Ch3 Question 98: For Each Of The Following Compounds, State

Ch3 Question 98 For Each Of The Following Compounds State Whether

Ch3 Question 98: For each of the following compounds, determine whether it is ionic or covalent. If the compound is ionic, write the symbols for the ions involved: (a) KClO4 (b) MgC2H3O2 (c) H2S (d) Ag2S (e) N2Cl4 (f) Co(NO3)2. Additionally, provide the chemical formulas for the following compounds: (a) barium chloride (b) magnesium nitride (c) sulfur dioxide (d) nitrogen trichloride (e) dinitrogen trioxide (f) tin(IV) chloride. Lastly, calculate the mass of HCl contained in 45.0 mL of an aqueous HCl solution with a density of 1.19 g/cm³ and containing 37.21% HCl by mass.

Paper For Above instruction

Introduction

Understanding the nature of chemical compounds and their compositions is fundamental in chemistry. Determining whether a compound is ionic or covalent involves analyzing the types of elements involved and their bonding characteristics. Additionally, accurately writing chemical formulas and calculating quantities such as mass in solutions are essential skills for chemical analysis and laboratory work. This paper addresses the classification of selected compounds as ionic or covalent, the writing of specific chemical formulas, and the calculation of HCl mass in a given solution, illustrating core principles of inorganic chemistry.

Classification of Compounds as Ionic or Covalent

The first step involves evaluating each compound's bonding type, primarily based on element types and their electronegativities. Generally, compounds formed between metals and nonmetals tend to be ionic, with electrons transferred from metal to nonmetal, resulting in positively and negatively charged ions. Conversely, compounds between nonmetals tend to be covalent, sharing electrons through covalent bonds.

(a) KClO4 (potassium perchlorate):

Potassium (K) is a metal, and perchlorate (ClO4⁻) is a polyatomic ion with nonmetals. The bond between K⁺ and ClO4⁻ is ionic, as it involves a metal cation bonding with a polyatomic anion.

Type: Ionic; Ions involved: K⁺ and ClO4⁻

(b) MgC2H3O2 (magnesium acetate):

Magnesium (Mg) is a metal cation, and acetate (C2H3O2⁻) is a polyatomic nonmetal ion. The ionic bond forms between Mg²⁺ and C2H3O2⁻.

Type: Ionic; Ions involved: Mg²⁺ and C2H3O2⁻

(c) H2S (hydrogen sulfide):

Both hydrogen and sulfur are nonmetals. The bond involves sharing electrons, characteristic of covalent bonds.

Type: Covalent

(d) Ag2S (silver sulfide):

Silver (Ag) is a metal, and sulfur is a nonmetal. The compound forms via ionic bonds between Ag⁺ and S²⁻ ions.

Type: Ionic; Ions involved: Ag⁺ and S²⁻

(e) N2Cl4 (dichlorine tetrachloride):

All elements are nonmetals, sharing electrons in covalent bonds.

Type: Covalent

(f) Co(NO3)2 (cobalt(II) nitrate):

Cobalt (Co) is a transition metal, and nitrate (NO3⁻) is a polyatomic ion. The bonding between Co²⁺ and nitrates is ionic.

Type: Ionic; Ions involved: Co²⁺ and NO3⁻

Writing Chemical Formulas of Compounds

The second task involves constructing chemical formulas based on the names of compounds.

(a) Barium chloride:

Barium (Ba²⁺), chloride (Cl⁻). To balance charges: 1 Ba²⁺ and 2 Cl⁻.

Formula: BaCl₂

(b) Magnesium nitride:

Magnesium (Mg²⁺), nitride (N³⁻). Least common multiple of charges is 6; thus, 3 Mg²⁺ and 2 N³⁻.

Formula: Mg₃N₂

(c) Sulfur dioxide:

Sulfur (S), oxygen (O). In sulfur dioxide, the formula is S with two oxygens.

Formula: SO₂

(d) Nitrogen trichloride:

Nitrogen (N), chlorine (Cl). The formula reflects three Cl atoms: NCl₃.

(e) Dinitrogen trioxide:

Two nitrogen atoms, three oxygen atoms.

Formula: N₂O₃

(f) Tin(IV) chloride:

Tin (Sn) with a +4 charge, chloride (Cl⁻). To neutralize +4, 4 Cl⁻ are needed.

Formula: SnCl₄

Calculating the Mass of HCl in a Solution

Given data:

- Volume of HCl solution = 45.0 mL

- Density of solution = 1.19 g/cm³ (equivalent to g/mL)

- HCl content = 37.21% by mass

First, calculate the mass of the entire solution:

Mass = Volume × Density = 45.0 mL × 1.19 g/mL = 53.55 g

Next, determine the mass of HCl in this solution:

Mass of HCl = 37.21% of total mass = (37.21 / 100) × 53.55 g ≈ 19.94 g

Thus, the solution contains approximately 19.94 grams of HCl.

Conclusion

This analysis highlights essential concepts in inorganic chemistry, including bond classification, compound nomenclature, chemical formula derivation, and quantitative calculations. Recognizing ionic versus covalent bonds informs us about compound properties. Accurate formula writing aids in chemical communication and stoichiometric calculations. Calculating quantities like HCl mass enables precise laboratory measurements, essential for applications in industry, research, and education. Mastery of these skills underpins broader chemical understanding and practical laboratory competency.

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