4.1 - Metallic Properties and Bonding

Metallic bonds form because metals

• "want" to give up valence electrons

• always share valence electrons

• have many valence electrons

• always gain valence electrons

In metallic bonds, the force of attraction is between

• positive and negative ions

• cations and electrons

• two different metals

• neutrons and electrons

Which metal atom provides the most electrons for the sea of delocalised electrons?

• Aluminium

• Sodium

• Calcium

• Magnesium

Which statement describes the lattice structure of a metal?

• The lattice consists of alternating positive ions and negative ions.

• The lattice consists of neutral atoms arranged in layers.

• The lattice consists of positive ions in a ‘sea of electrons’.

• The lattice consists of neutral atoms in a ‘sea of electrons’.

The diagram shows metallic bonding.

Which labels are correct?

• X: atomic nucleus

  Y: outer electron

• X: metal atom

  Y: delocalised electron

• X: metal cation

  Y: delocalised electron

• X: positive ion

  Y: negative ion

Another word for shiny

• Ductile

• Conductive

• Malleable

• Lustrous

Can be beaten into thin sheets

• Ductile

• Brittle

• Malleable

• Flexible

Having the ability to be drawn into a wire describes which property?

• Malleable

• Ductile

• Brittle

• Conductive

Which statement about metals is correct?

• Layers of positive ions can slide over each other making metals malleable.

• Metallic bonding consists of a lattice of negative ions in a sea of delocalised electrons.

• Metallic bonding consists of a lattice of positive ions in a sea of delocalised negative ions.

• Metals conduct electricity because positive ions are free to move.

Which statement about metals is not correct?

• Metals are malleable because the metal ions can slide over one another.

• Metals conduct electricity because electrons can move through the lattice.

• Metals are hard due to the strong attraction between the metal cations and the sea of delocalised electrons

• Metals have high melting points due to the strong attraction between metal cations.