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Unformatted text preview: the trends in vapor pressure as a function of temperature • draw a particle diagram representing vapor pressure • be able to draw particle diagrams that distinguish solid and liquid phases; be able to describe the motion in the phases • identify the 6 phase transitions and label them (evaporation, condensation, freezing, melting, sublimation, deposition) 7 Hunter College, CUNY •
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• identify the phases at higher temperature and lower temperatures recognize that heat and temperature are different concepts identify the different phases on a heating curve and recognize those that require the most energy locate gas, liquid, and solid regions in simple phase diagrams, and be able to read boiling points and freezing points from the diagrams describe the different types of intermolecular forces and the relative strengths of the interactions recognize the IMF present in a specific substance when given its name or structure describe the types of bonding in solids, particularly metallic bonds, network atomic bonds, molecular solids, and ionic solids write a chemical equation from viewing a unit cell compare the difference between a chemical equation for a unique molecule and the chemical equation for a solid – note the importance of the unit cell given a structure and chemical formula, identify the type of bonding in the solid • Unit 7: Stoichiometry (including math skills) Read Chapter 1, sections 1.1 1.6, Appendix A and Chapter 3, sections 3.1 3.11 • recall and apply the basic rules of significant figures, scientific notation and rounding • perform basic unit conversions for metric units or when given conversion factors • re arrange a basic algebraic expression to isolate any variable in the expression (i.e. PV=nRT) • revisit balancing a chemical equation and use the coefficients to predict the number of atoms or molecules produced or used in a chemical reaction • articulate what the coefficients mean in terms of number of reacting atoms or molecules AND in terms of combining ratios • write a definition of the mole in terms of a fixed number of particles – Every mole contains _?__ particles. (Av#) • recall the number of particles from gases and think of this as a fixed unit • scale up the coefficients to realize that they can refer to the number of atoms and molecules or even to the number of moles. • articulate that the atomic mass in the periodic table is the number of grams in a mole of the element. Alternatively the atomic mass in the periodic table is the number of grams in an Avogadro’s number of atoms. • use the periodic table (atomic mass) to determine the mass (in grams) of a single mole of different substances. • interpret the chemical formula to be able to compute the molar mass. • convert between moles and masses for an arbitrary amount of matter • convert between numbers of particles, moles and grams – any two! • balance chemical equations by moles • use the chemical equation to compute the maximum amount (theoretical yield) of products produced • use the chemical equation to compute the amount of reactants needed to produce a 100% yield • compute percent yields for any chemical reaction from actual yields and theoretical yields. • incorporate limiting reagent calculations into all stoichiometric calculations • obtain the empirical formula from mass measurements and chemical reactions • obtain molecular formulas from empirical formulas and molecular weight data • calculate the average mass number from the periodic table for any element based on isotope abundance 8 Hunter College, CUNY Unit 8...
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This note was uploaded on 02/24/2014 for the course CHEM 102 taught by Professor Peterpastos during the Winter '08 term at CUNY Hunter.
 Winter '08
 PETERPASTOS
 Chemistry, pH

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