PPT-Composition of Substances and Solutions Atomic Mass and Formula Mass;

Composition of Substances and Solutions Atomic Mass and Formula Mass Mole amp Molar Mass Percent Composition of Compounds Determination of Empirical amp Molecular Formulas Molarity Other Units for Solution Concentrations. Calculate the following percentage by mass:. percent = portion/total x 100. If two samples are the same substance, they should have the . same percent composition by mass.. A compound will have the same physical and chemical characteristics.. Harmful substance-many materials or substances used or created that could harm your health. These substances could be dusts, gases, or fumes that you breathe in, or liquids, gels or powders that come into contact with your eyes or skin. . The Molecular Nature of Matter and Change. Seventh Edition. Martin S. Silberberg and Patricia . G. Amateis. Copyright .  . McGraw-Hill Education. All rights reserved. No reproduction or distribution without the prior written consent of McGraw-Hill Education.. th. Grade Science. What are “Substances”? . Substances can be identified as either…. Elements. Compounds. Mixtures. So, what is a substance?. A substance cannot be further broken down or . p. urified by physical means.. A Dozen Elephants & . A Dozen Paper Clips. Would a dozen of each weigh the same amount? Give a reason for your answer.. Moles and Mass. The molar mass gives us the relationship between the number of moles and the mass of an element or compound.. Moles and Mass. The . molar mass . gives us the relationship between the . number of moles . and the . mass of an element or compound. .. We can . use the molar mass . to . calculate . the . mass. or . Compounds are ALWAYS composed of elements in fixed ratios. This is often referred to as the . Law of Definite Proportions.. This law states that elements are always present in the same proportions by mass in a compound. I.e. H. The Mole. Chemist’s counting number. amount. of a substance . 1 mole is equal to 6.022 x 10. 23. atoms or particles or molecules (Avogadro’s number). There are always 6.022 x 10. 23 . particles in . Atomic mass. Atoms of different elements have different masses. . Mass of a single atom is incredibly small so a special unit called atomic mass unit (. amu. ) is used. . Atomic Mass. Atoms are composed of three particles:. Atomic Mass. Empirical formula. Yield. CC9 . - Calculating Involving Masses . (p26-30). 1: O 2: C 3:Mg 4:Ca 5:N . 4. Empirical . formula . (. the . simplest ratio of atoms in a . Determining Molecular Formulas. Calculate the molecular formula of a compound whose molar mass is 60.0 g/mol and has an empirical formula of CH4N.. What you need:. Empirical Formula. Molar Mass. Calculate the molar mass of the empirical formula. (they are trivially simple, but they do give some interesting results if you ask the right questions). The Physical Principal – . Conservation of Mass. Bulk Silicate Earth . (the hypothetical homogeneous composition of the solid silicate Earth after core formation, but before any other differentiation process). Objectives:. -         . The student will determine percentage composition from formula data.. -         . The student will determine percentage composition of a hydrated salt.. In your notes…. Draw a model of an atom that best represents each component of that atom.. Foundations of Atomic Theory. Particle Theory of Matter. Democritus in 400 B.C.. Stated that nature’s basic particle was the atom (“indivisible” in Greek). .