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SNC2PI
CHEMISTRY UNIT TEST - 2012 -
NAME: _________________________________
MARK =
/95
**YOU MAY USE YOUR PERIODIC TABLE FROM YOUR NOTES**
PART A: MULTIPLE CHOICE (40 marks)
Answer the following questions on the Scantron Card provided, in pencil.
1.
There is no doubt that a chemical reaction has occurred if:
(a) there has been an overall volume change
(b) the form or state has been changed
(c) a new substance has been formed
(d) there has been a change of state
2.
The set of elements containing only nonmetals is:
(a) I, H, Ag
(b) C, Cl, S
(c) Al, Sr, K
(d) Br, Fe, He
3.
The set of elements containing only metals is:
(a) Cu, Br, Fe
(b) Zn, Li, Ca
(c) Sr, Al, Cl
(d) K, O, Ag
4.
An atom has a total of 18 protons and 18 electrons. These electrons are found in 3 orbits that have:
(a) 6 electrons each;
(b) 8, 8, and 2 electrons, moving out from the nucleus
(c) 2, 8, and 8 electrons, moving out from the nucleus;
(d) 2, 10, and 6 electrons, moving out from the nucleus;
5.
Which of the following atoms has the electron orbit arrangement “2 in the first orbit, 7 in the second”?
(a) Li
(b) Cl
(c) F
(d) Ne
6.
An atom becomes a negatively charged ion when it:
(a) loses neutrons
(b) gains electrons
(c) gains protons
(d) loses electrons
7.
When calcium metal is dropped into water, which gas or gases would be produced?
(a) oxygen and carbon dioxide gases
(b) hydrogen and oxygen gases
(c) hydrogen gas only
(d) carbon dioxide gas only
8.
What does the " —> " mean in the chemical equation: water —> hydrogen + oxygen
(a) reacts with
(b) produces
(c) a skeleton equation
(d) is balanced
9.
What does the " + " mean in the chemical equation: phosphorus + oxygen —> diphosphorus pentoxide
(a) a skeleton equation
(b) to produce
(c) reacts with
(d) a coefficient
10. In any chemical reaction, the total mass of the reactants is always equal to the total mass of materials
produced. This is known as the law of:
(a) conservation of mass
(b) chemical reactions
(c) constant proportion.
(d) conservation of energy
11. A balanced chemical equation takes into account the theory that:
(a) compounds and elements remain unchanged in a chemical reaction.
(b) atoms are neither created nor destroyed in chemical reactions.
(c) the total mass always increases during a chemical reaction.
(d) the mass of any gases involved can be ignored.
-212.
Predict the product(s) for the following single displacement reaction.
Li + CuO —> _________________
1. CuLi 2. CuO2 3. Li2O 4. Cu 5. Cu(OLi)2
(a) 3 and 4 only
(b) 1 and 2 only
13.
14.
(c) 5 only
(d) 4 and 5 only
In the following equation, the " X " represents:
Al2(SO4)3 + Ca(OH)2 —> X + CaSO4
(a) H2O
(b) Al
(c) Al(OH)3
(d) SO2
Classify the following equation as to reaction type.
AgNO3 + NaCl—> NaNO3 + AgCl
(a) decomposition
(b) double displacement
15.
(c) synthesis
(d) single displacement
What is the reaction type classification for the following equation?
2CaCO3 —> 3CO2 + 2Ca
(a) double displacement
(b) decomposition
16.
(c) synthesis
(d) single displacement
Which of the following is an example of a single displacement reaction?
(a) passing electricity through water to produce oxygen and hydrogen gases;
(b) putting copper into oxygen to produce copper (II) oxide;
(c) heating calcium carbonate to produce carbon dioxide and calcium oxide;
(d) putting sodium into water to produce hydrogen gas and sodium hydroxide;
17. If BaCl2 and Na2SO4 solutions are mixed together, a:
(a) single displacement reaction occurs.
(b) double displacement reaction occurs.
(c) neutralization reaction occurs.
(d) synthesis reaction occurs.
18. The products of the following reaction carried out in solution are:
Ca(NO3)2 + K2CO3 —> __________________
1. CaCO3 2. CaK2 3. KNO3 4. CO3(NO3)2
(a) 1 and 3
(b) 1, 2, and 4
(c) 2, 3, and 4
(d) 2 and 4
19. When the following equation is balanced, the coefficients for P and O2 in order are:
P + O2 —> P2O5
(a)
(b)
(c)
(d)
6, 4
4, 6
5, 4
4, 5
20. Which of the following equations is correctly balanced?
(a) 2H2O —> H2 + O2
(b) HgO —> Hg + O2
(c) C + O2 —> CO2
(d) 2Mg + Cl2 —> MgCl2
21. Metals ‘like’ to:
(a) Lose valence electrons to become an anion;
(b) Lose valence electrons to become a cation;
(c) Gain valence electrons to become neutral;
(d) Lose valence electrons to become neutral;
22. Metal and non-metal elements will either lose or gain valence electrons to closely resemble:
(a) Halogens
(c) alkali metals
(b) Noble gases
(d)
metalloids
23. Incomplete combustion is caused mainly due to:
(a) Lack of enough oxygen
(b) Not enough fuel
(c) Too much heat
(d) All of the above
3
24. An example of a double displacement reaction would be:
(a) KI + Pb(NO3)2  KNO3 + PbI2
(b) KClO3  KCl + O2
(c) H2 + O2  H2O
(d) None of these is a double displacement
25. The product(s) of the complete combustion of a hydrocarbon is/are:
(a) water, oxygen, and nitrogen dioxide
(b) water only
(c) carbon dioxide only
(d) water and carbon dioxide
26. Which reaction among the following is NOT a double displacement?
(a) H2SO4 + Ca(OH)2  CaSO4 + H2O
(b) Zn + HCl  ZnCl2 + H2
(c) KOH + HCl  KCl + H2O
(d) HNO3 + NaOH  H2O + NaNO3
Use the following diagrams to answer the next four (4) questions.
1
2
3
4
27. Diagram 1 above represents which of the following?
(a) poisonous and infectious causing immediate toxic effects
(b) poisonous and infectious causing other toxic effects
(c) corrosive material
(d) flammable and combustible material
28. Diagram 2 above represents which of the following?
(a) poisonous and infectious causing immediate toxic effects
(b) poisonous and infectious causing other toxic effects
(c) corrosive material
(d) flammable and combustible material
29. Diagram 3 above represents which of the following?
(a) corrosive warning
(b) explosive danger
(c) compressed gas
(d) biohazardous material
30. Diagram 4 represents which of the following?
(a) corrosive warning
(b) explosive danger
(c)
(d)
corrosive caution
biohazardous material
31. Which one of the following statements is TRUE regarding lab safety?
(a) All products used can be washed down the sink.
(b) Adding water to spilled acids and bases id the best way to reduce any potential harm.
(c) Goggles must be worn only when dealing with chemicals.
(d) If you break a piece of glassware, you should pick up all the pieces with your hands.
32.
A solid that forms when two liquids are mixed together is called a:
(a) precipitate;
(c) reactant;
(b) solution;
(d) electrolyte;
33.
When ionic compounds dissolve in water, they form:
(a) dissolved ions;
(c) electrolytes;
(b) homogeneous mixtures
(d) all of the choices;
34. Which of the following properties describe a molecular compound?
1. relatively low melting point;
2. very high melting point;
3. could be solid liquid or gas at room temperature depending on the molecule;
4. conducts electricity;
5. always dissolves in water
(a) 1 and 3 only
(b) 1, 4, and 5 only
(c) 1, 2, 3, 4, and 5
(d) 2 and 5 only
4
35. If a group I metal is added to water what product(s) is/are made?
(a) hydrogen gas.
(b) metal hydroxide.
(c) oxygen gas.
(d) only (a) and (b).
(e) both (b) and (c)
36.
Which of the following are correct about ionic bonds?
1. very strong;
2. found between a metal ion and a non-metal ion;
3. are electrostatic attraction;
4. found between two non-metal atoms;
5. are caused by the sharing of valence electrons.
(a) 2, 4, and 5 only
(b) 2, 3, and 4 only
37. Molecular compounds:
(a) have a lower melting point than ionic compounds
(b) contain two metal ions
(c) 1, 4, and 5 only
(d) 1, 2, and 3 only
(c) all dissolve in water
(d) all of the choices
38. A heterogeneous solution is said to:
(a) Have only one phase (layer)
(b) Have more than one phase
(c) Be a pure substance
(d) Both (a) and (c)
39. In order to light a Bunsen burner you must first:
(a) Turn on the gas
(b) Light the lighter/sparker
(c) ‘Choke’ off the air intake to limit oxygen flow
(d) Open up the air intake valve to let in more air
40. Examples of Metalloids are:
(a) group I and II elements
(b) halogens
(c) transition metals
(d) Boron, Silicon and Antimony
**ANSWER EACH OF THE FOLLOWING QUESTIONS IN THE SPACES PROVIDED**
PART B: SHORT ANSWER (57 marks) Answer the following questions in the spaces provided.
1.
A chemical reaction is represented by the following word equation:
magnesium + sulfuric acid —> hydrogen + magnesium sulfate
2.
(a) What are the
products of this reaction? (2 marks)
(b) What are the
reactants in this reaction? (2 marks)
An unknown white solid is discovered on the lab counter in room 2101. Miss Allen wants to know if it is ionic or covalent.
Describe how you could use its properties to determine if it is ionic or covalent. Be sure to use at least 3 specific
examples of properties (3 marks)
5
3.
Balance the following equations and give the reaction
type for each. If the reaction is already balanced write
“balanced”: (12 marks, 2 marks each)
a)
KOH +
b)
C6H12O6 +
c)
CuCO3 
H 2O 
NH4NO3 + H20 
N2 
H 2O +
HOH
REACTION TYPE: _______________________
CO2
REACTION TYPE: ________________________
CO2
e)
REACTION TYPE: ______________________
Li2O +
H2
NH4OH +
HNO3
Mg3N2
REACTION TYPE:
______________________
REACTION TYPE:
_____________________
REACTION TYPE:
_________________________
Identify each of the following as either an ionic compound or molecular compound or neither. (3 marks – ½ mark each)
(a)
(b)
(c)
(d)
(e)
(f)
5.
CuO +
Li +
Mg +
K2SO4 +
O2 —>
d)
f)
4.
H2SO4 —>
calcium hydroxide _________
table sugar _________
Na2CO3 __________
magnesium chloride ________
NO3 __________
LiOH __________
The molecule lithium
oxide is an ionic compound.
(a) Draw the dot diagrams of each atom of this molecule, clearly showing the electron transfer with arrows. (2 marks)
(b) Draw what the ions that are formed (use boxes around the ions with their ionic charge). (2 marks)
(c) Give the chemical formula for lithium oxide. (1 mark) __________________________________
6.
The molecule
oxygen dichloride is a molecular compound.
(a) Draw the dot diagrams of each
atom of the molecule, clearing showing the bonds. (3 marks)
(b) Draw the stick diagram of the molecule (2 marks)
7.
8.
Write the balanced chemical equation for the complete combustion of methane (CH4). (4 marks)
Examine these electron dot diagrams of three hypothetical elements.
X
Y
Z
a) Which element(s) is/are non-metals? How do you know? (2 marks)
b) Which element would you predict would NOT react with oxygen? Give reasons to support your answer.
(2 marks)
6
9.
Draw Bohr diagrams for i) an ATOM of sodium and
i) SODIUM ATOM
10.
ii) an ION of fluorine. (5 marks)
ii) FLUORIDE ION
Nomenclature: Fill in the chart in the spaces provided. (8 Marks)
1.
Cu2O
2.
CaCl2
3.
N2O3
4.
Hg(OH)2
Formula
Name
Name
Formula
1.
iron(II) oxide
2.
lithium iodide
3.
phosphorus pentabromide
4.
sodium carbonate
11. Identify the following pieces of Laboratory equipment. (4 Marks)
_____________
_____________
___________________
_______________
-7+1
+2
+3
-4
-3
-2
-1
Mono:
Di:
Tri:
Tetra:
Penta:
Hexa:
Prefixes
one
two
three
four
five
six
Roman Numeral
I
II
III
IV
V
VI
Common Polyatomic Ions
Negative Polyatomic Ions
PO43Phosphate
SO42Sulfate
CO32Carbonate
HCO31bicarbonate
NO21Nitrite
NO31Nitrate
OH1Hydroxide
Positive Polyatomic Ions
NH41+
Ammonium