Ch.10 - Molecular Shapes & Valence Bond TheoryWorksheetSee 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: NO3- :Molecular geometry?Ideal bond angle?Are polar bonds present?Is there an overall dipole?Octect rule violator and how?

Solution: NO3- :Molecular geometry?Ideal bond angle?Are polar bonds present?Is there an overall dipole?Octect rule violator and how?

Problem

NO3- :

Molecular geometry?

Ideal bond angle?

Are polar bonds present?

Is there an overall dipole?

Octect rule violator and how?

Solution
  • N will appear as our central atom since it is less electronegative than O

  • N will appear to have 3 Os single bonded on it however, each O atom will appear as negatively charged with 3 lone pairs in it

  • One O must have a double bond with N making it neutral while N as positively charged

  • This will give a total charge of -1

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