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# Mole Concept

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Sections
The Atom
Subatomic Particles
Isotopes
Ions
Atomic Mass
Periodic Table: Classifications
Periodic Table: Group Names
Periodic Table: Representative Elements & Transition Metals
Periodic Table: Element Symbols
Periodic Table: Elemental Forms
Periodic Table: Phases
Periodic Table: Charges
Calculating Molar Mass
Mole Concept
Law of Conservation of Mass
Law of Definite Proportions
Atomic Theory
Law of Multiple Proportions
Millikan Oil Drop Experiment
Rutherford Gold Foil Experiment

The Mole Concept involves the interconversions between different unit amounts of a substance.

###### Mole Concept

Concept #1: Mole Concept

Mole connects together atoms, ions, molecules and formula units.

Example #1: Which of the following compounds would not be associated with the term “formula unit”?

Concept #2: Converting between Moles and Particles

Converting between moles and particles requires Avogadro's Number: 1 mole = 6.022x1023 particles.

Example #2: How many moles of chlorine gas are there in 8.33 x 1037 molecules?

Concept #3: Converting between Mass and Moles

Example #3: How many grams of chlorine gas are there in 2.34 moles?

Example #4: How many grams of Clcontain 9.25 x 1024 molecules of Cl2?

Mole also serves to connect mass units to particles.

Practice: If a sample of sodium chloride, NaCl, contains 73.1 kg, what is its number of formula units?

Practice: Calculate the number of oxygen atoms found in 783.9 g NiCl2 • 6 H2O.

Practice: If the density of water is 1.00 g/mL at 25°C, calculate the number of water molecules found in 1.50 x 103 µL of water.

Practice: A cylindrical copper wire is used for the fences around a house. The copper wire has a diameter of 0.0750 in. How many copper atoms are found in 5.160 cm piece? The density of copper is 8.96 g/cm3. (V = π • r2 • h)