Chapter 11 The Mole

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# Chapter 11 The Mole - PowerPoint PPT Presentation

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

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### Chapter 11 The Mole

Section 11.1

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 x1023 particles (atoms or molecules)
Words used for counting:
• UnitNumerical ValueExample
• Dozen 12 Eggs in a carton
• Pair 2 Shoes
• Ream 500 Sheets of paper
• Gross 144 Pencils in a box
• Mole 6.02 x 1023 Particles
Never Changes
• 1 dozen is always equal to 12
• 1 mole is always equal to 6.02 ×1023
Avogardro’s number

•6.02 ×1023 is also called Avogadro’s number

•It was named after this guy:

Other names for a particle
• The mole is the SI unit used for counting the amount of a substance
• 1 mole = 6.02 ×1023particles

Particles can be atoms, ions, molecules, formula units, etc.

Multiplying a mole
• 0.5 moles = 3.01 ×10 23
• 1 mole = 6.02 ×10 23
• 2 moles = 1.20 ×10 24
• 3 moles = 1.80 ×10 24
• 4 moles = 2.41 ×10 24
How big is a mole
• 602, 000, 000,000,000,000,000,000 particles
• 602 SEXTILLION!!!!
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 16.00 grams
• –Ex. one mole of potassium atoms weighs 39.10 grams
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 12.00 Scientists measured out exactly 12 grams of carbon-12
• The sample had 6.02 ×1023atoms of carbon
• They set 6.02 ×1023to be one mole (like 12 is one dozen)
Steps for mole caluculations
• 2. (given) x ------------
• 3. 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
Example of time
• How many minutes are in 120 seconds?
Pg 311 examples
• 1. Determine the number of atoms in 3.00 moles(mol) of Zn?
• 2. Given 4.00 mole (mol) of AgNO3 determine the number of formula units(FMU).
Pg 311 examples continued…
• 3. Calculate the number of molecules in 11.5 mol of H2O.
• 4a) 5.75 x 1024 atoms Al how many moles?
On your own in your notes needs to be stamped for points
• 4b) 3.75 x1024 molecules CO2 How many moles?
• 4c) 3.58 x 1023 Formula units ZnCl2 How many moles?
• 4d) 2.50 x1020 atoms Fe. How many moles?

### 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.

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.
Examples
• EX: Find the molar mass of the following compounds:
• P2O5
• C6H12O6
• Fe2(SO4)3
• EX: Find the molar mass of the following compounds:
• N2O3
• KC2H3O2
• Ca3(PO4)2
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 NF3to moles
• 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
Particles to grams
• EX: Perform the following conversions:
• Convert 6.5 x 1024 particles of N to grams.
• Convert 2.8 x 1027 particles of Ca to grams.
• Convert 5.1 x 1022 particles of K to grams.
Grams to particles
• EX: Perform the following conversions:
• Convert 300.0 grams of H2CO3 to particles.
• Convert 20.0 grams of CuF2 to particles.

PP: Perform the following conversions:

• Convert 250.0 grams of Na2CO3 to particles.
• Convert 10.0 of CaF2 to particles.