My chemistry education in high school had large, gushing, bullet hole gaps. Here's what I've learned in four days at college (well, what I've taught myself, since the professor assumes that we know it already and just need refreshing). I could take Jesuit's 1st-semester finals now.
Monday: Ch. 2
- The electron's charge-to-mass ratio: e/m = 1.758820 x 108 c/g (coulumbs/gram)
- Mass ratios & Law of Multiple Proportions
- Atomic mass and natural abundance of isotopes
- Atomic weight. 1 atomic mass unit = 1.660539 x 10-24 g
[Naturally occurring carbon, for example, is a mixture of two isotopes, 12C (98.89%) and 13C (1.11 %). Individual carbon atoms therefore have a mass of either 12.000 or 13.03354 amu. But the average mass of the different isotopes of carbon is 12.011 amu.]
- The difference between covalent and ionic bonds
- homogeneous vs. heterogeneous
- Table sugar is named β-D-fructofuranosyl-α-D-glucopyranoside (We didn't need to know that)
- Metals form cations, nonmetals form anions.
- The metals that can form more than one kind of cations
- How to name binary molecular compounds, compounds with polyatomic ions, oxoacids and their oxoions
Tuesday: Statistics
General Introduction to Statistical Analysis of Data, new to most of us, thankfully.
- frequency analysis
- mean, median, mode
- variance
- standard deviation and normal distribution
- percent relative standard deviation a.k.a. confidence interval (chemistry always uses 95%)
- t-test for uncertainty/condfidence level
- formula for estimating how many data points are needed to obtain lower uncertainty
- Null hypothesis theory, determining if data differences are statistically significant or due to randomness
Wednesday: Ch.3
- Balancing Chemical Equations
- stoichiometry
- yields of chemical reactions
- reactions with limiting amounts of reactants
- molarity. M = solute (mol) / solution (L), stoichiometry with solutions, titration
- percent composition of each element in a compound
- molecular formula, molecular mass; formula unit, formula mass; mole, molar mass; empirical formula, empirical formula mass; mass ratio for molecules
Thursday: Ch.4, Reactions in Aqueous Solution
- precipitation reactions, oxidation-reduction reactions
- electrolytes in aqueous solution
- aqueous reactions and net ionic equations
- solubility rules
- identifying, balancing redox using oxidation-number method or the half-reaction method
- redox titration
2 comments:
Huh? I'd be totally, I mean totally lost. Glad I didn't have to take all that in college. I went the Humanities route & happy for it. G.
Yeah, it's not for everyone. It's not for Sammi. She's in Greek intro right now. Too bad Jeff transfered to Michigan, because he would have tutored me without asking.
Post a Comment