Second Exam Study Sheet Chem 111 Section 3 Fall 2013--A periodic table will be provided--Mathematical equations and values of constants will be provided on the exam --Topics in the book or lectures not mentioned here will not be covered on the exam1. Balancing chemical equations.2. Using balanced chemical equations to calculate amounts of reactants and products.3. Identifying limiting reactants, using them to calculate amounts of reactants and products.4. How ionic compounds dissolve: in waterHydration forces overcome ionic attractions, hydrated ions completely surroundedby shells of water molecules, arranged by coordination of the partial positive and negative charges of water to the solvated ion5. Trends (only) in solubility of ionic compounds: 1) the higher the charges on ions, the less soluble the compound2) the more matched in size the ions, the less soluble the compound6. Writing simple net ionic equations, spectator ions.7. The definition of hydrogen bonding: A hydrogen atom bonded to a very electronegative atom (either N, O, or F), is strongly attracted to an N, O, or F, atom in another molecule (or, in large molecules such as proteins, to a N, O, or F in the same molecule)8. Definitions of oxidation and reduction.9. Calculation of oxidation states (oxidation numbers) for atoms in compounds.10. Identifying redox reactions, what is oxidized and what is reduced, showing whichatoms change in oxidation state and how many electrons are transferred.11. Molarity: calculation of the molarities of reagents, using molarities to determine amounts or volumes of reactants and products.12. Acid-base titrations: finding the concentration or volume of an acid (or base) by titration with a base (or acid) of known concentration and volume.13. Definition of H of a reaction:Enthalpy: the heat exchanged under constant pressure during the reaction14. Sign of H: exothermic and endothermic reactions, which is associated with breaking or forming weak or strong bonds. That energy is needed to break bonds, energy is evolved when bonds form.15. Specific heat capacities: calculating energy exchange as temperature changes.16. Energy of phase changes: heat of fusion and heat of vaporization. Calculation of energy needed to change a phase for a given quantity of a material. That the temperature of a material remains constant during a phase change.17. Enthalpy change of reactions Hrxn: its dependence on stoichiometry, sign change for reverse reaction.18 Hess' Law: 1) Hrxn is equal to the sum of the H of all the individual steps of the reaction2) Hrxn depends only on the starting reactants and the end products and their states, and is independent of the pathway taken from one to the other Using Hess' Law to calculate enthalpy changes (Hrxn) for reactions19. Standard heats of formation Hfo: definition, writing the reaction for any compound that Hfois the enthalpy change for. Standard heats of formation: the change in enthalpy when one mole of a substance, in the standard state of 1 atm of pressure and temperature of 29815 K, is formed from its pure elements under the same conditions Value of it for all elements in standard state is zero20. The conditions known as "standard conditions, or "standard state".25 degrees centrigade, 1 atm21. Using given values of Hfo to calculate enthalpy changes for reactions. Hrxn = ∑nHfo (products) - ∑mHfo (reactants) (this equation not given on theexam)22. Definition of electromagnetic radiation. Wavelength and frequency of electromagnetic radiation, how they are related. Calculation of one from the other. Relationship of short or long wavelength and high or low frequency to the energy of the radiation.Electromagnetic radiation: energy that travels through space as a waveShort wavelengthhigh frequency, Long wavelength low frequency23. The electromagnetic spectrum: names and orders of the different wavelength regions.ROYGBIVRadio, Microwave, Infrared, Visible, Ultraviolet, Xrays, Gamma raysBiggest wavelengthsmallest wavelength24. Photons: definition, calculating the energy of, calculating the energy of any wavelength of light.Photon- 1 particle of lightE = hνh = Planck's constant, 6626 x 10-34 J ⋅s25. Description of the Bohr model of the atom: energy levels and principal quantum numbers, how electrons transit from one energy level to another (no calculations of this). Ground and excited states, absorption and emission.26. Using the de Broglie equation to calculate the wavelengths of matter in motion.m = mass in kg h = Planck's constant v = velocity in sec-27. Definition of an orbital: The space within which an electron having a certain energy, in an atom, is allowed to be, or, where it has a 90% probability of being28. The four quantum numbers: names, symbols, what each represents, allowed values of each, calculating three (ms does not need to be exactly specified, only that it is either 1⁄2 or - 1⁄2 ) quantum numbers of any electron. Number of orbitals, types of orbitals and number of electrons in each orbital, for any value of n.29. s, p, d, and f orbitals: shapes of each, quantum numbers of each, how many of each there are.30. What each magnetic quantum number represents (different orientation of the subshell orbitals, as, for example, along different axes)31. Energy level diagram for orbitals (Figure