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Chapter 11 The Mole Section 11.1 Please have a highlighter and your periodic table out.

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Presentation on theme: "Chapter 11 The Mole Section 11.1 Please have a highlighter and your periodic table out."— Presentation transcript:

1 Chapter 11 The Mole Section 11.1 Please have a highlighter and your periodic table out

2 Standard 3 3b-Students know the quantity one mole is set by defining one mole of carbon 12 atoms to have a mass exactly of 12 grams. 3c- Students know one mole equals 6.02 x10 23 particles (atoms or molecules)

3 Words used for counting: UnitNumerical Value Example Dozen 12 Eggs in a carton Pair 2 Shoes Ream 500 Sheets of paper Gross 144 Pencils in a box Mole 6.02 x Particles

4 Never Changes 1 dozen is always equal to 12 1 mole is always equal to 6.02 ×10 23

5 Avogardro’s number 6.02 ×10 23 is also called Avogadro’s number It was named after this guy: Amedeo Avogadro of Italy

6 Other names for a particle The mole is the SI unit used for counting the amount of a substance 1 mole = 6.02 ×10 23 particles Particles can be atoms, ions, molecules, formula units, etc.

7 Multiplying a mole 0.5 moles = 3.01 × mole = 6.02 × moles = 1.20 × moles = 1.80 × moles = 2.41 ×10 24

8 How big is a mole 602, 000, 000,000,000,000,000,000 particles 602 SEXTILLION!!!!

9 1 mole=atomic mass of each element The average atomic mass (on the periodic table) tells you how much one mole of an element weighs (it is also called the molar mass). –Ex. one mole of oxygen atoms weighs grams –Ex. one mole of potassium atoms weighs grams

10 How did scientist come up with this number? Carbon-12 has exactly 6 protons and 6 neutrons So it has an atomic mass of exactly Scientists measured out exactly 12 grams of carbon-12 The sample had 6.02 ×10 23 atoms of carbon They set 6.02 ×10 23 to be one mole (like 12 is one dozen)

11 Steps for mole caluculations 1. Start with what is given. 2. (given) x The units that are given are placed in the denominator 4. Your unknown is placed in the numerator 5. Multiply the top and divide by the bottom

12 Example of time How many minutes are in 120 seconds ?

13 Pg 311 examples  1. Determine the number of atoms in 3.00 moles(mol) of Zn?  2. Given 4.00 mole (mol) of AgNO 3 determine the number of formula units(FMU).

14 Pg 311 examples continued… 3. Calculate the number of molecules in 11.5 mol of H 2 O. 4a) 5.75 x atoms Al how many moles?

15 On your own in your notes needs to be stamped for points 4b) 3.75 x10 24 molecules CO 2 How many moles? 4c) 3.58 x Formula units ZnCl 2 How many moles? 4d) 2.50 x10 20 atoms Fe. How many moles?

16 Molar Mass and Mole to gram calculation Standard 3.d- Students know how to determine the molar mass of a molecule from its chemical formula and a table of atomic masses.

17 17 Molar Mass The molar mass of a compound can be calculated solving for the sum of the products of each elements’ mass times the number of atoms present.

18 18 Examples EX: Find the molar mass of the following compounds: -P 2 O 5 -C 6 H 12 O 6 -Fe 2 (SO 4 ) 3

19 19 On your own EX: Find the molar mass of the following compounds: -N 2 O 3 -KC 2 H 3 O 2 -Ca 3 (PO 4 ) 2

20 20 Moles to Grams EX: Perform the following conversions: -Convert 5.0 moles of Na to grams -Convert 12.0 moles of He to grams -Convert 213 grams of NF 3 to moles

21 21 On your own PP: Perform the following conversions: -Convert 6.50 moles of O to grams -Convert 25.0 moles of Fe to grams -Convert 0.40 moles of Ne to grams


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