7D Metallic Bonding Review

What is metallic bonding?

• The bonding between two different metals

• Chemical bonding in metals where electrons are delocalized

• Chemical bonding in metals where protons are delocalized

• A type of bonding found in non-metallic elements

How does metallic bonding contribute to the thermal conductivity of metals?

• Metallic bonding creates strong covalent bonds between metal atoms

• Metallic bonding causes the electrons to be tightly bound to the nucleus

• Metallic bonding allows for the free movement of electrons

• Metallic bonding results in the formation of insulating layers between metal atoms

Explain the relationship between metallic bonding and electrical conductivity in metals.

• High electrical conductivity is due to the delocalized electrons in metallic bonding.

• Metals have high electrical conductivity because of their strong covalent bonds.

• Electrical conductivity in metals is not related to metallic bonding.

• Low electrical conductivity is due to the delocalized electrons in metallic bonding.

Why are metals malleable?

• Metals are malleable because they have a rough surface

• Metals are malleable because their atoms are tightly packed together

• Metals are malleable because their atoms can slide past each other when a force is applied.

• Metals are malleable because they are made of soft materials

Tags

NGSS.HS-PS1-3

Define ductility and explain how metallic bonding relates to the ductility of metals.

• Metals have ductility because they are made of non-metallic elements

• Metallic bonding causes metals to be brittle

• Metals have ductility because metallic bonding allows for the movement of atoms in response to stress.

• Ductility in metals is due to covalent bonding

What type of bonding is present in metals?

• Hydrogen bonding

• Metallic bonding

• Ionic bonding

• Covalent bonding

How does the structure of metals contribute to their thermal conductivity?

• The density of the metal's structure allows for efficient heat transfer.

• The free movement of electrons within the metal's structure allows for efficient heat transfer.

• The color of the metal's structure contributes to efficient heat transfer.

• The hardness of the metal's structure allows for efficient heat transfer.

Discuss the role of free electrons in the electrical conductivity of metals.

• Free electrons in metals are responsible for the color of the metal.

• Free electrons in metals attract other metals to form alloys.

• Free electrons in metals allow for the flow of electric charge.

• Free electrons in metals cause the metal to become brittle.

Tags

NGSS.HS-PS2-5

NGSS.HS-PS3-5

What property of metallic bonding allows metals to be hammered into thin sheets?

• Transparency

• Brittleness

• Malleability

• Ductility

Explain the relationship between metallic bonding and the ability of metals to be drawn into wires.

• Metals are drawn into wires due to the presence of covalent bonding

• Metallic bonding causes metals to be brittle and unable to be drawn into wires

• Metallic bonding allows for the movement of electrons within the metal lattice, which gives metals their malleability and ductility.

• Metallic bonding has no effect on the ability of metals to be drawn into wires