Hydrogen Cyanide – HCN

Hydrogen Cyanide – HCN (2 points) Lewis Structure Diagram Required Information Total Number of Valence Electrons (Molecule): Answer Central Atom: Answer of Electron Sets: Answer Geometry of Electron Sets: Answer Bonding Electron Sets: Answer Non-bonding Electron Sets: Anspver Observed Shape (Molecular Shape): Answer Bond Angle: Answer Bond Polarity: Answer Molecular Polarity: Answer Molecular Model Carbon Disulfide – CS2 (2 points) Lewis Structure Diagram Required Information Total Number of Valence Electrons (Molecule): Answer Central Atom: Answer # of Electron Sets: Answer Geometry of Electron Sets: Answer Bonding Electron Sets: Answer Non-bonding Electron Sets: Anshver Observed Shape (Molecular Shape) Answer Bond Angle: Answer Bond Polarity: Answer Molecular Polarity: Answer 27 Molecular Model Formaldehyde – H2CO (2 points) Lewis Structure Diagram Required Information Total Number of Valence Electrons (Molecule): Answer Central Atom: Answer of Electron Sets: Answer Geometry of Electron Sets: Answer Bonding Electron Sets: Answer Non-bonding Electron Sets: Answer Observed Shape (Molecular Shape) Answer Bond Angle: Answer Bond Polarity: Answer Molecular Polarity: Answer Molecular Model Tetrafluoromethane – CF4(2 points) Lewis Structure Diagram Required Information Total Number of Valence Electrons (Molecule) Answer Central Atom: Answer # of Electron Sets: Answer Geometry of Electron Sets: Answer Bonding Electron Sets: Answer Non-bonding Electron Sets: Answer Observed Shape (Molecular Shape) Answer Bond Angle: Answer Bond Polarity: Answer Molecular Polarity: Answer Molecular Model Nitrogen Trifluoride – NF, (2 points) Lewis Structure Diagram Required Information Total Number of Valence Electrons (Molecule): Answer Central Atom: Answer # of Electron Sets: Answer Geometry of Electron Sets: Answer Bonding Electron Sets: Answer Non-bonding Electron Sets: Answer Observed Shape (Molecular Shape) Answer Bond Angle: Answer Bond Polarity: Answer Molecular Polarity: Answer Molecular Model Nitrogen Trichloride – NCIS (2 points) Lewis Structure Diagram Required Information Total Number of Valence Electrons (Molecule). Answer Central Atom: Answer # of Electron Sets: Answer Geometry of Electron Sets: Answer Bonding Electron Sets: Answer Non-bonding Electron Sets: Answer Observed Shape (Molecular Shape)! Answer Bond Anglet Answer Bond Polarity: Answer Molecular Polarity Answer Molecular Model Water – H20 (2 points) Lewis Structure Diagram Required Information Total Number of Valence Electrons (Molecule): Answer Central Atom: Answer # of Electron Sets: Answer Geometry of Electron Sets: Answer Bonding Electron Sets: Answer Non-bonding Electron Sets: Answer Observed Shape (Molecular Shape): Answer Bond Angle: Answer Bond Polarity: Answer Molecular Polarity: Answer um Molecular Model DU . Hydrogen Sulfide – H2S (2 points) Lewis Structure Diagram Required Information Total Number of Valence Electrons (Molecule) Answer Central Atom: Answer of Electron Sets: Answer Geometry of Electron Sets: Answer Bonding Electron Sets: Answer Non-bonding Electron Sets Answer Observed Shape (Molecular Shape) Answer Bond Anglet Answer Bond Polarity: Answer Molecular Polarity Answer ad Orang!

The Correct Answer and Explanation is :

Let’s go through each molecule step by step:

1. Hydrogen Cyanide (HCN):

• Total Number of Valence Electrons: H (1) + C (4) + N (5) = 10 electrons.
• Central Atom: Carbon (C).
• # of Electron Sets: 3 electron sets (2 bonding pairs, 1 lone pair on nitrogen).
• Geometry of Electron Sets: Linear.
• Bonding Electron Sets: 2 bonding pairs (C-H, C≡N).
• Non-bonding Electron Sets: 1 lone pair on nitrogen (N).
• Observed Shape (Molecular Shape): Linear.
• Bond Angle: 180°.
• Bond Polarity: C-H is nonpolar, C≡N is polar.
• Molecular Polarity: Polar due to the asymmetrical distribution of electrons from the C≡N bond.

2. Carbon Disulfide (CS2):

• Total Number of Valence Electrons: C (4) + S (6 * 2) = 16 electrons.
• Central Atom: Carbon (C).
• # of Electron Sets: 2 bonding sets (S=C=S).
• Geometry of Electron Sets: Linear.
• Bonding Electron Sets: 2 bonding pairs (S=C=S).
• Non-bonding Electron Sets: No lone pairs.
• Observed Shape (Molecular Shape): Linear.
• Bond Angle: 180°.
• Bond Polarity: C=S bonds are polar.
• Molecular Polarity: Nonpolar, because the linear shape results in the dipoles cancelling out.

3. Formaldehyde (H2CO):

• Total Number of Valence Electrons: H (1 * 2) + C (4) + O (6) = 12 electrons.
• Central Atom: Carbon (C).
• # of Electron Sets: 3 bonding sets (H-C=O).
• Geometry of Electron Sets: Trigonal Planar.
• Bonding Electron Sets: 3 bonding pairs (C-H, C=O).
• Non-bonding Electron Sets: No lone pairs.
• Observed Shape (Molecular Shape): Trigonal Planar.
• Bond Angle: 120°.
• Bond Polarity: C=O is polar, C-H is nonpolar.
• Molecular Polarity: Polar because of the asymmetry of the C=O bond.

4. Tetrafluoromethane (CF4):

• Total Number of Valence Electrons: C (4) + F (7 * 4) = 32 electrons.
• Central Atom: Carbon (C).
• # of Electron Sets: 4 bonding sets (F-C-F-F).
• Geometry of Electron Sets: Tetrahedral.
• Bonding Electron Sets: 4 bonding pairs (C-F).
• Non-bonding Electron Sets: No lone pairs.
• Observed Shape (Molecular Shape): Tetrahedral.
• Bond Angle: 109.5°.
• Bond Polarity: C-F bonds are polar.
• Molecular Polarity: Nonpolar because the symmetry of the tetrahedral shape cancels out the dipoles.

5. Nitrogen Trifluoride (NF3):

• Total Number of Valence Electrons: N (5) + F (7 * 3) = 26 electrons.
• Central Atom: Nitrogen (N).
• # of Electron Sets: 4 electron sets (3 bonding, 1 lone pair).
• Geometry of Electron Sets: Tetrahedral.
• Bonding Electron Sets: 3 bonding pairs (N-F).
• Non-bonding Electron Sets: 1 lone pair on nitrogen.
• Observed Shape (Molecular Shape): Trigonal Pyramidal.
• Bond Angle: 107°.
• Bond Polarity: N-F bonds are polar.
• Molecular Polarity: Polar due to the asymmetry caused by the lone pair.

6. Nitrogen Trichloride (NCl3):

• Total Number of Valence Electrons: N (5) + Cl (7 * 3) = 26 electrons.
• Central Atom: Nitrogen (N).
• # of Electron Sets: 4 electron sets (3 bonding, 1 lone pair).
• Geometry of Electron Sets: Tetrahedral.
• Bonding Electron Sets: 3 bonding pairs (N-Cl).
• Non-bonding Electron Sets: 1 lone pair on nitrogen.
• Observed Shape (Molecular Shape): Trigonal Pyramidal.
• Bond Angle: 107°.
• Bond Polarity: N-Cl bonds are polar.
• Molecular Polarity: Polar due to the lone pair and polar bonds.

7. Water (H2O):

• Total Number of Valence Electrons: H (1 * 2) + O (6) = 8 electrons.
• Central Atom: Oxygen (O).
• # of Electron Sets: 4 electron sets (2 bonding, 2 lone pairs).
• Geometry of Electron Sets: Tetrahedral.
• Bonding Electron Sets: 2 bonding pairs (O-H).
• Non-bonding Electron Sets: 2 lone pairs on oxygen.
• Observed Shape (Molecular Shape): Bent.
• Bond Angle: 104.5°.
• Bond Polarity: O-H bonds are polar.
• Molecular Polarity: Polar because of the bent shape and the polar bonds.

8. Hydrogen Sulfide (H2S):

• Total Number of Valence Electrons: H (1 * 2) + S (6) = 8 electrons.
• Central Atom: Sulfur (S).
• # of Electron Sets: 4 electron sets (2 bonding, 2 lone pairs).
• Geometry of Electron Sets: Tetrahedral.
• Bonding Electron Sets: 2 bonding pairs (S-H).
• Non-bonding Electron Sets: 2 lone pairs on sulfur.
• Observed Shape (Molecular Shape): Bent.
• Bond Angle: 92.1°.
• Bond Polarity: S-H bonds are polar.
• Molecular Polarity: Polar due to the bent shape and the polar bonds.

Each molecule’s Lewis structure and properties depend on electron sharing and the shape that minimizes repulsion between electron pairs (VSEPR theory).