FINAL EXAM REVIEW GUIDE
I.
INTRODUCTION
A.
Chemistry
1.
Know the definition
B.
Scientific Method
n
Understand the steps of scientific method, as well as be able to put
them
in the proper order.
-
Be able to distinguish the independent variable from the dependent variable
-
What is a “control” used for in an experiment ?
C.
Matter
1.
Know the definition
2. Know the 3 phases that matter exists in
D.
Understand and distinguish
between
1.
Physical vs Chemical changes
2. Mixtures : Heterogenous vs. Homogenous
3.
Elements vs.
Compounds
E.
Chemical Symbols
F. Law of Conservation of Mass ---- Understand the law and be able to apply it
II. SCIENTIFIC MEASUREMENT
A.
Quantitative
measurements vs. Qualitative measurements
B. Metric System
1.
Know the standard units
for lenght,
volume, and mass
2. Be able to convert within those units ( ex. Convert centimeters à millimeters )
C.
Density Mass___(g)__
Density = Volume
(cm3) 1 cm3
= 1 ml
Know how to find density of a metal in a lab
D.
Temperature
1. Convert from degrees celcius to Kelvin
2. Convert from Kelvin to
degrees celcius
E.
Significant digits
1. Understand the rules for
determining significant digits
2. Use significant digits in
your calculations when a problem requires you to.
F. Scientific notation - Be able to convert #’s to and from
scientific notation
III. ATOMIC STRUCTURE
A.
Know the definition of an
atom
B. Know and understand the 3 subatomic particles
1.
Proton ( + )
2. Neutron ( no charge )
3. Electron ( - )
C.
Understand atomic
structure ( where the subatomic
particles are located in the atom )
D. Understand and be able to apply the following :
1.
atomic #
2. Mass # ( aka atomic mass )
3. Isotopes
n
know definition as well as be able to find atomic mass from isotopes
4. Ions Define and differentiate cations from anions
E.
Periodic Table
1.
Understand the relationships
elements in the same group have
2. Understand the relationships elements in the same period have
3.
Metals vs.
Nonmetals
IV.
ELECTRONS IN ATOMS
n Be
familiar with some of the earlier models and who developed them
ex. Thomson’s plum pudding model
n Understand
the quantum mechanical model
n atomic
orbitals
s, p, d, f
n sublevels and # of
electrons
s 1
- 2. p
3 -6 .
d
5 - 10. f 7 - 14
n Electron
configurations
n Follow
the Aufbau principle, Pauli
exclusion principle,
and Hund’s rule.
n Both
methods
n boxes, shorthand config including noble gas configs.
V. CHEMICAL
PERIODICITY
n Be
familiar with the history of the periodic table
n understand
the trends
n atomic
size
n ionic
size
n ionization
energy
n electon affinity
n electronegativity
VI. BONDING
n Why
do elements form bonds ?
n Valence
electrons, octet rule
n electron
dot structures
n Ionic
bonds
- When diagramming, use the 3
step approach.
n Covalent
bonds
single,
double , triple
n VSEPR
Theory
know
the basic shapes produced
n Polar
vs. non polar bonds
n Difference
in electronegativities
n Polar
vs. non polar molecules
VII. NAMING IONIC COMPOUNDS &
MOLECULAR
COMPOUNDS
Be
able to derive the formula from the name, and the name from the formula
A.
Ionic Compounds
1.
Binary ( 1 metal (cation) + 1
non metal (anion ) )
n
Criss Cross method
n
anion ends in - ide
2.
Tertiary 3 or more elements--------contains a
polyatomic ion
n
Criss cross method
n
ends in - ate or - ite ( there are a few exceptions )
A.
Molecular compounds
1.
Binary (
2 non metals )
n
Use prefixes, do not criss cross
!!!!!!! These aren’t IONS
n
If 1st non metal only has 1 atom, it doesn’t get a prefix,
all other
elements get a prefix.
n
1st non metal retains the element’s name, 2nd
ends in ide
VIII. CHEMICAL REACTIONS
A.
Writing chemical reactions
B.
Balancing chemical reactions
C.
Be able to identify the type
of reaction
1. direct combination
(synthesis)
2.
decomposition
3.
single
replacement
4. double replacement