| Syllabus / Schedule | 
|
| Chem 109 |
|
Summer 2002 |
| Lecture Notes:: 6 June |
|
|
| PREVIOUS |
Note that formulae are more or less written with the elements ordered by charge (+ then -) and/or electronegativity (elements on the right side of the Periodic chart generally precede those on the left).
You should also know about the Stock system of nomenclature for cations and ionic compounds.
Note also the -ic -ous system. You only need a "reading" knowledge of this system for common elements such as iron, copper, lead, mercury, and tin.
Atoms are now known to consist of three different types of particles: electrons, protons and neutrons (the common form of one very important atom, hydrogen, has only two kinds: a proton and an electron). The protons and neutrons reside in a small inner portion called the nucleus while the electrons reside in a relatively large cloud centered on the nucleus. Important properties of these particles are listed in the table below:
|
Some important terms which you must know are:
Isotopes are forms of elements which differ only in the number of neutrons. This means different isotopes of the same element have essentially the same chemical properties but slightly different physical properties. They can also differ substantially in terms of their nuclear stability. Let's look at some examples of isotopes:
|
You should be able to fill in the blanks in a table like this with, the aid of a periodic table, on a quiz.
Determination of Atomic Mass: We want to be able to figure out the atomic mass of a sample with a particular isotopic composition.
Example: Cu occurs as an isotopic mixture of 69.09% 63Cu (mass = 62.93 amu) and 30.91% 65Cu (64.93 amu). What is the atomic mass of copper in this sample?
Assume the sample consists of 1 atom for convenience, then (0.6909 atoms)(62.93 amu/atom) + (0.3091 atoms)(64.93 amu/atoms) = 43.478 amu + 20.070 amu = 63.558 amu for 1 atom = 63. 558 amu/atom How about sig figs? 1 is a count, therefore exact. The two multiplications each have 4 sig figs so the calculations each have 4 sig figs (note I keep one extra, that is 5 sig figs, in the calculations to avoid rounding errors.) . For the addition we use the add/subt. rule and look at decimal place, for our four sig figs the hundredth's place is then the sig fig (again, during calculation its best to keep one extra sig fig to avoid rounding errors). The final answer then has 4 sig figs:
An example of the reverse problem can be found on the Final, number II.3.
Stoichiometry is the quantitative study of the composition of compounds (e.g. determining the ratios of atoms in a molecule) and/or the ratios of substances in chemical equations.
This is the SI unit of amount of substance. 1 mole = the number of carbon atoms in 12 g of 12C. This number, called Avogadro's Number, has been measured as 6.022 x 1023 mol-1 (current value: 6.022 141 99 x 1023mol-1). Notice that this number can refer to anything (a mole of eagles, a mole of pennies, etc.). In each case we are talking about 6.022 x 1023 items or entities.
For chemists a mole has two common uses:
Note that Avogadro's number, 6.022 x 1023 is thus the conversion factor from amu's to grams!
Atomic Mass:
Notice that atomic masses have two meanings:
Examples:
- What is the mass of 27 atoms of oxygen
- in amu's? (432.0 amu)
- in grams? (7.174 x 10-22g)
- Given 3.45 grams of copper
- how many moles of copper is this? (0.0543 mole)
- how many atoms of copper are there in this sample? (3.27 x 1022)
- A 2.34 mole sample of sulfur contains
- how many grams of sulfur? (75.0 g)
- how many atoms of sulfur? (1.41 x 1024)
| Syllabus / Schedule |
|
© R A Paselk
Last modified 6 June 2002
