express numbers in scientific notation to the appropriate number of
significant figures and with the correct units.
understand the difference between homogeneous and heterogeneous
mixtures and the difference between pure elements and pure compounds, giving examples.
understand the principles underlying methods to separate the
components of mixtures into pure substances; explain the principles of chromatography.
understand the difference between chemical and physical reactions.
understand early concepts in the development of
chemistry and how the ideas of specific people influenced the development of our concept of matter:
La Voisier Law of mass
conservation
Law of Constant Composition
Dalton - Law of Multiple Proportions; Atomic Theory
Law of Combining Volumes of Gases
Avogadro - Molecules; Avogadro's Hypothesis
Thompson - discovery of the electron; Plum Pudding model of the
atom
Millikan - oil drop experiment
Rutherford - nuclear model of the atom
explain in words and through geometric symbols for atoms/molecules
(a nanoscopic representation) how Dalton's Atomic Theory and Avogadro's Hypothesis can explain the Laws of Mass
Conservation, Constant Composition, Multiple Proportions, and Combining Volumes
(macroscopic observations)
describe the differences between laws and theories.
identify in an experiment the independent and
dependent variables, and those held fixed.
give an example of a scientific theory which must be
falsifiable, and a non-scientific theory, one that is not.
explain the difference between atoms, molecules, ions, and molecular
(polyatomic) ions. Give examples of each.
name ionic compounds and simple binary compounds of nonmetals.
describe how magnetic and electric fields affects the movement of
charged particles.
describe the atomic and molecular mass scales.
define isotopes and allotropes and give examples
use dimensional analysis to
convert between moles, molar mass, and number of particles.
explain periodic law embodied in the empirical arrangement of elements
in the periodic table
describe how the arrangement of electrons into shells explains the
organization of the periodic table
explain a graph showing ionization energies of the
element as a function of atomic number is consistent with a shell-like
structure for the arrangement of electrons around nuclei
describe the differences between ionic, polar covalent, and nonpolar
covalent bonds
Identify ionic, polar covalent, and nonpolar covalent bonds in
chemical structures
describe the meaning of electronegativity
write molecular and condensed formulas for molecules
draw Lewis structures for molecules and molecular ions
determine formal charge and partial charges in any
Lewis structure
know the formula and Lewis structures of common molecular ions
draw a mechanism with Lewis structures using curved
arrows to show electron flow in the forming and breaking of bonds in the
formation of products
write formulas for salts containing molecular ions
determine the formal charge on any atom/ion
explain how molecular ions often arise from the
reaction of water with oxyacids
describe atoms, molecules and their properties using
macroscopic, nanoscopic, symbolic, and mathematical representations
understand the relationships among mole, molecular or
atomic mass, and molar mass
write, balance, and interpret simple chemical equations,
define molarity, understand the relationships among moles, volume,
mass, and molarity,.
calculate:
average atomic weight of an element given abundancy of isotopes
% composition of a given element in a compound
number of particles, moles, or mass, given two of the three
quantities
empirical formula of a compound
molecular formula given the empirical formula and molecular weight
values of molarity, volume, mass given any two.
stoichiometric relations (moles, grams, or molarity)
under a variety of conditions including excess/limiting reagents and in
solution.
Note: Questions based on the lab might be expected.