1) Metal P + H2O = hydroxide of Metal P and H2 (moderate rate) (Metal P discovered in A.D. 1808)What is metal P? Give some reasons.2) Metal R + aqueous solution of Mercury nitrate = Metal Q + aqueous solution of nitrate of Metal RMetal R + dilute HCL = No reaction (Metal R discovered in B.C., year not recorded)What is metal R? Give some reasons.3) Oxide of Metal S + CO = S + CO2 (Metal S discovered in A.D. 1000)Oxide of S + H2 = No reactionWhat is metal S? Give some reasons.4) Arrange metals P, Q, S and Mercury in decreasing order of reactivity.5) How to balance Al + Fe(2+) = Al(3+) + Fe?
Malleability: Easily bent, and hammered into shape. - Conductivity: Conducts electricity well. - Ductility: Easily made into wire.
* Metals are elements that have atoms arranged in rows. The electrons are easily released from metal atoms so that layers of metal atoms exist in a 'sea' of electrons. * Examples of Metals are gold, copper, lead, zinc, iron, magnesium, sodium, calcium and mercury. * Physical Properties of Metals include shiny lustre, greyish - silver colour, hardness, good heat and electricity conductivity, high melting and boiling points, malleability (can be hammered into a sheet) and ductility (can be pulled into a wire). Some exceptions to these are the metals - sodium and calcium (very soft), gold and copper (yellowish colour), and mercury (low melting and boiling points). * Chemical Properties of Metals Some metals are more reactive than others. This is because very reactive metals lose electrons easily. Metals such as sodium are very reactive and are explosive in air. Metals such as gold are very unreactive, and therefore do not corrode or tarnish in air.
