🏷️ LIMITED TIME OFFER: GET 20% OFF GRADE+ YEARLY SUBSCRIPTION →
Log in
HomeClass Notes1,200,000CA670,000

CHM 2353 Lecture Notes - Lecture 7: Icosahedron, Improper Rotation, Oxidation State

43 views3 pages
erinpug43
7 Nov 2017
School
University of Ottawa
Department
Chemistry
Course
CHM 2353
Professor
Muralee Murugesu

For unlimited access to Class Notes, a Class+ subscription is required.

Document Summary

Oxidation numbers: hypothetical numbers assigned to an individual atom or ion present in a substance. Always reported for one individual atom or ion, not for groups of atoms or ions. Rule 1: oxidation number for an atom in its elemental form is always zero. Only one kind of neutral atom is present. Rule 2: the oxidation number of a monoatomic ion is the charge of the ion. Rule 3: all group 1a metals are +1. Rule 4: all groups 2a metals are +2. Rule 5: hydrogen is +1 when bonded to a nonmetal and -1 when bonded to a metal. Rule 6: oxygen is -2 (except when it combines with f), -1 in peroxides (o2-, h2o2), -1/2 in super oxides (o2-) Rule 8: the sum of the oxidations numbers of all atoms (or ions) in a neutral compound is 0.

Get access

Grade+20% off
$8 USD/m$10 USD/m
Billed $96 USD annually
Grade+
Homework Help
Study Guides
Textbook Solutions
Class Notes
Textbook Notes
Booster Class
40 Verified Answers
Class+
$8 USD/m
Billed $96 USD annually
Class+
Homework Help
Study Guides
Textbook Solutions
Class Notes
Textbook Notes
Booster Class
30 Verified Answers

Related Documents

CHM 2353 Lecture Notes - Lecture 8: Octahedral Molecular Geometry, Ethylenediamine, Ethylenediaminetetraacetic Acid
erinpug43
CHM 2353 Lecture Notes - Lecture 4: Trigonal Planar Molecular Geometry, Trigonal Pyramidal Molecular Geometry, Triangular Bipyramid
purplemarten11
CHEM 312
Final Exam
Study Guide
CHEM 312 Study Guide - Midterm Guide: Electron Affinity, Noble Gas, Electronegativity
bluecheetah583

Related Questions

Neutral compounds In a neutral compound, the sum of the oxidation states is zero. Note that the sign of the oxidation states and the number of atoms associated with each oxidation state must be considered. In H2O, for example, each hydrogen atom has an oxidation state of +1 and each oxygen atom has an oxidation state of −2 for a total of 2(+1)+(−2)=0.

Part A:

What is the oxidation state of an individual sulfur atom in BaSO4? Express the oxidation state numerically (e.g., +1).

Part B

What is the oxidation state of an individual nitrogen atom in HNO3? Express the oxidation state numerically (e.g., +1).

In an ion, the sum of the oxidation states is equal to the overall ionic charge. Note that the sign of the oxidation states and the number of atoms associated with each oxidation state must be considered. In OH−, for example, the oxygen atom has an oxidation state of −2 and the hydrogen atom has an oxidation state of +1, for a total of (−2)+(+1)=−1.

Part C:

What is the oxidation state of an individual phosphorus atom in PO33−? Express the oxidation state numerically (e.g., +1).

Part D:

What is the oxidation state of each individual carbon atom in C2O42−?

Oxidation Numbers

The oxidation number of an element is the "charge" the element would have if all of its bonds were completely ionic; that is, if the electron pairs of each bond were transferred to the more electronegative atom.

For monatomic ions the oxidation number is simply the charge of the ion. For covalently bonded elements the oxidation number is a bookkeeping device and does not mean that the element carries an actual charge.

Determine the oxidation state for each of the elements below.

The oxidation state of chlorine in hypochlorite ion ClO- is______
The oxidation state of chlorine in chlorine pentafluoride ClF5 is_____
The oxidation state of sulfur in sulfur dioxide SO2 is_______

PLEASE ANSWER ALL 5 QUESTIONS!!!!!!!!!!!