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It’s a beauty mark… It’s a small furry garden pest… No, wait… its how we count ATOMS!

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Presentation on theme: "It’s a beauty mark… It’s a small furry garden pest… No, wait… its how we count ATOMS!"— Presentation transcript:

1 It’s a beauty mark… It’s a small furry garden pest… No, wait… its how we count ATOMS!

2 The mass of 1 mole of a substance.

3 Calculate the molar mass of 1 mole of magnesium chloride. (first you need a formula) Calculate the molar mass

4 FORMULAS - review MgCl 2 The subscript is the number at the bottom of a formula. There is 1- Mg & 2 - Cl

5 How to calculate molar mass 1.Identify the # of atoms of each element 2.Multiply # atoms by the atomic mass of that element. (round to 2 #’s after the decimal) 3.Add them all together 4.Grams (g) is the unit

6 Molar Mass MgCl 2 Mg – 1 (24.31) = Cl – 2 (35.45) = or g/mol g MgCl 2 1 mole MgCl 2 =

7 Molar mass allows scientist a way to measure moles in a lab. Molar mass of Fe = Molar mass of O 2 = Molar mass of Cu(OH) 2 = Molar Mass

8 Calculate the molar mass: (you MUST write the formula correctly before answering) 1 mole of Ammonium phosphide 1 mole of Trinitrogen pentachloride

9 The percent BY MASS of each element in a compound – divide the element’s total mass (part) by the molar mass (whole) then multiple by 100 to get the percent. Ex: % composition of MgCl 2 Mg – 1 (24.31) = / x 100 = 25.53% Mg Cl – 2 (35.45) = / x 100 = 74.47% Cl Molar mass = g/mol Percent Composition (PART) (WHOLE) (PART)(WHOLE)

10 K – 1 (39.10) = / x 100 = 24.74% K Mn – 1 (54.94) = / x 100 = 34.76% Mn O – 4 (16.00) = / x 100 = 40.50% O molar mass KMnO 4 = Practice - Calculate the % comp of KMnO 4 :

11 1.Find the % comp of the element in the compound 2.Change the % to a decimal (move decimal 2 times to the left or divide by 100) 3.Multiply that decimal by the amount (g) of the sample. Ex: Calculate amount of chlorine in grams of MgCl 2. (use the % we found earlier) 74.47% Cl =.7447 x = grams Cl Calculating the amount of an element in a sample

12 H – 2(1.01) = 2.02 O – 1(16.00) = Molar mass H 2 O = Practice: Calculate the amount of oxygen in grams of water. / x100 = 88.79% O 88.79% O =.8879 x = grams O Complete % comp worksheet

13 The lowest whole number ratio (subscripts) of elements in a compound. Cannot be reduced!!! not empirical empirical Ex: C 6 H 12 O 6  CH 2 O Empirical Formula

14 Actual number of atoms in a chemical compound molecular EX: C 12 H 24 O 12 Molecular Formulas can be reduced to Empirical Formulas molecular empirical EX: C 12 H 24 O 12  CH 2 O Different molecular formulas can have similar empirical formulas molecular empirical EX: N 3 O 9  N 12 O 36  Molecular Formula Molecular formula: C 76 H 52 O 46 Empirical formula: ___________ NO 3

15 1.C 2 H 4 2.NO 3 3.S 9 Cl 12 4.C 3 Cl 9 5.N 4 S 9 PRACTICE: 1. Identify each as empirical (can’t be reduced) or molecular (can be reduced) 2. If its molecular – write the empirical molecular empirical CH 2 - empirical S 3 Cl 4 - empirical CCl 3 - empirical

16 Ex: A compound was found to be 54.53% Carbon, 9.15% Hydrogen, and 36.32% Oxygen. Find its Empirical Formula. Steps: Assume a 100g sample (change %  g) Use molar mass to find moles of each Divide all moles by the smallest number of moles Round each to the nearest whole # (sometimes you have to multiply to get a whole number - special) The resulting whole #are the subscripts for that element in the empirical formula Finding Empirical Formula from Percent Composition

17 63.5% Silver 8.2% Nitrogen 28.3% Oxygen 63.5 g Ag8.2 g N28.3 g O mole Ag.59 mole N1.77 mole O AgNO 3 Calculating Empirical Formula

18 60.00%C4.48%H 35.53%O 60.00g C4.48g H35.53g O mole C4.44 mole H2.221 mole N x4x4x4 984 C9H8O4C9H8O4 Calculating Empirical Formula (special)

19 1.Find the empirical formula 2.Calculate the molar mass of your empirical formula 3.Identify the molar mass of your molecular (GIVEN in the problem everytime!) 4.Divide the molecular mass / empirical mass 5.Round to the nearest whole # 6.Multiply the whole # by the subscripts in the Empirical formula Calculating Molecular Formula

20 If a compound has an empirical formula of NO 3 and a molecular mass of 186g – what is the molecular formula? Empirical formula: NO 3 molar mass: 62.01g Molecular mass (given) 186g empirical mass x NO 3 = N 3 O 9 Practice

21 For counting matter (quantity) in chemistry we use the mole Moles are used to correctly measure chemicals for reactions in a lab. Problem – no way to “physically” measure a mole. (no lab equipment measures moles) Solution – molar mass (balance) What is a mole?

22 Remember – Molar mass is the mass (grams) of 1 mole 1 mole Fe = _________grams Fe 2.5 mole Fe = ________ grams Fe grams Fe = _______ moles Fe Mass to mole = divide by molar mass Mole to mass = moletiply by mole mass Using Molar Mass

23 How many grams are in 15.7 mole MgCl 2 How many moles are in 0.75 grams of silver? What is the mass of 30.7 mole water? Using molar mass

24 In the lab, Mrs. Mathieson needs 2.57 moles of NaCl to do an experiment. How many grams would be needed to equal 2.57 moles of NaCl? After doing the experiment, Mrs. Mathieson has 1.02 moles of NaCl remaining – how many grams does that equal? Using molar mass

25 For counting matter (quantity) in chemistry we use the mole 1 mole = 6.02 x representative particles (particles are very tiny) This value is called Avogadro’s Number What is a mole?

26 ie. the smallest particle that retains chemical and physical properties 3 types depending on the compound : Atoms: Single element Molecules: covalent compound Formula Units: Ionic Compounds or ions What are REPRESENTATIVE PARTICLES ?

27 Remember there are 6.02 x particles (atoms, molecule, f.u) in 1 mole How many atoms are in 1 mole? How many atoms are in 2.10 moles of Copper? How many moles are in 4.21 x atoms of aluminum? Using Avagadro’s Number

28 For counting matter (quantity) in chemistry we use the mole 1 mole = 22.4 L of any gas This value is called Molar Volume What is a mole?

29 How many liters are in 1 mole of any gas? How many liters are in L of oxygen gas? How many moles are in moles of nitrogen gas? Using molar volume

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