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Holy Moley !

Holy Moley !. Mole Day : 10/23. Mole day is an unofficial holiday celebrated among chemists annually between 6:02am and 6:02pm on October 23 rd . Mole Day commemorates Avogadro’s Number (6.02 x 10 23 ), which is a basic measuring unit in Chemistry. What is Mole Day?.

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Holy Moley !

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  1. Holy Moley! Mole Day: 10/23

  2. Mole day is an unofficial holiday celebrated among chemists annually between 6:02am and 6:02pm on October 23rd. • Mole Day commemorates Avogadro’s Number (6.02 x 1023), which is a basic measuring unit in Chemistry. What is Mole Day?

  3. Avogadro’s number is used as a basic unit of measuring molecules in chemistry. • The atomic mass on the periodic table is the mass of 1 mole of an element. • In 1 mole of any given element or substance there are 6.02 x 1023molecules or atoms. • That means that there are 602,000,000,000,000,000,000,000 atoms of hydrogen in 1 gram of hydrogen! Why is this number so important in chemistry?

  4. The number is named after the scientist who first observed the relationship between the volume of a substance and the number of molecules, Amadeo Avogadro. • Avogadro was an Italian physicist who lived in the early 1800s. • In addition to observing the relationship between the amount of a substance and the molecules therein contained, Avogadro is also considered to be the father of physical chemistry. Why is it called Avogadro’s number?

  5. Avogadro’s number is like saying there’s a dozen eggs. • Ex: If there’s a dozen eggs, then there are 12 eggs. 1 dozen = 12 • If there is 1 mole of something, like Carbon, then there are 6.02 x 1023 atoms of Carbon. • In fact, there are 6.02 x 1023 atoms of Carbon in 1 gram of Carbon! Examples Using Avogadro’s number

  6. The unit “AMU” is used for atomic mass on the periodic table. • 1 AMU = 1 gram per mol (g/mol) • So, if you have a certain number of grams of an element, then you can figure out how many moles of that element you have (or visa versa). • Ex: If you have 2 grams of K (potassium), and the atomic mass of K is 39.0983 AMU or g/mol, then (2 grams) x (1 mol/39.0983 g) = 0.05 moles K. • Then, you can find the # atoms in 0.05 moles K by multiplying by 6.02 x 1023to get 3.01 x 1022 atoms. Examples Using Avogadro’s number (cont’d)

  7. 1. How many atoms of Calcium are in 1 mole of Calcium? • 2. How many molecules of water are in 1 mole of water? • 3. How many moles are in 3 grams of Silver (Ag)? • 4. How many atoms are in 3 grams of Silver (Ag)? Complete the following problems with a partner

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