Draw the Lewis structure for each of the following: (6.6)a. H₃COCH₃ (the atoms are in the order C O C)

Verified step by step guidance

1. Identify the total number of valence electrons in the molecule. Carbon (C) has 4 valence electrons, oxygen (O) has 6, and hydrogen (H) has 1. Calculate the total for H₃COCH₃.
2. Arrange the atoms with carbon (C) as the central atoms and oxygen (O) between them, as specified in the problem. Connect the atoms with single bonds initially.
3. Distribute the remaining valence electrons to satisfy the octet rule for each atom, starting with the outer atoms (hydrogens and oxygen) and then the central carbon atoms.
4. Check if all atoms have a complete octet (or duet for hydrogen). If any atom lacks a complete octet, consider forming double bonds if necessary.
5. Verify the structure by counting the total number of electrons used and ensuring it matches the total number of valence electrons calculated initially.

Key Concepts

Lewis Structures

Lewis structures are diagrams that represent the bonding between atoms in a molecule and the lone pairs of electrons that may exist. They use dots to represent valence electrons and lines to indicate bonds between atoms. Understanding how to draw Lewis structures is essential for visualizing molecular geometry and predicting the behavior of molecules in chemical reactions.

Valence Electrons

Valence electrons are the outermost electrons of an atom and are crucial in determining how atoms bond with each other. The number of valence electrons influences the atom's reactivity and the types of bonds it can form. For example, carbon has four valence electrons, allowing it to form four covalent bonds, while oxygen has six, typically forming two bonds.

Molecular Geometry

Molecular geometry refers to the three-dimensional arrangement of atoms within a molecule. It is influenced by the number of bonds and lone pairs around the central atom, which can affect the molecule's physical and chemical properties. Understanding molecular geometry helps predict the shape of the molecule, which is important for its reactivity and interactions with other molecules.