Transition Metals, Alloys, and Corrosion Flashcards
Describe the position of transition metals in the periodic table.
Transition metals are found in the d-block, between groups 2 and 3.
Describe some general physical properties of transition metals.
They have high melting points, high density, are hard, and conduct electricity.
Describe some general chemical properties of transition metals.
They form colored compounds, can act as catalysts, and have variable oxidation states.
Describe corrosion of metals as the result of oxidation.
Corrosion is the oxidation of metals, causing them to deteriorate over time.
Describe how rusting of iron occurs.
Iron rusts when it reacts with oxygen and water, forming iron oxide.
Explain how rusting can be prevented by excluding oxygen and/or water.
Rusting is prevented by applying coatings, oil, or grease to block oxygen and water.
Explain how sacrificial protection works.
A more reactive metal (like zinc) is attached to iron, which corrodes instead of the iron.
Recall what electroplating is.
Electroplating is coating an object with a thin layer of metal using electrolysis.
Recall some common examples of electroplating.
Examples include silver-plated cutlery and gold-plated jewelry.
Explain why metal objects may be electroplated.
Electroplating improves appearance, prevents corrosion, and reduces friction.
Recall the name of a common alloy.
Steel is a common alloy made from iron and carbon.
Describe what alloys are.
Alloys are mixtures of metals, or metals with non-metals, designed to improve properties.
Explain why iron is alloyed with other metals.
Alloying iron improves strength, durability, and corrosion resistance.
Recall common uses for aluminum, copper, and gold.
Aluminum is used in aircraft, copper in electrical wiring, and gold in jewelry.
Recall the names and compositions of common alloys containing aluminum or copper.
Brass (copper and zinc), bronze (copper and tin), and duralumin (aluminum and copper).
