Science 10 Chemistry Review_keyed Unit A: Chemistry Review
Multiple Choice
1. Which statement is not part of Dalton’s atomic theory?
(a) All matter is made up of small particles called atoms.
(b) Atoms are made up of protons, neutrons, and electrons.
(c) Atoms cannot be created, destroyed, or divided into smaller particles.
(d) A chemical reaction changes the way that atoms are arranged.
2. J. J. Thomson discovered that cathode rays are
(a) emitted from the nucleus of an atom
(b) a stream of charged atoms
(c) a result of nuclear reactions
(d) composed of tiny, negatively charged particles
3. Isotopes are best described as two atoms of the same element that
(a) become electrically charged
(b) differ in mass but are chemically alike
(c) give away electrons to become positively charged
(d) have the same mass but different chemical properties
4. The isotope
(a)
(b)
(c)
(d)
has
40 protons and 20 neutrons
20 protons and 40 neutrons
20 protons and 20 neutrons
40 electrons and 20 neutrons
5. Elements in the same period in the periodic table
(a) share similar properties
(b) have the same atomic weight
(c) cannot react with each other
(d) have the same number of energy levels
6. Which electron dot diagram correctly represents a nitrogen atom?
(a)
(b)
(c)
(d)
7. How many protons does an atom of silver contain?
(a) 47
(b) 108
(c) 61
(d) 60
8. An electron dot diagram shows
(a) unpaired electrons only
(b) valence electrons only
(c) electrons from the innermost energy level only
(d) all the electrons in an atom
Mrs. Steinbrenner Science 10 Chemistry Review_keyed Mrs. Steinbrenner 9. An atom is found to have seven valence electrons. To which family of elements in the periodic table
does this atom belong?
(a) noble gases
(b) halogens
(c) alkaline earth metals
(d) alkali metals
10. The nucleus of any atom, except hydrogen, is made up of
(a) only neutrons
(b) only protons
(c) equal numbers of electrons and protons
(d) neutrons and protons
11. Which of the following applies to metallic elements when they form positive ions?
a) they lose electrons and become anions
b) they lose electrons and become cations
c) they gain electrons and become anions
d) they gain electrons and become cations
12. The IUPAC name for MnO is
a) manganese oxide
b) manganese dioxide
c) manganese (II) oxide
d) manganese (IV) oxide
13. The common name for NH3 is
a) methane
b) ammonia
c) natural gas
d) nitrogen trihydride
14. Which of the following is a base?
a) H 2O(l)
b) NaOH(aq)
c) H2SO3(aq)
d) Na2SO3(aq)
15. One of the unique properties of water is a high level of cohesion. Cohesion is
a) an ionic compound
b) an attraction to solid substances
c) an attraction between like molecules
d) an attraction between dissimilar molecules
16. An acid has the following properties:
a) tastes sour and has no reaction with Mg
b) tastes bitter and has no reaction with Mg
c) tastes sour and reacts with Mg to produce bubbles
d) tastes bitter and reacts with Mg to produce bubbles
Science 10 Chemistry Review_keyed Mrs. Steinbrenner 17. Which of the following are typical of a solution having a pH of 12?
a) litmus is red; solution conducts electricity
b) litmus is blue; solution conducts electricity
c) litmus is red; solution does not conduct electricity
d) litmus is blue; solution does not conduct electricity
18. What is the systematic (IUPAC) name for the compound Fe2O3?
(a) iron(III) oxide
(b) iron oxide
(c) iron(II) oxide
(d) iron(II) trioxide
19. What is the systematic (IUPAC) name for the compound S2O3?
(a) sulfur oxide
(b) sulfur(III) oxide
(c) sulfur trioxide
(d) disulfur trioxide
20. What is the correct formula for the compound that contains magnesium and
phosphate ions?
(a) MgPO4
(b) Mg3PO4
(c) Mg2(PO4)3
(d) Mg3(PO4)2
21. Which compound has no covalent bonds?
(a) Na2SO4
(b) KCl
(c) HClO3
(d) CH3Cl
22. The name for H2SO3 (aq) is
(a) hydrosulfuric acid
(b) sulfuric acid
(c) sulfurous acid
(d) hydrogen sulfite acid
23. Substances with a pH above 7 are considered to be
(a) basic
(b) acidic
(c) salty
(d) ionic
Science 10 Chemistry Review_keyed Mrs. Steinbrenner 24. Which is not a characteristic of acids?
(a) bitter taste
(b) turn litmus red
(c) react with bases to form salts
(d) react with active metals to form H2 gas
25. Four compounds are dissolved in water. Which of the resulting solutions (A to D) are
good conductors of electricity?
A.
H2CO3(aq)
B.
NH4OH(aq)
C.
CH3OH(aq)
D.
NaCl(aq)
(a) A, B, and C only
(b) A and C only
(c) B and D only
(d) A, C, and D only
26. The attraction between the partial negative charge of one water molecule and the
partial positive charge of another water molecule is referred to as a(n)
(a) polar covalent bond
(b) ionic bond
(c) hydrogen bond
(d) hydrophobic bond
27. Which statement best explains the unusually high boiling point of water?
(a) Water contains H+ and OH– ions.
(b) The covalent O−H bond in water is very strong.
(c) The hydrogen bonds that hold water molecules together are strong.
(d) Water molecules interact with each other through ionic bonds.
28. The accepted IUPAC name for the orange compound (NH4)2Cr2O7(s) is
(a) ammonium chromate
(b) ammonium dichromate
(c) diammonium chromate
(d) ammonium chromium oxide
29. Which list includes only substances with no ionic bonds?
(a) N2O4, HBr, LiCN
(b) CO2, NH3, N2
(c) SO3, BaCl2, O2
(d) NaCl, CH4, Al(OH)3
Science 10 Chemistry Review_keyed Mrs. Steinbrenner 30. The reaction of solid copper(II) oxide with hydrogen gas at high temperatures
produces copper metal and water. Which chemical equation represents this
reaction?
(a) CuO2(s) + 2 H2(g) → Cu(s) + 2 H2O(l)
(b) Cu2O2(s) + 2 H2(g) → 2 Cu(s) + 2 H2O(l)
(c) CuO(s) + H2(g) → Cu(s) + H2O(l)
(d) Cu2O(s) + 2 H(g) → 2 Cu(s) + H2O(l)
31. In a chemical reaction, solid iron metal reacts with chlorine gas to produce solid
iron(III) chloride. Which equation is the correctly balanced chemical equation for this
reaction?
(a) 2Fe(s) + 3Cl2(g) → 2FeCl3(s)
(b) Fe(s) + Cl2(g) → FeCl2(s)
(c) 6Fe(s) + Cl2(g) → 2Fe3Cl(s)
(d) 2Fe(s) + 2Cl2(g) → 2FeCl2(s)
32. How would you classify the following reaction?
HNO3(aq) + NaOH(aq) → H2O(l) + NaNO3(aq)
(a) combustion reaction
(b) formation reaction
(c) decomposition reaction
(d) double replacement reaction
33. The molar mass of Al2(SO4)3 (s) is
(a) 123.04 g/mol
(b) 150.02 g/mol
(c) 278.02 g/mol
(d) 342.14 g/mol
34. The amount (in mol) of 1.40 g of copper is
(a) 0.0220 mol
(b) 0.500 mol
(c) 1.40 mol
(d) 45.3 mol
35. The mass of 0.500 mol of sodium hydroxide (lye), NaOH(s), is
(a) 20.0 g
(b) 40.0 g
(c) 80.0 g
(d) 200.0 g
Science 10 Chemistry Review_keyed Mrs. Steinbrenner Matching
Match each description in column A with the correct term in column B. Write the letter for the
term on the line beside the description.
A
B
f 1.
substance that dissolves in water to release hydrogen ions
k 2.
ion that consists of one or more different atoms joined by
covalent bonds
g 3.
process that takes place when acids and bases are mixed
i 4.
substance that is used to identify whether a solution is
acidic or basic
e 5.
compound that is formed of non-metals joined only by
covalent bonds
A j 6. An insoluble solid formed by a chemical reaction in solution. d 7. A chemical reaction in which energy is absorbed. k 8. The total mass of the reacting substances must equal the
total mass of the resulting substances.
a 9. f 10.
An organic compound that contains only the elements carbon and hydrogen. The amount of a substance that contains as many
elementary entities as exactly 12 g of carbon-12.
(a) ionic compound
(b) molar mass
(c) anion
(d) cation
(e) molecular compound
(f) acid
(g) neutralization
(h) base
(i) litmus paper
(j) electron
(k) polyatomic ion
B (a) hydrocarbon (b) exothermic reaction (c) open system (d) endothermic reaction (e) combustion reaction (f) mole (g) molar mass (h) neutralization reaction (i) Avogadro’s number (j) precipitate (k) law of conservation of mass (l) law of conservation of energy Science 10 Chemistry Review_keyed Mrs. Steinbrenner Fill-in the Blanks
Use the following terms and symbols to complete the sentences below. Some terms and
symbols will be used more than once, and some not at all.
H+
OH–
NH4+
sour
bitter
sweet
red
blue
orange
turns pink
remains colourless
lower
higher
Arrhenius
greater than
less than
conduct
do not conduct
(a) According to Arrhenius, acids are substances that dissolve in water to release H+ ions.
(b) They are characterized by a pH value less than 7.
(c) The lower the pH value, the more acidic a solution is.
(d) When an acid is added, blue litmus turns a red colour and phenolphthalein remains
colourless.
(e) Acidic solutions conduct electricity.
(f) According to Arrhenius, bases are substances that dissolve in water to release OH- ions.
(g) Acids are responsible for the sour taste in foods.
(h) Bases are characterized by a pH value greater than 7.
(i) The higher the pH value, the more basic a solution is.
(j) When a base is added, red litmus turns a blue colour and phenolphthalein turns pink.
(k) Basic solutions conduct electricity.
(l) Bases are responsible for the bitter taste in foods.
Science 10 Chemistry Review_keyed Mrs. Steinbrenner Chemical Nomeclature
No.
Chemical
Formula
Name of Compound
No.
Chemical
Formula
Name of Compound
1
NH4Cl
ammonium chloride
21
AlPO4
aluminum phoshpate
2
KMNO4
potassium
permanganate
22
CO
carbon monoxide
3
HCl (aq)
hydrochloric acid
23
SO3
sulfur trioxide
4
FeSO4
iron (II) sulfate
24
K 2S
potassium sulfide
5
CuNO3
copper (I) nitrate
25
HgS
mercury (II) sulfide
6
Li2CO3
lithium carbonate
26
NO2
nitrogen dioxide
7
CH4
methane
27
HCl(aq)
hydrochloric acid
8
Mg(OH)2
magnesium hydroxide
28
P 2O 5
diphosphorus pentoxide
9
CaO
calcium oxide
29
H2SO4(aq)
sulfuric acid
10
Li3N
lithium nitride
30
NaOH(aq)
aqueous sodium
hydroxide
11
SiO2
silicon dioxide
31
CuSO4
copper (II) sulfate
12
N2 (g)
nitrogen gas
32
CS2
carbon disulfide
13
ZnO
zinc oxide
33
K2Cr2O7
potassium dichromate
14
HBrO3
hydrogen bromate
34
HI
hydrogen iodide
15
Fe2(CO3)3
iron (III) carbonate
35
NaH
sodium hydride
16
H 2S
hydrogen sulfide
36
N 2O 5
dinitrogen pentoxide
17
NH3 (l)
ammonia
37
KClO4
potassium perchlorate
18
MgCH3COO
magnesium acetate
38
SnF2
tin (II) fluoride
19
Ag2SO4
silver sulfate
39
Na2B4O7
sodium tetraborate
*tetraborate ion is B4O72-
20
CH3OH
methanol
40
HClO4(aq)
hydrogen perchlorate
Science 10 Chemistry Review_keyed Mrs. Steinbrenner Balancing
Balance the following chemical reactions.
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
4K(s)
P4(s)
8Cu(s)
2Mg(s)
4Fe(s)
4P4(s)
2C(s)
N2(g)
6Li(s)
S8(s)
+
+
+
+
+
+
+
+
+
+
O2 (g)
10Cl2(g)
S8(s)
3O2(g)
O2(g)
5S8(s)
O2(g)
2O2(g)
N2(g)
8O2(s)
2K2O(s)
4PCl5(s)
8CuS(s)
2MgO(s)
2Fe2O3(s)
8P2S5(s)
2CO(g)
2NO2(g)
2Li3N(s)
8SO2(g)
Complete and balance the following chemical reactions.
1.
2.
3.
4.
5.
2Al(s)
2H2(g)
4Al(s)
Ca(s)
8Zn(s)
+
+
+
+
+
3Br2(l)
O2(g)
3O2(g)
Cl2(g)
S8(s)
2AlBr3(s)
2H2O(l)
2Al2O3(s)
CaCl2(s)
8ZnS(s)
Translate, complete and balance the following reactions:
1. Magnesium and oxygen react in a formation reaction
2Mg(s) + O2(g)  2MgO(s)
2. Aluminum and oxygen react in a formation reaction
4Al(s) + 3O2(g)  2Al2O3(s)
3. Lead (II) chloride decomposes
PbCl2(aq)  Pb(s) + Cl2(g)
Science 10 Chemistry Review_keyed Mrs. Steinbrenner Use this page to make extra study notes:
What do I need to know for the exam? Evolution of atomic theory, who contributed what. isotopes and nuclear notation Lewis dot diagrams – atoms and ions trends on the PTOE (ie. groups, periods, reactivity patterns, ion charge patterns) how are ions formed; positive and negative bond theories (ionic vs. molecular) properties of ionic, molecular, acids and bases (including Arrhenius definition of A and B) properties of water (density anomalies, adhesion, cohesion, specific heat capacity – due to H bonding) naming compounds from formula predicting formula from name classifying chemical reactions predicting chemical reactions balancing chemical reactions the mole (avogadro’s #) using (n=m/M) to solve for an unknown variable (n, m, M)