IIIIIIIV The Mole I. Molar Conversions

A. What is the Mole? n A counting unit n Similar to a dozen, except instead of 12, it’s 602 billion trillion 602,000,000,000,000,000,000,000 n 6.02 X (in scientific notation) n This number is named in honor of n Amedeo Avogadro (1776 – 1856) n Amedeo Avogadro (1776 – 1856),

n 1 mole of hockey pucks would equal the mass of the moon! A. What is the Mole? n 1 mole of pennies would cover the Earth 1/4 mile deep! n 1 mole of basketballs would fill a bag the size of the earth!

How does a Mole relate? n 1 Mol = 6.02 x particles n If I had 1 mol of cookies, how many cookies would I have? n If I had 1 mol of cars, how many cars would I have? n If I had 1 mol of Aluminum, how many atoms would I have? n Note that the NUMBER is always the same, but the MASS is very different!

= 6.02 x C atoms = 6.02 x H 2 O molecules = 6.02 x NaCl “formula units” 6.02 x Na + ions and 6.02 x Cl – ions A Mole of Anything A Mole of Anything Contains 6.02 x particles 1 mole C 1 mole H 2 O 1 mole NaCl

Avogadro's Number n That means in grams of Hydrogen, there are:  6.02x10 23 atoms OR  602,000,000,000,000,000,000,000 n And that grams of Flourine, there are:  6.02x10 23 atoms OR  602,000,000,000,000,000,000,000

Molar Mass n Describes the mass of 1 mole of an element or compound. n Atomic mass tells the...  grams per mole (g/mol), used to describe the mass of one mole of an element or chemical compound. n Round to 2 decimal places!

B. Molar Mass Examples n carbon n aluminum n zinc g/mol g/mol g/mol

B. Molar Mass Examples n water n sodium chloride H2OH2O  2(1.01) = g/mol  NaCl  = g/mol

B. Molar Mass Examples n sodium bicarbonate n sucrose  NaHCO 3  (16.00) = g/mol  C 12 H 22 O 11  12(12.01) + 22(1.01) + 11(16.00) = g/mol

C. Multiple Moles Examples n 2 moles of water n 3.4 moles of sodium chloride  2 x (H 2 O)  2 x (2x(1.01) )  = g  The units of grams is because we now have multiple moles…  3.4 x (NaCl)  3.4 x ( )  = g