Chemists use the mole to count atoms, molecules, ions, and formula units. Section 1: Measuring...
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Transcript of Chemists use the mole to count atoms, molecules, ions, and formula units. Section 1: Measuring...
Chemists use the mole to count atoms, molecules, ions, and formula units.
Section 1: Measuring Matter
KWhat I Know
WWhat I Want to Find Out
LWhat I Learned
• 8(A) Define and use the concept of a mole.• 8(B) Use the mole concept to calculate the number of atoms,
ions, or molecules in a sample of material.• 2(G) Express and manipulate chemical quantities using
scientific conventions and mathematical procedures, including dimensional analysis, scientific notation, and significant figures.
Measuring MatterCopyright © McGraw-Hill Education
Essential Questions
• How is a mole used to indirectly count the number of particles of matter?
• What is a common everyday counting unit to which the mole can be related?
• How can moles be converted to number of representative particles and vice versa?
Measuring MatterCopyright © McGraw-Hill Education
Review• molecule
New• mole• Avogadro’s number
Measuring MatterCopyright © McGraw-Hill Education
Vocabulary
Counting Particles
Chemists need a convenient method for accurately counting the number of atoms, molecules, or formula units of a substance. The mole is the SI base unit used to measure the amount of a substance. 1 mole is the amount of atoms in 12 g of pure carbon-12, or 6.02 ×1023 representative particles, which is any kind of particle – an atom, a molecule, a formula unit, an electron, an ion, etc. The number is called Avogadro’s number.
Measuring MatterCopyright © McGraw-Hill Education
Converting Between Moles and Particles
Conversion factors must be used.Moles to particles:
• Number of molecules in 3.50 mol of sucrose:
Measuring MatterCopyright © McGraw-Hill Education
Converting Between Moles and Particles
Particles to molesUse the inverse of Avogadro’s number as the conversion factor.
Measuring MatterCopyright © McGraw-Hill Education
Measuring MatterCopyright © McGraw-Hill Education
PARTICLES-TO-MOLES CONVERSION
Use with Example Problem 1.
Problem Zinc (Zn) is used as a corrosion-resistant coating on iron and steel. It is also an essential trace element in your diet. Calculate the number of moles of zinc that contain 4.50 × 1024 atoms.
ResponseANALYZE THE PROBLEMYou are given the number of atoms of zinc and must find the equivalent number of moles. If you compare 4.50 × 1024 atoms Zn with 6.02 × 1023, the number of atoms in 1 mol, you can predict that the answer should be less than 10 mol.
KNOWN
Number of atoms = 4.50 × 1024 atoms Zn
1 mol Zn = 6.02 × 1023 atoms Zn
UNKNOWN
Moles Zn = ? mol
SOLVE FOR THE UNKNOWN
Use a conversion factor—the inverse of Avogadro’s number—that relates moles to atoms.
• Apply the conversion factor.
Measuring MatterCopyright © McGraw-Hill Education
PARTICLES-TO-MOLES CONVERSION
EVALUATE THE ANSWER
Both the number of Zn atoms and Avogadro’s number have three significant figures. Therefore, the answer is expressed correctly with three digits. The answer is less than 10 mol, as predicted, and has the correct unit, moles.
SOLVE FOR THE UNKNOWN
• Substitute the number of Zn atoms = 4.50 × 1024. Multiply and divide numbers and units.
Measuring MatterCopyright © McGraw-Hill Education
Review
Essential Questions
• How is a mole used to indirectly count the number of particles of matter?
• What is a common everyday counting unit to which the mole can be related?
• How can moles be converted to number of representative particles and vice versa?
Vocabulary•mole•Avogadro’s number