CHEM 6A Lecture 7: CHEM W3 Lec 10/16/17
33 views2 pages
3 Jun 2018
School
Department
Course
Professor
Representation of Compounds
Type
Chemical formula
Name
Structural Drawing
ionic
NaCl
Sodium choride
Ch 15 (68)
FeCl3
Iron (III) chloride
molecular
H2O
water
Lewis structures (ch
7-9)
N2O5
(as molecules)
Dinitrogen
pentaoxide
Or
Dinitrogen pentoxide
Pre-Chapter 3: The Mole
● The amount of a substance that contains as many particles (e.g. atoms, molecules) as
there are 12C atom in exactly 12 grams of 12C
● Avogadro’s number:
NA = 6.022 * 1023/mol
● 1 mol of molecules = 6.022 * 1023 molecules
● 1 mol of eggs = 6.022 * 1023 eggs
E.g. Consider 2.06 mol of H2O
a. How many molecules are there?
2.06 mol * 6.022*1023 = 1.24 * 1024 molecules
mol
b. How many # atoms are there?
1.24 * 1024 molecules * 2 H atoms = 2.48 * 1024 H atoms
1 H2O molecule
c. How many grams of H are there?
2.48 * 1024 H atoms * 1.008 amu * 1.661 * 10-22kg * 1000g = 4.15g
H atom amu kg
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Document Summary
The amount of a substance that contains as many particles (e. g. atoms, molecules) as there are 12c atom in exactly 12 grams of 12c. 1 mol of molecules = 6. 022 * 1023 molecules. 1 mol of eggs = 6. 022 * 1023 eggs. 1. 24 * 1024 molecules * 2 h atoms. 2. 48 * 1024 h atoms * 1. 008 amu * 1. 661 * 10-22kg * 1000g = 4. 15g. Mass in grams of 1 mole of particles (g/mol) For elements, mm (in g/mol) = atomic mass (in amu) For compounds, mm (in g/mol) = formula mass (in amu) H2o 2 mol of h atoms, 1 mol of o atom (1 mol) 2. 06 mol h2o * 2 mol h * 1. 008g h = 4. 15g. A chemical formula shows the elements present in a compound and their relative proportions. An empirical formula shows the simplest whole number ratio of atoms. A molecular formula shows the actual number of atoms in one molecule.
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