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Unit 2 Review - 2016
Topics Covered:
% mass (MOE/MOC x 100)
Alloy
Atoms
Atomic mass
Average atomic mass
Atomic number
Basic mixture
Chemical property
Chemical reaction
Colloid
Compound
Distillation
Element
Electrons
Gas
Heterogeneous mixture
Homogeneous Mixture
Isotopes
Isotopic symbols
Law of conservation of mass
Law of definite proportions
Liquid
Mass number
Mass
Mass #
Matter
Mixture
Neutrons
Protons
Physical change
Physical property
Product
Reactant
Solid
Solution
Substance
Suspension
Tyndall effect
Examples:
Atomic #
9
Mass #
# protons
14
47
55
# neutrons
10
15
25
# electrons
Symbol
25
Fill in the table:
Particle
Proton
Neutron
Electron
Charge
Mass
FROM HERE ON, SHOW ALL WORK ON A SEPARATE SHEET OF PAPER!!!!!!!!!!
1. Calculate the approximate atomic mass for lead using the following info ( note: 1 p + = 1.007276 amu, and
1 n0 = 1.008664 amu)
82 p
122 n
1.37%
82 p
124 n
26.26%
82 p
125 n
20.82%
82 p
126 n
51.55%
2. Which subatomic particle identifies an atom as that of a particular element?
3. Copper has two isotopes Cu-63 (abundance = 69.2%, mass = 62.930 amu) and Cu-65 (abundance =
30.8%, mass = 64.928 amu). Calculate the atomic mass – SHOW WORK!!
4. Show the isotopic symbols for each isotope mentioned in the question above.
5. Why is an element electrically neutral?
6. How can there be 1000 different atoms when there are only about 100 different elements?
7. What is the difference between the mass number and the atomic number of an atom?
8. Identify the following matter as substances or mixtures. Then identify each as an element, compound,
homogeneous, or heterogeneous mixture. Then JUSTIFY your answer.
A
B
C
D
9. What state of matter do each of the following diagrams represent? JUSTIFY your answer.
A
B
C
10. Explain the law of conservation of mass.
11. In the complete reaction of 22.99 g of sodium with 35.45 g of chlorine, what mass of sodium chloride is
formed? SHOW ALL WORK
12. A 12.2 g sample of X reacts with a sample of Y to form 78.9 g XY. What is the mass of Y that reacted?
SHOW ALL WORK
13. Describe the structure of a typical atom. Identify where each subatomic particle is located.
14. Describe the separation technique that could be used to separate the following mixtures.
a. Two colorless liquids with different polarities/attractive forces for mobile phase of a liquid.
b. Salt dissolved in water
c. Two substances that form a heterogeneous suspension with a solid.
15. Classify each of the following as a chemical or physical property
a. Iron and oxygen form rust
b. Iron is more dense than aluminum
c. Magnesium burns brightly when ignited
d. Oil and water do not mix
e. Mercury melts at -39 degrees Celsius
16. Classify each example as a physical or a chemical change
a. Crushing an aluminum can
b. Aluminum combining with oxygen to form aluminum oxide
c. Leaves changing color
d. Sugar dissolving in water
e. Baking a cake
17. 8.35 x 10-6 mg = ______________________ kg (show all work using dimensional analysis).
18. How many ks are in 3,500 years? (show all work using dimensional analysis).
19. What type of mixture is a metal alloy? Justify your answer, then draw a diagram of what a metal alloy
might look like at the atomic level. Be sure to label the parts.