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. Lesson 28. Warm up. Submit Mole Conversion packages in basket, and copy the following upon arrival. Write-Pair-Share. What is the percent of the total composition of each ingredient in the following recipe (masses are fictitious):. vs.. Gram Formula Mass. AMUs . vs. Grams. Aim: . How can we find the . formula mass . and . gram formula mass . of a compound?. Essential Questions:. How can we find the formula mass and gram formula mass of a compound?. 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.. Atoms and Reactions Lesson 1. 1.1.2. Atomic Masses. WARM UP:. Work out the relative molecular mass of:. Calcium carbonate - CaCO. 3. Magnesium chloride - MgCl. 2. . Methane – CH. 4. Copper sulphate - CuSO. What you need to know:. Relative formula mass. Empirical formula. % composition by mass. Use balanced equations to calculate masses of reactants and products. Yields. Quick . quiz – molecular mass and empirical formula. Why Study Chemistry?. . Think about current issues in the news.. . . . . . . 2. Why Study Chemistry?. . Think about current issues in the news.. Energy sources. . . 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.. Atomic Mass. What is an elements atomic mass?. The weighted average of its naturally occurring isotopes. .. When looking at an element on the periodic table of elements, where is atomic mass found?. Usually the top left hand corner of each elements box. However, on the periodic table that you will use for your AP Exam(s), this number will be located below each elements chemical symbol.. In a group, calculate the percentage of flasks, owls, . Marios. , pencils & stars. What if this was related to mass? Calculate the % by mass for each of the objects.. 100 g. 20 g. 5. 0 g. 2 g. 6. 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 . Mr. Guerrero. Stoichiometry. Homework, due on the day of chapter exam. . Zumdahl. Text, 9. th. ed. . page 126: . #10, 13, 18, 38, 40, 46, 50, 66, 74, 84, 86, 88, 100, 106, 122, 124, 126.. Write out all conceptual(non-math) questions & answer in complete sentences.. BASIC CHEMISTRY. CHM 138. Dalton’s Atomic Theory (1808). 1.. . Elements are composed of extremely small particles called . atoms. . . 2. All . atoms. of a given element are . identical, having the same size, mass and chemical properties. 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:. and Solutions. Atomic Mass and Formula Mass;. Mole & Molar Mass;. Percent Composition of Compounds;. Determination of Empirical & Molecular Formulas;. Molarity. Other Units for Solution Concentrations.