Name:
Period:
Chemistry Semester 1 Final Review 2015
Unit 1: Nature of Science and Lab Safety
1. Define chemistry.
2. Define and give an example of an observation and an inference.
3. Identify the dependent and independent variables in the following hypothesis:
“If I share a hat with Alfred, I will get head lice.”
4. Define hypothesis, theory and law. How are each unique?
Unit 2: Measurement
5. Define mass, volume, and density.
6. What is the formula to calculate density?
7. Complete the following table about the SI system.
SI Unit
SI Symbol
Tool(s) to Measure
Time
Volume
Amount of Substance
N/A
Distance
Temperature
Mass
8. Define precision and accuracy. How do the two concepts differ?
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Name:
Period:
9. Define and give an example of a qualitative observation and a quantitative
observation.
10. How can you determine the number of significant figures in a number? Give
examples.
11. Complete the following table about calculations.
Explanation
Example
Addition/Subtraction
with Sig Figs
Multiplication/Division
with Sig Figs
Addition/Subtraction
with Scientific
Notation
Multiplication with
Scientific Notation
Division with Scientific
Notation
12. How do unit conversions within the metric system work? Give examples.
13. How are mass and weight different?
Unit 3: Matter and Classification
14. Complete the following table about types of properties.
Definition
Physical
Properties
Chemical
Properties
15. Complete the following table about types of changes.
Definition
Physical
Change
Chemical
Change
Examples
Evidence
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16. Complete the following table about types of matter.
Definition
Period:
Example
Pure Substance
Mixture
Element
Compound
Heterogenous
Homogenous
17. Make a flow chart to relate matter, pure substances, mixtures, compounds,
elements, heterogeneous mixtures, and homogeneous mixtures.
Unit 4: Nomenclature
18. Summarize the rules for naming ionic compounds.
19. Summarize the rules for naming covalent compounds.
20. Complete the following table about compounds names and formulas.
Formula
Name
Formula
Name
Zinc chloride
AgBr
Carbon tetrahydride
C2H4
Na3PO4
Magnesium sulfide
CoF2
Barium nitrite
Ca3P2
NH4Cl
Triphosphorus pentachloride
SiBr6
Iron II sulfate
NO2
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Unit 5: Atomic Structure and Nuclear Change
21. How did the model of the atom progress through time?
Period:
22. Complete the following table about the subatomic particles.
Subatomic Particle
Charge
23. Complete the following table using a Periodic Table.
Isotopic
Atomic Atomic
Mass
Notation
Number
Mass
Number
Location
#p
#n
#e
Tungsten
Tin
24. Define radiation and explain why an atom will go through radiation.
25. Complete the following table about radiation.
Greek
Emitted
Stopped by
Symbol
Effect on
mass #
Effect on
atomic #
Alpha
Beta
Gamma
26. Define half-life and draw a graph to represent the concept of half-life.
27. Define fission and fusion. Compare and contrast the two concepts.
Unit 6: Electron Configuration
28. Draw the Bohr model for Be, N, Na, S, and Ar.
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29. Draw the Lewis structure for He, B, P, K, Se, C, I, and Ar.
Period:
30. State the three rules of electron configuration (Aufbau’s Principle, Pauli Exclusion
Principle, and Hund’s Rule).
31. Use the box and arrow method to do electron configurations for Li, N, and V.
32. Write out the electron configuration for Ne, Mg, and Fe.
33. Give the valence electron configuration for Ca, Br, Bi, and Sn.
Unit 7: Periodicity
34. Describe where each family is found on the periodic table:
 Alkali Metals
 Metals
 Alkaline Earth Metals
 Nobel Gasses
 Halogens
 Nonmetals
 Metalliods
 Transition Metals
35. Complete the following table about trends in the Periodic Table.
Definition
Group Trend
Period Trend
Atomic Size
Electronegativity
Ion Size
Ionization Energy
Metallic Properties
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