Predict the products for each of the following reactions. If...

Predict the products for each of the following reactions. If no reaction happens, write “no reaction.” Write a total ionic equation for each reaction that does happen. a. $\mathrm{AuCl}_{3}(a q)+\mathrm{Ag}(s) \rightarrow$ b. $\mathrm{AgNO}_{3}(a q)+\mathrm{CaCl}_{2}(a q) \rightarrow$ c. $\mathrm{Al}(s)+\mathrm{NiSO}_{4}(a q) \rightarrow$ d. $\mathrm{Na}(s)+\mathrm{H}_{2} \mathrm{O}(l) \rightarrow$ e. $\mathrm{AgNO}_{3}(a q)+\mathrm{NaCl}(a q) \rightarrow$

Predict the products for each of the following reactions. If no reaction happens, write “no reaction.” Write a total ionic equation for each reaction that does happen.
a. $\mathrm{AuCl}_{3}(a q)+\mathrm{Ag}(s) \rightarrow$
b. $\mathrm{AgNO}_{3}(a q)+\mathrm{CaCl}_{2}(a q) \rightarrow$
c. $\mathrm{Al}(s)+\mathrm{NiSO}_{4}(a q) \rightarrow$
d. $\mathrm{Na}(s)+\mathrm{H}_{2} \mathrm{O}(l) \rightarrow$
e. $\mathrm{AgNO}_{3}(a q)+\mathrm{NaCl}(a q) \rightarrow$

Key Concepts

Single Replacement Reactions

Single replacement reactions involve an element, typically a metal, replacing another element in a compound. This type of reaction is commonly guided by the activity series, which ranks metals by their reactivity. When a more reactive metal comes into contact with a compound containing a less reactive metal, the more reactive metal displaces the less reactive one, forming a new compound and leaving the displaced metal in its elemental form.

Double Replacement Reactions

Double replacement reactions, also known as metathesis reactions, involve the exchange of ions between two compounds. In aqueous solutions, the cations and anions of the reactants swap partners, often resulting in the formation of a precipitate, a gas, or a weak electrolyte such as water. These reactions are typically predicted using solubility rules to determine if an insoluble compound (precipitate) will form.

Redox Reactions

Redox (reduction-oxidation) reactions involve the transfer of electrons between reacting species. In these reactions, one substrate is oxidized (loses electrons) and another is reduced (gains electrons). Metal displacement reactions are a common example where the oxidation state of the metal changes as it goes from elemental form to an ionic form or vice versa.

Alkali Metal Reactions with Water

Alkali metals react vigorously with water due to their high reactivity. In these reactions, the alkali metal typically donates an electron to water, forming a hydroxide and liberating hydrogen gas. The reactions are highly exothermic and can sometimes be explosive, emphasizing the need for careful handling of these metals.

Total Ionic Equations

Total ionic equations represent all the ions present in an aqueous reaction while excluding the molecules that do not dissociate, illustrating the actual chemical species involved in the reaction. By breaking down soluble compounds into their constituent ions, these equations make it easier to identify the spectator ions and understand the underlying reaction mechanism in aqueous solutions.

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