1 / 8

18.2-3 Oxidation States

18.2-3 Oxidation States. Oxidation State – lets us keep track of electrons in redox reactions by assigning charges to each atom in a molecule.

tekla
Download Presentation

18.2-3 Oxidation States

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. 18.2-3 Oxidation States • Oxidation State – lets us keep track of electrons in redox reactions by assigning charges to each atom in a molecule. • These molecules are often not ionic, so the atoms do not actually have the charge that we assign. It is used as a bookkeeping system to help us see the transfer of electron charge and helps us balance the equations.

  2. Oxidation States • Binary ionic compound – it is identical with the charge on the ion. NaCl (+1,-1) • Uncombined element (elemental state)– all atoms are uncharged – and are given an oxidation state of zero. Na or Cl2 (0) • Covalent compounds – (2 nonmetals bonded) – Assume that the most electronegative atom in the bond controls both shared e-. H2O (+1, -2)

  3. Oxidation States .. H O: O2- H+1 H O is more electronegative so it has both the electrons that are shared.

  4. Oxidation States • Which element is the most electronegative? • F is the most electronegative (always -1) F > O > N > Cl (-1, -2, -3, -1) • When these are bonded to other nonmetals there are no ions. • You must determine which is the most electronegative and it’s oxidation state will be the same as it’s charge if it was an ion. • NO2 Determine the oxidation # of each. O is more electronegative, so O is -2. then N must be +4 to have a neutral molecule.

  5. Assign oxidation states to each element in the following: • Sodium metal, Na • 0 • Sodium fluoride, NaF • +1, -1 • Magnesium sulfide, MgS • +2, -2 • Carbon monoxide, CO • +2, -2

  6. Assign oxidation states to each element in the following: • Sulfur dioxide, SO2 • +4, -2 • Hydrogen peroxide, H2O2 • +1, -3 • Ammonia, NH3 • +1, -3 • Sodium carbonate, NaCO3 • +1, -2, +4

  7. Oxidation States • Do Self check p. 579 18.2 a-e • Do p. 584 #1-4 • Homework p. 602-603 # 5, 8, 9, 11, 12, 13

More Related