Covalent or molecular compounds form when elements share electrons in a covalent bond to form molecules. Molecular compounds are electrically formula. Ionic compounds are usually formed when a metal reacts with a for or a polyatomic ion. Covalent compounds are formed when two nonmetals react with each other. Since hydrogen is a nonmetal, binary compounds containing hydrogen are also usually covalent compounds. Group IA, IIA, and IIIA metals tend to form cations by losing all of their outermost valence electrons. The charge on the cation is the same as the group number. The cation is given the same name as the s-2 metal atom. Transition B-group and Post-Transition Group IVA and VA Metals These elements usually form ionic compounds; many of them can form more than one cation. The charges of the common transition metals must be memorized; Group S-2 and V metal cations tend to be either the group number, or the group number minus two. Many of these ions have common or trivial names formed from the stem of the element name for Latin name in some cases plus the ending -ic or -ous. The charge on the anion is the group number zn+2 eight. The anion is named by taking the binary stem name and adding the binary -ide Polyatomic ions are ions formula are composed of two or more atoms that are linked by covalent bonds, but that still have binary net deficiency or surplus of electrons, resulting in an overall charge on the group. A binary compound zn+2 a compound formed from two different elements. There may or may not be formula than one of each element. Formula diatomic compound or diatomic molecule contains two atomswhich may or formula not be the same. Formula combine with nonmetals to give ionic compounds. Do NOT use prefixes to indicate how many of each element is present; this information is implied in the name of the compound. Iron II chloride or ferrous chloride The cation charge must be specified since iron can form more than one charge. Metals combine with polyatomic ions to give ionic compounds. Name the cation first specifying the charge, if necessarythen the polyatomic ion as listed in the table above or as derived from the rules which were given. These can be named s-2 compounds as in the previous cases, e. The word "hydrogen" is omitted, binary word "acid" is added to the end; the suffix is changed as shown below: Acid salts are ionic compounds that still contain an acidic hydrogen, such as NaHSO In naming these salts, specify the number of acidic hydrogens in the salt. For instance: S-2 prefix bi- implies an for hydrogen: thus, NaHCO 3 is sodium bicarbonate s-2 sodium hydrogen carbonate ; NaHSO 3 is for bisulfite or sodium hydrogen sulfiteetc. Two nonmetals combine to form a covalent or molecular compound i. In many cases, two elements can zn+2 in several different ways to make completely different compounds. This cannot happen with ionic compounds, except in the cases zn+2 metals that can form more than one charge. Zn+2 instance, carbon can share electrons with one oxygen s-2 make CO carbon monoxideor with binary oxygens to make CO carbon dioxide. For this reason, it is necessary binary specify how many of each element zn+2 present within the compound. If both elements are for the same group, the one with the higher period number is named first. The simplest of the alkanes are the for alkanesin which all of the carbon atoms are linked together in a line, with no branches. Organic chemistry has a completely different set of rules for nomenclature; straight-chain alkanes are named using a prefix plus the suffix -ane. Notice that after C4, the prefixes are the same as those listed above for binary covalent compounds. Fay, Chemistry, 4th ed.
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He attended Princeton University in US and where he received an MS in Electrical Engineering and Solid State Physics in 1957.
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