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          ARRoGANT                CoURiERS      WiTH     ESSaYS

Grade Level:       Type of Work           Subject/Topic is on:
 [ ]6-8                 [ ]Class Notes    [Jarvis Collegiate Chem  ]
 [ ]9-10                [ ]Cliff Notes    [Exam                    ]
 [x]11-12               [ ]Essay/Report   [                        ]
 [ ]College             [x]Misc           [                        ]

 Dizzed: 10/94  # of Words:2429  School: ?              State: ?
ФФФФФФФФФ>ФФФФФФФФФ>ФФФФФФФФФ>Chop Here>ФФФФФФФФФ>ФФФФФФФФФ>ФФФФФФФФФ>ФФФФФФФФФ
                       JARVIS COLLEGIATE INSTITUTE                              

                                CHEMISTRY


Grade 12.   
Time: 1 1/2 hours.   
11.30 a.m. to 1:00 p.m.  
Tues  June 20 1989

NAME                                    HOME FORM             

Circle your teacher's name and indicate the period you take Chemistry.



Marks.  Part A = ___     Part B = ___    Total Marks = ___
                  30               55                   85


                           INSTRUCTIONS TO STUDENTS.

1.   Answer Part A on the answer sheet at the bottom of page 5.
     DO NOT detach the answer sheet.

2.   There is a periodic table at the back of the exam.  You may
     detach this.

3.   The questions in Part 1 are worth 1 mark each.

4.   Answer all the questions from Part B in the given space.



Part A.  Answer all questions in Part A on the answer grid at the
         bottom of page 5.                                             


1. Which of the following properties is not characteristic of metals?

   a)   They are dull in appearance
   b)   They are malleable
   c)   They are ductile
   d)   They are good conductors of heat.
     

2. The following is a list of the usual charge found on the ions 
   of a series of elements:

          V3+       W2+       X+        Z2-    
    
     Which elements are likely to be metals?

     a)   V and W       b)   V,  W and X.    
     c)   X  and Y    d)  Y and Z


3.   Which of the following is not a postulate of the kinetic 
     molecular theory?

a)   There are no attractive forces between the molecules
b)   Gases consist of extremely small particles called molecules
c)   Molecules of different gases have the same average velocity 
     at the same temperature
d)   All collisions of gas molecules are perfectly elastic


4. 2.00 L of dry hydrogen gas is collected at 27.0oC and 100 kPa 
   pressure.  The volume of this hydrogen measured at 227oC and 
   220 kPa pressure would be

  a)   2.00  x  220  x   27  L       b)   2.00  x  100  x  300  L
                100     227                        220     500

  c)   2.00  x  220  x  300  L       d)   2.00  x  100  x  500  L
                100     500                        220     300

5. If the temperature of a fixed mass of gas is kept constant 
   while the volume is decreased

a)   the average kinetic energy of the particles decreases
b)   the average kinetic energy of the particles increases
c)   the number of collisions per second increases
d)   the number of collisions per second decreases

6. The compound in the following list which is the best example 
   of an ionic solid at room temperature is,

a)   calcium bromide       (CaBr2)
b)   boron trifluoride     (BF3)
c)   tetrachloromethane    (CCl4)
d)   phosphorus(V) oxide   (P2O5)


7. Which one of the following items correctly indicates both the 
   correct electron dot (Lewis) diagram and the correct structural 
   (line) diagrams for the molecules illustrated.

                       H                   H
                                             
     a)   CH4       H  C  H             H  C  H 

                       H                   H

                         
     b)   NH3       H  N  N             H  N  H

                       H                   H

     c)   CO2       :O::C::O:           O  C  O

     d)   H2O       H  O:               H  O
                       
                       H                   H


8. A metal which does NOT readily liberate hydrogen gas from cold 
   water is

     a)   magnesium     b)   sodium       
     c)   potassium     d)   calcium



9. 1.00 L of a particular gas, at STP, has a mass of 4.80 g.
     Its molar mass is

     a)    0.210 g      b)   4.80 g       
     c)   108 g         d)   22.4 g


10   When the skeleton equation

          Al2(SO4)3    +    Ca(OH)2         Al(OH)3   +    CaSO4

     is balanced with the smallest whole numbers, the coefficient of
     Ca(OH)2 is

     a)   1              b)   2         c)   3         d)   4

11   Which of the following statements describing the 
     characteristics of the elements in the Periodic Table is TRUE?

a) The sequence of the elements Si, P, Cl shows increasing metallic 
   character.
b) The sequence of the elements Li, Na, K shows decreasing metal
   character.
c) The sequence of the elements C, N, O shows decreasing atomic 
   radius.
d) The sequence of the elements Ti,  V,  Cr  shows increasing
   electropositivity.

12   In general the valence electrons of metals are

a)   few in number and weakly held
b)   few in number and strongly held
b)   many in number and weakly held
d)   many in number and strongly held

13 Successive ionization energies, in kJ/mol, for an unknown element
   are given below.

E1  =  711      E2  =  1421        E3  =  7733         E4  =  9196

To which family of the Periodic Table does the element belong?

a)   IV          b)    III           c)   II           d)   I 


14 Benzoic acid,  C6H5COOH, is a component of candle wax. It burns 
   according to the unbalanced equation:

          C6H5COOH   +   O2          CO2    +    H2O

  When the equation is balanced for 1 mole of C6H5COOH the coefficient
  for oxygen is

   a)   6 1\2     b)   7 1/2          c)   8 1/2          d)  15

15 The reaction between gaseous hydrogen chloride and water is best
   represented by

a)   HCl(g)    +   H2O(l)          H22+(aq)    +   Cl-(aq)

b)   HCl(g)    +   H2O(l)          H2(g)     +    HClO(aq)

c)   HCl(g)    +   H2O(l)          H+(aq)    +    ClO-(aq)

d)   HCl(g)    +   H2O(l)          H3O+(aq)   +    Cl-(aq)


16  Which of the following will form an acidic solution when 
    dissolved in water?

a)   CO2     b)   Na2O      c)   O2     d)  H2


17 The best example of a molecular solid in which the 
   intermolecular bonding is only London dispersion forces is

a)   potassium iodide  (KI)        b)   carbon dioxide (CO2)
c)   water             (H20)       d)   ammonia        (NH3)


18 The products formed when potassium hydroxide reacts with 
   sulphuric acid are

a)   a salt and hydrogen           b)   sulphur dioxide and water
c)   a metallic oxide and water    d)   a salt and water


19  Which one of the following groups of elements will all produce 
    acidic solutions when their oxides are dissolved in water?

a)   Cl   S    Br  N               b)   S    P    Ca   Na
c)   N    Mg   K   Ni              d)   Li   Mg   Na   Cu


20   Real gases behave most like ideal gases when

a)   the pressure is high and the temperature is low
b)   the pressure is low and the temperature is high
c)   the pressure is low and the temperature is low
d)   the pressure is high and the temperature is high

21 Equal masses of hydrogen and oxygen are placed in a sealed 
   container.
   Which of the following statements about the system is TRUE?

a) since there are more hydrogen molecules, the mass of the hydrogen is 
   greater
b) since both the hydrogen and the oxygen are at the same temperature
   both have the same average molecular velocity
c) since the oxygen molecule is 16 times heavier than the hydrogen
   molecule, the hydrogen molecules are, on the average, moving
   4 times faster than the oxygen molecules.
d) since they are both at the same temperature , both exert the same 
  pressure

22             2KClO3     2KCl   +   3O2

How many moles of oxygen are produced during the decomposition of 8.0 
mol of KClO3?

a)   5.3            b)    24           c)   48            d)   12


23  Both copper metal and sodium chloride have high melting points. 
    Solid copper conducts electricity well but sodium chloride will 
    conduct electricity only when melted or dissolved in a polar 
    solvent.The difference in electrical conductivity of the two 
    solids is best explained by the

a) stronger bonding forces between particles of NaCl than in Cu
b) greater mobility of electrons in solid Cu than in solid NaCl
c) greater number of atoms in a mole of NaCl than in a mole of Cu       
d) solubility of sodium chloride in water


Questions 24, 25 and 26 refer to the following table which lists some
properties of substances

     Substance . Melting   .  Electrical conductivity . Water
                 Point (oC)   in solid   in liquid      solubility

         A         776          low          high           high
         B        -198          low          low            low
         C         961          high         high           low
         D        1640          low          low            low

24   Which substance is most likely to be an ionic solid?

a)   A         b)   B         c)   C         d)   D

25   Which substance is most likely to be a network solid

a)   A         b)   B         c)   C         d)   D

26   Which substance is most likely to be a metal

a)   A         b)   B         c)   C         d)   D

27   The number of moles of nitrogen gas present in 21 g of the gas is

a)   0.67      b)   0.75      c)   1.3      d)   1.5

28   The density of carbon dioxide gas (relative molecular mass 44) 
     at STP is

a)  0.509 g/L     b)  0.986 g/L     c)  1.79 g/L      d)  1.96 g/L


29 The concentration of NaOH in an aqueous solution containing 
   4.0 g of NaOH dissolved in 100 mL of solution is


30 Scientists prefer to measure quantities per mole rather than per 
   gram because    

a) one mole of any substance has the same mass as a mole of any other
   substance
b) the gram is too small a unit to be used in the laboratory
c) a mole of any substance contains the same number of particles as a 
   mole of any other substance
d) a mole of any substance has the same volume as any other substance
   measured at STP.




Part B. Answer all questions in this section in the blank spaces 
        provided.
          

1.   Name ANY FIVE of the following compounds.  (l mark each).


a)  H2SO3(aq) __________________   b)  (NH4)2SO4 ______________________


c)  Fe(OH)3   __________________   d)  Zn(CH3CO2)2  ________________

5

e)  SF6 ________________________   f)  Ca(ClO)2  ____________________


g)  Cu(NO3)2.6H2O  ___________________________________________



2.   Write the formula for ANY FIVE of the following compounds.

a)   lead(II) phosphate             ______________

b)   potassium chlorate             ______________

c)   tetraphosphorus heptasulphide  ______________

5
d)   nitrous acid                   ______________      

e)   magnesium hydrogen carbonate   ______________

f)   sodium periodate               ______________

g)   barium hydroxide octahydrate   ______________


                        Part B is continued on page 6.


                            ANSWERS TO PART "A".                                                         

Answer each of the questions in Part A by writing the letter that 
corresponds to the most correct answer in each case in the brackets          
provided.    USE CAPITAL (UPPER CASE) LETTERS ONLY.

                            PART A.

1 (  )    2 (  )    3 (  )    4 (  )    5 (  )    6 (  )    7 (  )

8 (  )    9 (  )   10 (  )   11 (  )   12 (  )   13 (  )   14 (  )

15 (  )   16 (  )   17 (  )   18 (  )   19 (  )   20 (  )   21 (  )

22 (  )   23 (  )   24 (  )   25 (  )   26 (  )   27 (  )   28 (  )

29 (  )   30 (  )


.
3. Write a balanced equation to represent each of the following 
  reactions.

a) The formation of a precipitate when aqueous solutions of                 
   calcium nitrate and aluminum sulphate are mixed.

3
    _______________________________________________________________


b) The formation of carbon dioxide by the reaction of hydrochloric
   acid on marble (calcium carbonate).

3
    _______________________________________________________________



4. Draw an electron dot (Lewis) diagram for the following molecules:-


   a)   NF3                            b)   O2             



4


5. Draw Lewis structures (line representation) for molecules of:-      


   a)  Ethylene  CH2CH2                       b)   HCN


4


     

PLEASE NOTE.  IN QUESTIONS 6, 7 AND 8 THERE IS CHOICE.
              DO ONLY THE NUMBER OF QUESTIONS ASKED FOR.             
              EXTRA ANSWERS WILL NOT BE MARKED SO BE SURE TO       
              CROSS OUT ALL BUT THE SELECTIONS YOU WISH MARKED.


6. Answer any FOUR of the following questions.  (2 marks each).


a) In volumetric analysis the "Stoichiometric Point" and the "End 
   Point" of a titration are rarely the same. Explain why this is so.


b) How does the pH scale enable us to assess the acidity or the 
   basicity of an aqueous solution?


8 






.
c) Equal volumes of acid A and acid B,  both at the same 
   concentration,
   were tested with a conductivity apparatus.   The light bulb glowed 
   brightly with acid B and only dimly for acid A.   Comment on the 
   relative strength of these two acids.  Explain the observations.
   




d) If a bottle of ammonia was spilled in a room its odour would
   eventually be detected throughout the room.   Explain this 
   observation in terms of kinetic molecular theory.                    













e) How is water, a molecular substance, able to interact with, and
   dissolve, ionic solids?













f) Explain the difference between temperature and heat.
   Illustrate your answer with an everyday example.











g) What one feature of an element is the most important in deciding 
   on 
   its placement in a "Chemical Family"?    Explain how this feature 
   is illustrated in the "Alkali Metal" family.









.
h) If a half filled flask of water is sealed does the process of 
   evaporation stop? Explain your answer.











 
7. Clearly explain ANY THREE of the following statements on the
   basis of          
   chemical and physical concepts introduced in this years' course.
   (3 marks each).

a) H2O and CO2 are both triatomic molecules, however, the H2O 
   molecule
   is highly polar whereas the CO2 molecule is not.











b) HOCl is acidic in aqueous solution but NaOH is basic when dissolved
   in water.




9 






c) Adding crushed limestone (CaCO3) to lakes that have become acidified
   by acid rain can raise the pH of the water.












d) Gasoline contains a very small amount of compounds of nitrogen but
   the emissions from automobile exhausts cause significant amounts of
   polluting oxides of nitrogen.










.
e) Why does the air that escapes from a car tire have a lower 
   temperature than the air that is still in the tire but under pressure?









f) Substances which are not ionic are often soft and pliable.









8. Calculate ANY FOUR of the following, showing all the steps 
   involved in the calculation.  (2 marks each).

a) If a mixture containing 100 mL of propane (C3H8) and 1000 mL of 
   oxygen is ignited and returned to room temperature and pressure 
   what gases will remain and what volume will each gas occupy?                                 

     Equation.    C3H8    +    5O2        3CO2    +    4H2O.











b) What volume of oxygen,  measured at STP,  is produced by the 
   electrolytic decomposition of l kmol of Al2O3?

      Equation.           2Al2O3       4Al   +   3O2
 



8




c) What is the mass of 5.0 L of freon-11 (CFCl3) measured at STP?










d) What is the concentration of KOH in mol/L if 22.44 g of KOH is
   dissolved in enough water to make exactly 2 L of solution?






e) The density of a gas is 2.41 g/L at STP what is the molecular 
   mass of the gas?









 
f) A scuba diver's tank has a volume of about 13 L. When fully 
   charged with compressed air the pressure of the air in the tank 
   is about 150 times greater than atmospheric pressure. When the 
   air in the tank is released at atmospheric pressure and constant 
   temperature what will be the volume of the air?














9. A welder's tank of compressed acetylene (C2H2) contains 3000 g of
   fuel.
   
a) Calculate the mass of oxygen required for the complete combustion of
   all the acetylene in the tank given the following equation for the
   reaction.          

     2C2H2(g)  +    5O2(g)        4CO2(g)   +   2H2O(g)
     
     Clearly set out all steps in your calculation.






3










b) What volume of carbon dioxide will be produced at 900oC and 
   101.3kPa? Clearly show all steps in your calculation.
          



3
 
