(a)
Interpretation:
To determine the name of binary ionic compound BeO.
Concept Introduction:
The naming of the ionic compound takes place in the way that the name of metal cation will remain same to that of metal while for anion the name of negative charged species end with suffix ‘ate’ for the case of elements such as P, S etc and name of negative charged species end with suffix ‘ide’ for the case of elements such as halides.
(b)
Interpretation:
To determine the name of binary ionic compound MgI2.
Concept Introduction:
The naming of the ionic compound takes place in the way that the name of metal cation will remain same to that of metal while for anion the name of negative charged species end with suffix ‘ate’ for the case of elements such as P, S etc and name of negative charged species end with suffix ‘ide’ for the case of elements such as halides.
(c)
Interpretation:
To determine the name of binary ionic compound Na2 S.
Concept Introduction:
The naming of the ionic compound takes place in the way that the name of metal cation will remain same to that of metal while for anion the name of negative charged species end with suffix ‘ate’ for the case of elements such as P, S etc and name of negative charged species end with suffix ‘ide’ for the case of elements such as halides.
(d)
Interpretation:
To determine the name of binary ionic compound Al2 O3.
Concept Introduction:
The naming of the ionic compound takes place in the way that the name of metal cation will remain same to that of metal while for anion the name of negative charged species end with suffix ‘ate’ for the case of elements such as P, S etc and name of negative charged species end with suffix ‘ide’ for the case of elements such as halides.
(e)
Interpretation:
To determine the name of binary ionic compoundHCl.
Concept Introduction:
The naming of the ionic compound takes place in the way that the name of metal cation will remain same to that of metal while for anion the name of negative charged species end with suffix ‘ate’ for the case of elements such as P, S etc and name of negative charged species end with suffix ‘ide’ for the case of elements such as halides.
(f)
Interpretation:
To determine the name of binary ionic compoundLiF.
Concept Introduction:
The naming of the ionic compound takes place in the way that the name of metal cation will remain same to that of metal while for anion the name of negative charged species end with suffix ‘ate’ for the case of elements such as P, S etc and name of negative charged species end with suffix ‘ide’ for the case of elements such as halides.
(g)
Interpretation:
To determine the name of binary ionic compound Ag2 S.
Concept Introduction:
The naming of the ionic compound takes place in the way that the name of metal cation will remain same to that of metal while for anion the name of negative charged species end with suffix ‘ate’ for the case of elements such as P, S etc. and name of negative charged species end with suffix ‘ide’ for the case of elements such as halides.
(h)
Interpretation:
To determine the name of binary ionic compound CaH2.
Concept Introduction:
The naming of the ionic compound takes place in the way that the name of metal cation will remain same to that of metal while for anion the name of negative charged species end with suffix ‘ate’ for the case of elements such as P, S etc. and name of negative charged species end with suffix ‘ide’ for the case of elements such as halides.
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Chapter 5 Solutions
Introductory Chemistry: A Foundation
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- For the following pairs of ions, use the principle of electrical neutrality to predict the formula of the binary compound that the ions are most likely to form. Na+andS2e.Cu2+andBr K+andClf.Al3+andI Ba2+andO2g.Al3+andO2 Mg2+andSe2h.Ca2+andN3arrow_forwardWrite the formula for each of the following compounds: a. ammonium hydrogen phosphate b. mercury(I) sulfide c. silicon dioxide d. sodium sulfite e. aluminum hydrogen sulfate f. nitrogen trichloride g. hydrobromic acid h. bromous acid i. perbromic acid j. potassium hydrogen sulfide k. calcium iodide l. cesium perchloratearrow_forwardFor the following processes that show the formation of ions, use the periodic table to indicate the number of electrons and protons present in both theionand theneutral atomfrom which the ion is made. a.CaCa2++2e b.P+3eP3 c.Br+eBr d.FeEe3++3e e.AlAl3++3e f.N+3eN3arrow_forward
- Name the compounds in parts ad and write the formulas for the compounds in parts eh. a. NaBr b. Rb2O c. CaS d. AlI3 e. strontium fluoride f. aluminum selenide g. potassium nitride h. magnesium phosphidearrow_forwardName the compounds in parts a-d and write the formulas for the compounds in parts eh. a. Hg2O b. FeBr3 c. CoS d. TiCl4 e. tin(II) nitride f. cobalt(III) iodide g. mercury(II) oxide h. chromium(VI) sulfidearrow_forwardThe formulas MgO and CO look very similar. What is the name for each compound? Why do we name them differently?arrow_forward
- A small crystal of CaCl2 that weighs 0.12 g contains 6.5 1020 formula units of CaCl2. What is the total number of ions (cations and anions) that make up this crystal?arrow_forwardSulfur dioxide, SO2, is a molecular compound that contributes to acid rain, and CaCO3 is an ionic compound that can neutralize acid rain. Explain the difference in the meanings of these two formulas.arrow_forwardThese questions concern the work of J. J. Thomson: From Thomson’s work, which particles do you think he would feel are most important in the formation of compounds (chemical changes) and why? Of the remaining two subatomic particles, which do you place second in importance for forming compounds and why? Come up with three models that explain Thomson’s findings and evaluate them. To be complete you should include Thomson’s findings.arrow_forward
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