Honors Chem IA
Review for Unit 1 Exam
1.
What does Dalton’s Atomic Theory state? Be able to describe this theory.
2.
Define the Law of Conservation of Mass / Energy and explain how this law can predict quantities of
products in a chemical reaction.
3.
How does a hypothesis differ from a theory and a law? What two characteristics must be true of a
hypothesis?
4.
Be able to utilize the “classification of matter” flowchart. Differentiate between “pure matter” and
mixtures. Provide two examples of each: “pure compound” and “pure element”
5.
What is the difference between hetero- and homogeneous mixtures? Give two examples of each.
6.
How do you read the calibrations on instruments in lab? Think about the number of SigFigs.
7.
How many SigFigs are in the following?
a. 90909
d. 0.0009
b. 90009
e. 9.0000
c. 90000
f. 0.0909
g. 6.09x1023
h. 0.99000
i. 10000
j. 1000.
k. 100001.00
l. 0.000123
8.
Calculate the following and report your answer in the correct number of SigFigs (put into scientific
notation where appropriate)
a. 6.767 + 4.1
e. convert 49.0℃ to ℉
i. convert 44.52℉ to K
b. 555.5 – 6.004
f. convert 289K to ℃
j. convert 35.67 cm to m
c. 7.1 x 23.65
g. convert 32.5℉ to ℉
k. convert 700.0 kL to mL
d. 10.4 / 22.34
h. convert 332 K to ℉
l. convert 1000 cg to kg
9.
Convert the following using the Factor Label Method (dimensional analysis) – SHOW ALL WORK
a.
55.4kg to lbs
b.
3009.99 cm to inches
c.
How many meters are in a football field?
10. What is the difference between “extensive” and “intensive” properties? Provide an example of each.
11. Compare and contrast “accuracy” vs. “precision.” Give three data measurements that are accurate and not
precise, three data measurements that are precise and not accurate, and three that are both.
12. Scientific Notation: convert to scientific notation or expand out of scientific notation (watch SigFigs!)
a. 1.005x105
c. 9,700,000
e. 0.0000896
g. 9x10-5
-3
b. 4.12x10
d. 500,982
f. 0.004
h. 9x105
13. What is the difference between chemical and physical properties? How can these be used to separate
mixtures? Provide and define six different types of separation techniques that we discussed.
14. How are physical changes and chemical changes different? Provide two examples of each.
15. What is an element? How is this different from a compound or molecule?
16. Discuss the interactions between particles on the molecular scare within solids, liquids, and gases. How are
they different when considering kinetic and potential energy? Which phase has the highest kinetic energy?
Draw a picture of each of the three phases illustrating the molecular interactions and speed.
17. What is the difference between crystalline and amorphous solids? Discuss the arrangement and
organization of the molecules.
18. Perform the following calculations:
a. An object displaces 22.8 mL of water when placed into a graduated cylinder. Its mass was
previously determined to be 440.04 g. What is its density? Using this value, identify it.
b.
A sample of aluminum has a mass of 34.5 grams. What volume will it occupy?
19. What happens to the molecular speed as you increase the temperature? What, then, does this do to the
volume?
20. What is density? Using what you just determined in question #17:
a. What can you say about the density of a substance as you increase or decrease its temperature?
How? Why?
b. Explain or draw what is happening on the molecular scale. Maybe think about water (solid, liquid,
gas) as an example to simply your explanations.
c. Why is knowing the temperature important when performing analytical analyses – trying to
determine the identity of a substance?