Chapter 7: Aqueous solution reactions: Know the solubility chart and how to determine if something is soluble in water. Write a molecular, complete and net ionic equation for: A solution of barium chloride and sodium phosphate are added. Chapter 8: Types of Reactions: Redox – transfer of electrons from 1 substance to another Mg + Cl2 MgCl2 CH4 + O2 CO2 + H2O Double Replacement: AB + XY AY + XB Acid-Base: HA + BOH Acid-Carbonate: HA + BCO3 BA + HOH + CO2 BA + HOH Zn + HCl ZnCl2 + H2 Single Replacement: ZnCl2 + H 2 ??? Combustion: HC + O 2 CO2 + H2O Metal + O2 Metal Oxide A + B AB AB A + B Synthesis: Decomposition Chapter 9: Moles Convert 10.0 g Al to moles 10.0 g Al x 1 mole = .37 mole Al 27.0 g Convert 10.0 g Al to atoms 10.0 g Al x 1 mole Al 27.0 g x 6.02 x 1023 atoms Al = 2.23 x 1023 atoms Al 1 mole Al Define atomic mass Define molar mass What is the molar mass of water? 3 Convert 22 g H2O to moles H2O 22 g H2O x 1 mole H2O 18 g H2O = 1.2 mole H2O Convert 22 g H2O to molecules of H2O 22 g H2O x 1 mole H2O x 6.02 x 1023 molecules H2O = 7.2 x 1023 molecules 18 g H2O 1 mole H2O How many atoms of H are in 22 grams of H2O? 22 g H2O x 1 mole H2O x 6.02 x 1023 molecules H2O x 2 atoms H 18 g H2O 1 mole H2O 1 molecule H2O = 1.4 x 1024 atoms of H A compound has a molar mass of 216 g/mole and for every 6.22 g of Nitrogen, it has 17.8 g of Oxygen. Determine its empirical and molecular formula. Empirical formula: 6.22 g N x 1 mole = .444 mole N / .444 mole = 1 mole x 2 = 2 mole N 14 g 17.8 g O x 1 mole = 1.11 mole O / .44 mole 16 g = 2.5 mole x 2 = 5 mole O Therefore, the empirical formula is N2O5, which has a molar mass of 28 + 80 = 108 g/mole 216 = 2 108 2 (N2O5) = N4O 10 (check to see that N4O10 weighs 216 g/mole) Determine the percent composition of N in ammonium nitrate. NH4NO3 has %N = gN g everything 2 mole N 4 mole H 3 mole O = = 28.0 g = 4.0 g = 48.0 g 80.0 g 28.0 x 100 = 35 % Nitrogen 80.0 4 Chapter 10: Stoichiometry: 12.15 g of Mg is added to 16 g O 2. Predict the g of MgO formed 12.15 g Mg x Avail: 1 mole = .50 mole Mg 24.3 g Mg .50 16 g O2 x 1 mole = .50 mole O2 32 g O2 .50 2 Mg + O2 2MgO Case 1 Case 2 .50 1.0 .25 .50 .50 1.0 which doesn’t work? .50 mole MgO x 40.3 g MgO = 20. g MgO forms 1 mole MgO % Yield: Regarding the problem above, the reaction is completed, and 17 g MgO is formed from the experiment. What is the theoretical, actual and percent yield? = 17 x % Yield = actual theoretical 20 Theoretical = 20. g 100 = 85 % Actual = 17 g Chapter 11: Atomic Theory Properties of waves: (wavelength, amplitude, frequency, speed) Different types of light are determined by their wavelength…radio, uv, infrared, visible, x-ray,.. Electron principle energy levels n = 1 , 2 , 3 , … Sub energy levels: s p d f Electron configuration and orbital diagram for: S How many unpaired electrons? S-2 Size: Increases going down a group, decreases going left to right Ionization Energy – the energy required to remove an electron from an atom. decreases going down a group, increases going left to right across a period. Electronegativity – increases toward fluorine 5 Chapter 12: Bonding Intramolecular – bond between atoms to form a molecule Covalent Polar Covalent Ionic bond between HCl? electronegativity difference 0 - .2 .2 - 1.7 > 1.7 H2O? NaF? Intermolecular – bond between 2 molecules Lewis structures of molecules: What is the shape of: H2S? CO2? PH 3? molecular shapes: Linear Trigonal Planar Tetrahedral Trigonal Pyramidal Bent Chapter 13: Gases Know the relationship between pressure and volume plus temperature and volume. Combined Gas Law: deals with changing conditions. P1V 1 = P2V2 T1 T2 Calculate the volume of 2 liters of gas at 100 oC and 3 atm if it is changed to STP. (3 Atm) (2 L) (373 K) = (1 Atm) (V2) (273 K) V2 = 4.4 Liters 2 Liters of gas at 3 atm is converted to 1 atm of pressure. What is the volume? (3 Atm) (2 L) = (1Atm) (V2) Temperature is not changed, and is eliminated in the equation. V2 = 6 Liters 6 Pressure units and conversions Convert 275 mm Hg to atm 275 mm Hg x 1 torr 1 mm Hg x 1 atm = .362 atm 760 torr Ideal Gas Law: P V = n R T used mostly when moles, grams, molecules or atoms are included in the problem. Determine the volume of 2.0 g of He at STP 2.0 g He x 1 mole = .5 mole He 4.0 g (1 atm) (V) = (.50 mole) (.0821) (273) 11.2 liters R = .0821 (atm) 8.31 (kPa) 62.36 (torr) Partial Pressure: 2 mole of H2 and 3 mole of N2 are placed into a container with a total pressure of 1.0 Atm. What is the partial pressure of the H2? Pi = Xi Pt PH2 = 2 (1 atm) = .4 atm 5 Gas Stoichiometry: 3 Liters of CH4 are mixed with 2 Liters of O2 at STP. How many moles of CO2 will form at STP? Avail: 3 L CH4 Case 1 3 Case 2 1 + 2 L 2O2 CO2 + 6 won’t work 2 1 1 Liter of CO2: 2H2O PV = nRT (1 atm) (1 Liter) = n (.0821) (273) n = .0446 mole CO2 forms Kinetic Molecular Theory: 1. 2. 3. 4. Gas particles are small relative to the space they travel in. Molecules move in straight line motion, changed by collisions. Collisions are elastic. Velocity of molecules is dependant on temperature. Diffusion: movement of gas molecules from high to low concentration. Lighter molecules have higher average velocity than heavy molecules, therefore, light molecules diffuse faster. (Taco Bell) 7 Chapter 14: Solids and Liquids ∆Hfusion = 6.02 kJ/mole ∆Hvaporization = 40.6 kJ/mole How much energy is required to warm 18 g ice at 0oC to 100oC steam? 18 g x 1 mole x 6.02 kJ x 1000 J = 6,020 J 18 g 1 mole 1 kJ q = 18 g x 4.184 J x 100 oC g oC = 7,531 J 18 g x 1 mole x 40.6 kJ x 1000 J = 40,600 J 18 g 1 mole 1 kJ 6,020 + 7,531 + 40,600 = 54,151 J Polarity of a molecule is determined by its shape and the electronegativity of the elements that make it up. Intermolecular Bonds: 1. 2. 3. 4. Dipole-Dipole Hydrogen London Ionic What type of bonding would be found in molecules of: HCl? H2S? H2? H2O? Vapor Pressure – function of molecular weight and strength of intermolecular bonding. Which has higher vapor pressure, CH3OCH3 or CH3CH2OH? (Can you name these compounds?) Solids are classified by their bonding: Ionic – metal + non-metal Molecular – non-metals Atomic – network or metallic (diamond or iron) What type of solid is: NH3? BaO? 8 Chapter 15: Solutions Dissociation Concentration is usually measured by Molarity, M M = mole solute Liters solution Calculate the molarity of 11.5 g NaOH dissolved in 1.5 Liters solution 11.5 g NaOH x 1 mole = .2875 mole NaOH 40.0 g M = .2875 mole = .19 M NaOH 1.50 L Solution Stoichiometry What mass of KNO3 is formed from .0035 mole Ba(NO3)2 added to 265 mL .010 M K2CrO4? .010 M = mole .265 L M = mole Liter mole = .00265 Avail: .0035 mole Ba(NO3)2 Case 1 .0035 Case 2 .00265 .00265 mole + K2CrO4 .0035 .00265 BaCrO4 + .00265 2KNO3 (2)(.00265) = .0053 .0053 mole KNO3 x 101.1 g = .53 g KNO3 will form 1 mole Chapter 16: Kinetics, Equilibrium and Solubility A + B C 350 200 100 What is Ea and ∆H for the forward reaction? Is this endothermic or exothermic? What about the reverse reaction? ( C A + B) 9 Equilibrium – Forward and reverse reaction occur at the same rate Write the Equilibrium expression for 2H2O(l) ↔ 2H2(g) + O2(g) K = [H2]2 [O2] Small K means that reaction favors reactants, large K favors product formation. LeChateliers Principle A(s) + 3B(g) ↔ 2C(g) + D(aq) + energy add B remove A increase P lower temperature The solubility of PbF 2 is 2.5 x 10-3 mole/Liter. Calculate Ksp PbF2(s) ↔ Pb+2 2.5 x 10-3 2F- + (2) 2.5 x 10-3 = 5 x 10-3 Ksp = [Pb+2] [F-]2 [2.5 x 10-3][5 x 10-3]2 = 6.3 x 10-8 Chapter 17 – Acids and Bases Acid – H+ donor Base - H+ acceptor Write an equation of water + ammonia. Strong acids dissociate completely, weak acids barely dissociate. Write an equation of HCl HF + H2O + H2O Know the list of strong acids. 10 Auto-ionization of water: H2O + H2O H 3O+ + OH- Kw = 1 x 10-14 = [H+][OH-] What is the [H+] and pH of a .25 M NaOH solution? NaOH Na+ + OHInit Final .25 0 0 .25 0 .25 1 x 10-14 = [H+][.25] [H+] = 4 x 10-14 pH = (-1) log 4 x 10-14 = 13.4 Does this make sense? Mg + Cl2 MgCl2 What is oxidized? What is reduced? What is the oxidizing agent? What is the reducing agent? 11