Metallic Bond Mastery

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Quiz on metallic bonds and properties

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Faith

Kenya

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Metallic Bond Mastery


Froggy Jumps Metallic Bond MasteryOnline version Quiz on metallic bonds and properties by Faith 1 How does a metallic bond form in a metal lattice? a Delocalized electrons are shared by a lattice of cations. b Ions exchange electrons with neighboring ions. c Electrons are localized around individual atoms forming ions. 2 Why can metals conduct electricity? a Ions shuttle charges only at high temperatures. b Free-moving electrons carry charge throughout the structure. c Bound electrons cannot move, only the lattice conducts. 3 Why do metals conduct heat well? a Only the atoms at the surface conduct heat in metals. b Delocalized electrons rapidly transfer kinetic energy. c Heat travels only via lattice vibrations in metals. 4 What gives metals malleability and ductility? a Rigid crystal lattice prevents any movement of atoms. b Delocalized electrons cushion and allow atom layers to slide. c Strong ionic bonds hold layers rigidly together. 5 Why are ionic compounds typically brittle? a Their electrons are delocalized like metals. b They form metallic bonds that crack easily. c Relief of stress creates ionic lattice fracture with oppositely charged layers. 6 How does electron sea model explain malleability? a Electrons form fixed bridges between ions. b A sea of electrons allows layers to glide past each other. c Ions are free to move individually under stress. 7 What happens to metallic bonds when heated? a Bonds break and metal becomes ionic. b Cations vibrate; electrons still move freely, aiding conduction. c All electrons become fixed to atoms when heated. 8 Which property distinguishes metals from ionic solids? a Metallic bonding with electron delocalization. b Ions are never present in metallic solids. c Covalent sharing of electrons between nonmetals. 9 How does alloying affect metallic bonding? a Introduces different-sized atom networks, hindering dislocations. b Increases ionic character drastically. c Removes delocalized electrons entirely. 10 Which statement best describes durability of metals? a Ions lock positions rigidly, preventing any movement. b Delocalized electrons reduce friction and enable plastic deformation. c Electron sea makes metals insoluble in all solvents.

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Metallic Bond Mastery

Froggy Jumps

About this activity

Created by

Download the paper version to play

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Metallic Bond MasteryOnline version

by Faith

How does a metallic bond form in a metal lattice?

Why can metals conduct electricity?

Why do metals conduct heat well?

What gives metals malleability and ductility?

Why are ionic compounds typically brittle?

How does electron sea model explain malleability?

What happens to metallic bonds when heated?

Which property distinguishes metals from ionic solids?

How does alloying affect metallic bonding?

Which statement best describes durability of metals?