Science (086) — AI-generated practice question

The fundamental tendency is that metals lose electrons easily to form positive ions (cations). This is driven by their need to attain a stable electronic configuration.

In ionic compound formation (e.g., NaCl): Sodium loses one electron to chlorine, forming Na⁺ and Cl⁻ ions. The oppositely charged ions attract each other, forming the ionic compound NaCl.

In electrolytic extraction of reactive metals: Highly reactive metals like sodium or magnesium have such strong affinity for oxygen that carbon cannot reduce their compounds. Electrolysis of molten chlorides is used; the metal cations (Na⁺) gain electrons at the cathode and are deposited as pure metal: Na⁺ + e⁻ → Na.

Thus, the same tendency — losing electrons to form cations — leads to compound formation in nature and enables isolation through forced electron gain during electrolysis.

Source: Chapter 3, Sections 3.3 and 3.4.5

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• The examiner wants you to name the tendency (metals lose electrons / form positive ions) and then link it explicitly to both processes.
• For NaCl: electron transfer → ionic bond. For electrolysis: metal ions already exist in molten ore; cathode supplies electrons to reduce them back to metal.
• The contrast is key: in NaCl formation the metal gives away electrons; in electrolysis, those same cations are given back electrons artificially — both driven by the metal's tendency to exist as cations.
• Always write the cathode half-reaction when discussing electrolytic extraction; it fetches a dedicated mark.