Understanding Metallic Bonding Properties

Which of the following best describes the electron sea model in metallic bonding?

• Electrons are shared between two specific atoms.

• Electrons are localized around individual atoms.

• Electrons are delocalized and shared among all atoms.

• Electrons are transferred from one atom to another.

Answer explanation

The electron sea model describes metallic bonding where electrons are not tied to individual atoms but are delocalized, allowing them to move freely and be shared among all atoms, which explains the conductivity and malleability of metals.

What property of metals is explained by the freedom of movement of delocalized electrons?

• Brittleness

• Conductivity

• Low density

• Transparency

Answer explanation

The freedom of movement of delocalized electrons in metals allows them to conduct electricity efficiently. This property, known as conductivity, is a key characteristic of metallic substances.

Why do metals exhibit malleability?

• Because their atoms are rigidly fixed in place.

• Because their atoms can slide past each other easily.

• Because their atoms are tightly bonded to nonmetals.

• Because their atoms are arranged in a random pattern.

Answer explanation

Metals exhibit malleability because their atoms can slide past each other easily. This ability allows metals to be shaped without breaking, unlike rigid structures where atoms are fixed in place.

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How does the electron sea model account for the high melting points of metals?

• The strong attraction between localized electrons and protons.

• The weak attraction between delocalized electrons and protons.

• The strong attraction between delocalized electrons and protons.

• The weak attraction between localized electrons and protons.

Answer explanation

The electron sea model describes metals as having delocalized electrons that move freely. This strong attraction between these delocalized electrons and the positively charged protons in the metal lattice accounts for their high melting points.

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Which of the following is NOT a property of metals explained by metallic bonding?

• High volatility

• Ductility

• Conductivity

• Malleability

Answer explanation

High volatility is not a property of metals explained by metallic bonding. Metals are typically stable and do not easily vaporize, while ductility, conductivity, and malleability are key characteristics resulting from metallic bonding.

Explain why metals are good conductors of electricity using the electron sea model.

• Electrons are tightly bound to atoms, preventing flow.

• Electrons are free to move, allowing easy flow of electric current.

• Electrons are transferred to nonmetals, creating a current.

• Electrons are shared between two atoms, restricting flow.

Answer explanation

The electron sea model explains that in metals, electrons are not bound to individual atoms but are free to move throughout the structure. This mobility allows for easy flow of electric current, making metals good conductors.

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Predict what would happen to the malleability of a metal if its electrons were not delocalized.

• Malleability would increase.

• Malleability would decrease.

• Malleability would remain unchanged.

• Malleability would become infinite.

Answer explanation

If electrons are not delocalized, they cannot move freely, which is essential for a metal's malleability. This lack of mobility would hinder the ability of the metal to deform under stress, leading to decreased malleability.

How does the electron sea model explain the ductility of metals?

• Electrons are fixed, allowing atoms to break easily.

• Electrons are free, allowing atoms to stretch without breaking.

• Electrons are transferred, making metals brittle.

• Electrons are shared, causing metals to shatter.

Answer explanation

The electron sea model describes electrons as free to move, which allows metal atoms to slide past each other when stress is applied. This mobility enables metals to stretch and deform without breaking, explaining their ductility.

Using the electron sea model, explain why metals have low volatility.

• The weak attraction between electrons and protons.

• The strong attraction between electrons and protons.

• The weak attraction between electrons and nonmetals.

• The strong attraction between electrons and nonmetals.

Answer explanation

Metals have low volatility due to the strong attraction between electrons and protons in the electron sea model. This strong attraction stabilizes the metallic structure, making it less likely for metal atoms to escape into the gas phase.

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What happens to the melting point of metals as you move across the transition metals from scandium to zinc, and why?

• It consistently increases due to more electrons.

• It consistently decreases due to fewer electrons.

• It varies due to changes in electron configurations.

• It remains constant due to stable electron configurations.

Answer explanation

The melting point of transition metals varies from scandium to zinc due to changes in electron configurations, which affect metallic bonding and stability, leading to different melting points.

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