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Chapter 14: Problem 85

Why does brass cause your skin to turn green?

Short Answer

Expert verified
Brass causes skin to turn green due to the oxidation of the copper within the alloy when it reacts with the natural oils and sweat on your skin and forms a layer of copper carbonate or copper chloride which appears green.

Step by step solution

01

Understand the Composition of Brass

Brass is an alloy of copper and zinc, but sometimes it contains other metals. It's important to note that the copper in the alloy is the cause for the green tint on the skin when wearing a brass jewelry.
02

Chemical Reactions with Skin

The natural oils and sweat on human skin cause the copper molecules in brass to oxidize. This oxidation, in combination with the skin鈥檚 natural acids, causes a chemical reaction which results in a greenish color on the skin.
03

Green Colour Explanation

This green color is actually copper chloride (or copper carbonate), which our bodies have no problem dealing with in small amounts. This is non-hazardous and can simply be washed off.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Copper Oxidation
Copper oxidation is a chemical process that occurs when copper is exposed to the environment. Over time, copper reacts with oxygen in the air, causing it to lose electrons in a reaction known as oxidation. The visible result is the formation of a layer of copper oxide on the surface. This thin layer is what gives copper its teal or green color, commonly seen on the Statue of Liberty.
  • Oxidation is accelerated in moist environments.
  • Copper oxide is a natural protective layer.
  • This layer prevents further corrosion of the copper material underneath.
Understanding oxidation can help in appreciating why items like copper cookware or jewelry might change color over time and why certain measures, such as coatings or polishing, are used to maintain their appearance.
Alloy Properties
Alloys are mixtures of two or more metals, designed to benefit from the characteristics of each component. Brass, for example, is an alloy mainly composed of copper and zinc. This mixture results in a metal that is both durable and corrosion-resistant, making it widely used for decorative and functional purposes.
  • Brass is malleable and has good acoustic properties, which is why it is used in musical instruments.
  • Its non-magnetic properties make it essential for electronic devices.
  • The zinc addition helps in preventing easy rusting and enhances the metal's strength.
The properties of alloys like brass are determined not just by the choice of metals but also by the proportion in which they are combined. This allows for customization to fit specific applications and is why alloys are so prevalent in manufacturing industries.
Chemical Reactions with Skin
When wearing metal jewelry like brass, it often reacts with the skin. This is primarily due to the copper content undergoing a reaction with the natural oils and sweat produced by the skin. The acidity of the sweat and oil facilitates copper oxidation, resulting in the formation of copper salts such as copper chloride or copper carbonate.
  • This is often perceived as a green discoloration on the skin.
  • The green tone is harmless and can be washed off with mild soap and water.
  • Reaction intensity varies depending on individual's skin chemistry.
The reason behind the green mark is the metal ions interacting with skin compounds. Knowing this helps in making informed choices about jewelry and potentially preventing unwanted discolorations by applying barrier creams or choosing different metals like gold or silver for sensitive skin.

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Most popular questions from this chapter

The following table gives the results of reactions between five metals and solutions of their nitrate salts. NR means "no reaction" and MD means "metal displaced from solution." From these results, arrange the five metals in order of decreasing chemical activity. \begin{tabular}{lccccc} \hline & \(\mathrm{Ag}(s)\) & \(\mathrm{Fe}(s)\) & \(\mathrm{Hg}(l)\) & \(\mathrm{Mn}(s)\) & \(\mathrm{Ni}(s)\) \\ \hline \(\mathrm{AgNO}_{3}(a q)\) & \(-\) & \(\mathrm{MD}\) & \(\mathrm{NR}\) & \(\mathrm{MD}\) & \(\mathrm{MD}\) \\ \(\mathrm{Fe}\left(\mathrm{NO}_{3}\right)_{2}(a q)\) & \(\mathrm{NR}\) & \(-\) & \(\mathrm{NR}\) & \(\mathrm{MD}\) & \(\mathrm{NR}\) \\ \(\mathrm{Hg}\left(\mathrm{NO}_{3}\right)_{2}(a q)\) & \(\mathrm{MD}\) & \(\mathrm{MD}\) & \(-\) & \(\mathrm{MD}\) & \(\mathrm{MD}\) \\ \(\mathrm{Mn}\left(\mathrm{NO}_{3}\right)_{2}(a q)\) & \(\mathrm{NR}\) & \(\mathrm{NR}\) & \(\mathrm{NR}\) & \(-\) & \(\mathrm{NR}\) \\ \(\mathrm{Ni}\left(\mathrm{NO}_{3}\right)_{2}(a q)\) & \(\mathrm{NR}\) & \(\mathrm{MD}\) & \(\mathrm{NR}\) & \(\mathrm{MD}\) & \(-\) \end{tabular}

What is an oxidation-reduction reaction?

In the following oxidation-reduction reactions, identify the oxidizing agent, the reducing agent, and the number of electrons transferred. (a) \(\mathrm{I}_{2}(a q)+2 \mathrm{OH}^{-}(a q) \longrightarrow \mathrm{I}^{-}(a q)+\mathrm{IO}^{-}(a q)+\mathrm{H}_{2} \mathrm{O}(l)\) (b) \(\mathrm{Cr}(s)+2 \mathrm{H}^{+}(a q) \longrightarrow \mathrm{Cr}^{2+}(a q)+\mathrm{H}_{2}(g)\) (c) \(2 \mathrm{Cr}_{2} \mathrm{O}_{7}{ }^{2}(a q)+16 \mathrm{H}^{+}(a q) \longrightarrow\) \(4 \mathrm{Cr}^{3+}(a q)+3 \mathrm{O}_{2}(g)+8 \mathrm{H}_{2} \mathrm{O}(l)\) (d) \(3 \mathrm{Fe}^{3+}(a q)+\mathrm{Al}(s) \longrightarrow 3 \mathrm{Fe}^{2 *}(a q)+\mathrm{Al}^{34}(a q)\)

The reaction that occurs in a common dry cell battery is as follows: $$ \begin{aligned} \mathrm{Zn}(s)+2 \mathrm{MnO}_{2}(s)+2 \mathrm{NH}_{4}^{+}(a q) & \longrightarrow \\ \mathrm{Zn}^{2 *}(a q) &+\mathrm{Mn}_{2} \mathrm{O}_{3}(s)+2 \mathrm{NH}_{3}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \end{aligned} $$ What gets oxidized in this battery? What gets reduced? What is the oxidizing agent? What is the reducing agent?

The reaction that occurs in gas grills involves the burning of propane: $$ \mathrm{C}_{3} \mathrm{H}_{\mathrm{s}}(g)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(g) $$ Assign oxidation numbers to all of the reactants and identify the oxidizing and reducing agents.
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