The Chemistry MOLE By: Mark Silverman

1. The Chemistry MOLEBy: Mark Silverman The most beautiful and only beautiful mole! http://www.moleday.org/index.htm

2. Instructions • Dark or colored background = just take it in • White background = take notes

3. The Ten Mole Commandments • Thou shalt not use 6.02 x 10^23 in vain. • Thou shalt not use the term mole if thou has no true knowledge of the term mole. • Thou shalt not kill a mole. • Thou shalt not covet your neighbor's mole. • Thou shall always remember to celebrate Mole Day. • Thou shalt not disparage Mole Day. • Thou shalt not use a mole out of season. • Thou shall always honor the one who introduced thou to Mole Day. • You shall always keep sacred 10/23. • Thou shall always remember these commolments • or thou will never properly celebrate Mole Day.  

4.  A Dictionary of Mole demoleition – The destruction which moles bring about in your yard. dismole – being gloomy on Mole Day molearchy – government in which moles are in complete control; under this government Mole Day is celebrated three times a year and chemistry is the only scientific subject taught in school molect – the obsessive collection of Mole Day stuff including T-shirts, lawn decorations, pins, and endless other things molectomy – the study of a mole's insides or removal of a mole moleism – the continual reverence of moles moleodic – a word describing the Mole Day songs which are played over the loudspeaker remoletly – obscurely having to do with a mole remolte control – a devise used by moles to watch all their favorite television shows, such as Bill Nye the Science Guy and the Discovery Channel, particularly used by lazy papa moles sophmole – anyone in the tenth grade who is taking Chemistry already

5. Mole Humor Q: Why is it bad to tell mole jokes? A: It's mole-itically incorrect Q: What did Avogadro teach his students in math class? A: Moletiplication Q: What kind of fruit did Avogadro eat in the summer? A: Watermolens Q: Why was there only one Avogadro? A: When they made him, they broke the Moled Q: What do you get when you have a bunch of moles acting like idiots? A: A bunch of Moleasses

6. Q: What kept Avogadro in bed for two months? A: Moleonucleosis Q: What line from Shakespeare do high school moles have to memorize? A: "To mole or not to mole, this is the question." Q: What element do moles love to study in chemistry? A: Molybdenum Q: What is Avogadro's favorite kind of music? A: Rock 'N' Mole And finally…Q: What was Avogadro’s favorite Mexican food? You got it!...A: Molé!

7. Moletoons

8. The Ugly Moles The Biology Mole Would you kiss this face??? Introducing Scalopus aquaticus …and look what they eat!!! A face only a mother could love!

9. The Naked Mole Rat Kiss me, I’m really a Prince… Please??? Warning!!! This is not a mole. This is another example of how non-chemistry use of the word “mole” is Ugly!! If you are sensitive please do not look at the picture that’s about to appear. Are you ready? No vomiting please… Proof positive that the Biology Mole is Ugly!!!!

10. The Medical Mole Its ugly! It can be dangerous! Its something we want to get rid of!

11. The Spy Mole Corporate moles cost us money!

12. An enemy of the people! The Rosenbergs got the DEATH sentence! Moles include international spies, corporate spies, and couriers who smuggle drugs and international secrets

13. The Martian Mole All it does is dig holes on Mars… for goodness sake!

14. The Chemistry Mole is the only beautiful and perfect mole! It is part of the underlying and fundamental organization and design of the universe

15. The concept of The Mole is incredibly useful! The bad news is that when you first start using it,you won't know what you're doing.It's like taking the first few faltering steps on an unknown planet. The good news is that by following a few simple rules,you'll be able to do amazing calculations,win friends and influence people (and get full marks in a test!).

16. The Mole Defined • The mole is, simply put, the gram atomic or gram molecular mass of a substance. • Its simple. The atomic mass in grams is one mole of substance. • So 1.008 g of H = 1 mol H • 1 mol C = 12.01 g C • Ok your turn: 16.00 g O = ? Mol O • That’s right 1 mol O, see you got it!

17. OK, so water is two hydrogen, 2 x 1.008 amu = 2.016 amu + 1 oxygen = 16.00 amu. In total 18.016 amu. • So 1 mol H2O = 18.016 g H2O, see its easy! • Now you try: How many grams are in 1 mol of sodium chloride? • 22.99 + 35.45 = 58.44 g/mol, very good! http://www.chemistrycoach.com/moles.htm

18. Amedeo Avogadro Lorenzo Romano Amedeo Carlo Avogadro, conte di Quaregna e di Cerreto (1776 - 1856), was born in Turin, Italy (Sometimes known today as Torino). http://www.bulldog.u-net.com/avogadro/avoga.html

19. Amedeo Avogadro Avogadro - his contribution to chemistry • In order to understand the contribution that Avogadro made, we must consider some of the ideas being developed at this time. Chemistry was just beginning to become an exact science. The Law of Definite Proportions and the Law of Multiple Proportions were well accepted by 1808, at which time John Dalton published his New System of Chemical Philosophy. • Dalton proposed that the atoms of each element had a characteristic atomic weight, and that it was atoms that were the combining units in chemical reactions. Dalton had no method of measuring atomic weights unambiguously, so made the incorrect assumption that in the most common compound between two elements, there was one atom of each. • At around this time, Gay-Lussac was studying the chemical reactions of gases, and found that the ratios of volumes of the reacting gases were small integer numbers. Dalton still equated particles with atoms, and could not accept how one particle of oxygen could yield two particles of water. This was a direct threat to the relatively new atomic theory, and therefore Dalton tried to discredit the work of Gay-Lussac. • In 1811, Avogadro published an article in Journal de physique that clearly drew the distinction between the molecule and the atom. He pointed out that Dalton had confused the concepts of atoms and molecules. The "atoms" of nitrogen and oxygen are in reality "molecules" containing two atoms each. Thus two molecules of hydrogen can combine with one molecule of oxygen to produce two molecules of water. • Avogadro suggested that equal volumes of all gases at the same temperature and pressure contain the same number of molecules which is now known as Avogadro's Principle. • The work of Avogadro was almost completely neglected until it was forcefully presented by Stanislao Cannizarro at the Karlsruhe Conference in 1860. He showed that Avogadro's Principle could be used to determine not only molar masses, but also, indirectly, atomic masses. The reason for the earlier neglect of Avogadro's work was probably the deeply rooted conviction that chemical combination occurred by virtue of an affinity between unlike elements. After the electrical discoveries of Galvani and Volta, this affinity was generally ascribed to the attraction between unlike charges. The idea that two identical atoms of hydrogen might combine into the compound molecular hydrogen was abhorrent to the chemical philosophy of the early nineteenth century.

20. Amedeo Avogadro • It was long after Avogadro that the idea of a mole was introduced. Since a molecular weight in grams (mole) of any substance contains the same number of molecules, then according to Avogadro's Principle, the molar volumes of all gases should be the same. The number of molecules in one mole is now called Avogadro's number. It must be emphasised that Avogadro, of course, had no knowledge of moles, or of the number that was to bear his name. Thus the number was never actually determined by Avogadro himself. • As we all know today, Avogadro's number is very large, the presently accepted value being 6.0221367 x 1023. The size of such a number is extremely difficult to comprehend. There are many awe-inspiring illustrations to help visualize the enormous size of this number. For example: • An Avogadro's number of standard soft drink cans would cover the surface of the earth to a depth of over 200 miles. • If you had Avogadro's number of unpopped popcorn kernels, and spread them across the United States of America, the country would be covered in popcorn to a depth of over 9 miles. • If we were able to count atoms at the rate of 10 million per second, it would take about 2 billion years to count the atoms in one mole.

21. Now the amazing part: • 1 mol of anything, yes anything, is always 6.022 x 1023 particles. This works for atoms, molecules, formula units, ions, anything! • Think about what this means! The total number of protons and neutrons in any substance measured out in grams always contains the same number of particles. Weird and wild, huh! • The mole is based on the number of atoms in 12 g of 12C.

22. Sum it up • 6.022 x 1023 is known as Avogadro’s number. • gam or gmm = 1 mol = 6.022x 1023 particles. • Another amazing fact! Any gas at standard temperature and pressure (STP = 0 oC and 760 mm Hg) contains exactly 1 mole of particles in a 22.4 L volume. This is Avogadro’s Principle. Wow! • This is known as the molar volume of a gas.

23. Moles can also show concentration: • Mstands for molarity. • A 1 molar or 1 M solution contains one mol per liter • (1 mol/L) of a solution.

24. Conversions Conversion Factor mol < ------ > mass (g) molar mass in g/mol mol < ------ > particles (atoms, Avogadros’s number = 6.022 x 1023 molecules, formula units, particles/mol ions, etc.) mol < ------ > volume in L of gas molar volume of a gas = 22.4 L/mol at STP (0 oC and 1 atm) mol < ------- > volume (L), for Molarity (M) in mol/L concentration of solute in a solution mass (g) < ------ > volume (mL) Density in g/mL or g/cm3 , etc. *Remember: “Moles in the middle!!!” also known as the “mole bridge.” “If its not from moles or too moles you have to go through moles.”

25. How to solve mass and mole problems: Step1: Plan Step 2: Identify conversion factor Step 3: Draw a cross Step 4: Put given over 1 Step 5: Place units to cancel Step 6: Put conversion in cross Step 7: solve arithmetic

26. Practice! • How many grams of Ca are in 3.55 mol? • Plan: • Solution: • How many formula units of NaOH are in 30.0 g? • Plan: • Solution: • If you have 4.65 x 1025 formula units of Na, how many grams will you have? (5 points) • Plan: • Solution:

27. Don’t let all this molest you! I will now show you how to begin solving problems with moles. • Now we just need to remember how to use conversion factors, sig figs, and scientific notation. Ouch! We will do: • mol  particles (atoms, molecules, etc.) • g  mol • mol  g • particles  mol • Have moles of fun!!

28. Mole Day History Mole Songs • Unofficial holiday celebrated among chemists • October 23, between 6:02 AM and 6:02 PM, making the date 6:02 10/23 • The time and date are derived from Avogadro's number, which is approximately 6.02×1023, defining the number of particles(atoms or molecules) in one mole of substance. • http://www.ehow.com/how_2181979_celebrate-mole-day.html

29. Announcement… • In order to properly celebrate Mole Day, you will be doing a MOLE Project! • Yea!!!

30. Mole Day Project Idea #1 Create a Creative Stuffed Mole

31. Samples

32. Samples

33. Mole Day Project Idea # 2 Create a Stuffed Element Mole

34. Mole Day Project Jacques Cousteau Leonardo Davinci Idea #3 Create a Famous Stuffed Mole

35. Mole Day Project Idea #4 Create a Mole Shirt Idea #5 Create a Mole Hat Idea #6 Mole Piñata or Sculpture Idea #7 Make a Mole Cake or Cookies

36. Cake Samples Mole-asses cookies http://projects.washingtonpost.com/recipes/2008/12/10/mole-cookies/