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# The Mole

### CAVA Chem 302 303 S1U6L2 Mole Number Relationships

Question | Answer |
---|---|

A mole is a unit for measuring [...] of particles such as atoms or compounds. | A mole is a unit for measuring numbers of particles such as atoms or compounds. |

A mole is just like a 'dozen', or a 'pair', or a 'hundred'.... just a much [...] number. | A mole is just like a 'dozen', or a 'pair', or a 'hundred'.... just a much bigger number. |

Think of [...] as just a name for a certain number: 6.022 * 10^23 | Think of mole as just a name for a certain number: 6.022 * 10^23 |

Chemists defined a mole as the amount of a substance that contains as many particles as there are atoms in exactly [...] g of carbon-12. | Chemists defined a mole as the amount of a substance that contains as many particles as there are atoms in exactly 12 g of carbon-12. |

True or False: No one is absolutely sure where the term mole came from. [...]! | True or False: No one is absolutely sure where the term mole came from. TRUE! |

There are [...] things in a mole. | There are 6.022 * 10^23 things in a mole. |

A mole is just a name for 6.022 * 10^23 of anything; just as a [...] is a name for 12 of anything. | A mole is just a name for 6.022 * 10^23 of anything; just as a dozen is a name for 12 of anything. |

If you have a 12 eggs, you can say you have a dozen eggs; If you have 6.022 * 10^23 eggs, you can say you have a [...] of eggs. | If you have a 12 eggs, you can say you have a dozen eggs; If you have 6.022 * 10^23 eggs, you can say you have a mole of eggs. |

6.022 * 10^23 is called [...]'s Number; it's named after a famous chemist. | 6.022 * 10^23 is called Avogadro's Number; it's named after a famous chemist. |

Moles are useful because a mole of any element weighs the same as the element's atomic mass in [...]. | Moles are useful because a mole of any element weighs the same as the element's atomic mass in grams. |

The periodic table tells you how much 1 [...] of any element weighs in grams. | The periodic table tells you how much 1 mole of any element weighs in grams. |

Think of the periodic table of the elements as the periodic table of [...]. | Think of the periodic table of the elements as the periodic table of how much a mole of anything weighs in grams. |

A mole of H2O would contain within itself, [...] mole of O and [...] moles of H. | A mole of H2O would contain within itself, one mole of O and two moles of H. |

A mole of H2O would weigh the same as [...] mole of O plus [...] moles of H. | A mole of H2O would weigh the same as one mole of O plus two moles of H. |

Sulfur (S) has an average atomic mass of 32.06 amu. Therefore, 1 mole of sulfur weighs 32.06 [...]. | Sulfur (S) has an average atomic mass of 32.06 amu. Therefore, 1 mole of sulfur weighs 32.06 grams. |

Aluminum (Al) has an average atomic mass of 26.98 amu. Therefore, 1 mole of aluminum weighs [...] grams. | Aluminum (Al) has an average atomic mass of 26.98 amu. Therefore, 1 mole of aluminum weighs 26.98 grams. |

Gold (Au) has an average atomic mass of 196.97 amu. Therefore, [...] mole of gold weighs 196.97 grams. | Gold (Au) has an average atomic mass of 196.97 amu. Therefore, 1 mole of gold weighs 196.97 grams. |

Technically, a mole is defined as the number of atoms of carbon-12 that weigh [...] grams. That number is 6.022 * 10^23. | Technically, a mole is defined as the number of atoms of carbon-12 that weigh 12 grams. That number is 6.022 * 10^23. |

For some reason, chemists love the carbon isotope carbon-[...]. | For some reason, chemists love the carbon isotope carbon-12. |

Created by:
mr.shapard