Chapter Two Chemical Compounds
Chapter two discussed chemical compounds and their different representations whether naming and or through formula format. From such information, the amount of atoms, moles, and or determining charges can be found. All formulas can convey a limited amount of information depending on which structure has been selected to represent the compound. Compounds are usually shown by a chemical formula. Once compounds have bonded through the attraction of protons and electrons, if the bond is ionic or covalent may be shown now. An ionic compound forms when a metal and nonmetal bond explaining the electron transfer and attraction of charged ions. On the other hand, a covalent compound, forms when two nonmetals attract to each other, when some of their atoms share an electron. Ionic and …show more content…
An exception for the first element is enforced only if the required prefix is mono-. Another quintessential factor of writing the name or formula are polyatomic ions. Polyatomic ions are single ions that contain more than one atom. The name and or charge of a polyatomic ion does not vary/change. Common polyatomic ions include nitrite (NO2-) or sulfate (SO4^2). Similar to ionic and covalent compounds, the naming system is unique to its characteristics. Depending on the elements group on the periodic table, the ending of the anion will have –ate, although the amount of oxygen within the formula will determine if the name requires a prefix. Acids depend on the presence of a hydrogen atom which becomes the first element and if the acid contains only two elements, binary, or an oxygen atom which becomes an oxyacid. Binary acids end with –ic; an oxyacid includes –ous when the original ending ended in –ite and –ic when the original ending ended in –ate. Within the compound, an element may require the mass of one mole. One mole of anything equals 6.022 x 1023, also known as Avogadro’s number. The mass of one mole can be determined by Molar mass= 1
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