Chemistry: The Molecular Nature of Matter and Change
Chemistry: The Molecular Nature of Matter and Change
8th Edition
ISBN: 9781259631757
Author: Martin Silberberg Dr., Patricia Amateis Professor
Publisher: McGraw-Hill Education
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Chapter 2, Problem 2.96P

(a)

Interpretation Introduction

Interpretation:

The formulas for ammonium and ammonia are to be determined.

Concept introduction:

Covalent bonds are formed by the sharing of electrons between two or more atoms. In covalent bonding, there is a mutual attraction between two nuclei and the two electrons that reside between them. The elements that engage in covalent bond formation are present at the rightmost corner of the periodic table. These elements are non-metals. The interaction between two non-metal elements leads to the formation of a covalent bond.

(a)

Expert Solution
Check Mark

Answer to Problem 2.96P

The formula for ammonia is NH3. The formula for ammonium is NH4+.

Explanation of Solution

Ammonia is a covalent compound in which three hydrogen atoms are covalently bonded to a nitrogen atom. It is denoted by the molecular formula NH3.

The ammonium ion is a molecule of ammonia in which one hydrogen ion H+ is added as follows:

NH3+H+NH4+

The difference between ammonia and ammonium is, while the former is a neutral molecule, the latter is an ion with +1 charge.

Conclusion

The formula for ammonia is NH3. The formula for ammonium is NH4+.

(b)

Interpretation Introduction

Interpretation:

The formulas for magnesium sulfide, magnesium sulfite, and magnesium sulfate are to be determined.

Concept introduction:

The general rules for naming ionic compounds are as follows:

1) In ionic compounds, the cations are named before the anions.

2) In binary ionic compounds, the name of the cation is the same as the name of the metal. The name of the anion includes the root name of the non-metal and a suffix -ide.

3) In polyatomic ions in which a non-metal is bonded to one or more oxygen atoms. In two oxoanions in the family, the ion with fewer oxygen atoms has the non-metal root name and a suffix -ite added to it whereas the ion with more oxygen atoms has the non-metal root name and the suffix -ate added to it.

(b)

Expert Solution
Check Mark

Answer to Problem 2.96P

The formula for magnesium sulfide is MgS. The formulas for magnesium sulfite and magnesium sulfate are MgSO3 and MgSO4 respectively.

Explanation of Solution

Magnesium sulfide is a binary ionic compound. It is formed as follows:

Mg2++S2MgS

The sulfide ion is represented by the formula S2. The 2 charge on the sulfide ion is balanced by a magnesium ion. Magnesium belongs to the 2A(2) group in the periodic table, therefore on losing two electrons the charge on the magnesium ion is +2. Therefore the formula for magnesium sulfide is MgS.

Sulfate and sulfite are polyatomic oxoanions. The charge on both sulfate and sulfite is 2 on each. In oxoanions, the ion with fewer oxygen atoms has the non-metal root name and a suffix -ite added to it whereas the ion with more oxygen atoms has the non-metal root name and the suffix -ate added to it. Therefore the formulas for sulfate and sulfite are SO42 and SO32 respectively.

The formation of magnesium sulfate and magnesium sulfite occur as follows:

Mg2++SO42MgSO4

Mg2++SO32MgSO3

The 2 charge on the sulfate and sulfite ions are balanced by a magnesium ion with +2 charge. Therefore the formulas for magnesium sulfate and magnesium sulfite are MgSO4 and MgSO3 respectively.

Conclusion

The formula for magnesium sulfide is MgS. The formulas for magnesium sulfite and magnesium sulfate are MgSO3 and MgSO4 respectively.

(c)

Interpretation Introduction

Interpretation:

The formulas for hydrochloric acid, chloric acid, and chlorous acid are to be determined.

Concept introduction:

The general formula for naming binary acids is,

Prefix hydro-+non-metal root+suffix -ic+acid

The general rules for naming the members of a family with four oxoanions are as follows:

1) The anion with the most number of oxygen atoms has the refix per-, the non-metal root and the suffix -ate.

2) The anion with one fewer oxygen atom has the non-metal root and the suffix -ate.

3) The anion with two fewer oxygen atoms has the non-metal root and the suffix -ite.

4) The anion with three fewer oxygen atoms has the prefix hypo-, the non-metal root, and the suffix -ite.

(c)

Expert Solution
Check Mark

Answer to Problem 2.96P

The formula for hydrochloric acid is HCl. The formulas for chloric and chlorous acids are HClO3 and HClO2 respectively.

Explanation of Solution

Hydrochloric acid is a binary acid formed by the association of a hydrogen ion with +1 charge and chloride ion with 1 charge as follows:

H++ClHCl

Therefore the formula for hydrochloric acid is HCl.

The oxoanions of chlorine are ClO, ClO2, ClO3, ClO4

The anion ClO4 has the most number of oxygen atoms. Therefore it is the perchlorate ion. The anion ClO3 has one fewer oxygen atom, therefore it is the chlorate ion. The anion ClO2 is the chlorite ion and the anion ClO is the hypochlorite ion.

In the ion chlorate, the root name chlor denotes the non-metal chlorine (Cl). The formula for chlorate ion is ClO3. On associating with a hydrogen ion with +1 charge, the formation of chloric acid occurs as follows:

ClO3+H+HClO3

The suffix -ate in the anion chlorate is replaced by the suffix -ic

In the ion chlorite, the root name chlor denotes the non-metal chlorine (Cl). The formula for chlorite ion is ClO2. On associating with a hydrogen ion with +1 charge, the formation of chlorous acid occurs as follows:

ClO2+H+HClO2

The suffix -ite in the anion chlorite is replaced by the suffix -ous.

Therefore the formulas for chloric and chlorous acids are HClO3 and HClO2 respectively.

Conclusion

The formula for hydrochloric acid is HCl. The formulas for chloric and chlorous acids are HClO3 and HClO2 respectively.

(d)

Interpretation Introduction

Interpretation:

The formulas for cuprous bromide and cupric bromide are to be determined.

Concept introduction:

The general rules for naming ionic compounds with different charges on the same metal are:

1) The root name of the metal is followed by the suffix -ous for the ion with a lower charge.

2)The root name of the metal is followed by the suffix -ic for the ion with a higher charge.

(d)

Expert Solution
Check Mark

Answer to Problem 2.96P

The formulas for cuprous bromide and cupric bromide are CuBr and CuBr2 respectively.

Explanation of Solution

The element bromine belongs to the 7A(17) group in the periodic table. Therefore, an atom of bromine has the tendency to gain an electron to form a bromide ion as follows:

Br+eBr

The two ions formed by the copper element are Cu+ and Cu2+. The Cu+ ion has one fewer charge on it. Therefore it is the cuprous ion. The Cu2+ ion is the cupric ion.

To balance the +1 charge on the cuprous ion, one bromide ion with 1 charge combines with it to form the molecule of cuprous bromide as follows:

Cu++BrCuBr

To balance the Chemistry: The Molecular Nature of Matter and Change, Chapter 2, Problem 2.96P charge on the cupric ion, two bromide ions associate with one cupric ion to form the molecule of cupric bromide as follows:

Cu2++2BrCuBr2

Conclusion

The formulas for cuprous bromide and cupric bromide are CuBr and CuBr2 respectively.

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Chapter 2 Solutions

Chemistry: The Molecular Nature of Matter and Change

Ch. 2.5 - Prob. B2.1PCh. 2.5 - Prob. B2.2PCh. 2.6 - Prob. 2.6AFPCh. 2.6 - Prob. 2.6BFPCh. 2.7 - Prob. 2.7AFPCh. 2.7 - Prob. 2.7BFPCh. 2.8 - Prob. 2.8AFPCh. 2.8 - Prob. 2.8BFPCh. 2.8 - Prob. 2.9AFPCh. 2.8 - Prob. 2.9BFPCh. 2.8 - Prob. 2.10AFPCh. 2.8 - Prob. 2.10BFPCh. 2.8 - Prob. 2.11AFPCh. 2.8 - Prob. 2.11BFPCh. 2.8 - Prob. 2.12AFPCh. 2.8 - Prob. 2.12BFPCh. 2.8 - Prob. 2.13AFPCh. 2.8 - Prob. 2.13BFPCh. 2.8 - Prob. 2.14AFPCh. 2.8 - Prob. 2.14BFPCh. 2.8 - Prob. 2.15AFPCh. 2.8 - Prob. 2.15BFPCh. 2.8 - Prob. 2.16AFPCh. 2.8 - Prob. 2.16BFPCh. 2.8 - Determine the name, formula, and molecular (or...Ch. 2.8 - Prob. 2.17BFPCh. 2.9 - Prob. B2.3PCh. 2 - Prob. 2.1PCh. 2 - List two differences between a compound and a...Ch. 2 - Which of the following are pure substances?...Ch. 2 - Classify each substance in Problem 2.3 as an...Ch. 2 - Explain the following statement: The smallest...Ch. 2 - Prob. 2.6PCh. 2 - Can the relative amounts of the components of a...Ch. 2 - Prob. 2.8PCh. 2 - Prob. 2.9PCh. 2 - Prob. 2.10PCh. 2 - Prob. 2.11PCh. 2 - Prob. 2.12PCh. 2 - In our modern view of matter and energy, is the...Ch. 2 - Prob. 2.14PCh. 2 - Which of the following scenes illustrate(s) the...Ch. 2 - Prob. 2.16PCh. 2 - Prob. 2.17PCh. 2 - Prob. 2.18PCh. 2 - Prob. 2.19PCh. 2 - Fluorite, a mineral of calcium, is a compound of...Ch. 2 - Prob. 2.21PCh. 2 - Prob. 2.22PCh. 2 - Prob. 2.23PCh. 2 - Prob. 2.24PCh. 2 - Prob. 2.25PCh. 2 - Prob. 2.26PCh. 2 - Prob. 2.27PCh. 2 - Dolomite is a carbonate of magnesium and calcium....Ch. 2 - Prob. 2.29PCh. 2 - Which of Dalton’s postulates about atoms are...Ch. 2 - Use Dalton’s theory to explain why potassium...Ch. 2 - Prob. 2.32PCh. 2 - The following charges on individual oil droplets...Ch. 2 - Prob. 2.34PCh. 2 - When Rutherford’s coworkers bombarded gold foil...Ch. 2 - Prob. 2.36PCh. 2 - Prob. 2.37PCh. 2 - Prob. 2.38PCh. 2 - Prob. 2.39PCh. 2 - Prob. 2.40PCh. 2 - Prob. 2.41PCh. 2 - Prob. 2.42PCh. 2 - Write the notation for each atomic depiction: Ch. 2 - Write the notation for each atomic depiction: Ch. 2 - Draw atomic depictions similar to those in Problem...Ch. 2 - Prob. 2.46PCh. 2 - Prob. 2.47PCh. 2 - Prob. 2.48PCh. 2 - Chlorine has two naturally occurring isotopes,...Ch. 2 - Prob. 2.50PCh. 2 - Prob. 2.51PCh. 2 - Prob. 2.52PCh. 2 - Prob. 2.53PCh. 2 - Prob. 2.54PCh. 2 - Prob. 2.55PCh. 2 - Prob. 2.56PCh. 2 - Prob. 2.57PCh. 2 - Prob. 2.58PCh. 2 - Prob. 2.59PCh. 2 - Prob. 2.60PCh. 2 - Prob. 2.61PCh. 2 - Prob. 2.62PCh. 2 - Prob. 2.63PCh. 2 - Prob. 2.64PCh. 2 - Prob. 2.65PCh. 2 - Prob. 2.66PCh. 2 - Prob. 2.67PCh. 2 - Prob. 2.68PCh. 2 - Prob. 2.69PCh. 2 - Prob. 2.70PCh. 2 - What monatomic ions would you expect radium (Z =...Ch. 2 - Prob. 2.72PCh. 2 - Prob. 2.73PCh. 2 - Prob. 2.74PCh. 2 - Prob. 2.75PCh. 2 - The radii of the sodium and potassium ions are 102...Ch. 2 - Prob. 2.77PCh. 2 - What information about the relative numbers of...Ch. 2 - Prob. 2.79PCh. 2 - Prob. 2.80PCh. 2 - Prob. 2.81PCh. 2 - Prob. 2.82PCh. 2 - Prob. 2.83PCh. 2 - Prob. 2.84PCh. 2 - Prob. 2.85PCh. 2 - Prob. 2.86PCh. 2 - Prob. 2.87PCh. 2 - Prob. 2.88PCh. 2 - Give the systematic names for the formulas or the...Ch. 2 - Prob. 2.90PCh. 2 - Prob. 2.91PCh. 2 - Prob. 2.92PCh. 2 - Prob. 2.93PCh. 2 - Prob. 2.94PCh. 2 - Prob. 2.95PCh. 2 - Prob. 2.96PCh. 2 - Prob. 2.97PCh. 2 - Prob. 2.98PCh. 2 - Prob. 2.99PCh. 2 - Prob. 2.100PCh. 2 - Prob. 2.101PCh. 2 - Prob. 2.102PCh. 2 - Prob. 2.103PCh. 2 - Prob. 2.104PCh. 2 - Prob. 2.105PCh. 2 - Prob. 2.106PCh. 2 - Prob. 2.107PCh. 2 - Prob. 2.108PCh. 2 - Prob. 2.109PCh. 2 - Prob. 2.110PCh. 2 - Prob. 2.111PCh. 2 - Prob. 2.112PCh. 2 - What is the difference between a homogeneous and a...Ch. 2 - Prob. 2.114PCh. 2 - Prob. 2.115PCh. 2 - Prob. 2.116PCh. 2 - Which separation method is operating in each of...Ch. 2 - Prob. 2.118PCh. 2 - Prob. 2.119PCh. 2 - Prob. 2.120PCh. 2 - Prob. 2.121PCh. 2 - Prob. 2.122PCh. 2 - Ammonium dihydrogen phosphate, formed from the...Ch. 2 - Prob. 2.124PCh. 2 - Prob. 2.125PCh. 2 - Prob. 2.126PCh. 2 - Prob. 2.127PCh. 2 - Prob. 2.128PCh. 2 - The following scenes represent a mixture of two...Ch. 2 - Prob. 2.130PCh. 2 - Prob. 2.131PCh. 2 - Prob. 2.132PCh. 2 - Prob. 2.133PCh. 2 - Prob. 2.134PCh. 2 - Prob. 2.135PCh. 2 - Prob. 2.136PCh. 2 - Prob. 2.137PCh. 2 - Prob. 2.138PCh. 2 - Prob. 2.139PCh. 2 - Prob. 2.140PCh. 2 - Prob. 2.141PCh. 2 - Prob. 2.142PCh. 2 - Prob. 2.143PCh. 2 - Prob. 2.144P
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