Ionic and Metallic Bonds

In metallic bonds electrons are:

• shared

• move around the nuclei randomly

• transferred

Malleability and ductility are characteristics of compounds with

• covalent bonds

• metallic bonds

• ionic bonds

• alloy bonds

Alloys are important because

• their properties are often superior to the component elements

• their properties are a blend of the component elements

• they never corrode

• they are less expensive than their component elements.

Why are metals good conductors?

• they have mobile electrons

• they have mobile atoms

• they have crystal structures that can rearrange

• they have mobile protons

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Malleability means

• the ability to be drawn into a wire

• the electrons of metals are mobile

• the ability to be hammered into a shape

• the ability to be a conductor of electricity

In metals, the valence electrons are

• attached to the most positive ions

• shared by all of the atoms

• are bonded to the least electronegative element

• shiny

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Metals are ductile because metallic bonds

• hold the layers of ions in rigid positions

• maximizes the repulsive force in a metal

• allows planes of protons and electrons to slide past one another

• are easily broken

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Metals are hard because metals have a

• sea of electrons that tightly hold the nuclei together

• they form triple bonds

• low melting point

• high luster

The positive ions tend to _____________ electrons.

• lose

• gain

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The negative ions tend to _____________ electrons.

• lose

• gain

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