Draw the Lewis structure for HNO2

/ Exams & Certification / By

Draw the Lewis structure for HNO2 from the skeletals Wis structure for HNO2 from the skeletal structure presented below. If the valence his are filled to the usual limit (maximum of 8) how many non-bonding valence electrons are in the molecule? HONO a. 6.2 c. 6 d. 10 e. 14 Question: Please do the followings for these molecules: 1- Name the molecule A only 2- Draw the lewis structures (show the details of your work, step by step) 3- Determine the electron Geometry and Molecular Geometry (Shape) for central atom 4- Identify single bonds, double bonds and lone pairs B. HC F A. PI3

The Correct Answer and Explanation is :

Let’s tackle your questions one by one, starting with molecule A (PI₃):

Step-by-step breakdown:

  1. Name of Molecule (PI₃):
  • The chemical formula PI₃ is phosphorus triiodide. Phosphorus (P) is bonded to three iodine (I) atoms.
  1. Lewis Structure: Steps for drawing the Lewis structure for PI₃:
  • Step 1: Count the valence electrons:
    • Phosphorus (P) is in Group 15, so it has 5 valence electrons.
    • Each iodine (I) is in Group 17, so each iodine has 7 valence electrons.
    • Total valence electrons = 5 (from P) + 3×7 (from I) = 26 electrons.
  • Step 2: Draw the skeletal structure:
    • Phosphorus will be the central atom since it is less electronegative than iodine.
    • Place three iodine atoms around phosphorus.
  • Step 3: Connect the atoms with single bonds:
    • Place a single bond (2 electrons) between phosphorus and each iodine atom.
  • Step 4: Distribute the remaining electrons:
    • After placing three single bonds (6 electrons), we have 20 electrons left.
    • Distribute the remaining electrons as lone pairs on the iodine atoms.
    • Each iodine gets three lone pairs, using up 18 electrons.
    • This leaves two electrons, which are placed as a lone pair on phosphorus.
    Lewis structure of PI₃:
        I
        |
    I - P - I
        |
       (2 lone pairs on P)
  1. Electron Geometry and Molecular Geometry:
  • Electron Geometry: The electron geometry considers both bonding and lone pairs around the central atom. With three bonds and one lone pair around phosphorus, the electron geometry is tetrahedral.
  • Molecular Geometry: The molecular geometry only considers the positions of the atoms. Since one of the positions is occupied by a lone pair, the molecular geometry is trigonal pyramidal.
  1. Identify Single Bonds, Double Bonds, and Lone Pairs:
  • Single Bonds: There are three single bonds between phosphorus and iodine atoms.
  • Lone Pairs: Phosphorus has one lone pair, and each iodine has three lone pairs.

For B (HC F):

You didn’t provide a clear molecular formula for this compound. If this refers to a simple hydrofluorocarbon such as CH₃F (methyl fluoride), here’s a breakdown:

  1. Name of Molecule (CH₃F):
  • The molecule is called methyl fluoride, where a carbon atom (C) is bonded to three hydrogens (H) and one fluorine (F).
  1. Lewis Structure: Steps for drawing the Lewis structure for CH₃F:
  • Step 1: Count the valence electrons:
    • Carbon (C) is in Group 14, so it has 4 valence electrons.
    • Hydrogen (H) has 1 valence electron, and there are 3 hydrogens.
    • Fluorine (F) is in Group 17, so it has 7 valence electrons.
    • Total valence electrons = 4 (from C) + 3×1 (from H) + 7 (from F) = 10 electrons.
  • Step 2: Draw the skeletal structure:
    • Carbon will be the central atom, and it will bond with three hydrogens and one fluorine.
  • Step 3: Connect the atoms with single bonds:
    • Place a single bond (2 electrons) between carbon and each hydrogen, and another single bond between carbon and fluorine.
  • Step 4: Distribute the remaining electrons:
    • After placing the single bonds (8 electrons), there are 2 electrons left, which go to fluorine as a lone pair.
    Lewis structure of CH₃F:
       H
       |
   H - C - F
       |
       H
  1. Electron Geometry and Molecular Geometry:
  • Electron Geometry: With four bonds (three to hydrogen and one to fluorine), the electron geometry is tetrahedral.
  • Molecular Geometry: Since there are no lone pairs on the central carbon atom, the molecular geometry is also tetrahedral.
  1. Identify Single Bonds, Double Bonds, and Lone Pairs:
  • Single Bonds: There are four single bonds: three C-H bonds and one C-F bond.
  • Lone Pairs: Fluorine has three lone pairs.

Let me know if you’d like the image generated for PI₃ or CH₃F!

Related Posts

Scroll to Top