SCH4U Grade 11 Diagnostic
Multiple Choice
____
1. A Sn-120 ion with a 4+ charge has:
a) 54 electrons, 50 protons, and 70 neutrons
b) 50 electrons, 54 protons, and 70 neutrons
c) 46 electrons, 50 protons, and 70 neutrons
d) 50 electrons, 54 protons, and 120 neutrons
e) 46 electrons, 50 protons, and 120 neutrons
____
2. Elements X and Y are in the same chemical family. Element X has a first ionization energy of 7.646 eV.
Element Y has a first ionization energy of 5.695 eV. Which is more reactive?
a) X
b) Y
c) They are equally reactive.
d) not enough information
e) X will be more reactive provided it reacts with another member of its family.
____
3. Which of the following atoms is believed to contain three lone pairs of electrons?
a) H
d) C
b) Al
e) Cl
c) B
____
4. A student records the following evidence in a lab book.
Unknown Substance
Pure State
Solubility in Water
Solution Conductivity
I
solid
high
low
II
solid
low
low
III
solid
high
none
IV
solid
high
high
Which of the substances shown in the table above is most likely an ionic compound?
a) I
d) IV
b) II
e) none of the above
c) III
____
5. Which of the following is the proper Lewis structure for NaCl?
a)
d)
b)
e)
c)
____
6. 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) XF
d) X4F
b) XF2
e) XF4
c) X4F2
____
7. Which ion has the correct name and formula?
a) nitrite, NO3b) perchlorate, ClO5c) hydrogen carbonate, HSO3d) hyposulfite, SO32e) phosphite, PO33-
____
8. Determine the sum of the reactant coefficients when the following equation is balanced:
H3PO4 + BaCO3
Ba3(PO4)2 + H2O + CO2
a) 8
d) 5
b) 9
e) 2
c) 6
____
9. Which of the following combinations would result in the formation of a precipitate?
a) acetic acid and potassium hydroxide solutions
b) magnesium nitrate and sodium sulfide solutions
c) sulfuric acid and barium hydroxide solutions
d) sodium sulfate and copper(II) chloride solutions
e) sodium chloride and ammonium nitrate solutions
____ 10. Classify the following reaction: H2O + SO3  H2SO4
a) combustion
d) single displacement
b) synthesis
e) double displacement
c) decomposition
____ 11. Which metal would not displace lead, Pb, in a lead nitrate, Pb(NO3)2, solution?
a) copper, Cu
d) magnesium, Mg
b) potassium, K
e) none of the above
c) lithium, Li
____ 12. Which ion could a technician add to water to test for chloride ions, Cl–?
a) Na+
d) Cu2+
+
b) Ag
e) K+
+
c) NH4
____ 13. The molar mass of Ca3(PO4)2 is
a) 245.60 g/mol
b) 310.18 g/mol
c) 219.21 g/mol
d) 341.52 g/mol
e) 249.67 g/mol
____ 14. The number of moles of H in three moles of copper(II) sulfate pentahydrate, CuSO4.5H2O, is
a) 2
d) 30
b) 6
e) 50
c) 10
____ 15. Which formula cannot be an empirical formula?
a) HO
d) CH
b) CH2O
e) N2O4
c) NH2
____ 16. The limiting reagent of a chemical reaction is
a) the reactant of a chemical process that is not consumed completely
b) the product of a chemical process that is consumed completely
c) the product of a chemical process that is not consumed completely
d) the reactant of a chemical process that is consumed completely
e) none of the above
____ 17. Potassium chloride and oxygen gas are formed upon heating potassium chlorate. The following balanced
equation shows this decomposition process: 2KClO3
2KCl + 3O2
The number of moles of KClO3 required to produce 5.0 mol of oxygen is
a) 1.0
d) 3.3
b) 2.0
e) 5.0
c) 3.0
____ 18. If 2.0 mol of aluminum are allowed to react with 2.8 mol of bromine, determine which of the statements below
is true, given the following balanced equation: 2Al + 3Br2
2AlBr3
a) The aluminum will react completely.
b) The bromine is the reagent in excess.
c) The bromine is the limiting reagent.
d) The aluminum is the limiting reagent.
e) Both (a) and (d) are true.
____ 19. If 226.1 g of tin(II) chloride was the actual amount obtained in a reaction for which the theoretical yield was
288.0 g, the percentage yield is
a) 71.15%
d) 84.11%
b) 78.51%
e) 86.77%
c) 81.98%
____ 20. Which of the following mixtures would not conduct electricity?
a) an acidic solution
d) sugar dissolved in water
b) Gatorade solution
e) salt dissolved in water
c) a basic solution
____ 21. Intermolecular forces are
a) forces among molecules
b) covalent bonds
c) ionic bonds
d) forces within molecules
e) none of these
____ 22. The separation of ions that occur as ionic compounds dissolve in water is known as
a) dissociation
d) dissolving
b) separation
e) deportation
c) protonation
____ 23. The parts of a water molecule that surround the sodium ions when NaCl dissolves are the
a) positive hydrogen ends
d) positive oxygen ends
b) negative hydrogen ends
e) chloride ions
c) negative oxygen ends
____ 24. A solution that has a relatively large quantity of solute dissolved in the solvent is
a) homogenous
d) mixed
b) dilute
e) saturated
c) concentrated
____ 25. Which piece of lab equipment is used to obtain a small, accurate volume from a stock solution for a dilution
procedure?
a) graduated cylinder
d) beaker
b) pipet
e) none of the above
c) buret
____ 26. The equation C1V1=C2V2 is saying that the moles of solute _____________ when a solution is diluted.
a) increases
b) stays the same
c) decreases
____ 27. A bottle contains 3 L of 12 mol/L H2SO4 solution. After half of the contents are used up, the remaining solution
has a concentration of
a) 18 mol/L
d) 3 mol/L
b) 12 mol/L
e) none of the above
c) 6 mol/L
____ 28. As the temperature of a solution increases, the solubility of solids _____ and the solubility of gases _____.
a) doesn't change, doesn't change
d) decreases, decreases
b) increases, decreases
e) decreases, increases
c) increases, increases
____ 29. Nitric acid is classified as a strong acid because
a) it has high electrical conductivity
b) it ionizes about 50%
c) ionizes more than 99%
d) both a and c
e) it has a higher concentration than other acids
____ 30. How much more acidic is vinegar (pH = 2.0) than coffee (pH = 5.0)?
a) 3.0
d) 2.5
b) 1000
e) 0.4
c) 100
____ 31. According to Arrhenius, an acid is defined as:
a) a chemical that ionizes to release OH- ions in water
b) a chemical that reacts with a base in a neutralization reaction
c) a chemical that ionizes to release OH+ ions in water
d) a chemical that ionizes to release H+ ions in water
e) a chemical that ionizes to release electrons in water
____ 32. During an acid-base titration that uses an acid-base indicator, the point at which the experimenter stops adding
titrant to the analyte due to the observation of a sharp, permanent colour change is called the
a) mixed point
d) fixed point
b) equivalence point
e) last point
c) end point
____ 33. A gas is
a) always reactive
b) always diatomic in structure
c) highly compressible
d) a state with low miscibility with other gases
e) only found at elevated temperatures
____ 34. Assuming constant volume and amount of gas, the pressure of an ideal gas such as N2, increases with
temperature because the
a) volume of N atoms increases
d) molecules of N2 move more rapidly
b) density of the gas decreases
e) collisions are less elastic
c) density of the gas increases
____ 35. For a gas, which pair of variables are inversely proportional to one another if all other conditions remain
constant?
a) P and T
d) n and V
b) P and V
e) n and P
c) V and T
____ 36. Which of the following graphs represents the plot of volume versus temperature (in K) at constant pressure?
a) A
b) B
c) C
d) D
e) E
____ 37. An unknown gas has a density of 1.95 g/L at STP. What is the molar mass of this gas knowing that the universal
gas constant is 8.31 kPa L/mol K?
a) 22.4 g/mol
d) 23.8 g/mol
b) 11.4 g/mol
e) 140 g/mol
c) 43.7 g/mol
____ 38. A rigid container contains 2.50 mol O2, 0.50 mol N2, and 1.00 mol CO2. The total pressure of the system is 200
kPa. The partial pressure exerted by the O2 in the mixture is
a) 100 kPa
d) 200 kPa
b) 125 kPa
e) none of the above
c) 150 kPa
____ 39. The chemical formula of iron(II) perchlorate is:
a) Fe2ClO3
d) Fe(ClO2)2
b) Fe2(ClO3)2
e) Fe(ClO4)2
c) Fe3(ClO4)2
____ 40. Solid phosphorus, P4(s), reacts with chlorine gas to produce solid phosphorus pentachloride. If 187.82 g of
phosphorus reacts with 521.19 g of chlorine, what mass of the excess reactant should remain unreacted?
a) 64.75 g
d) 96.76 g
b) 23.94 g
e) 0 g since the reactant amount ratio matches
the stoichiometric ratio
c) 82.51 g
Short Answer
41. A monatomic ion with a 2+ charge has a mass number equal to 62. If the number of neutrons for the ion is 1.21
times larger than the number of protons, how many moles of electrons are there?
42. Which element accounts for more than half of the total mass of a human body? Explain. (include some
calculations in your explanation as well)