Metallic bonding-exercises
 

Consider the lattice structure of Na and Mg. The relative size of both ions in the lattice structure is similar. Explain in terms of electrostatic attraction why the melting point of Na is approximately 98 oC while the melting point of Mg is approximately 648 oC?

Give reasons why aluminium has a melting point of approximately 660 oC while boron has a melting point of close to 2,300oC.

Explain the changes that happen to the metal lattice when it is work hardened.

 

What is quenching and how does this change the property of the metal?

Consider the diagram on the right of a metal lattice. It shows metals ions with a smaller non-metal atom scattered amongst the ions.

What is the general name given to such a metal?

Explain how the metal's properties change?
Explain why metals, such as copper, are good conductors of electricity and heat.

Tungsten metal is used in incandescent light globes.

Name two properties of tungsten that make it useful for this purpose.
1)

2)

What is the mass of gold in a 40 gram 18 carat gold ring?
What name can best be used to describe the metal in the ring?
What is the metallic bonding model ?
What properties of metals are not able to be explained by the metallic bonding model?
Negative chlorine ions are attracted to the anode and form chlorine gas. Positive sodium ions are attracted to the cathode and form sodium metal. Power source Water molecules orient themselves to expose their negative end to the positive ion.Water molecules orient themselves to expose their negative end to the positive ion. Water molecules orient themselves to expose their negative end to the positive ion.Water molecules orient themselves to expose their negative end to the positive ion. Water molecules orient themselves to expose their negative end to the positive ion. Water molecules orient themselves to expose their negative end to the positive ion.Water molecules orient themselves to expose their negative end to the positive ion. The water molecules orient themselves to expose their positive end to the negative ion. The water molecules orient themselves to expose their positive end to the negative ion. The water molecules orient themselves to expose their positive end to the negative ion. The fluorine atom attracts the electrons towards it unevenly and results in this end of the molecule having a slightly negative charge. The fluorine atom attracts the electrons towards it unevenly and results in this end of the hydrogen atom having a slightly positive charge. Hydrogen molecule Hydrogen molecule Hydrogen molecule