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exam 2 study guide - Ch. 4-Types of reactions: combination...

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Ch. 4-Types of reactions: combination (x + y = z), decomposition (z = x+y), single replacement aka displacement (x + yz = xz + y) metals should not have negative oxidation numbers oxidizing agent- losses electrons reducing agent-gains electrons Ch. 7-Wavelength=distance per second s orbital holds up to 2 electrons and atomic orbital size is 1. ..p orbital holds up to 6 electrons and atomic orbital size is 3…d orbital holds up to 10 electrons and atomic orbital size is 5…f orbital holds up to 14 electrons and atomic orbital size is 7 number of orbitals = number of m values = 2l + 1 Ch. 8- Hund’s Rule - When orbitials of equal energy are available, the electron configuration of the lowest energy has the maximum number of unpaired electrons with parallel spins = you can move 1 electron to make a whole set half full but you can not put an electron back in the s orbit paramagnetic-series with unpaired electrons diamagnetic series-all paired ionization energy- energy it takes to remove an electron from an element group 2A: diamagnetic; group 3A: paramagnetic, group 1A: paramagnetic, group 8A: diamagnetic Ch.9- the greater the oxidation number, the smaller the element is lattice energy-the enthalpy change that accompanies he separation of 1 mol of ionic solid into gaseous ions (ΔH° lattice
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This note was uploaded on 04/21/2008 for the course CHEM 1035 taught by Professor Jgdillard during the Fall '07 term at Virginia Tech.

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exam 2 study guide - Ch. 4-Types of reactions: combination...

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