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Chapter 9: Problem 12

The term "molar mass" was introduced in Chapter 3 What is the advantage of using the term "molar mass" when we discuss ionic compounds?

Short Answer

Expert verified
The term 'molar mass' is advantageous when discussing ionic compounds because it allows for easy conversion between the number of ions (an atomic scale concept) and the amount of ionic compound necessary for a reaction (a macroscopic or lab scale concept). By knowing the molar mass, one can understand how much of an ionic compound is needed for a reaction or how many ions will be produced from a given amount of compound.

Step by step solution

01

Understand the Term 'Molar Mass'

Molar mass is the mass of one mole of a substance, generally expressed in grams or kilograms per mole (\(g/mol\) or \(kg/mol\)). It's a way to convert between the atomic scale (microscopic) and the lab scale (macroscopic).
02

Understand 'Ionic Compounds'

Ionic compounds are chemical compounds consisting of ions held together by electrostatic forces termed ionic bonding. Each compound is neutral overall, but consists of positively charged ions called cations and negatively charged ions called anions.
03

Identify why 'Molar Mass' is Useful for Ionic Compounds

Molar mass is extremely useful in discussing ionic compounds because it allows us to easily calculate how much of an ionic compound is needed for a reaction (in the lab scale), starting from the number of ions (at the atomic scale), or vice versa. So it provides a convenient bridge between the atomic and macroscopic worlds.

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Most popular questions from this chapter

What is lattice energy and what role does it play in the stability of ionic compounds?

Write Lewis dot symbols for the following ions: (a) \(\mathrm{Li}^{+},(\mathrm{b}) \mathrm{Cl}^{-},(\mathrm{c}) \mathrm{S}^{2-},(\mathrm{d}) \mathrm{Sr}^{2+}\) (e) \(\mathrm{N}^{3+}\).

Distinguish among single, double, and triple bonds in a molecule, and give an example of each.

Draw Lewis structures of these organic molecules: (a) methanol \(\left(\mathrm{CH}_{3} \mathrm{OH}\right) ;\) (b) ethanol \(\left(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{OH}\right)\); (c) tetraethyllead \(\left[\mathrm{Pb}\left(\mathrm{CH}_{2} \mathrm{CH}_{3}\right)_{4}\right]\), which was used in "leaded" gasoline; (d) methylamine \(\left(\mathrm{CH}_{3} \mathrm{NH}_{2}\right)\) (e) mustard gas \(\left(\mathrm{ClCH}_{2} \mathrm{CH}_{2} \mathrm{SCH}_{2} \mathrm{CH}_{2} \mathrm{Cl}\right)\), a poison- ous gas used in World War I; (f) urea \(\left[\left(\mathrm{NH}_{2}\right)_{2} \mathrm{CO}\right]\), a fertilizer; (g) glycine \(\left(\mathrm{NH}_{2} \mathrm{CH}_{2} \mathrm{COOH}\right)\), an amino acid.

Draw three resonance structures for the chlorate ion, \(\mathrm{ClO}_{3}^{-}\). Show formal charges.
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