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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

Chapter 11 The Mole

Section 11.1

Please have a highlighter and your periodic table out

standard 3
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
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
Never Changes
  • 1 dozen is always equal to 12
  • 1 mole is always equal to 6.02 ×1023
avogardro s number
Avogardro’s number

•6.02 ×1023 is also called Avogadro’s number

•It was named after this guy:

Amedeo Avogadro of Italy

other names for a particle
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
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
How big is a mole
  • 602, 000, 000,000,000,000,000,000 particles
  • 602 SEXTILLION!!!!
1 mole atomic mass of each element
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
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
Steps for mole caluculations
  • 1. Start with what is given.
  • 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
Example of time
  • How many minutes are in 120 seconds?
pg 311 examples
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
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
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

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
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
Examples
  • EX: Find the molar mass of the following compounds:
  • P2O5
  • C6H12O6
  • Fe2(SO4)3
on your own
On your own
  • EX: Find the molar mass of the following compounds:
  • N2O3
  • KC2H3O2
  • Ca3(PO4)2
moles to grams
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
on your own1
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
particles 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
Grams to particles
  • EX: Perform the following conversions:
  • Convert 300.0 grams of H2CO3 to particles.
  • Convert 20.0 grams of CuF2 to particles.
slide25

PP: Perform the following conversions:

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