Ch.9 - Bonding & Molecular StructureWorksheetSee 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
Sections
Chemical Bonds
Lattice Energy
Lattice Energy Application
Born Haber Cycle
Dipole Moment
Lewis Dot Structure
Octet Rule
Formal Charge
Resonance Structures
Additional Practice
Bond Energy

Solution: Toothpastes containing sodium hydrogen carbonate (sodium bicarbonate) and hydrogen peroxide are widely used. Write Lewis structures for the hydrogen carbonate ion and hydrogen peroxide molecule, with

Solution: Toothpastes containing sodium hydrogen carbonate (sodium bicarbonate) and hydrogen peroxide are widely used. Write Lewis structures for the hydrogen carbonate ion and hydrogen peroxide molecule, with

Problem

Toothpastes containing sodium hydrogen carbonate (sodium bicarbonate) and hydrogen peroxide are widely used. Write Lewis structures for the hydrogen carbonate ion and hydrogen peroxide molecule, with resonance forms where appropriate.

Solution

Let’s start with the formulas for hydrogen carbonate ion and hydrogen peroxide.


Carbonate is a polyatomic anion with the formula CO32-.

Hydrogen carbonate is another polyatomic anion which has a hydrogen attached to the carbonate ion.

H+ + CO32- → HCO3-


Peroxides are compounds of oxygen where oxygen is present as O22-.

For a compound, the two negative charges need to be balanced with two H+ ions.

2H+  O22-   = H2O2


To write Lewis structures of molecules, we will recall the following rules:

  • The atom of least electronegativity is the center atom.
  • This does not apply to H as it can form only one bond.


Let’s start by calculating the number of valence electrons.


https://lh4.googleusercontent.com/SL6xYnDXs_t0VVvP7TlpYgK30eERVTKBnGiOOHocQG5fq1aO0iB3CJhv3Nq07CggQh8S849oJBk3F74QAZbimcHQpwDbjdvqldXfq-m6gySSDgHCVL-iNFSb41yKV2R1gLFdzoOE


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