Unit 2: Matter & Change
Possible Pts.
Name:___________________________
Practice
Test A
Hr:_________
Score
Possible Pts.
Objective 1
40
Objective 4
45
Objective 2
40
Objective 5
40
Objective 3
40
Score
Total
Objective 1: Read and express information given in Chemical Formulas. (5pts per box)
Formula
Name & Number of molecules
Number of each type of atom
(NH4)2Cl
Ammonium Chloride
5 P2S3
Phosphorus Sulfide
4 LiNO3
Lithium Nitrate
3 W2(SO3)3
Tungsten nitride
Objective 2: Distinguish between chemical and physical changes, as well as chemical
and physical properties. (4pts each)
Explain why it’s a Chemical or Physical Property?
Tape is sticky=
Paper will turn brown if left in sun=
Magnesium is silver and shiney=
Copper turns green if left outside=
Explain Why it’s a Chemical or Physical Change?
Hair gets cut=
Light bulb burns out, turns black inside=
Toasting bread nice and brown=
Melting butter on toast=
Use the following statement to distinguish between chemical and physical properties.
Explain your reasoning with complete sentences and thoughts: (8pts)
Sulfur is a yellow, brittle powder that smells like rotten eggs. When it is heated with grey magnetic iron, it produces iron
sulfide, which is black and no longer magnetic.
Objective 3: Classify Matter as a pure substance or mixture. (10 pts each)
Directions: Classify each type of matter as an element, compound, homogeneous mixture, or
heterogeneous mixture. Explain why.
1. Sodium Chloride (NaCl): ______________________
 Why:
2. Salt Water: ______________________
 Why:
3. Muddy Water: ______________________
 Why:
4. Titanium (Ti) : ______________________
 Why:
Objective 4: Balancing Chemical Equations (3 pts/element, 45 total)
Directions: Prove the law of conservation of mass by balancing the following equations
using only coefficients.(3 pts/element, 45 total)
1)
____ K + ____ Cl2  ____ KCl
2)
____ Al + ____ HCl  ____ H2 + ____ AlCl3
3)
____ N2 + ____ F2  ____ NF3
4)
____ SO2 + ____ Li2Se  ____ SSe2 + ____ Li2O
5)
____ Na3PO4 + ____ CaCl2  ____ NaCl + ____ Ca3(PO4)2
Objective 5. Multiple Choice (2 points each) Fill in a correct answer for each question
_____1. How do you calculate % error?.
_____2. In a can of pop, what is the solvent?
_____3. This type of matter can be separated by physical methods.
_____4. In the chemical/physical change lab, what did you produce when blowing CO 2 bubbles into
the water using the straw?
_____5. In the ink separation lab, we proved that markers were in fact which of the following.
_____6. If something is to be classified as a homogeneous mixture, it must have which attribute.
_____7. To be soluble means that something can _____________.
_____8. In the salt water separation lab, we proved that dissolving is ______________.
_____9. When you did the 8 station chemical physical change lab, what evidence was needed to
determine that a chemical change had taken place?
_____10. How do you calculate % yield?.
_____11. In our classroom, which type of matter is most common?
_____12. What does a balanced equation prove about matter?
_____13. A physical property is measured how?
_____14. How is a chemical property determined?
For Questions 15-20, interpret the following equation
Na2CO2(aq) +
2HCl(aq)
−>
2NaCl(s)
+
H2O(l)
+
CO2(g)
_____15. In the above equation, Na2CO2 & HCl are…
_____16. In the above equation, NaCl is a .
_____17. In the above equation, (aq) stand for...
_____18. In the above reaction, you would see...
_____19. In the above equation, how many molecules of NaCl are yielded?
_____20. In the above equation, the number of atoms of reactants is ______________ the number
of atoms of products.