Resource: Metals in Hydrochloric Acid

An acid is a chemical compound that, when dissolved in water, has a pH of less than 7.0. Acidic compounds contain positively charged hydrogen ions—hydrogen atoms containing protons but no electrons—which readily react with other compounds. Examples of common acids are acetic acid, or vinegar, and sulfuric acid, which is used in car batteries. Monoprotic acids, which include hydrochloric acid, only give up one proton per acid molecule, while polyprotic acids can give up more than one proton per acid molecule.

When bare-metal surfaces are immersed in an acidic aqueous solution (a solution in which the solvent is water), the hydrogen ions in the acid attract and bond with negatively charged electrons from the metal to produce what is called an oxidation-reduction reaction. Hydrogen gas, which forms as two released electrons attach to two hydrogen ions, bubbles off, and metal atoms (now positively charged ions) are released into the solution. Through this oxidation-reduction reaction, the metal is said to corrode, or gradually wear away.

Metals consist of stacked layers of tightly packed, interacting atoms arranged in geometric patterns. Whereas non-metals tend to gain electrons in chemical reactions, metals tend to lose them. The gauge of just how readily a metal loses electrons is known as its redox potential, which is determined by its atomic structure.

Electrons inhabit various energy levels, or shells. The electron configuration shown in the periodic table indicates how many electrons are found in each shell, from innermost to outermost. Atoms of elements in the left-hand column have one electron in their outer shell, while atoms of elements in the right-hand column have eight electrons in their outer shell. Generally speaking, single electrons in an outer shell can easily be taken away from the atom with the application of very little energy. This makes atoms of elements in the left-hand column very reactive. On the other hand, it is very difficult to add or remove electrons from an atom that has eight electrons in its outer shell. The atoms of these elements, found in the column to the far right, are non-reactive. Knowing this helps explain why some metals, such as tin and copper, corrode less readily than others, such as magnesium and iron.

Because some metals are more prone to corrosion, engineers have learned to use certain techniques during an item's manufacture to protect it from structural decay. One method involves plating, or painting over a metal with a coating. This technique prevents electrochemical reactions from occurring. When exposed to oxygen in air or water, for example, two elements, aluminum and chromium, form a self-renewing, microscopically thin layer, known as an oxide film, which protects the underlying metal from corrosion. The alloy stainless steel, known for its sleek, shiny surface and tremendous strength, contains a high concentration of chromium.

To learn more about elements and why metals appear where they do in the Periodic Table, check out Periodic Table of the Elements, Periodic Table of the Elements Chart, and Graphing the Periodic Table.

To learn about the crystalline structure of metal and other ways in which metals are subject to weaken and fail, check out The Structure of Metal.

To learn more about how acid present in rainfall can affect the natural environment, check out How Caves Form and Acid Lake.

To learn more about metal alloys, check out Elements of Steel.

• Why do you think silver does not react in any of the solutions?
• What determines the reactivity of zinc?
• How would you classify the level of reactivity of the various metals in HCl?
• Can you explain why some metals reacted in these solutions while others did not? Could the Periodic Table help?
• How would you explain what happens on the molecular level in terms of electron movement?