1 / 13

Chapter 2

Chapter 2. Atoms, Molecules, and Ions. History. Greeks, BC AD, Alchemy, beginning of element disc. 1600’s Boyle, gases 1800’s more scientists, more laws developed and more elements discovered. Fundamental Chemical Laws. Law of Conservation of Mass

ezra-perry
Télécharger la présentation

Chapter 2

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Chapter 2 Atoms, Molecules, and Ions

  2. History • Greeks, BC • AD, Alchemy, beginning of element disc. • 1600’s Boyle, gases • 1800’s more scientists, more laws developed and more elements discovered

  3. Fundamental Chemical Laws • Law of Conservation of Mass • Mass cannot be created or destroyed but can be changed from one form to another

  4. Law of Definite Proportions • A given compound always contains exactly the same proportions of elements by mass • Take H2O, water. There is no other way to make water. It must always be 2 Hydrogen atoms and one Oxygen atom. • Or 1.008 g H to 16.00 g of O • 1 : 15.87 proportion of H:O by mass

  5. Carbon and Oxygen • CO is always 1 g carbon to 1.33g oxygen (12.0 g 60 16.00g) • CO2 is always 1 g carbon to 2.66 g oxygen

  6. Think of Any Other Compound? • Law of Definite Proportions applies • MgO (24.31 : 16.00 or 1 : 0.6581) • NaCl • KBr • H2O2

  7. Law of Multiple Proportions • When two elements form a series of compounds, the ratio of the masses of the second element that combine with 1 g of the first element can always be reduced to small whole numbers

  8. Example N and O • The amount of N that combines with O is • Compound A, N2O, 2 N : 1 O • Compound B, NO, 1 N : 1 O • Compound C, NO2, 1 N : 2 O • All obey the Law of Definite Proportions

  9. Problems • You react 100 g Compound A with 20 g Compound B to make one product. What is the mass of the product? • A. 10 g B. 100 g C. 120 g D. > 120 g

  10. 3 A + B ---- C + D • If you react 4 moles A with 2 moles B what products (moles of C, D) would you get.

  11. What is the difference between the Law of Definite Proportions and the Law of Multiple Proportions?

More Related