0110 F24 Outline of Possible Exam 2 Material PDF

0110 F24 Outline of Possible Exam 2 Material Section 4.2 Classifying Chemical Reactions Determine whether a redox reaction has occurred o assign oxidation states o identify species that is ▪ oxidized ▪ reduced...

0110 F24 Outline of Possible Exam 2 Material Section 4.2 Classifying Chemical Reactions Determine whether a redox reaction has occurred o assign oxidation states o identify species that is ▪ oxidized ▪ reduced ▪ the reducing agent ▪ the oxidizing agent Balance redox reactions in o acidic conditions o basic conditions Recognize that single displacement and combustion reactions are redox reactions. Recognize that decomposition reactions and combination reactions might be redox. Section 4.3 Reaction Stoichiometry Use stoichiometric coefficients to o determine the moles of each reactant required for a reaction (Example 4.8) o relate masses of reactants to masses of products (Example 4.10) o relate masses of reactants to each other (Example 4.11) Section 4.4 Reaction Yields Identify the limiting reactant (Example 4.12) o Recognize that theoretical yield is determined by the limiting reactant. Calculate percent yield (Example 4.13) Section 4.5 Quantitative Chemical Analysis Explain the techniques of o titration o gravimetric analysis o combustion analysis Determine the concentration of a solution of an acid or base from titration data (Example 4.14) Determine the concentration of a solute from gravimetric analysis data (Example 4.15) Determine empirical formulas from combustion analysis data (Example 4.16) 0110 F24 Outline of Possible Exam 2 Material Chapter 5 Thermochemistry Section 5.1 Energy Basics Define and identify examples of kinetic energy potential energy thermal energy Covert between temperature scales Celsius, C Fahrenheit, F Kelvin, K Be familiar with the units for energy o Calorie (cal) o Joule (J) Distinguish between heat capacity specific heat molar heat capacity Determine, from C = q/∆T or q = c x m x ∆T specific heat heat capacity molar heat capacity mass heat temperature (initial or final) Complete all the examples and example checks in the section Section 5.2 Calorimetry Explain how calorimetry is used to measure heat transfer Distinguish between endothermic and exothermic processes system and surroundings Understand and apply the idea that qreaction = −qsolution Explain how a bomb calorimeter is used. Understand that a nutritional calorie (Calorie) equals 1 kcal. Complete all the examples and example checks in the section. 0110 F24 Outline of Possible Exam 2 Material Section 5.3 Enthalpy State the first law of thermodynamics. Explain and apply the following terms and concepts internal energy expansion work (pressure volume work) state function enthalpy (H) and enthalpy change (∆H) standard state conditions standard enthalpy of combustion (∆HC) standard enthalpy of formation (∆Hf) Hess’s law Write thermochemical equations. Manipulate thermochemical equations. Complete enthalpy of combustion calculations. Determine the heat of reaction from standard enthalpies of formation. Complete all the examples and example checks in the section Chapter 6 Electronic Structure and Periodic Trends Section 6.1 Electromagnetic Energy Convert between wavelength and frequency. Understand the relationships between energy wavelength frequency Know the regions of the electromagnetic spectrum. Recognize constructive and destructive interference. Determine the number of nodes in a standing wave. Distinguish between a continuous spectrum and a line spectrum. Explain the ultraviolet crisis photoelectric effect wave particle duality of light the contributions of o Balmer o Rydberg o Bohr Section 6.2 The Bohr Model Describe the Bohr model of the atom. Distinguish between the ground state and the excited state of an electron. 0110 F24 Outline of Possible Exam 2 Material Use the Rydberg equation to calculate energy of transitions. Section 6.3 Development of Quantum Theory Relate wave-particle duality of light to that of an electron. Understand and apply quantum numbers. Describe the four quantum numbers and their significance principal quantum number, n angular momentum quantum number, l magnetic quantum number, m spin quantum number, ms Understand the deBroglie wavelength Heisenberg uncertainty principle Pauli exclusion principle Section 6.4 Electronic Structure of Atoms Write electron configurations for atoms and ions. orbital diagrams for atoms and ions. Apply The Aufbau principle Hund’s rule Distinguish between valence electrons and core electrons. Identify Main group elements Transition elements Inner transition elements Section 6.5 Periodic Variations in Element Properties Describe, explain, and apply periodic trends in covalent radius effective nuclear charge ionic radii ionization energy electron affinity metallic character Recognize isoelectronic species. 0110 F24 Outline of Possible Exam 2 Material Chapter 7 Chemical Bonding and Molecular Geometry Section 7.1 Ionic Bonding Distinguish between cations, anions, atoms, and molecules. Explain how cations and anions form. Identify properties of ionic compounds. Compare properties of ions and atoms. Identify binary ionic compounds. Explain what is represented by the formula of an ionic compound. Recognize that attractive forces between ions are isotropic (the same in all directions). Explain the inert pair effect. Write electron configurations for atoms. anions. cations. Section 7.2 Covalent Bonding Explain how covalent bonds differ from ionic bonds. Compare the properties of molecular compounds with those of ionic compounds. Explain how covalent bonds form. Recognize the factors that affect bond length. that bond breaking is endothermic. that bond making is exothermic. Distinguish between polar covalent and pure covalent bonds. Differentiate between effective nuclear charge. electronegativity. electron affinity. Recognize trends in effective nuclear charge. electronegativity. electron affinity. Recognize polyatomic ions as charged molecules. 0110 F24 Outline of Possible Exam 2 Material Section 7.3 Lewis Symbols and Structures Write Lewis symbols from valence shell electron configurations. Show formation of ions with Lewis symbols. Distinguish between lone pair electrons and bonding electrons. Explain what the octet rule is. Distinguish between single bonds double bonds triple bonds Draw Lewis structures. Recognize the exceptions to the octet rule electron deficient species hypervalent species Section 7.4 Formal Charge and Resonance Assign formal charge to atoms in molecules. Use formal charge to determine which Lewis structures are best. Explain what resonance is. how resonance structures differ from isomers. what a resonance hybrid is.