ࡱ> jmic uObjbj 4V^\^\! \LP(TTTTTCY eOOOOOOOTtW^O]mCCmmOTTPPm"TTOmONwJNTܱiiL0OfP0POLLWA|W`NNZWNmmmmmmmOOmmmPmmmmWmmmmmmmmm > ^: Study Guide for Chemistry 1A Final Exam (American Chemical Society (A.C.S.) Chemistry Exam) 70 multiple choice questions, 110 minutes Bring a green color scantron, non-programmable calculator, pencil(s) and eraser. You are not allowed to write or make any markings on the ACS exam paper. Scratch paper will be provided. Chapter 1 Matter and Measurements Classification of matter Recognize the different states of matter (solids, liquids and gases) and give characteristics of each. Physical properties and chemical properties SI units and Metric Units Know how to find density, mass or volume if two of the three quantities are known. Convert temperatures between Celsius, Kelvin and Fahrenheit scales. Use dimensional analysis in calculations, conversions, etc. Know the differences between accuracy and precision. Be able to report a value correctly using the appropriate number of significant figures. Use the concept of percent in chemistry. Understand the difference between qualitative and quantitative measurements. Chapter 2 Atoms, Molecules and Ions Atomic Theory -Know the main contributions of Dalton, Thomson, Rutherford and Millikan. Atomic number, mass number, and isotopes. Understand the definitions of cation (positive charge) and anion (negative charge) Calculation of number of protons, electrons and neutrons for neutral and charged species. Predicting the ionic charges on atoms in groups 1A-3A and 5A-8A. Recognize that transition metal elements often exist in a variety of positively charged oxidation states. List of elements that exist as diatomic molecules Be able to recognize chemical compounds and identify the number and identity of atoms/ions in the compound. Naming compounds: ionic, covalent (molecular), acids and hydrates. Chapter 3 - Stoichiometry: Calculations with Chemical Formulas and Equations Writing chemical equations and balancing chemical equations. Types of chemical reactions and predicting product of chemical reactions. Avogadro number and conversion from number of atoms/ molecules to moles and vice versa. Formula weight, molecular weight and molar mass. Conversion of grams to moles, moles to grams, number of atoms/molecules to grams, grams to number of atoms/molecules. Percent composition and use of percent composition in calculation of empirical formulas. Calculation of empirical formula, molecular formula. Combustion analysis data for calculation of empirical formula. Use experimental data to calculate the number of water molecules in a hydrated compound. Stoichiometry: (mole-mole, mass-mass, mole-mass, mass mole, mass-number of molecules problems), Limiting reactants Yields of reactions (actual/experimental, theoretical, percent yield), Chapter 4- Aqueous Reactions and Solution Stoichiometry Properties of aqueous solutions electrolytes (weak and strong, non-electrolytes) Precipitation reactions solubility rules Writing net ionic equations Acids and bases neutralization reactions Calculation of oxidation number of an element in a compound. Know the definitions of reduced, oxidized, reducing agent and oxidizing agent. Be able to recognize an oxidation-reduction reaction. Concentration of solutions mass percent, molarity Interconverting molarity, moles and volume. Concentration of electrolytes (SA-C) Conversion of mass percent to molarity and molarity to mass percent Dilution calculations (M1V1 = M2V2) Solution stoichiometry and titration calculations using solution concentrations and volumes. Chapter 5 - Gases Basic Gas Laws: Boyles, Charles, Avogadros, Combined Ideal Gas law PV = nRT; MM= DRT/P; P1V1/n1T1 = P2V2/n2T2 STP conditions and calculations of molar mass, molecular weight, and gas density. Gas Stoichiometry Daltons Law of Partial Pressures and Vapor pressure due to water Grahams Law of Effusion and Diffusion Relationship of rate of effusion to molecular speed of gas molecules and to molecular weight of gas molecules. Deviations from ideal behavior (high P, low T) Chapter 6 - Thermochemistry Kinetic and potential energy Units of energy (calories, joules) and energy changes. Exothermic and endothermic reactions. Enthalpy and enthalpy (heat) of reaction ((Hrxn). Standard states. Relating (H to quantity of reactants and products Standard enthalpies of formation ((Hf() ( elements in standard states ( compound (1 mol in standard state) Using (Hf( to calculate (H(rxn and calculation of (Hf( of reactant or product when other (H values are given. ((H(rxn = ( n(Hf( (products) - ( m(Hf( (reactants)) Using Hesss law to calculate of (H for reactions. Calorimetry and specific heat (q = mC(T) Heats of solution. Chapter 7 Electron structure of atoms Electromagnetic radiation and relationship between energy, wavelength and wavelength for the different regions, Use the equation relating wavelength (l), frequency (n) and the speed of light (c). (E = hn; n = c/l). Quantum Theory, the Bohr atom, discrete energy levels, line spectra, emission spectra. Quantum mechanics: the allowed values for quantum numbers (n, l, ml, ms) Uncertainty principle, Pauli Exclusion Principle, Shape and meaning of atomic orbitals. Electron configurations of atoms (ground state and excited state) and ions Hund's rule, valence electrons, diamagnetism and paramagnetism. Relating Electron configuration to position of the element on the Periodic Table. Chapter 8 - Periodic Properties of the Elements Periodic trends in physical and chemical Properties. Valence electrons. Periodic variation in specific physical properties: Atomic Radius, Ionic Radius, Ion size in an isoelectronic series. Ionization Energy. Predicting the element of a certain period from the given successive ionization energies. Understand Electron Affinity and meaning of sign associated with its value. Chapter 9 - Basic Concepts of Chemical Bonding Lewis Dot Symbols for elements or ions and Lewis structures for compounds. Ionic Bonding, Covalent Bonding. Lattice Energy of Ionic Compounds (as a periodic property) Electronegativity (as a periodic property) and as a measure of bond polarity. Formal Charge calculation Resonance, multiple covalent bonds, bond length, bond energy. Octet Rule, Exceptions to the Octet Rule. Bond Dissociation Energy and calculation of (H. ((Hrxn = ( (bond enthalpies of bonds broken) - ( (bond enthalpies of bonds formed) Chapter 10- Molecular Geometry and Bonding Theories Valence Shell Electron Pair Repulsion Model (VSEPR). Predict Molecular Geometry (see Table 9.2 p 337 and 9.3 p 340), electron domain geometry, bonding domains (electron pairs) and nonbonding domains or lone pairs for molecules. Predict the bond angle in the molecule and predict if the molecule is polar or nonpolar. Hybridization of atomic orbitals and predicting the hybridization of an atom in a molecule. Bond angles in hybrid orbitals. Sigma (s) bonds and pi (p) bonds and type of overlap in these bonds. Molecular orbital theory  bonding orbitals and antibonding orbitals. Bond order and stability Calculation of bond order. Bond order = (no. of bonding electrons  no. of antibonding electrons) Chapter 11- Liquids and Intermolecular Forces Types of Intermolecular Forces: Ion-Dipole, Dipole-Dipole, Hydrogen Bonds, London dispersion forces and polarizability. Properties related to Intermolecular Forces: 1. Vapor Pressure; 2. Normal Boiling Point; 3. Molar Heat of Vaporization; 4. Surface Tension; 5. Viscosity. 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Factors that affect solubility, Solute-solvent interactions Important problems involving calculations to focus while reviewing: Density calculation Percent error Mass to mole; mole to number of atoms, mass to number of atoms/molecules/formula units Stoichiometric calculations: Mole to Mole, Mole to Mass , Mass to Mole, Mass to Mass Calculations involving solutions Titrations Calculations involving gases Limiting reagent Theoretical yield and percent yield Empirical and molecular formulas Gas Law problems Solution concentration and dilution Thermochemistry : (H(rxn, (H(f, Hesss Law, bond enthalpies, specific heat related problems. 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