Nonmetal carbonates

In principle, any element whose Ellingham line lies below the Ellingham line of a specified element, is capable of reducing the oxide of the specified element to the elemental state. In practice, however, only the nonmetals, carbon, hydrogen and silicon, and the met-... 

Nonmetals carbon, nitrogen, oxygen, silicon, phosphorus, sulfur, chlorine, bromine, and iodine... 

Although the electrochemistry of organic compounds is the focus of the next chapter, several carbon molecules are more appropriate to the present discussion of nonmetals. Carbon dioxide (C02, 0=C=0) and carbon monoxide (CO, C = 0 ) are the products of hydrocarbon combustion, and cynanide ion (CN NC", N = C ) is unique with respect to a stable carbon-centered anion. 

These reactions are discussed in treatises on organic chemistry. Hydrogenolysis of metal- or nonmetal-carbon bonds are used for small-scale specialty chemical syntheses ... 

The pattern metal-metalloid-nonmetal-noble gas is typical for the main group elements in each period. Period 2 begins with a metal, lithium, and ends with a noble gas, neon. In between are the metal beryllium the metalloid boron and the nonmetals carbon, nitrogen, oxygen, and fluorine. Remember that the most active metals. Groups 1 and 2, are in the s region of the periodic table. The metalloids, nonmetals, and less active metals are in the p region of the periodic table. 

It should be noted that in groups IVA, VA, and VIA, the elements at the top are nonmetals (carbon, nitrogen, and oxygen) and those at the bottom are metals (lead, bismuth, and polonium). The stairstep cuts these groups in two, separating metals from nonmetals with metalloids in the middle. 

It s important to realize, however, that an element s properties may not fall neatly into our categories. For instance, the nonmetal carbon in the form of graphite is a good electrical conductor. Iodine, another nonmetal, is a shiny solid. Gallium and cesium are metals that melt at temperatures below body temperature, and mercury is a liquid at room temperature. And iron is quite brittle. Despite such exceptions, we can make several generalizations about metallic behavior. 

All three categories of elements occur within Group 4A(14), from the nonmetal carbon (C) through the metalloids silicon (Si) and germanium (Ge) and down to the metals tin (Sn) and lead (Pb) [Group 4A(14) Family Portrait, p. 434]. 

The second-row nonmetals carbon through fluorine form stable molecules when they are surrounded by enough electrons to fill the valence orbitals—that is, the one 2s and the three 2p orbitals. Eight electrons are required to fill these orbitals, so these elements typically obey the octet rule they are surrounded by eight electrons. An example is the F2 molecule, which has the following Lewis structure ... 

In Figure 8.1, electrical resistivities (inversely proportional to conductivities) of the solid main group elements are plotted. At the far left are the alkali metals, having low resistivities (high conductances) at the far right are the nonmetals. Metals contain valence electrons that are relatively free to move and thereby conduct current. In most cases, non-metals contain mnch more localized electrons and covalently bonded pairs that are less mobile. Oraphite (Section 8.6.1), an allotrope (elanental form) of the nonmetal carbon, is an exception that has a mnch greater ability to condnct than most nonmetals because of delocalized electrons. 

Group 14 (IV A) (the carbon group) includes a nonmetal (carbon), silicon, and germanium, which are metalloids (Si behaves as a nonmetal mostly, but Ge behaves as a metal) and the typical metals, tin and lead. These elements have 4 electrons in the outer energy level, 2 of which are in the last p orbitals (p ) (Table 2.4). These 4 electrons are usually shared silicon and germanium can form +4 ions, tin and lead can form +2 ions, and only carbon can form -4 ions. 

PowerLecture Determining the Atomic Radius of a Nonmetal (Carbon)... 

Sarah informs her customer that aspirin is acetylsali-cylic acid and has the chemical formula, C9H8O4. Aspirin is a molecular compound, often referred to as an organic molecule because it contains the nonmetals carbon (C), hydrogen (H), and oxygen (0). Sarah shows her customer the chemical structure of aspirin, and explains that aspirin is used to relieve minor pains, to reduce inflammation and fever, and to slow blood clotting. Some potential side effects of aspirin may include heartburn, upset stomach, nausea, and an increased risk of a stomach ulcer. 

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