Chapter 11:.

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Presentation transcript:

Chapter 11:

By count By mass By volume A. Measuring Matter What are three methods for measuring the amount of something? By mass By volume

B. Words for Numbers What are some words you know that are used to identify an amount of something?

C. What is a Mole 1 mole = 6.02 x 1023 particles 602,000,000,000,000,000,000,000 Particles = molecules, atoms, or formula units

D. Moles to Particles Use dimensional analysis to answer the following questions (1 mole = 6.02 x 1023 particles) 1. How many moles is 2.17 x 1023 atoms?

D. Moles to Particles 2. How many moles is 5.50 x 1048 formula units

E. Particles to Moles How many atoms are there in 3.0 moles of copper atoms? How many molecules are there in 1.5 moles of water?

F. The Definition of the Mole Avogadro defined the mole as: 1 mole, 6.02 x 1023 particles, is exactly 12.0 g of carbon – 12 Recall: 12 amu = mass of 1 carbon – 12 atom The carbon – 12 isotope is used as the standard for both amu and the mole

Review! Using your periodic table…what is the atomic mass of the following elements and compounds? Ca Fe Cu Ar P

G. Atomic Mass vs. Molar Mass Atomic Mass (amu) Molar Mass (g/mol) Mass of 1 atom 1 atom of carbon = 12.01 amu Mass of 1 mole 1 mole of carbon = 12.01 g

H. Molar Mass of a Compound To calculate, sum up the atomic mass of each element in the compound. The atomic mass is the molar mass in g/mol

Practice Mg 1 24.305 amu 24.305 amu Cl 2 35.453 amu 70.906 amu Element Find the molar mass of magnesium chloride MgCl2 Element # of Atoms Atomic Mass (amu) Total Mass (amu) Mg 1 24.305 amu 24.305 amu Cl 2 35.453 amu 70.906 amu Total Mass (amu) = 95.211 amu Molar Mass (g/mol) = 95.211 g/mol

Practice Calculate molar mass of the following: KOH HCl H2SO4 Ca(OH)2