Time Allowed:   90 Minutes

This test is designed to give you an indication of what you would be expected to know in enrolling into first-year chemistry. Attempt all of the questions, but do not guess randomly. Use only a non-programmed calculator and a periodic table as test aids.

1. The quadratic equation 4x2+2x-1=0 was obtained from a calculation of chemical equilibrium. What is the concentration, x, in mol/L?

(a) 0.809
(b) -0.309
(c) 0.309
(d) 0.618
(e) none of the above

2. The following functions are often used in chemical kinetics   

(i) linear function: y=x,
(ii) quadratic function: y=x2,
(iii) reciprocal function: y=1/x,
(iv) exponential function: y=ex,
(v) logarithmic function:  y=ln x.
Match the functions with the following graphs in alphabetical order.

A   B   C   D   E

(a) A--i, B--iii, C--iv, D--v, E--ii
(b) A--iv, B--iii, C--ii, D--i, E--v
(c) A--ii, B--v, C--iv, D--iii, E--i
(d) A--iii, B--iv, C--v, D--ii, E--i
(e) A--ii, B--iii, C--v, D--iv, E--i

3. Two aqueous NaCl solutions were combined in a 1.00 L container. One solution was of concentration 80.0 g/L and the other, 30.0 g/L. If the total mass of NaCl was 50.0 g, what volume of the 80.0 g/L solution was required?

(a) 0.125 L
(b) 0.600 L
(c) 0.375 L
(d) 0.400 L
(e) 0.625 L

4. How many electrons, protons, and neutrons does an atom with atomic number 10 and mass number 21 have?

(a) 10,10,11
(b) 10,10,21
(c) 21,10,11
(d) 10,21,11
(e) 21,10,10

5. Which of the following elements is the most metallic?

(a) Silicon
(b) Boron
(c) Sodium
(d) Arsenic
(e) Selenium

6. Which of the following is a salt?

(a) HBr
(b) CBr4
(c) H2SO4
(d) NH4Br
(e) CH3Br

7. What is the name of (NH4)2SO4?
(a) Ammonium sulfide
(b) Diammonium sulfite
(c) Ammonium sulfite
(d) Diammonium sulfide
(e) None of the above

8. Ammonia at room temperature is:
(a) a white solid
(b) a clear colourless liquid
(c) a white gas
(d) a cloudy pungent liquid
(e) a colourless gas

9. What is the oxidation number of N in NH3OH+ ion?

(a) -2
(b) -1
(c) 0
(d) +1
(e) +2

10. The percentage by weight of iron in Fe2O3 is:

(a) 23%
(b) 40%
(c) 67%
(d) 70%
(e) 78%

11. Which element has the smallest atomic radius?

(a) Ca
(b) Ga
(c) Ge
(d) As
(e) Se

12. Which element has the highest ionization energy?

(a) Li
(b) Na
(c) Be
(d) Mg
(e) Ca

13. Which element has the electronic configuration 1s22s22p63s23p3?

(a) Na
(b) Mg
(c) Cl
(d) As
(e) P

14. Which of these molecules has the greatest ionic character in its bonding?

(a) OF2
(b) BF3
(c) NF3
(d) CF4
(e) BeF2

15. The shape of BF3 is:

(a) tetrahedral
(b) linear
(c) trigonal planar
(d) pyramidal
(e) square planar

16. The following discoveries were vital in establishing quantum theory:

(i) Bohr's model of Hydrogen atom   
(ii) Dalton's atomic theory   
(iii) Rutherford's gold-foil experiment   
(iv) Thomson's cathode-ray experiment   
(v) Balmer's series of Hydrogen atom.
Match these discoveries with the following in alphabetical order:
(A) Atom can not be divided further  
(B) Discovery of electrons  
(C) Discovery of nuclei  
(D) En=-R/ n2  
(E) Discovery of line spectra.
Your answer is

(a) A--i, B--iii, C-ii, D--v, E--iv
(b) A--ii, B--iii, C-v, D--iv, E--i
(c) A--v, B--ii, C-iv, D--i, E--iii
(d) A--ii, B--iv, C-iii, D--i, E--v
(e) A--ii, B--v, C-iv, D--iii, E--i

17. Arrange the following discoveries in a chronological order:

(i) Bohr's model of Hydrogen atom  
(ii) Dalton's atomic theory  
(iii) Rutherford's gold-foil experiment  
(iv) Thomson's cathode-ray experiment  
(v) Balmer's series of Hydrogen atom

(a)(i) (iii) (ii) (v) (iv)
(b) (iii) (i) (v) (iv) (ii)
(c) (v) (ii) (iv) (i) (iii)
(d) (iii) (iv) (ii) (v) (i)
(e) (ii) (v) (iv) (iii) (i)

18. Which of the following always occur when an Arrhenius acid solution is completely neutralized with a base?

(i) There is an increase in pH  
(ii) A salt is formed  
(iii) Heat is evolved  
(iv) A gas is produced   
(v) All indicators change colour

(a) (i) (ii) (iii)
(b) (i) (iii) (v)
(c) (ii) (iii) (iv)
(d) (ii) (iii) (v)
(e) (ii) (iv) (v)

19. What happens to the mass of an iron bar when it rusts?
(a)There is no change since mass is always conserved
(b) The mass decreases since the rust is less dense than iron
(c) The mass increases during winter and decreases in summer
(d) The mass increases because the rust is a compound of hydrate of ferric oxide
(e) It cannot be predicted since the rusting process is not completely understood

20. The limiting reagent in a reaction
(a)has the lowest coefficient in a balanced reaction
(b)is the reactant which has the fewest number of moles
(c)has the lowest ratio of the moles available to the coefficient in a balanced reaction
(d)has the smallest mass in grams
(e)has the highest ratio of the moles available to the coefficient in a balanced reaction

21. 10.00 grams of A when mixed with 8.00 grams of B gives 18.00 grams of C. In an experiment 20.0 g of A is mixed with 10.0 g of B. How many grams of C will be formed?

(a) 10.0
(b) 20.0
(c) 30.0
(d) 18.0
(e) 22.5

22. How many grams of KOH are required to prepare 250 mL of 2.0 molar KOH solution?

(a) 0.5 g
(b) 14 g
(c) 28 g
(d) 56 g
(e) 112 g

23. Which equilibrium is shifted to the left by an increase in external pressure but to the right by an increase in temperature?

(a) N2(g) + 3H2(g) 2NH3(g) + Heat
(b) 2NO2(g) + Heat 2NO(g) + O2(g)
(c)PCl3(g)+Cl2(g)+Heat PCl5(g)
(d) CaO(s) + CO2(g) CaCO3(s) + Heat
(e) H2(g) + I2(g) 2HI(g) + Heat

24. The pH of black coffee is about 5.0. How many times greater is the [H+] in coffee than in neutral water which has a pH of 7.0?

(a) 200
(b) 100
(c) 5.0
(d) 1.4
(e) 0.01

25. The pH of a 0.20 M solution of a weak acid HA is 3.70. What is the value of the ionization constant Ka of this acid?

(a) 7.0 × 10-4
(b) 4.0 × 10-6
(c) 2.0 × 10-7
(d) 1.8 × 10-5
(e) 1.3 × 10-2

26. Tripling the absolute temperature and doubling the pressure on exactly two litres of an ideal gas alters its volume to

(a) 1/3 L
(b) 4/3 L
(c) 8/9 L
(d) 3 L
(e) 12 L

27. How many Faradays of electricity, i.e., moles of electrons, are required to reduce two moles of MnO4- to two moles of Mn2+?

(a) 2
(b) 4
(c) 6
(d) 8
(e) 10

28. A radioactive substance decays at such a rate that after 96 minutes only 1/8 of the original amount remains. The half-life of this substance is:

(a) 12 min
(b) 24 min
(c) 32 min
(d) 48 min
(e) 64 min

29. A reaction has an activation energy of 40 kJ and an overall energy change of -100 kJ in the forward direction. The activation energy in kJ of the same reaction in the reverse direction would be:

(a) -40
(b) 60
(c) 60
(d) 140
(e) -140

30. Which of the following procedures can be safely performed in the laboratory?
(a) Diluting concentrated sulphuric acid by adding distilled water into it
(b) Evaporating a solution of sulphur in carbon disulphide over Bunsen flame
(c) Igniting a jar of hydrogen gas
(d) Bubbling carbon dioxide through concentrated sulphuric acid
(e) Adding a small piece of potassium to dilute nitric acid

31. Which of the following describes your high-school chmistry course?
(a) Greater Toronto---OAC
(b) Other Ontario---OAC
(c) Ontario---Grade 11
(d) Other Canadian Province
(e) Outside Canada

32. Which of the following describes the type of your high-school course?
(a) Full Year Day
(b) Semester Day
(c) Night School
(d) Summer School
(e) Correspondence


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Web created by:   C. C. Wan
Created: Fri Jun 23 2000