Fall Final Review
Topics Covered:
Scientific Method
Matter
Measurement
Lab Safety / Equipment
Atomic Theory
Atomic Structure
Periodic Table / Periodic Properties
Electrons
Ionic Bonding
Naming Compounds (nomenclature)
Scientific Method:
Define:
Theory:
Law:
Independent/manipulated Variable:
Control
Dependant / responding Variable:
What are the steps of the scientific method?
Matter and Measurement
Define
Matter:
Mixture:
Homogeneous:
Heterogeneous:
Compound:
Chemical Property:
Chemical Change:
Physical Property:
Physical Change:
Distillation:
Condensation:
Evaporation:
List the states of matter and the characteristics of each state.
Sublimation:
What is the difference between a substance and a mixture?
1.Which of these are composed of two or more different substances that are chemically combined
in a definite ratio?
A Compounds
B Mixtures
C Element
D Solutions
2.What is the mass of a 500.00 mL sample of seawater with a density of 1.025 g/mL?
3.This pipette is filled with a 20% NaOH solution. The solution has a
density of 1.23 g/mL. According to this information, what is the mass
of this NaOH?
solution?
4.What is the density of a block of wood with a mass of 350g and a
volume of 185cm3?
5. Which of the following will allow measurement of a liquid’s volume with the greatest precision?
A 50 mL cylinder graduated in 1 mL increments
B 100 mL
cylinder graduated in 0.5 mL increments
C 100 mL cylinder graduated in 1 mL increments
D 200 mL cylinder graduated in 5 mL increments
6.What volume should be reported for the solution in this graduated
cylinder?
How many significant figures in the measurement?
Which one is the estimated digit?
Write the measurement in scientific notation.
PRECISION AND ACCURACY
Accuracy:
Precision:
1) For which compound are the measurements accurate but not precise?
2) For which compound are the measurements precise but not accurate?
3) For which compound are the measurements both accurate and precise?
4) For which compound are the measurements neither precise nor accurate
1. Convert each of the following into scientific notation.
172000
__________ 0.000984
into decimal form.
___________200.0 x 102
__________ 2. Convert each
1.56 x 104 ______________ 3.6 x 10-2 _______________
736.9 x 105 _____________ 0.0059 x 105 ____________ 3. Calculate the following. Give the
answer in correct scientific notation.
a) 2.34 x 1065
b) 313.0
+ 9.2 x 1066
- 1.2 x 103
4. Calculate the following. Give the answer in correct scientific notation.
a) 8.95 x 1076/ 1.25 x 1056
b) (4.5 x 1029)(2.45 x 10100)
5. Give the number of significant figures in each of the following.
a) 1.05 g ______ b) 0.0003040 mm ______
6. Round each of the following to 3 significant figures.
77.0653 _________ 6,300,178.2 ______________ 0.00023350 _________
Metric Conversion Practice
4 m = _____mm
49 cm = _____m
16 kg = _____g
97 cm = _____mm
437 mg = _____g
25 l = _____ml
Atomic Theory:
Describe the contribution/models of the following scientists:
Dalton
Bohr
Rutherford
Thomson
Heisenberg
Atomic Structure:
Define:
Proton
neutron nucleus electron atom
mass number atomic mass unit
atomic number atomic mass
isotope
label the following structure:
Identify the elements represented below:
_____________ _____________ _______________ ____________________
Periodic Table / Periodic Properties:
Define:
Period
Group
Metal
Non-metal
Metalloid
Halogen
Noble gas
transition metals
representative elements
Group A
Group B
The modern periodic table is arranged in order of increasing ______________
Electrons:
What are valence electrons? Why are they important?
What is the octet rule? What does it have to do with the noble gases?
What happens to the amount of energy in an electron as it moves closer to the nucleus?
Period
Principle
energy
levels
Energy
sublevels
orbitals
1
2
3
4
How many electrons can each orbital hold?
S = ____max
p = ____max
d = _____max f = ______max
Write the electron configuration for the following elements: Fluorine, Silver, Ba, and Uranium.
Draw the orbital diagrams for the following elements: Silicon, Calcium, Radon and Plutonium.