Ch.4 - Chemical Quantities & Aqueous ReactionsWorksheetSee all chapters
All Chapters
Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds

Solution: Using Lewis formulas, assign oxidation states to the atoms ina) H2CO (g)H =C =O =b) CH3OH (l)C =H =O =H =  (last H)

Problem

Using Lewis formulas, assign oxidation states to the atoms in

a) H2CO (g)

H =

C =

O =

b) CH3OH (l)

C =

H =

O =

H =  (last H)

Solution

We’re asked to assign the oxidation states of each atom in the structure of two molecules.

First, let's remember some of the general rules about oxidation states or numbers:

  • In an ion, all the oxidation numbers must add up the charge of the ion.
  • In a neutral compound, all oxidation numbers must add to zero.
  • For a Hydrogen atom bonded with non-metals, H = +1.
  • For a Hydrogen atom bonded with metals (or Boron), H = -1.
  • For Oxygen, O = -2 (except when its a peroxide or superoxide)
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