DRAW IT Draw Lewis dot structures for each hypothetical molecule shown below, using the correct number of valence electrons for each atom. Determine which molecule makes sense because each atom has a complete valence shell and each bond has the correct number of electrons. Explain what makes the other molecule nonsensical, considering the number of bonds each type of atom can make. a.

Verified step by step guidance

1. Step 1: Identify the number of valence electrons for each atom in the molecules. For example, Carbon (C) has 4 valence electrons, Hydrogen (H) has 1 valence electron, and Oxygen (O) has 6 valence electrons.
2. Step 2: Draw the Lewis dot structure for each molecule by placing the valence electrons around each atom. Start by placing single bonds (pairs of electrons) between atoms to form the basic structure.
3. Step 3: Ensure that each atom has a complete valence shell. For Hydrogen, this means 2 electrons (1 bond), and for Carbon and Oxygen, this means 8 electrons (4 bonds for Carbon, 2 bonds and 2 lone pairs for Oxygen).
4. Step 4: Check if each bond has the correct number of electrons. Each single bond should have 2 electrons, each double bond should have 4 electrons, and each triple bond should have 6 electrons.
5. Step 5: Determine which molecule makes sense by verifying that all atoms have a complete valence shell and that the number of bonds is appropriate for each type of atom. Identify any molecule that does not meet these criteria and explain why it is nonsensical.

Key Concepts

Lewis Dot Structures

Lewis dot structures are diagrams that represent the valence electrons of atoms within a molecule. Each dot corresponds to a valence electron, and the arrangement of these dots illustrates how atoms bond together. Understanding how to draw these structures is crucial 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 key to determining how an atom will bond with others. The number of valence electrons influences the atom's reactivity and the types of bonds it can form, whether ionic or covalent. Knowing the valence electron count for each atom involved in a molecule is essential for constructing accurate Lewis dot structures.

Octet Rule

The octet rule is a chemical principle stating that atoms tend to bond in such a way that they each have eight electrons in their valence shell, achieving a stable electron configuration similar to that of noble gases. This rule helps predict the types of bonds that will form between atoms and is fundamental in assessing the validity of a proposed molecular structure. Molecules that do not satisfy the octet rule may be considered nonsensical or unstable.