6.4 Metallic Bonding

What is the basis of a metallic bond?

• the attraction of neutral metal atoms.
• the attraction between protons and neutrons.
• the attraction between positive metal ions and interlocking electrons.
• the attraction between positive metal ions and free floating electrons.

There are more metals than non metals in the periodic table.

• True
• False

At room temperature, most metals are

• liquid
• solid
• gas
• an alloy

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What does malleable mean?

• able to be shaped
• will break easily
• can be used for wire
• is shiny

Which of these is NOT an alloy?

• bronze
• copper
• brass
• stainless steel

Electrons that are free to move in metals

• delocalized electrons
• oxidation number
• chemical bond
• salts

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What is the ability of a substance to be pulled into a thin strand?

• Malleability
• Ductility 
• Conductivity
• Solubility

Why do metals have high melting points?

• They don't
• The negatively charged electrons act as a glue to hold the positively charged ions together.
• All the electrons become delocalised

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Why do metals conduct

• They are shiny
• The electrons are held tightly within the lattice
• The electrons are delocalised and able to move
• The electrons are shared between two metal ions

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Why are alloys generally used to make everyday objects?

• Alloys are often stronger and less active than pure metals.
• Alloys have higher melting point than pure metals.
• Alloys are less expensive to produce than pure metals.
• Alloys have ionic bonds instead of metallic bonds.

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