CHEM-C 117 Midterm: C117 Exam 2 Study Guide (Mar. 2)
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9-10 additional examples and information/study guide for exam 2. Bond energy- energy needed to break bond (endothermic: = (cid:1828)(cid:4666)(cid:1854)(cid:1867)(cid:1866)(cid:1856)(cid:1871) (cid:1854)(cid:1870)(cid:1867)(cid:1863)(cid:1857)(cid:1866)(cid:4667) (cid:1828)(cid:4666)(cid:1854)(cid:1867)(cid:1866)(cid:1856)(cid:1871) (cid:1858)(cid:1867)(cid:1870)(cid:1865)(cid:1857)(cid:1856)(cid:4667) Subtracting products accounts for exothermic bond formation. Pay attention to number of bonds and moles of each item. Bond h and cl (formed bond energy) Use bond energies to calculate the enthalpy change for h2(g) + f2(g) 2hf(g). dashes in parentheses are bond lines, 544 kj released for every mole of this reaction: ex. Draw lewis structures to see all bonds (esp. if bond types not given) 42 kj released for every mole of this reaction. Sodium must lose an electron (first ionization energy) Chlorine must gain an electron (electron affinity) Sodium is a solid, chlorine is a gas. Sodium must be converted to a gas (not really happening, but you need the energy required to do so to split sodium atoms up from a solid- heat of sublimation)
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