1 / 5

Understanding Ion Formation and Oxidation Numbers in Chemistry

This document explains the concepts of ion formation and oxidation numbers, essential for understanding chemical behavior. Ion formation occurs when an atom loses or gains electrons in its outer shell, leading to positive or negative oxidation numbers. The relationship between electron configuration and oxidation states is discussed, emphasizing how atoms with nearly full outer shells attract electrons from those with fewer electrons. Through examples like N2O3, the document illustrates how to determine oxidation numbers and balance them in neutral compounds.

varden
Télécharger la présentation

Understanding Ion Formation and Oxidation Numbers in Chemistry

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. Ion Formation and Oxidation Numbers Kelsey Ward Teresa Chan Jordan Allen Carl Evans Sam Pape

  2. Background • Ion formation is caused when an atom loses or gains electrons in its outer shell • Oxidation number is how many electrons it lost or gained When an atom gains or loses electrons it forms ions. Losing electrons makes it positive a positive oxidation number and gaining them makes it negative.

  3. Explaining the Relationship • A single electron in the outer energy level has less attraction towards the nucleus than an atom with the outermost energy level almost full. When forming an ion, atoms with an almost full outermost energy level take electrons from atoms with a single electron in the outermost energy level. The Oxidation number is the result of ion formations.

  4. Figuring Out Oxidation Numbers • Example: N2O3 a. N is +, O is -b. N is most likely +5, O is most likely be -2c. The oxidation numbers add up to 2(+5) + 3(-2) = +4. But the molecule is neutral. http://www.chemistrycoach.com/oxno.htm

  5. As the number of rows increases the likelihood for them to gain an electron increases. This is because there are less electrons in the outer shell in the first column because it increases. For example, an atom in the 1A column would be likely to lose its electron to an atom in the 17A column.

More Related