Midterm 1 Review


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KNOW EVERYTHING ON THIS LIST, DO YOUR PROBLEM SETS, AND YOU SHOULD BE A-OK FOR THE EXAM! DON’T MAKE THE BIG MISTAKE OF GOING INTO DETAILS IN AREAS WHERE YOU DON’T NEED TO (esp with respiration) 1. Atoms and Molarity -know atomic mass, atomic number, how they are symbolized The mass number of an element is written as the upper number, the atomic number is the bottom number - mass number = protons + neutrons - atomic number = # of protons - mass number – atomic number = # of neutrons - # of protons = # of neutrons **Know which ones can we change and still have the same element: neutrons -cation/anion/isotope -how to calculate neutrons -given an atom, figure out how many unpaired valence electrons the atom has and how many bonds it can form, also how which atom is this given atom similar to? (ie: how many unpaired valence electrons does oxygen have? Draw your shells! This is in case it’s an atom that you don’t know the valence electrons of.) -Make sure you fill in your S orbitals first, then the P orbitals. - remember the charges on cations, like Mg, Na, and how many anions they'll need to form a molecule with a net charge of 0 -know how to calculate molarity, a typical question:"given a substance with an atomic mass of X daltons(same as grams), how many grams of that substance do you need to put into a 1 liter solution to make a 1 molar solution" -Energy levels of Electron **Every atom has electron shells, the first energy shell has the lowest energy and they go up as u go out -energy needs to be absorbed by the atom in order for electron to travel out -energy needs to be released by the atom for electrons to fall towards the nucleus ** electrons can only fall in discrete steps **electrons that are further away from the nucleus have higher potential energy 2. Bonds - Covalent bonds involve sharing a pair of valence -The number of valence electrons determines how many covalent bonds are formed - Single and double covalent bonds
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This note was uploaded on 07/14/2009 for the course BILD BILD1 taught by Professor Bever during the Spring '08 term at UCSD.

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