Write the balanced net ionic equations for the reactions...

Name: Problem 60, Chapter 11: Chemistry
Uploaded: 2021-10-27T21:16:37-08:00
Duration: 1 min 37 s
Channel: Ronald Prasad
Description: Write the balanced net ionic equations for the reactions given. Then, using the reactants shown in parentheses, convert each balanced net ionic equation to a balanced formula unit equation. (a) Zn(s)+Cu^2+ ⟶Cu(s)+Zn^2+ (Zn. and .CuSO4) (b) Cr(s)+H^+ ⟶Cr^3++H2( g) (Cr. and .H2 SO4)

Write the balanced net ionic equations for the reactions given. Then, using the reactants shown in parentheses, convert each balanced net ionic equation to a balanced formula unit equation. (a) $\mathrm{Zn}(\mathrm{s})+\mathrm{Cu}^{2+} \longrightarrow \mathrm{Cu}(\mathrm{s})+\mathrm{Zn}^{2+} \quad\left(\mathrm{Zn}\right.$ and $\left.\mathrm{CuSO}_{4}\right)$ (b) $\mathrm{Cr}(\mathrm{s})+\mathrm{H}^{+} \longrightarrow \mathrm{Cr}^{3+}+\mathrm{H}_{2}(\mathrm{~g}) \quad\left(\mathrm{Cr}\right.$ and $\left.\mathrm{H}_{2} \mathrm{SO}_{4}\right)$

Write the balanced net ionic equations for the reactions given. Then, using the reactants shown in parentheses, convert each balanced net ionic equation to a balanced formula unit equation.
(a) $\mathrm{Zn}(\mathrm{s})+\mathrm{Cu}^{2+} \longrightarrow \mathrm{Cu}(\mathrm{s})+\mathrm{Zn}^{2+} \quad\left(\mathrm{Zn}\right.$ and $\left.\mathrm{CuSO}_{4}\right)$
(b) $\mathrm{Cr}(\mathrm{s})+\mathrm{H}^{+} \longrightarrow \mathrm{Cr}^{3+}+\mathrm{H}_{2}(\mathrm{~g}) \quad\left(\mathrm{Cr}\right.$ and $\left.\mathrm{H}_{2} \mathrm{SO}_{4}\right)$

Key Concepts

Conversion between Net Ionic and Formula Unit Equations

Converting a net ionic equation to a formula unit equation involves reintroducing the spectator ions to reconstruct the complete representational formula of the reaction. This conversion is essential to show the full context of the reactants and products as they exist in solution, providing a complete picture of the chemical reaction.

Spectator Ions

Spectator ions are ions that are present in the same form on both the reactant and product sides of a chemical equation. They do not participate in the actual chemical change and are omitted in the net ionic equation but are included in the complete formula unit (molecular) equation.

Balancing Chemical Equations

Balancing chemical equations is the process of making sure that the number of atoms for each element and the overall charge are the same on both the reactant and product sides of the equation. This often involves using the half-reaction method in redox reactions to separately balance the oxidation and reduction processes before combining them into a complete, balanced equation.

Redox Reaction

A redox reaction involves the transfer of electrons between species, resulting in oxidation (loss of electrons) and reduction (gain of electrons). In these reactions, one element’s oxidation state increases while another’s decreases, which is a central concept in understanding the reactivity and balancing of redox equations.

Net Ionic Equation

The net ionic equation shows only the species that actually participate in the chemical reaction, omitting spectator ions that do not undergo any chemical change. It simplifies the reaction by focusing solely on the reactive ions, allowing for easier analysis and understanding of the underlying chemical process.

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