CHEM 1332 2nd EditionExam # 1 Study Guide Lectures: 1 - 9Lecture 1 (August 29)What are the three main states of matter and describe them in macroscopic ad microscopic- Solid in the macroscopic view has a definite shape and volume. A solid in the microscopic view the particles are in a regular arrangement with strong attraction as four balls held together by springs. Liquid in the macroscopic view has a definite volume, but adopts the shape its container. Liquid in the microscopic view has a more random arrangement and has an ok attraction as four balls held together by stretchy wire. Gas in the macroscopic view hasno definite volume and takes the shape of its container. Gas in the microscopic view has a random arrangement with no attraction as just fours balls with no attachment.What is the change in heat equation?It is q=m x c x T m is mass, c is specific heat and the last part is change in temperatureIdentify the different stages of a curve?The first step the equation is q=m x c x T m is the mass c is the specific heat and T is the temperature. Step two q=Hfus x n where H fus is heat fusion and n is moles. Step three q= m x cliq x T where c liq is the specific heat of a liquid. Step four q= Hvap x n this step is longer because it takes more time to turn a liquid into gas than a solid to liquid. H vap is heat vaporization. Step five q=m x cgas x T where cgas is the specific heat of gas.Lecture 2 (September 3) What is a phase diagram?-The phase diagram is a pressure vs. temperature graph. The melting point on the diagram is where the solid and liquid interface usually that slope is almost vertical and it is essentially independent of pressure. Some species like water the line is a little negative of the vertical. The boiling point is where the liquid and gas interface an it is very dependent of pressure. A liquid boils when the vapor pressure is equal to the atmospheric pressure. The triple point is where allthree states coexist.What are IPFs?- Inter-particle forces (IPF) affect the physics of melting point, boiling point, change in heat fusion,change in heat vapor, viscosity and surface tension these as the (IPF) is stronger they increase. Vapor pressure has the opposite affect as IPF is stronger vapor pressure goes down. Ionic bonds are very very very strong bonds and have higher boiling and melting points. Metallic bonds very very very strong bonds described as a sea of electrons have high boiling and melting points mercury is one of the few metals that is liquid at room temperature. Network covalent bonds are very very very very strong bonds have high melting and boiling points an examples are diamonds and graphites.Lecture 3 (September 5)What is a discrete molecule?- Discrete molecule is a type of inter-particle force particularly inter-molecular force. One type is polar molecules in this type of molecule it has different ends, one end is slightly positive and theother is slightly negative. This creates an attraction between the two molecules that is called a dipole-dipole attraction it is a very weak attraction and does not have very high melting points.What is London Dispersion forces?- This type of force one electron density cloud approaches another it distorts the molecule. This isthe dominant intermolecular force and they are mostly weak bonds. They have low melting points.What is a hydrogen bond?- This is a special type of dipole-dipole force that is of molecules that have an H atom bonded to asmall highly electronegative atom with lone electron pairs specifically N,O, or F. Relatively strongbond.When does polarizability increase and decrease?- It increases down a group and decreases across a period.What are some equations for parts of solute over parts of solution?- First example is mass percentage of (solute/solvent) is equal to the mass of the (solute/solvent) over the total mass times a 100. The next is volume percentage of (solute) is equal to the volume of the (solute) over the total volume times a 100. The mole fraction of (solute/solvent) is equal to the mole of (solute/solvent) over the total moles. Molarity is equal to moles of the solute over liters of the solution the issue with this concentration is that volume changes with temperature. Molality is equal to moles of a solute over kilograms of solventLecture 4 (September 10)What are colligative properties?- Colligative properties are properties that depend on the amount of solute and they are vapor pressure, boiling point, freezing point and osmotic pressure.What are the vapor pressure effects?- The vapor pressure of a nonvolatile nonelectrolyte solution is always lower than the vapor pressure of the pure solvent. The equation for these changes is Raoult’s Law Vapor pressure of asolution is equal to mole fraction of solvent times vapor pressure of solute. Another case is the vapor pressure of a solution is equal to the mole fraction of solvent times the vapor pressure of the solvent plus mole fraction of solute times vapor pressure of the solute. This occurs when solvent that is soluble is dissolved in solventWhat are the effects of boiling point?- A solution boils at a higher temperature than the pure solvent. The equation for change in boiling point is bp=kbpxm where kbp is a boiling point constant that depends upon the solute. What are the effects of freezing point?- The solution freezes at a lower temperature than the pure solvent. The equation for this is fp=kfpxm where kfp is the freezing point constantLecture 5 (September 12)What are the effects of osmotic pressure?- It is when solutions of a higher and lower concentrations are separated by a semi-permeable membrane one that allows solutes but not solvent to pass through. The net flow of water into the solution increases its volume and thus decreases its concentration. The equation is osmotic pressure= MRT and M is the molar mass R is a constant and T is temperature.What are the effects of breaking and making imfs?- The breaking of imfs is endothermic while the making is exothermic. In a exothermic reaction it is nice because a solute is soluble in a solution. In this case the imfs of a solution are greater than the solute and solvent. In a reaction that is a little endothermic the solute is still soluble. The imfs in the solute and solvent are about equal to the solution. In a reaction that is very endothermic it is nasty and the solute is insoluble in the solvent. In this reaction the imfs in the solution are