Metal Reactivity and Extraction Quiz

Metal Reactivity and Extraction

• Metals vary in their reactivity, some reacting easily, others not.
• Reactivity series: A list ordering metals from most to least reactive. A more reactive metal can displace a less reactive one from its compounds. Reactivity is a substance's tendency to undergo a chemical reaction.
• Reactive metals readily form new substances. E.g., Sodium reacts rapidly with air, losing its shine. This is due to the high reactivity of sodium.
• Unreactive metals, like gold and platinum, resist reacting with air even at high temperatures. These metals are unreactive, meaning they do not easily take part in chemical reactions.
• Metal reactivity affects extraction methods. Reactivity affects what reactions the metal participates in. Metals can react with water, acid, and oxygen.

Extracting Metals

• Metal ores: Natural rocks containing usable amounts of metals or metal compounds.
• Extraction method depends on metal's reactivity and ore stability.
• In all cases, metal ions gain electrons to form metallic atoms.

Extracting Unreactive Metals

• Heating the ore is enough to extract the metal.
• Example: Heating silver oxide produces silver metal and oxygen.
  • Word equation: silver oxide → silver + oxygen
  • Chemical equation: 2 Ag₂O(s) → 4 Ag(s) + 2 O₂(g)

Extracting Reactive Metals

• Ores of reactive metals need carbon or carbon monoxide.
• Carbon is more reactive than some metals, so can extract them from their oxides.
• Example metals: zinc, iron, tin, lead, and copper(least reactive of these).
• General word equation: metal oxide + carbon → metal + carbon dioxide
• Practical example: extracting copper from copper oxide.
• Mix copper oxide powder with carbon powder.
• Heat strongly in a crucible (covered to prevent oxygen reaction with carbon).
• Filter out the copper pieces via water.
• Word equation: copper oxide + carbon → copper + carbon dioxide
• Chemical equation: 2 CuO(s) + C(s) → 2 Cu(s) + CO₂(g)

Extracting Very Reactive Metals

• Melting and electrolysis (using direct current) are crucial for very reactive metals, including those used in solutions or solutions themselves.
• Ions get electrons at the negative electrode, forming metal atoms.
• Electrolysis can also extract less reactive metals like copper.
• Example: Magnesium is a very reactive metal. It ignites when heated and burns with a brilliant white flame.

Test your knowledge on the reactivity of metals and their extraction methods. This quiz covers the reactivity series, how different metals react, and the extraction processes for both reactive and unreactive metals. Challenge yourself with questions that explore the science behind metal ores and chemical equations involved in metal extraction.