![]() ![]() Rutherford did not identify it as an element and several other contemporary scientists also investigated it and proposed the names burnt air and phlogisticated air. Even though 78% of the Earth’s atmosphere is nitrogen gas, it was only discovered in 1772 by Daniel Rutherford who called it noxious air. Display:Ĭarbon fibre, anthracite coal, charcoal, graphite brushes from a motor and graphite electrodes, low density polyethylene and different allotropes of carbon: diamonds (loose), diamond-tipped drill bit, graphite, fullerenes (carbon nanotubes), graphene (in solution) Nitrogen – N – element 7 History:Īmmonia, nitric acid and nitrate salts were known, in some cases, since ancient times. Carbon has a crucial biological role and all plant and animal products contain carbon. Carbon fibres are used in woven materials. Uses:Ĭarbon’s main industrial uses are as a fuel (coal, oil, and gas) and for making plastics, it is combined with iron to make steel, and diamonds are used in cutting and drilling tools. They proposed the name carbone after the Latin carbo meaning charcoal. Vandermonde did the same with graphite, previously believed to be a type of lead. Similarly, in 1786, Claude Louis Berthollet, Gaspard Monge, and C. In 1772, Antoine Lavoisier showed that diamonds and charcoal produced the same reaction products when burnt. Display:Ĭarbon was known since prehistoric times in the form of charcoal, however it was not known that diamonds and graphite are the same element. Boron compounds such as borax and boric acid are used domestically as cleaning products, insecticides, and food additives amongst other uses. Uses:īoron is used as an additive in glass, particularly fiberglass and borosilicate glass, and in ceramics. The name boron was adopted by analogy with carbon. In 1808 boron was isolated independently by Joseph Louis Gay-Loussac and Louis Jacques Thenard, and Humphry Davy who proposed the name boracium, after the mineral borax. ![]() Together with groups 17 and 18, these elements form the p-block.Īlthough boron-containing minerals were known historically, boron compounds were not used widely prior to the 19th century when the mineral borax became widely available. The lighter group 15 elements can form anions with a -3 charge, and the lighter group 16 elements can form anions with a -2 charge. Group 15 elements have 5 valence electrons in their outer shell, and group 16 elements have 6.The lighter of these elements can form both cations with a +4 charge, and anions with a -4 charge. Group 14 elements have 4 valence electrons in their outer shell.Group 13 elements have 3 valence electrons and mostly form cations with a +3 charge.As a result, these groups contain non-metals like nitrogen, oxygen and sulfur, all the semimetals, and metals like aluminium, tin, lead, and bismuth. The metallic properties of these elements decrease along each period and increase down each group. The thing they have in common is the progressive filling of a p-orbital. Groups 13-16 don’t really fit together in any nice way, so let’s look at them one by one. Why are elements in Groups 13-16 categorised together? The charges of most monatomic ions derived from the main group elements can be predicted by simply looking at the periodic table and counting how many columns an element lies from the extreme left or right.In this article, we give you the history and uses for the elements in Groups 13-16. Ions such as these, which contain only a single atom, are called monatomic ions. ![]() Conversely, elements in groups 17, 16, and 15 often react to gain one, two, and three electrons, respectively, to form ions such as Cl −, S 2−, and P 3−. Because the lanthanides and actinides formally belong to group 3, the most common ion formed by these elements is M 3 +, where M represents the metal. In addition, the elements in group 13 lose three electrons to form cations, such as Al 3 +, again attaining the same number of electrons as the noble gas closest to them in the periodic table. Similarly, K +, Ca 2 +, and Sc 3 + have 18 electrons each, like the nearest noble gas: argon. They then have the same number of electrons as the nearest noble gas: neon. The planes of an NaCl crystal reflect the regular three-dimensional arrangement of its Na+ (purple) and Cl− (green) ions.Ĭonsistent with a tendency to have the same number of electrons as the nearest noble gas, when forming ions, elements in groups 1, 2, and 3 tend to lose one, two, and three electrons, respectively, to form cations, such as Na + and Mg 2 +. ![]()
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