CHEM 151 1st EditionExam 1 Study Guide Lectures: 2 - 11Lecture 2 (August 28)Properties can be broken up into two different categories: extensive and intensive. An extensiveproperty is dependent on the amount of material. It can also be called quantitative. An intensive property is dependent on the type of material. It can also be called qualitative. There are four methods of separation: distillation, extraction, filtration, and chromatography. Below are the factors that each method is based upon. (For example, distillation is based on the difference in boiling points.) - Distillation = boiling point- Extraction = solubility- Filtration = size- Chromatography = absorptionLecture 3 (August 30)Phase transitions:Lecture 5 (September 4)Phase Diagrams:Top image is a general phase diagram for a given substance. Bottom image is a phase diagram for water, which has differences from a normal phase diagram.-Water does not have a super critical fluid region.-The line separating the solid region from the liquid region points in the opposite direction for water. Lecture 6 (September 6)Basic assumptions about a particulate model of matter:1. Any macroscopic sample is composed of a large number of particles.(1 mL of water = 3.34 x 1022 molecules) 2. Particles are constantly moving. (Translation, rotation, vibration, etc.)3. Particles interact with each other. The nature and strength of the interactions depends on distance. Important equations to remember:T (K) = T (˚C) + 273.15 ; to convert temperature from degrees Celsius to KelvinKE = ½ m v2 ; to calculate kinetic energy using mass and volume Interparticle Forces:1. Solids (strongest)2. Liquids3. Gases (weakest)Lecture 7 (September 9)Gases at high temperature and low pressure we assume:Kinetic-Molecular Theory:1. Particles are moving (have KE) but do not interact (no PE).2. Only interact with walls of container.3. Particles are points with mass but no volume.Ideal Gas Law: PV = nRT P=pressure (atm)V=volume (L)n=number of moles (mol)R=gas constant= 0.08206 ((L atm)/(mol K))T=temperature (K)Units given on variables are the most commonly used units, and therefore if possible, values should be converted before plugging into the equation.Variables on the same side of the equation are inversely proportional.Variables on opposite sides of the equation are directly proportional.Lecture 8 (September 11)Elemental substances consist of only one type of atom. Elemental atom- Na for example Elemental molecule- non-metals; Cl2 for exampleLecture 9 (September 13)A mixture can be made up of two elements, two compounds, or an element and a compound. There are two types of mixtures: Homogenous: uniform distributionHeterogeneous: non-uniform distributionSTP (Standard Temperature Pressure)T=273.15 KP=1.00 atmLecture 10 (September 16)An example of a balanced equation and its importance: Na2 + Cl  NaCl (unbalanced) Na2 + 2Cl  2NaCl (balanced)Too much sodium will cause an explosion.Too much chlorine will result in you being poisoned. You can see from the balanced equation that for every sodium molecule, you will need two chlorine molecules.Lecture 11 (September 18)Avogadro’s Number: 6.022 x 1023 particles/molTo calculate molar mass of a compound:(using C2H6O)2 moles of C: 12.01 x 26 moles of H: 1.008 x 61 mole of O: 16.00 x 1*add all together to get final valueMolar mass (C2H6O) = 46.07