CHM 143 Lecture Notes - Lecture 4: Lead, Atomic Orbital, Roman Numerals
15 Sep 2016
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29cm x cm 1 m x 1m = 29cm x cm 10^-2 x 10^-2= 2. 9x 10^-3m^2. 1cm 1cm: density as a conversion factor: d=m/v can use ration in reciprocal form. 703g/ml=mg/200. ml m= 141g 200. ml x . 703 g m= 141g ml. Start with section 2. 3 before that is background that we won"t be tested on. Law of conservation of mass: matter cannot be created or destroyed during a chemical reaction/process. #atoms each element start = #atoms of each element when reaction done. Law of definite proportions: all samples of a specific type of matter, will have the same proportion of the elements it"s composed of, no matter the source. Ex: h20 = 2 hydrogen & 1 oxygen always. 18g h20 will decompose into its elements and always produce. Based on mass; mass ratio is different than the ratio of the # of atoms. *if not produced then probably not h20. Mass ratio 58. 5g nacl= 23. 0g na & 35. 5g cl.
