Define:
Molecule, Elements, Compounds, Empirical Formula, Molecular formula, intensive and extensive properties,
atomic number, mass number, atomic symbol, accuracy, precision, significant figure, ion, cation, anion,
isotope, separations techniques, distillations, evaporations, filtration, decantation, chemical reaction, scientific
method, hypothesis, Dalton’s Atomic Theory, Gold Foil Experiment, solid-sphere model, planetary model,
quantum-mechanic model.
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
11.
12.
13.
14.
What does Dalton’s Atomic Theory State?
What is the Law of Conservation of Mass / Energy? How can this be used to help predict quantities of
products in a chemical reaction / change?
What is a “pure substance” – provide two examples of “pure elemental” and two of “pure compound”.
Compare and contrast “heterogeneous mixture” and “homogeneous mixture.” Provide three examples of
each.
Define and thoroughly compare solids, liquids, and gases. Be sure to discuss the amount of average kinetic
energy (molecular motion) of each. You may want to draw a picture to illustrate the molecules positions in
relation to one another (spaces between molecules and compressibility)
What is the scientific method? What are the five main steps we discussed? What is a hypothesis? Why is
“observations” not a necessarily a step? What are observations? What is the difference between a “law”
and a “theory”?
What is a chemical change? What is a physical change? Provide three examples of each.
What is the difference between a chemical and physical property? Provide three examples of each.
Name one chemical property of hydrogen gas, H2(g).
Compare and contrast extensive and intensive properties
Math and SigFigs
a. Scientific Notation
i. 898,990,000
iii. 842,399
iv. 0.0000345
vii. 0.00000009884
ii. 5.5323x104
iv. 3.43x10-2 vi. 9.9x10-6
viii. 3.2345x107
b. SigFigs and calculations
i. How many SigFigs are in the following:
1. 0.0090990
D. 1.0950009
2. 123.33
E. 0.098012
3. 9.91452x1023
F. 738.000
ii. Round each of the previous values to 3 SigFigs:
iii. Perform the following calculations expressing your answers in the correct number of
SigFigs:
1. 7.87 x 8.8 =
C. 100.9 – 0.293 =
2. 5.55 + 18.8 =
D. 9008.9 / 55.0 =
What is the difference between accuracy and precision? Draw a picture to explain.
What is accuracy? What is precision? Which is more important? Can you be both accurate and precise?
(You may want to draw pictures to supplement your understandings).
a. If the actual value is 9.70g and you measure three trials: 9.24g, 9.21g, and 9.22g. is your data
accurate, precise or both?
b. Actual is 5.22mL and you measure 5.21mL, 4.90mL, and 5.88mL. Accurate, precise, or both?
How do you read measurements (like a ruler, grad cylinder, triple beam, etc.) to the correct number of
SigFigs?
15. What is Density? What is the relationship between mass, volume, and density?
a. Calculate the density of a sample with a mass of 15.7g and a volume of 12.2mL
b. What volume will 10.09 grams of aluminum take up? (you will need to use your books to find the
density)
16. Temperature conversions:
a. 593C to K
c. 201F to C
e. 55.4F to C
g. 82.99C to K
b. 55.55F to K
d. 100.1F to K
f. 273.15K to C
h. 385K to F
17. Read the following measurements:
Length: _________________
Mass: _________________
Volume: ________ & ________
18. Nomenclature!!! Be VERY GOOD at naming compounds and molecules
Name / Formula
Molar Mass (g/mol)
Compound or
Molecule?
Na2O
N3O7
NO3
magnesium nitrite
aluminum phosphide
Cobalt(II)hydroxide
dinitrogen trioxide
19. How do you calculate protons, neutrons, and electrons? How about in ions? Isotopes? There are about 10
questions pertaining to this information!!!
20. Metric conversions: Be able to convert between all prefixes in the SI system. (Kilo-, hecta-, etc.)
21. Where are the alkali metals located? Alkaline earth metals? Transition metals? Metalloids? Halogens?
Noble gases?
22. What are the charges AND number of valence electrons for each of the groups?
23. (3 calc questions) Calculate average atomic masses of atoms when give the percent abundance and the
masses of the abundances. What instrument is used to make these calculations? Why are the peaks not at
the decimal values from the table?
24. What is the law of definite proportions? What does it state?
25. What is the law of multiple proportions? What does this state? Compare to the law of definite proportions.
26. Where are the metals located on the periodic table? Where are the nonmetals located?
27. Give several properties of METALS, METALLOIDS, and NONMETALS.
28. How would you separate a salt, water, sand, iron mixture? Explain this process step by step.
29. Balance a chemical reaction (basic, basic) just illustrate the law of conservation of mass. What you put in,
you better get out!!