Chapter 3_Part 1_ Composition of Substances and Solutions_Formula Mass and the Mole_ SP21.pdf.pdf

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1Chapter 3 -Composition of Substancesand Solutions1Part 1: The MoleOutline - Chapter 32Module 53.1 Formula Mass and the Mole Concept3.2 Determining Empirical and Molecular FormulasModule 63.3 Molarity3.4 Other Units for Solution Concentrations3Textbook Readings and Practice Problems - Chapter 3Part 1Readings: Sections 3.1-3.2Problems: 3, 5, 9, 15, 17, 21, 23, 27, 29, 33, 35, 37, 39, 414Formula Mass (FM)Theformula massof a substance is the sum of the averageatomic masses of all the atoms in the substance’s formula.The formula mass of a covalent substance may be correctlyreferred to as amolecular mass.The average mass of a chloroform molecule, CHCl3, is 119.37 amu, which is the sumof the average atomic masses of each of its constituent atoms. The model shows themolecular structure of chloroform.Source: OpenStax, Chemistry 2e1234
25Table salt, NaCl, contains an array of sodium and chloride ions combined in a 1:1ratio. Its formula mass is 58.44 amu.Formula Mass (FM)Theformula massof an ionic substance is the sum of theaverage atomic masses of all the atoms in the substance’sformula.Source: OpenStax, Chemistry 2eThe MoleThe mole (mol) is defined as the amount of a substance containingthe same number of discrete entities (such as atoms, molecules, orions) as the number of atoms in a sample of pure carbon-12weighing exactly 12 g.The mole provides a link between the mass of a sample and thenumber of atoms, molecules, or ions in that sample.1 mole of anything = 6.022 x 1023units (atoms, molecules, ions) ofthat thing.

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Term
Spring
Professor
AnthonyS.Drager
Tags
Atom, Mole, Molecule, Atomic mass unit, Empirical Formulas

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