Each question is followed by up to five lettered responses (A-E). For each question choose the response which is the best answer to the question.

1. From the following table of ionisation energies deduce which element is most likely to form M3+ ions in the gaseous phase.
                                                Ionisation energy /kJ mol-1
   

   Elements

   1st

   2nd

   3rd

   
   
   1.   ?                  502        4560          6918
   2.   ?                  748         1463            7741
   3.   ?                  558          1827         2759
   4.   ?                  1003        2261          3432
   5.   ?                   422        3060       4431

2. Five ionisation energies (in kJ mol-1) are listed:
        830      872       1100       1178       376
   Which one of the following could have such values?
   

   1.   ?    the first ionisation energies for the elements from GroupsV, VI, VII, 0 and I
   2.   ?    the first ionisation energies for elements with atomic numbers 1-5
   3.   ?    successive ionisation energies for boron
   4.   ?    the first ionisation energies for the elements in Group I starting with lithium

3. Which one of the following does not affect the first ionisation energy of an atom?
   

   1.   ?    atomic radius
   2.   ?    electronegativity
   3.   ?    nuclear charge
   4.   ?    shielding

4. Which one of the following equations represents the first ionisation energy of potassium?
   

   1.   ?    K(s)   =  K+(s)   +   e-
   2.   ?    K(s)   =   K+(g)   +   e-
   3.   ?    K+(g)   =   K2+(s)   +   e-
   4.   ?    K(g)   =   K+(g)   +   e-

5. Which one of the following has the largest first ionisation energy?
   

   1.   ?    carbon
   2.   ?    fluorine
   3.   ?    neon
   4.   ?     nitrogen

6. The first six successive ionisation energies , in kJ mol^-1, of an element Z are
        590, 1100, 4900, 6500, 8100 and 10500.
   Which ion is formed when Z reacts with chlorine?
   

   1.   ?    Z⁺
   2.   ?    Z²⁺
   3.   ?    Z^-
   4.   ?    Z^2-

7. Which one of the following equations represents the second ionisation energy of chlorine?
   

   1.   ?    Cl(g)   =   Cl²⁺ (g)   +   2e^-
   2.   ?    Cl(g)   +   2e^-   =   Cl^2- (g)
   3.   ?    Cl^-(g)   =   Cl^2-(g)   +  e^-
   4.   ?    Cl⁺(g)   =  Cl²⁺(g)   +   e^-

8. In which one of the following series of elements is there the smallest variation in the value of the first ionisation energy?
   

   1.   ?     K to Br
   2.   ?    Sc to Zn
   3.   ?     Li to F
   4.   ?     F to I

9. The first six ionisation energies of an element Y are as follows:
           786, 1580, 3230, 4360, 16 000, 20 000 kJ mol^-1
   Which one of the following statements is consistent with these data?
   

   1.   ?    The chemistry of Y and its compounds is similar to that of aluminium and its compounds.
      
   2.   ?     Y forms a chloride with the molecular formula YCl
   3.   ?    The outer electronic configuration of an atom of Y is ns²np²
   4.   ?     Y is in Group I of the Periodic Table.
      

10. The first ionisation energy for carbon is greater than it is for sodium. One of the factors responsible is that the
    

    1.   ?     shielding provided by the inner quantum shells of sodium is greater
    2.   ?     outer quantum shell is further from the nucleus in carbon atoms than in sodium atoms
    3.   ?     nuclear charge on carbon is greater
    4.   ?     number of electrons in the outer quantum shell of carbon is greater than in sodium
       

11. An element has successive ionisation energies of 99, 1800, 14800 and 21000 kJ mol^-1.
    To which group of the Periodic Table does the element belong?
    

    1.   ?    IV
    2.   ?    III
    3.   ?    I
    4.   ?    II

12. The first four ionisation energies of an element Z are;
          738, 1451, 7733 and 10541 kJ mol^-1.
    Which one of the following ions is most likely to be formed when Z reacts with fluorine?
    

    1.   ?     Z⁺
    2.   ?    Z³⁺
    3.   ?     Z²⁺
    4.   ?     Z⁴⁺