General Chemistry Principles, Patterns, and Applications, 2011

S T R U C T U R E A N D R E A C T I V I T Y
1. PF 3 reacts with F 2 to produce PF 5 , which in turn reacts with F − to give salts that contain the PF − 6 ion. In
contrast, NF 3 does not react with F 2 , even under extreme conditions; NF 5 and the NF − 6 ion do not exist. Why?
2. Red phosphorus is safer to handle than white phosphorus, reflecting their dissimilar properties. Given their
structures, how do you expect them to compare with regard to reactivity, solubility, density, and melting
point?
3. Bismuth oxalate [Bi 2 (C 2 O 4 ) 3 ] is a poison. Draw its structure and then predict its solubility in H 2 O, dilute HCl,
and dilute HNO 3 . Predict its combustion products. Suggest a method to prepare bismuth oxalate from
bismuth.
4. Small quantities of NO can be obtained in the laboratory by reaction of the iodide ion with acidic solutions of
nitrite. Write a balanced chemical equation that represents this reaction.
5. Although pure nitrous acid is unstable, dilute solutions in water are prepared by adding nitrite salts to
aqueous acid. Write a balanced chemical equation that represents this type of reaction.
6. Metallic versus nonmetallic behavior becomes apparent in reactions of the elements with an oxidizing acid,
such as HNO 3 . Write balanced chemical equations for the reaction of each element of group 15 with nitric
acid. Based on the products, predict which of these elements, if any, are metals and which, if any, are
nonmetals.
7. Predict the product(s) of each reaction and then balance each chemical equation.
a. P 4 O 10 (s) + H 2 O(l) →
b. AsCl 3 (l) + H 2 O(l) →
c. Bi 2 O 3 (s) + H 2 O(l) →
d. Sb 4 O 6 (s) + OH − (aq) →
e. a. C 2
H 5
( ) 3
Sb( l) + O 2 ( g) - ® D
f. SbCl 3 (s) + LiAlH 4 (soln) →
8. a. Ca s
( ) + N 2
O( g) - ® D
9. Write a balanced chemical equation to show how you would prepare each compound.
a. H 3 PO 4 from P
b. Sb 2 O 5 from Sb
c. SbH 3 from Sb
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