Chapter 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

Electrons that are free to move in metals are called ..

• delocalized electrons

• oxidation number

• chemical bond

• salts

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 electricity and heat? Because ..

• 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

Why does the melting point of metals increase across period 3, from Sodium (Na) to Aluminium (AI)?

• Size of atoms gets smaller

• Attraction force between nuclei and free electron increases

• Increased space between the valence electrons in the "sea"

• Increased number of valence electrons contributed to the "sea"

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Why do metallic compounds conduct electricity as solids?

• core electrons are mobile, allowing electricity to flow through the metal

• valence electrons are mobile, allowing electricity to flow through the metal

• protons are mobile, allowing electricity to flow through the metal

• the metal cations are mobile, allowing electricity to flow through the metal

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