Question

Liquefied metals contain (a) metal anions only (b) metal cations only (c) metal kernels and mobile electrons (d) metal atoms only

Short answer

Liquefied metals contain metal kernels and mobile electrons (c).

Step-by-step solution

Understanding the Problem

The question is asking about the nature of liquefied metals, specifically what components they contain. We need to identify which of the options accurately describes the composition of liquefied metals.

Analyzing Metal Components

Metals, when they are in solid form, consist of a lattice of metal cations surrounded by a 'sea' of delocalized electrons. To see if the same applies to liquefied metals, we analyze the components likely to persist in their liquid state.

Metal Cation and Electron Sea Model

Metals have a unique bonding through a structure of positive metal cations and free electrons that move throughout. Upon melting, this structure becomes more fluid, yet still consists of these elements as opposed to isolated atoms or ions.

Evaluating Each Option

- (a) Metal anions are unlikely because metals generally lose electrons to form cations. - (b) Metal cations form part of the structure, but the model also involves electrons. - (c) The correct model includes metal kernels (cations) and a sea of mobile electrons that are free to move. - (d) Metal atoms alone can't accurately describe the structure due to electron presence.

Key concepts

Metal Cations

When discussing liquefied metals, metal cations play a crucial role in understanding their structural composition. Metal cations are positively charged ions formed when metal atoms lose electrons. This loss of electrons is a fundamental process that enables metal atoms to bond with one another in solid states and in liquids.
For liquefied metals, the metal cations maintain their structure even when the metal is in a liquid state. They become part of what is referred to as metal kernels, which is a more stable configuration of metal ions and nearby electrons. These cations do not simply float around individually but are part of a collective framework with other cations and roaming electrons.
In essence, metal cations are the backbone of metallic bonding. Without them maintaining a stable positive charge, the unique properties of metals like conductivity and malleability would be impossible. This is crucial for understanding that liquefied metals aren't just molten blobs but structured entities much like their solid counterparts.

Electron Sea Model

The Electron Sea Model is a central concept when discussing metal bonding in both solid and liquid states. It describes how metals are bonded through a lattice framework of positive metal cations engulfed by free electrons, often termed the 'sea of electrons.' These free electrons are not bound to any particular atom and can move freely throughout the structure.
This movement is critical because it provides metals with several characteristic properties:

• High electrical conductivity: As electrons move freely, they facilitate the easy flow of electric current.
• Malleability and ductility: The sea of electrons allows the metal atoms to slide past each other without breaking the metallic bond.

When metals are liquefied, the Electron Sea Model persists albeit in a more fluid form. The positive cations are part of the flowing liquid, and the free electrons continue their erratic dance, ensuring that the structure remains conductive and robust without losing metallic bonds.

Metal Bonding in Liquids

Metal bonding in liquids involves the same principles as those found in solid metals: a network of metal cations and free-floating electrons. However, when metals are melted, these bonds become dynamic, allowing for fluidity while maintaining their metallic characteristics.
In liquefied metals, the metal cation lattice found in solid form is not as rigid but still effectively holds the metal kernels in a cohesive structure. The free electrons continue to flow unimpeded, ensuring consistent metallic properties such as conductivity remain even in this fluid state.
Understanding metal bonding in liquids is important because it explains why metals behave similarly in both solid and molten forms. It also sheds light on their ability to conduct electricity and heat while being shaped and manipulated without breaking the intrinsic metallic bonds. The flow and movement of electrons and cations are the hallmarks of metal bonding, showcasing an elegant dance of stability and change.