CHEM 210 1nd Edition Lecture 9 Outline of Last Lecture I. Covalent BondsII. Different Types of Chemistry FormulasIII. Naming CompoundsOutline of Current Lecture IV. Naming CompoundsV. Brief Introduction to Stoichiometry A. The MoleCurrent LectureIn chemistry, it is very important to learn how to name compounds. In the previous lecture, we learned how to name a few and we will continue here. For example, the name forFe(ClO4)2 would be Iron II perchlorate. This is because ClO4 has a negative one charge associated with it, with the name perchlorate. Since there are two of them, the charge on iron must be a positive two, to balance out the two negative one charges. Hence, the roman numeral II (two).Na2SO3 would be sodium sulfite. Sulfite (SO3) has a negative charge, and since there is one of them, the overall charge is 2-. Na (sodium) has a positive one charge, so in order to balance out with the sulfite, we must give Na a subscript of 2, giving it an overall charge of 2+.There are also ways to change compounds into acids by adding hydrogen to them. Br on its own is bromine. When you add an H, causing the formula to be HBr, it then becomes hydrobromic acid. IO3 with an H added to it (HIO3) becomes iodic acid.Arsenic (CN) becomes hydrocyanic acid when you add an H (HCN). These notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best used as a supplement to your own notes, not as a substitute.Lets work on naming two more compounds and then calculating their mass.P4S3 is known as tetraphosphorus trisulfide.NH4NO3 is named ammonium nitrate.To find the molecular mass, you simply multiply the number of each element, or subscript, by itsatomic mass.P4S3 would be (4 X 30.794) + (3 X 32.065) = 123.176 + 96.195 = 219.371The MoleThe Mole, or Avogadro’s number is equal to 6.022 X 10 ^ 23.A mole is equal to the amount of substance that contains the same number of entities as there are atoms in exactly 12 grams of carbon
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