2. Properties of Metals and Non-Metals Done By: Sherrell Mungal

3. Metals

4. Physical Properties  Metals are solid except for mercury, which is liquid at room temperature.  They are malleable and ductile meaning it can be bent or put out of shape without breaking.  Very good conductors of electricity and heat.  They have high densities, melting points and when struck, a sound comes out from it. (Metallic sonority)  They have a characteristic metallic lustre.

5. Reactions of Metals  Metal + Oxygen  Metal Oxide  Metal + Steam  Metal oxide + hydrogen  Metal + Water  Metal hydroxide + hydrogen  Metal + Acid  Salt + hydrogen N.B Metals react with dilute non-oxidising acids. Examples are HCL (Hydrochloric acid) & H 2 SO 4 (Sulphuric Acid)

6. The Reactivity Series  This is simply a listing of metals in order of their reactivities. In this listing only common metals are placed but note that all metals can make up the reactivity series.  Following the arrow, we can see the decreasing reactivity. In this listing Potassium is the most reactive metal while, at the bottom of the list, Platinum is the least reactive. MetalSymbol PotassiumlK SodiumlNa MagnesiumlMg AluminumlAl ZinclZn IronlFe TinlSn LeadlPb HydrogenlH CopperlCu SilverlAg GoldlAu PlatinumVPt

7. Uses of the Reactivity Series  This shows a comparison of reactivity with metals.  To predict displacement reactions between metals and their salts. A metal higher up in the series is able to displace one lower down from its salt. Mg (s) + CuO (s)  MgO (s) + Cu (s) Mg (s) + CuO (s)  MgO (s) + Cu (s) Magnesium + Copper oxide  Magnesium oxide + Copper Magnesium + Copper oxide  Magnesium oxide + Copper  To predict how salt reacts with heat in a chemical reaction. Metals higher up in the series tend to form salts that are more thermally stable than those lower down. Salts of metals lower down decompose according to general equations.  To determine the most suitable method of extraction of metal from its ore.

8. Non- Metals  Anything that isn’t classified as a metal is referred to as a non- metal.  There are two types of non-metals, 1) Non-metal elements (chlorine, sulphur, carbon, oxygen etc) & 2) Non-metal compounds (sodium chloride, sulphur dioxide, ammonia, nitric acid etc)

9. Physical Properties  They are considered poor conductors of heat and electricity.  They are brittle  Dull in colour  Low in sonority

10. Facts  Ionic substances are only considered conductors when aqueous or in its molten form  Graphite is a well known non-metal which shares some properties of metals (it is a good conductor of electricity and has a shiny appearance), however it is very brittle and has low sonority.

11. Chemical Properties  Reacts with air or oxygen on heating to produce covalent acidic oxides. e.g. S (s) + O 2 (g)  SO 2 (g) N.B The only non-metal that reacts at room temperature is phosphorus to form phosphorus trioxide P 4 O 6  Reacts with metals to produce ionic compounds. e.g. Fe (s) + S  FeS (s)  Do not react with dilute acids  Do not react with water. The exception however is chlorine which reacts with water to give an acidic solution know as chlorine water. Cl 2 + H 2 O  HCl (aq) +HOCl (aq)