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Chapter 4: Problem 15

What is the difference between an ionic equation and a molecular equation?

Short Answer

Expert verified
An ionic equation represents compounds as dissociated ions, showing all the particles as they realistically exist in the solution. A molecular equation, on the other hand, shows the reaction occurring between the neutral compounds as a whole and not as separated ions.

Step by step solution

01

Understanding Molecular Equation

A molecular equation is a balanced chemical equation where the ionic compounds are expressed as molecules instead of component ions.
02

Understanding Ionic Equation

An ionic equation is a chemical equation where the electrolytes in aqueous solution are written as dissociated ions.
03

Key Differences

The key difference between these two lies in the fact that the ionic equation shows all the particles involved in the reaction as they realistically exist in the solution, while the molecular equation shows the neutral compounds as whole rather than as separated ions.

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Most popular questions from this chapter

The concentration of \(\mathrm{Cu}^{2+}\) ions in the water (which also contains sulfate ions) discharged from a certain industrial plant is determined by adding excess sodium sulfide \(\left(\mathrm{Na}_{2} \mathrm{~S}\right)\) solution to \(0.800 \mathrm{~L}\) of the water. The molecular equation is $$ \mathrm{Na}_{2} \mathrm{~S}(a q)+\mathrm{CuSO}_{4}(a q) \longrightarrow_{\mathrm{Na}_{2} \mathrm{SO}_{4}(a q)+\operatorname{CuS}(s)} $$ Write the net ionic equation and calculate the molar concentration of \(\mathrm{Cu}^{2+}\) in the water sample if \(0.0177 \mathrm{~g}\) of solid \(\mathrm{CuS}\) is formed.

For the complete redox reactions given here, (i) break down each reaction into its half-reactions; (ii) identify the oxidizing agent; (iii) identify the reducing agent. (a) \(2 \mathrm{Sr}+\mathrm{O}_{2} \longrightarrow 2 \mathrm{SrO}\) (b) \(2 \mathrm{Li}+\mathrm{H}_{2} \longrightarrow 2 \mathrm{LiH}\) (c) \(2 \mathrm{Cs}+\mathrm{Br}_{2} \longrightarrow 2 \mathrm{CsBr}\) (d) \(3 \mathrm{Mg}+\mathrm{N}_{2} \longrightarrow \mathrm{Mg}_{3} \mathrm{~N}_{2}\)

Give oxidation numbers for the underlined atoms in the following molecules and ions: (a) \(\underline{\mathrm{Cs}_{2} \mathrm{O}},\) (b) \(\mathrm{Ca} \underline{\mathrm{I}}_{2}\), (c) \(\underline{\mathrm{Al}_{2} \mathrm{O}_{3}}\) (d) \(\mathrm{H}_{3} \mathrm{As} \mathrm{O}_{3},\) (e) \(\underline{\mathrm{Ti} \mathrm{O}_{2}},\) (f) \(\underline{\mathrm{Mo}} \mathrm{O}_{4}^{2-}\), (g) \(\underline{\mathrm{Pt} \mathrm{Cl}_{4}^{2-}}\) (h) \(\underline{\mathrm{Pt}} \mathrm{Cl}_{6}^{2-}\) (i) \(\underline{\operatorname{Sn} F}_{2}\) (j) \(\underline{\mathrm{ClF}_{3},}\) (k) \(\underline{\mathrm{Sb}} \mathrm{F}_{6}^{-}\)

Is it possible to have a reaction in which oxidation occurs and reduction does not? Explain.

Which of the following processes will likely result in a precipitation reaction? (a) Mixing a \(\mathrm{NaNO}_{3}\) solution with a \(\mathrm{CuSO}_{4}\) solution. (b) Mixing a \(\mathrm{BaCl}_{2}\) solution with a \(\mathrm{K}_{2} \mathrm{SO}_{4}\) solution. Write a net ionic equation for the precipitation reaction.
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