Periodic trends questions

Assignment: Question Topic 3.2 : Periodic trends

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1

Explain why the atomic radius of sodium (Z = 11) is bigger than the atomic radius of chlorine (Z = 17).

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2

Explain why the atomic radius of the elements increases upon descending group 17 (F → I).

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3

Suggest how the values for the atomic radii of the noble gases given in Section 9 in the IB Chemistry data booklet have been obtained.

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4

Suggest two reasons why the ionic radius of a sodium ion is much smaller than the atomic radius of a sodium atom.

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5

Three negative ions are the phosphide ion, P3−, the sulfide ion, S2– and the chloride ion, Cl–.
Place these three ions in order of increasing size (smallest first) and explain your logic.

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6

Give the equations for the reaction of water with:

i.  sodium oxide, Na2O.

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ii. magnesium oxide, MgO

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iii. phosphorus(V) oxide, P4O10

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iv. sulfur(VI) oxide, SO3.

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7

Describe and explain (with a relevant equation) what will be observed when chlorine water is added to:
 

i.   a solution of chloride ions.

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ii.  a solution of bromide ions.

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iii. a solution of iodide ions.

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8

State what will be observed when sodium metal is placed in water and give the equation for the reaction.

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9

Suggest one reason why caesium is more reactive than lithium when it is placed in water.

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10

State what will be observed when a piece of warm sodium metal is lowered into in a gas jar containing chlorine gas and give the equation for the reaction.

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11

Aluminium oxide, Al2O3, has a high melting point and it reacts with both hydrochloric acid and sodium hydroxide.
What can be deduced about the chemical nature of aluminium oxide from this information?

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