1. METALS Metals are…Solid at room temperature, except mercury, which is liquid ! Metals have…medium to high melting points Metals are…shiny when they cut. Metals are…good conductors of heat and electricity. Metals are…usually strong & malleable so they can be hammered into shape.

2. METALS

3. Metals in columns 1, 2, 3 are electron donors. NonMetals in columns 5, 6, 7 receive Electrons.

4. Metals The first widely used metal was copper – first mined and used on the island of Cyprus around 5000 years ago –Low melting point –Easily extracted from its ores Aluminium (most common metal in the earth’s crust) –Difficult and expensive to extract –Now widely used due to technological advances

5. Metallic Bonding Formed between atoms of metallic elements Good conductors in all states, lustrous, relatively high melting points, malleable. Examples; Na, Fe, Al, Au, Co

6. Structure of Metals Metallic atoms have low electronegativities - lose their valence electron(s) easily Once a metallic atom loses its outer shell electron(s) it becomes a positively charged cation. Metallic lattice structures are made up of an array of cations. The electrons from each metallic atom are found in a common pool and are free to move between all the cations and are called delocalized electrons.

7. Metallic Bonding - A Sea of Delocalized Electrons

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10. Structure of Metals Electrostatic forces of attraction between the positively charged cations (positive ions) and the negatively charged electrons hold the lattice together. A metal is therefore a seen as a rigid framework of cations immersed in a ‘sea’ of delocalized electrons that serve as the glue holding the three-dimensional framework together.

11. Properties of Metals 1. Lustre –due to mobile electrons within the lattice being able to reflect light causing the metal to shine 2. Conduction of heat – electrons are able to gain kinetic energy in hotter areas of the metal and are able to quickly transfer it to other parts of the metal lattice because of their freedom of movement. Heat causes the delocalized electrons to move faster and the ‘bumping’ of these electrons with each other (and the nuclei) transfers the heat.

12. Properties of Metals 3.Conduction of electricity – When an electric field is applied to a metal, one end of the metal becomes positive and the other becomes negative. All the electrons experience a force toward the positive end. The movement of electrons is an electric current.

13. Properties of Metals 4. Malleability an ductility – metals are malleable and ductile, rather than brittle, as a result of the non- directional nature of metallic bonds. The attractive forces exerted between the positive metal ions and the mobile electrons occur in all directions. This means that layers of atoms can move past one another without disrupting the force between the positive ions and the negative sea of electrons. The nature of the metal does not change when the metal becomes thinner.

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15. Properties of Metals 5.Melting point and hardness – The generally high melting points and hardness of metals indicate that metallic bonding is quite strong. Melting points and hardness increase with an increase in the number of outer shell electrons, since there is a greater attractive force between the cations and the electrons.