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Atomic Weight, Molecular Weight, Formula Weight and Molar Mass

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## Atomic Weight, Molecular Weight, Formula Weight and Molar Mass

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**Atomic Weight, Molecular Weight, Formula Weight and Molar**Mass Dr. C. Yau Spring 2014 loosely based on Chap 4 Sec 1of Jespersen 6th edition 1 1**Examine the periodic table. What is the atomic weight (AW)**of carbon? Atomic Weight or Atomic Mass The atomic weight of C is or 12.01 u/atom It means that each C atom weighs12.01 u. (In this class you should make it a habit to look up AW to 4 sig. fig.) 2**Molecular Weightor Molecular Mass**The AW of C is 12.01 u/atom The AW of O is 16.00 u/atom. Therefore, the mass of one molecule of CO2 would be 12.01 + 2(16.00) = 44.01 u/molecule. (Always round to 4 sig. fig.) We call this the molecular weight (MW) or molecular mass. What is the MW of methane (CH4)? Ans. 16.04 u/molecule 3 3**Formula Mass**If we add up the atomic mass of Na and Cl we get 22.99 + 35.45 = 58.44. What is wrong with saying… the molecular weight of NaCl is 58.44 u/molecule? 4 4**Formula Mass**For molecular substances, the smallest unit is the molecule. For ionic substances, the smallest unit is the "formula unit" abbreviated f.u. e.g. If you pluck out the smallest unit out of water, you would have a water molecule. 5 5**Formula Mass**When you pluck out the smallest unit of table salt you would have a formula unit of NaCl. Na+Cl- Na+ClNa+ClNa+Cl ClNa+ClNa+ClNa+ Na+ClNa+ClNa+Cl We often simply write NaCl, but it is understood that Na is Na+ and Cl is Cl-. There are no molecules in an ionic compound! 6 6**Summary:**Atomic Weight (AW) = mass of one atom (for atoms) in units of amu/atom Molecular Weight (MW) = mass of one molecule (for molecular substances) in units of amu/molecule Formula Weight (FW) = mass of one f.u. (for ionic compounds) in units of amu/f.u. AW, MW and FW 7**Calculate the formula weight of…**(and give the proper units) cobalt(III) sulfide ammonium sulfate Calculate the molecular weight of… (CH3CH2)3N Calculations of AW, MW and FW 8**Calculate the formula weight of…**Na2SO42H2O This is known as a hydrate. The dot in the formula does NOT mean you multiply anything. The dot means there are 2 water molecules attached to each f.u. of Na2SO4. What is its formula weight? 9**The Mole Concept**One mole is defined as the number of atoms in exactly 12 g of C-12 atoms. Remember that C-12 refers to the isotope…. exactly 12 g C 6.022x1023 C atoms It turns out that there are 6.022x1023 C atoms in those 12 grams. So…. 1 mole = 6.022x1023(not an exact number, but in 4 sig. fig.) MEMORIZE THIS NOW! 10 10**1 mole = 6.022x1023**This number is known as Avogadro's number Note: Mole is abbreviated mol NOT m (which stands for meters) Note: It is a NUMBER. It is NOT a mass. It does NOT have the unit of grams. The Mole Concept 11**The Mole Concept**We all know… 1 dozen eggs = 12 eggs 1 dozen atoms = 12 atoms In the same way, we use the word "mole"… 1 mole eggs = 6.022x1023 eggs Obviously that is a VERY big number of eggs. There would be no occasion to be talking about a mole of eggs. When do you we use "moles?" 12**The Mole Concept**1 mol atoms = 6.022x1023 atoms 1 mol molecules = 6.022x1023 molecules 1 mol electrons = 6.022x1023 electrons The "mole" is not a mass itself, just a number of items. Why do we bother with such a strange number? Let us take a look at the periodic table. 13 13**The Mole Concept**The atom is a very, very small particle. You can fit 7000 atoms on the dot of an i. It is too small to see with the naked eye, and too small to hold in your hand or weigh on the balance. We must use a much larger quantity of atoms: a mole of atoms. 14 14**The Mole Concept**From the periodic table, we can get the atomic weight for Ag. This mass can be given in two units: 107.9 u per atom or 107.9 g per mole of atoms One atom of silver weighs 107.9 u, which is 0.0000000000000000000001079 gram Get the picture? You cannot weigh a single atom of silver, but you CAN weigh a mole of Ag atoms. 107.9 g is about 3.8 ounces. 15 15**The Mole Concept**Cu Ag From the periodic table we see that… Ag is 107.9 g/mol Cu is 63.55 g/mol What does 107.87 g of Ag have in common with 63.55 g of Cu? They both contain the same number of atoms: 6.022x1023 Ag atoms and 6.022x1023 Cu atoms, in other words, 1 mole Ag and 1 mol Cu. 16 16**The Mole Concept**Earlier we were talking about the AW, MW and FW. Now we are going to add one more…. MM = molar mass Whenever you see "molar" you should think "per mole." Molar mass = mass per mole (for 1 mol) with units of g/mol KNOW THIS WELL! SEE THIS IN YOUR DREAMS….AND NIGHTMARES! 17 17**Molar Mass (MM)**The atomic mass from the periodic table can be used with two units: amu/atom or g/mole (or g mol-1) REMEMBER: Whenever you see a fractional unit (such as amu/atom, g/mol, g/mL) you should think "conversion factor"! The g/mol gives you the link between MASS AND # of MOLES. 18 18**Molar Mass (MM)**The FW ofCo2(SO4)3 is 406.7 amu/f.u. Its MM = 406.7 g/mol 2(58.93)+3(32.07)+12(16.00) = 406.7 We had calculated the MW of… (CH3CH2)3N to be 101.2 amu/molecule Its MM = 101.2 g/mol 2x3C + 5x3H + N = 6(12.01) + 15(1.008) + 14.01 = 101.2 19 19**Molar Mass (MM)**Note that we no longer need to distinguish between f.u. and molecules in the units of MM. It is understood that for Co2(SO4)3 its MM = 406.7 g/mol of f.u. and for (CH3CH2)3N its MM = 101.2 g/mol of molecules. 20 20**Use of MM in Dimensional Analysis**Conversion factors from MM: e.g. MM (N) = 14.01 g/mol e.g. MM (HCl) = 36.45 g/mol 21 21**Use of MM in Dimensional Analysis**When do we use MM? Whenever you see a fractional unit (such as g/mol or g mol-1) you should think "conversion factor"! MM is the link between mass & moles massmoles of particles moles of atoms moles of f.u. moles of molecules e.g. mol Cu mol CuCl2 mol PBr3 22 22**Use of MM**Example 4.1 p.109 Titanium(IV) oxide is one of the best sunscreens because it completely blocks ultraviolet radiation from reaching the skin. In an experiment to prepare TiO2, we start with 23.5 g sample of titanium. How many moles of Ti do we have?**Example 4.2 p.110**We need 0.254 mol of iron(III) chloride for a certain experiment. How many grams do we need to weigh? Do Practice Exercises 4.1 & 4.2 on p.110 (Note: Ans to Pract. Exercises are at the back of the book.)**Use of Avogadro's Number in Dimensional Analysis**Conversion factors from Avogadro's number: Note that X can be anyTHING, such as CO2, K2SO4, electrons, Na+, etc…. as long as it is EXACTLY the same on top as on the bottom. BUT it cannot be a unit, such as g or mL. 25 25**Use of Avogadro's Number in Dimensional Analysis**You use Avogadro's number ONLY if you have to go between the macroscopic and the particulate (sub-microscopic) levels. particulate levelmacrosopic level (conceptual, (observable) non-observable) atoms moles of atoms f.u. moles of f.u. molecules moles of molecules u g, mg, lbs, oz 26 26**Use of Avogadro's Number**Example 4.3 p.111 Tungsten wire is the filament inside most incandescent light bulbs. In a typical light bulb, the tungsten filament weighs 0.635 g. How many atoms of tungsten are there in such a light bulb flame? First ask yourself... “Do I need Avog. #?”**Example 4.4 p.112**Carbon tetrachloride was used as a dry-cleaning fluid until it was found to be carcinogen. What is the average mass in grams of one molecule of carbon tetrachloride (CCl4)? “Do I need Avog. #?”**Use of Avogadro's Number**Example What is the mass in grams of 2.01 mole of NaCl? Example How many anions are in 7.82 g of MgCl2? Example What is the weight in grams of 158 molecules of CO2? REMEMBER! ASK YOURSELF… DO I NEED AVOGADRO'S NUMBER IN THIS PROBLEM? Do Practice Exercises 4.3 & 4.4 on p.112