METALLIC BONDING

Gap-fill exercise.

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Fill in all the gaps, then press "Check" to check your answers. If available use the "Hint" button to get a free letter if an answer is giving you trouble. You can also click on the "[?]" button if available to get a clue. Note that you will lose points if you ask for hints or clues!
   2 delocalised electrons      3      attraction      closely packed      conductivity      delocalised      densed      ductile      easily lose      gp 2      Gp 3      group 1      hammered      higher      increases      ionisation energy      ions      lattice      layers      lose      malleable      mobile      move around      negatively      no longer attached      not strongly held      number of valence electrons increase      positive ions      positively charged      positively charged metal      range      same period      sea of delocalised      slide past      stretched into thin wires      strong electrostatic bonding      stronger      transfers this energy      valence      valence electrons are highly mobile      vibrate faster   
Metallic Bonding

Metals can easily their electrons. For instance a sodium atom can one electron to give a sodium ion.

What is the evidence?

Metals have low . This is an indication that the valence electrons are . So they can easily lose them.

In metallic structures we can visualise these electrons been and free to . They are not attached to any one atom either. As the valence electrons are to any one atom what results is that the atoms become which have achieved the stable octet configuration.

Metallic bonding is thus made up of the between the metal in a and valence electrons.
They are arranged in a structure.

Metals have characteristic properties. They include high electrical . This is because the and any voltage applied can move the electrons along.

Metals also have high thermal conductivity. When a metal is heated particles in the metal structure will . The delocalised electrons in the metal lattice readily as they move through the lattice.

Metals are which means they can be easily into shape. They are also which means they can be .

This is because the metal cations are arranged in that can easily each other. The electrostatic forces between the cations and the charged electrons are not affected.

Metals exhibit a of melting and boiling points.

Some metals have melting and boiling points than others.
Take for instance Na, Mg and Al. Their melting points are 98, 650 and 660 deg C respectively. They belong to the but Na belongs to , Mg in and Al in . The number of valence electron in Na is one, in Mg 2 and that of Al is . This means that Mg can have for every Mg atom.

As the the electrostatic forces in the metallic bond gets and the result is melting point and boiling point.

Finally due to between the electrons and the cations the ions become . For that reason metals are usually . They are said to have high density. As the number of valence electrons per atom the density also .

We can see that it is the case because the density for Na is 0.97 g/mL, for Mg it is 1,74 g/mL and for Al it is 2.7 g/mL. They are in the same period.

 

 

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