Some metals, such as gold and silver, are so unreactive they occur largely uncombined with other elements, and are relatively simple to obtain. This is because they can react with the compounds in metal ores, and displace the metals, aiding with their extraction. You’ll notice in the graphic that carbon and hydrogen are also shoehorned in between entries in the list, despite being non-metals. This is illustrated below:Ĭopper sulfate + zinc → zinc sulfate + copperĪs well as helping us predict the outcomes of these reactions, the reactivity series also gives us an insight into why different metals are extracted from their ores in different ways. Conversely, if we try and react a metal compound with a metal lower in the reactivity series, no reaction will take place. If a metal compound reacts with a metal that’s above it in the reactivity series, a displacement reaction will occur, and the more reactive metal will take the place of the less reactive metal in the compound. What use does this series have beyond ranking the reactivity of metals, though? Well, for one, it can help us predict the outcome of certain chemical reactions. The metals designated as the transition metals in the periodic table are much less reactive, and metals such as gold and platinum prop up the bottom of the series, exhibiting little in the way of chemical reaction with any everyday reagents. They’re closely followed by the marginally less reactive group two metals. Group 1 metals, the most reactive metals in the periodic table, head up the rankings. The reactivity series offers a ranking of the metals in order of their reactivity. Caesium, the most reactive metal in the periodic table, reacts extremely violently – hence why it can’t be demonstrated in a classroom! This can be compared to other common metals, such as iron and copper, which produce no reaction when dropped into water. Lithium fizzes gently, sodium fizzes vigorously, and potassium’s reaction is so energetic it bursts into a lilac flame as it zips across the water’s surface. In this demonstration, small pieces of three different metals from group 1 of the periodic table are dropped into a large bowl of water. Metals have a range of reactivities – to illustrate this, you have to look no further than the classic alkali metals in water demonstration commonly used in chemistry classes. This graphic places a selection of common metals into order of reactivity, as well as showing their reactions with air, water and steam. It’s also a useful tool in predicting the products of simple displacement reactions involving two different metals, as well as providing an insight into why different metals are extracted from their ores in different manners. Groups of nonmetals include the nonmetals, halogens, and noble gases.The metal reactivity series is a commonly taught concept in chemistry, placing the metals, as its name suggests, in order of reactivity from most reactive to least reactive. Groups of metals include the alkali metals, alkaline earth metals, transition metals, basic metals, lanthanides, and actinides. Elements may be further subdivided into groups. While all of the metals except mercury are solid under ordinary conditions, nonmetals may be solids, liquids, or gases at room temperature and pressure. In contrast, most nonmetals are poor conductors of heat and electricity, tend to be brittle solids, and can assume any of a number of physical forms. Metals are generally good conductors of heat and electricity, are malleable and ductile, and have a lustrous metallic appearance. These elements are found along a zig-zag line that runs from the upper left of group 13 to the bottom right of group 16. Elements that have some properties of metals and some properties of nonmetals are called metalloids or semimetals. The far right side contains the nonmetals, plus hydrogen displays nonmetal characteristics under ordinary conditions. They are found on the lefthand side of the table. Another way to categorize elements is according to whether they behave as metals or nonmetals.
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