January 30: Ch.2.7 reviewed.
Click here for 32 practice
items
. Ch.3.1: Chemical Equations; balancing of equations. Read
text on margins of page 69 in BLB - very important! Ch.3.2: Types of chemical reactions, eg.: combustion in
oxygen (fancy phrase for burning), combination and decomposition reactions,
double replacement reactions, etc... Look up in BLB
examples of each type. Ch.3.3: Atomic and Molecular Weights:
recall how average atomic masses were calculated from isotopic masses (our
January 25 lecture, or read it on pages 74-76 in BLB). Ch.3.4 The mole: definition of a
mole, the Avogadro's number, NA; calculating of molar mass and
using molar mass to convert between moles and grams of substances, and moles
and numbers of "building blocks" Solve all the sample exercises and
practice problems from Ch.3.1-4, and the recommended questions from
BLB
.
January 28: Ch. 3.5: Empirical Formulas
from Analyses; Ch. 2.7: Naming Inorganic Compounds:
MEMORIZE
ACIDS, both their FORMULAS and NAMES
FIGURE OUT
the FORMULAS, CHARGES and NAMES of the anions which result from the ionization
of acids.
For each H atom in a formula of an acid, there will be
one negative charge in its anion, eg: HCl (hydrochloric acid) has
1 H atom, Cl- (chloride) has a -1
charge, H2SO4 (sulfur
ic acid) has 2 H atoms, SO42- (sulf
ate) has a -2 charge, H3PO3 (phosphor
ous acid) has 3 H atoms, PO33- (phosph
ite) has a -3 charge, etc... Cations: Associate the charge
of a simple monoatomic metal cation with its placement in the periodic table
. eg: sodium, Na, is in the FIRST main group, it forms a +1 cation, etc... Combine your knowledge of the
names, formulas and charges of anions and cations to name ionic inorganic
compounds. January 25: Ch.2 started: Read through and
understand the three laws: conservation of mass, constant proportions and
multiple proportions; Ch. 2.2-2.3: Atomic Structure: Sub-atomic particles (protons, neutrons and electrons)
and their charges and masses (amu); Mass Number, A and Atomic Number, Z;
know the difference and information each carries;Isotopes; Ch. 3.3: Calculation of average
atomic masses from abundances and isotopic masses; Ch. 2.4: The Periodic Table: there are trends in properties
of atoms (both chemical and physical) and a deep meaning behind the placement
of an element in the periodic table. Figs. 2.13, 2.18. Learn how to draw information
about elements from their location in the periodic table; Ch. 2.5-2.6: Empirical vs Molecular formula - started
. January 23: Introduction; Hand-outs: course syllabus and write-up on cross proportions; Use any method of solving problemsthat works for
you. Possibly give the cross-proportions a
chance! Significant figures for additions and subtractions as
well as multiplications and divisions. Note, there are differences in approach.
Need a check for (in)sanity? Check this web site:
http://www.essbasetools.com/instest.htm
. My ex-students from the GWN (great white north) sent this one to me.
