Download sch3u unit 1 test: matter

SCH3U UNIT 1 TEST: MATTER
SECTION A: KNOWLEDGE/UNDERSTANDING (27 marks)
11. The IUPAC name for NO2 is
a.nitrite
b.nitrate
c.dinitrogen oxide
d.nitrogen dioxide
Multiple Choice
Answer the following questions by circling the correct response on the answer sheet
provided. (1 mark each)
1. The subatomic particle that has the smallest mass is the
a.electron
b.proton
c. neutron
d.nucleus
12. The IUPAC name for P2I4 is
a.
phosphorus iodide
b.
diphosphorus tetraiodide
c.
tetraphosphorus diiodide
d.
phosphorus pentaiodide
13. Which of the following formulas does NOT represent a molecular compound?
a.
CO(g)
b.
Co(s)
c.
CO2(g) d.
CH4(g)
2. The atomic mass of barium is due to the number of
a. neutrons and electrons in the nucleus
b. electrons in the nucleus
c. protons and neutrons in the nucleus d. protons and electrons in the atom
14. Which of these will experience dipole-dipole interactions?
a. CH4, methane
b. carbon monoxide
c. oxygen gas
d. silver nitrate
15. The name of HBrO3 (s) is
a. bromic acid
b. hydrogen perbromate
d. hydrogen bromate
3. All fluorescent lights, when analyzed in a spectrometer, exhibit the same lines in the
yellow, green, and blue spectral regions. This is evidence that
a. Fluorescent lights contain fluorine gas.
b. There are no gases present in fluorescent lights.
c. The same elements are present in all fluorescent lights.
d. Air is present in all fluorescent lights.
4. Choose the pair of elements that will form a compound with the most ionic character
a. Li & O b. C & O c. F & F d. Cl & Br
5. In the alkali metals group, as the atomic number increases
a. the electronegativity increases
b. the electronegativity decreases
c. the atomic radius decreases
d. the electron affinity increases
6. In a neutral atom
a. the number of protons is always equal to the number of neutrons
b. the number of neutrons is always equal to the number of electrons
c. the number of protons is always equal to the number of electrons
d. the atomic number is always equal to the number of neutrons
c. bromous acid
16. Which of the following will form a formula unit?
a. C and F
b. C and O
c. K and F
d. K and Na
17. A compound composed of sodium, sulfur, and oxygen would be named
a.
sodium peroxide b.sulfuric acid
c.sodium sulfide
d.sodium sulfate
18. A metallic element X forms a carbonate with the formula X(CO3)2. The corresponding
fluoride compound of element X would have the formula
a.
XF4
b.
XF2
c.
X4F2
d.
X4F
19. The reaction of silver nitrate with zinc would be classified as a
a.
combustion reaction
b.synthesis reaction
c.
double displacement reaction
d.single displacement reaction
20. When baking soda is heated, sodium carbonate, water, and carbon dioxide gas are
formed. This reaction can be classified as
a.synthesis
b.combustion
c.decomposition
d.single displacement
7. Consider the equation X(g) + energy  X+ + e–. The "energy" represents
a.
electron affinity
b.
heat of sublimation
c.
ionization energy
d.
sublimation energy
21. Which of the following always indicates that a chemical reaction has taken place?
a.
production of a gas
b.
absorption of heat
c.
change in colour
d.
appearance of a new substance
8. Electron affinity increases as you go from left to right on the periodic table because
a.
atomic radius decreases
b.
ionization energy decreases
c.
of the periodic law
d.
all of the above
22. Which metal would not displace lead, Pb, in a lead nitrate, Pb(NO3)2, solution?
a. copper, Cu
b. potassium, K
c. lithium, Li
d. magnesium, Mg
9. When fluorine forms an ionic bond it tends to
a. lose electrons b. gain electrons c. share electrons d. lose protons
10. Copper (II) hydroxide is composed of
a. 2 elements, 2 atoms
b. 2 elements, 3 atoms
c. 3 elements, 4 atoms
d. 3 elements, 5 atoms
True and False.
On your answer sheet, circle A for true, B for false.
b) Potassium metal is added to water. (3 marks)
c) Butane, C4H10 (g), reacts with atmospheric oxygen. (4 marks)
23. ___ The radius of an ion is always larger than the atomic radius of
the original atom.
24. ___Most of the metals found above hydrogen in the activity series
are found as elements in the ground.
4. Write the complete chemical, total and net ionic equations for a
double displacement reaction between calcium chloride and sodium
phosphate. (8 marks)
SECTION C: APPLICATION (9 marks)
25. __ Gold is a highly reactive metal.
26. ___ Barium hydroxide produced in a double displacement reaction
will precipitate out.
27. ___ Hydrogen is in the activity series because it classifies as a
metal.
SECTION B: THINKING/INQUIRY (30 marks)
1. Draw the following Lewis symbols/Lewis structures (2 marks each)
a) oxygen atom
b) chloride ion
c) hydrogen gas
d) carbon tetrafluoride
e) calcium chloride
f) sodium hydroxide
2. Predict the products and write a balanced chemical equation for the
following chemical reactions:
a) Copper wire is added to an aqueous solution of silver nitrate. (3 marks)
1. Beakers A and B are filled with substances that are liquid at room
temperature. The substance in beaker A experiences London dispersion
forces. The substance in beaker B experience dipole-dipole interactions.
Compare and contrast the two force types. Which substance will boil at
a lower temperature and why? (5 marks)
2. For a science fair project, a student wants to design a simple device
for removing certain gases from polluted air. He knows that polar
molecules dissolve well in water, so he bubbles polluted air through a jug
of water to remove unwanted gases. For his project, the student uses air
containing the following gases:
1. N2(g)
2. O2(g)
3. HF(g)
4. NH3(g)
5.
6.
7.
8.
CH4(g)
OCl2(g)
C3H8(g)
CH3OCH3(g)
Which gases will dissolve? (4 marks)
SECTION D: COMMUNICATION (10 marks)
* an additional 4 marks will be awarded for clarity, correct spelling,
neatness and organization of answers throughout test
1. Explain how first ionization energy is related to atomic radius. (3
marks)
2. Describe what are polar covalent bonds. (3 marks)