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Chapter 22: Problem 119

Explain the important distinctions between each pair of terms: (a) acid salt and acid anhydride; (b) azide and nitride; (c) white phosphorus and red phosphorus; (d) ionic hydride and metallic hydride.

Short Answer

Expert verified
Acid salts are formed by partially replacing the replaceable hydrogen atoms of an acid molecule, while Acid anhydrides are dehydrated acids. Azides contain the group -N3 and Nitrides are compounds of nitrogen with less electronegative elements. White phosphorus is a reactive solid and red phosphorus is a non-toxic solid used where a controlled ignition is required. Ionic hydrides have hydrogen bonded with a more electropositive element so it has a charge of -1, while Metallic hydrides are formed with transition metals where hydrogen present doesn't have charge of -1.

Step by step solution

01

Understand Acid Salt vs Acid Anhydride

An acid salt is a type of salt which is formed by partial replacement of replaceable hydrogen atoms of an acid molecule. On the other hand, Acid anhydrides are compounds that provide an acid when combined with water. They are technically 'dehydrated acids' and can convert back into acids by absorbing water. Acid Anhydrides are generally formed by removing water from an acid.
02

Understand Azide vs Nitride

Azides are compound containing the group -N3 or individual ions carrying a charge of -1/3. In terms of resonance, azides can be described as a resonance hybrid of two structures. Nitrides on the other hand, are binary compounds of nitrogen with less electronegative elements – elements from the first three groups of the periodic table. For example: Sodium Nitride (Na3N) , Aluminum Nitride (AlN).
03

Understand White Phosphorus vs Red Phosphorus

White phosphorus and red phosphorus are different forms of phosphorus, known as allotropes. White phosphorus is a waxy, highly reactive solid that is typically stored in water to prevent it from spontaneously combusting in the air. Red phosphorus, on the other hand, is an amorphous non-toxic solid that is used in matches, pyrotechnics, and other applications where a controlled ignition is required.
04

Understand Ionic Hydride vs Metallic Hydride

Ionic hydrides are compounds in which hydrogen is bonded with a more electropositive element so that it exhibits a charge of -1. Metallic hydrides are formed with transition metals. In these types of hydrides, the hydrogen is present in 'interstitial sites' in the metal lattice and does not have a charge of -1. Instead, they feature delocalised electrons (like metallic bonding).

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Most popular questions from this chapter

Explain why the volumes of \(\mathrm{H}_{2}(\mathrm{g})\) and \(\mathrm{O}_{2}(\mathrm{g})\) obtained in the electrolysis of water are not the same.

On the basis of molecular orbital theory, would you expect \(\mathrm{NH}_{2}^{+}\) to be linear or bent?

Two of the following, through a reaction occurring in a weakly acidic solution, produce the same gaseous product. They are (a) \(\mathrm{CaH}_{2}(\mathrm{s}) ;\) (b) \(\mathrm{Na}_{2} \mathrm{O}_{2}(\mathrm{s})\) (c) \(\mathrm{NaOH}(\mathrm{s}) ;(\mathrm{d}) \mathrm{Al}(\mathrm{s}) ;(\mathrm{e}) \mathrm{NaHCO}_{3}(\mathrm{s}) ;(\mathrm{f}) \mathrm{N}_{2} \mathrm{H}_{4}(1)\).

Use information from this chapter and previous chapters to write plausible chemical equations to represent the following: (a) the reaction of silver metal with \(\mathrm{HNO}_{3}(\mathrm{aq})\) (b) the complete combustion of the rocket fuel, unsymmetrical dimethylhydrazine, \(\left(\mathrm{CH}_{3}\right)_{2} \mathrm{NNH}_{2}\) (c) the preparation of sodium triphosphate by heating a mixture of sodium dihydrogen phosphate and sodium hydrogen phosphate.

Which of the following reactions are likely to go to completion or very nearly so? (a) \(\mathrm{H}_{2} \mathrm{O}_{2}(\mathrm{aq})+2 \mathrm{I}^{-}(\mathrm{aq})+2 \mathrm{H}^{+}(\mathrm{aq}) \longrightarrow\) \(\mathrm{I}_{2}(\mathrm{s})+2 \mathrm{H}_{2} \mathrm{O}(1)\) (b) \(\mathrm{O}_{2}(\mathrm{g})+2 \mathrm{H}_{2} \mathrm{O}(1)+4 \mathrm{Cl}^{-}(\mathrm{aq}) \stackrel{-}{\longrightarrow}\) \(2 \mathrm{Cl}_{2}(\mathrm{g})+4 \mathrm{OH}^{-}(\mathrm{aq})\) (c) \(\mathrm{O}_{3}(\mathrm{g})+\mathrm{Pb}^{2+}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\mathrm{l}) \longrightarrow\) \(\mathrm{PbO}_{2}(\mathrm{s})+2 \mathrm{H}^{+}(\mathrm{aq})+\mathrm{O}_{2}(\mathrm{g})\) (d) \(\mathrm{HO}_{2}^{-}(\mathrm{aq})+2 \mathrm{Br}^{-}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\mathrm{l}) \longrightarrow\) \(3 \mathrm{OH}^{-}(\mathrm{aq})+\mathrm{Br}_{2}(1)\)
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