Draw the Lewis Dot structure of each of the following molecules

Draw the Lewis Dot structure of each of the following molecules (15 points): Acetic acid (CH3COOH) Ethanol (CH3CH2OH) Acetone (CH3COCH3) Draw the Lewis Dot structures of each of the following molecules (15 points): SF6 BF3 XeF4

The Correct Answer and Explanation is:

1. Acetic Acid (CH₃COOH)

Acetic acid consists of a carboxyl group (-COOH) attached to a methyl group (-CH₃).

Step-by-step Lewis structure:

• Carbon (C) is the central atom and forms four bonds (one with the oxygen in the carboxyl group, and three in the methyl group).
• The two hydrogens in the -CH₃ group bond to the carbon.
• The oxygen atom in the carboxyl group forms a double bond with carbon and a single bond with another oxygen.
• The second oxygen atom is bonded to hydrogen (hydroxyl group).

The structure:

mathematicaCopyEdit   H   O
   |   ||
H - C - C - O - H
   |
   H

2. Ethanol (CH₃CH₂OH)

Ethanol contains a hydroxyl group (-OH) attached to an ethyl group (-CH₂CH₃).

Step-by-step Lewis structure:

• The central carbon in the -CH₂ group bonds with two hydrogens and one carbon from the ethyl group.
• The second carbon in the -CH₃ group bonds with three hydrogens.
• The oxygen is bonded to the second carbon in the chain and a hydrogen atom to form the hydroxyl group.

The structure:

mathematicaCopyEdit   H   H
   |   |
H - C - C - O - H
   |   |
   H   H

3. Acetone (CH₃COCH₃)

Acetone is a simple ketone, where a central carbonyl group (C=O) is bonded to two methyl groups (-CH₃).

Step-by-step Lewis structure:

• The central carbon atom forms a double bond with oxygen.
• Each of the two methyl groups is attached to the central carbon via single bonds and contains three hydrogens.

The structure:

mathematicaCopyEdit   H   H
   |   |
H - C - C = O
   |   |
   H   H

4. Sulfur Hexafluoride (SF₆)

SF₆ is an example of an octahedral molecule, where sulfur is surrounded by six fluorine atoms.

Step-by-step Lewis structure:

• Sulfur is the central atom and forms single bonds with six fluorine atoms.
• Each fluorine atom has three lone pairs to satisfy the octet rule.

The structure:

rCopyEdit        F
        |
F - S - F
        |
        F
        |
        F
        |
        F

5. Boron Trifluoride (BF₃)

BF₃ is a trigonal planar molecule where boron is surrounded by three fluorine atoms.

Step-by-step Lewis structure:

• Boron is the central atom and forms single bonds with three fluorine atoms.
• Fluorine atoms each have three lone pairs of electrons.

The structure:

rCopyEdit    F
    |
F - B - F
    |
    F

6. Xenon Tetrafluoride (XeF₄)

XeF₄ is a square planar molecule with xenon as the central atom, bonded to four fluorine atoms.

Step-by-step Lewis structure:

• Xenon forms single bonds with four fluorine atoms.
• The fluorine atoms each have three lone pairs of electrons.
• Xenon has two lone pairs, which occupy opposite corners of the square planar geometry.

The structure:

rCopyEdit      F
      |
  F - Xe - F
      |
      F

Explanation:

• Octet rule: Most elements (except hydrogen and helium) follow the octet rule, which means they form bonds in such a way as to have eight electrons in their outermost shell.
• Bonding: Covalent bonds form when atoms share electrons. Each bond corresponds to a shared pair of electrons.
• Lone pairs: Electrons that are not involved in bonding are shown as lone pairs. These are critical in determining the molecule’s geometry and reactivity.
• Valence electrons: The number of valence electrons (electrons in the outer shell) influences how atoms bond. For example, hydrogen has 1, carbon has 4, oxygen has 6, nitrogen has 5, and halogens like fluorine have 7 valence electrons.