Determine whether or not each metal dissolves in 1 M HNO3. For those metals that do dissolve, write a balanced redox equation for the reaction that occurs. a. Au

Verified step by step guidance

1. Identify the reactivity of gold (Au) with nitric acid (HNO3). Gold is a noble metal and is known for its resistance to corrosion and oxidation.
2. Understand that nitric acid is a strong oxidizing agent, but gold does not react with it under normal conditions because it is below hydrogen in the reactivity series.
3. Recognize that gold does not dissolve in 1 M HNO3 alone. However, it can dissolve in aqua regia, a mixture of concentrated nitric acid and hydrochloric acid.
4. Since gold does not dissolve in 1 M HNO3, there is no need to write a balanced redox equation for this reaction.
5. Conclude that gold remains undissolved in 1 M HNO3 due to its low reactivity and noble nature.

Key Concepts

Redox Reactions

Redox reactions involve the transfer of electrons between two species, resulting in oxidation (loss of electrons) and reduction (gain of electrons). In the context of metals dissolving in acids, the metal typically undergoes oxidation while the acid's hydrogen ions are reduced. Understanding the electron transfer process is crucial for balancing redox equations.

Metal Reactivity

The reactivity of metals determines their ability to dissolve in acids like HNO3. More reactive metals, such as zinc or magnesium, readily react with acids, while noble metals like gold (Au) are less reactive and often do not dissolve. Knowing the position of metals in the reactivity series helps predict their behavior in chemical reactions.

Balanced Chemical Equations

A balanced chemical equation represents a chemical reaction with equal numbers of each type of atom on both sides of the equation. For redox reactions, this involves ensuring that both mass and charge are conserved. Writing a balanced equation for the dissolution of a metal in acid requires identifying the oxidation states and the products formed during the reaction.