
Interpretation:
The chemical formula for the given compounds isto be written.
Concept introduction:
The naming of a chemical compound is based on the charges of the cations and anions. For naming ionic compounds, the name of the cation is written after the name of ananion.
To form a compound from the given anion and cation, first identify the charges on thecation and the anion, as chargestransfer to the subscript of the other ion, which means the charge on the cation transfers to the subscript of the anion and the charge of the anion goes to the subscript of the cation.

Answer to Problem 84QP
Solution:
(a) CuCN
(b) Sr(ClO2)2
(c) HBrO4
(d) HI
(e) Na2(NH4)PO4
(f) KH2PO4
(g) IF7
(h) P4S10
(i) HgO
(j) Hg2I2
(k) SeF6
Explanation of Solution
a) Copper (I) cyanide
The copper (I) cation has a charge of +1 always, and the cyanide anion, CN-, has a charge of −1.
So, the compoundcopper (I) cyanide is formed from the cation Cu+ and the anion CN-, the charge of copper (I) transfers to the subscript of cyanide and charge of cyanide goes to the subscript of copper (I) and the ions combine in a ratio of one-to-one. Therefore, the correct formula for compoundcopper (I) cyanideis CuCN.
Hence, the formula for copper (I) cyanide is CuCN.
b) Strontium Chlorite
The strontium cation has charge of +2 and chlorite anion has charge of −1.
So, the compoundstrontium chlorite is formed from the cation Sr+2 and the anion ClO-2. The charge of strontium goes to the subscript of chlorite and the charge of chlorite transfers to the subscript of strontium and the correct formula of the compound strontium chlorite is Sr(ClO2)2.
Hence, the formula for strontium chlorite is Sr(ClO2)2.
c)Perbromic acid
The compoundperbromic acidis formed from bromium oxide and hydrogen. Therefore, formula ofperbromic acidis HBrO4.
Hence, the formula for perbromic acidis HBrO4.
d) Hydroiodic acid
The hydrogen cation has a charge of +1 always, and the iodine anion has a charge of −1.
So, the compoundhydroiodic acidis formed from cation H+ and anion I-. The charge of hydrogentransfers to the subscript of iodine and charge of iodine goes to the subscript of hydrogen, which makes the formula of the compoundhydroiodic acidto be HI.
Hence, the formula for hydroiodic acidis HI.
e) Disodium ammonium phosphate
The compounddisodium ammonium phosphate is formed fromsodiumNa+ cation and ammonium phosphate (NH4)PO42- anion. There is a disodium ion present, which means there are two sodium atoms and ammonium phosphate present, which makes the formula of the compounddisodium ammonium phosphateto be Na2(NH4)PO4.
Hence, the formula for disodium ammonium phosphateis Na2(NH4)PO4.
f) Potassium dihydrogen phosphate
The compoundpotassium dihydrogen phosphateis formed from the potassium K+ cationand the hydrogen phosphate anion. The formula of the compoundpotassium dihydrogen phosphateis KH2PO4.
Hence, the formula for potassium dihydrogen phosphateis KH2PO4.
g) Iodine heptafluoride
The compoundiodine heptafluoride is formed from iodine and fluorine. There is an iodine atom present and heptafluoride means there are seven fluoride atoms present, which makes the formula of the compoundiodine heptafluorideto be IF7.
Hence, the formula for iodine heptafluorideis IF7.
h)Tetra phosphorous decasulfide.
The compoundtetra phosphorous decasulfideis formed from the phosphorus cation and the sulphur anion. There are tetra phosphorus present, which means there are four phosphorus atoms and decasulfide means there are10sulfur atoms are present, which makes the formula of the compoundtetra phosphorous decasulfideto be P4S10.
Hence, the formula for tetra phosphorous decasulfideis P4S10.
i) Mercury (II) oxide
The mercury cation has a charge of +2 always and the iodide anion has a charge of −1.
Mercury (II) oxideis formed from the cation Hg2+ and the anion O2-. The charges of the cation and anion negate each other as it is the same and the charge of mercury transfers to the subscript of oxide and the charge of oxidetransfers to the subscript of mercury, which makes the formula of the compoundmercury (II) oxideto be HgO.
Hence, the formula for mercury (II) oxideis HgO.
j) Mercury (I) iodide
The mercurycation has a charge of +2 always, and the iodide anion has a charge of −1.
So, mercury (I) iodide is formed from the cation Hg2+ and the anion I2-. The charge of mercury transfers to the subscript of iodide and the charge of iodide transfers to the subscript of mercury, which makes the formula of the compoundmercury (I) iodideto be Hg2I2.
Hence, the formula for mercury (I) iodideis Hg2I2.
k)Selenium hexafluoride
The selenium cation has a charge of +6 always, and the fluoride anion F− has a charge of −1.
So, the selenium hexafluoride is formed from the cation Se6+ and the anion F−. The charge of selenium goes to the subscript of fluoride and the charge of fluoridetransfers to the subscript of selenium, which makes the formula of the compoundselenium hexafluorideto be SeF6.
Hence, the formula for selenium hexafluorideis SeF6.
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Chapter 2 Solutions
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