Draw in all missing lone pairs for the following molecules.
(d)

Verified step by step guidance

1. Step 1: Identify the atoms in the molecule that typically have lone pairs. In this structure, chlorine (Cl) is the atom that will have lone pairs because it is a halogen and typically has three lone pairs when bonded to one other atom.
2. Step 2: Recall that chlorine has seven valence electrons. When it forms a single bond, one electron is shared with the bonded atom, leaving six electrons to be arranged as three lone pairs.
3. Step 3: Draw the three lone pairs around the chlorine atom. These lone pairs should be evenly spaced to minimize electron repulsion, forming a tetrahedral-like arrangement with the bond.
4. Step 4: Examine the rest of the molecule. The positively charged carbon (indicated by the '+' sign) does not have lone pairs because it has lost an electron, resulting in a formal positive charge.
5. Step 5: Verify the structure to ensure that all atoms follow the octet rule where applicable, and that the formal charges are consistent with the given structure.

Key Concepts

Lone Pairs

Lone pairs are pairs of valence electrons that are not involved in bonding and are localized on a single atom. They play a crucial role in determining the geometry and reactivity of molecules. Understanding how to identify and represent lone pairs is essential for accurately drawing molecular structures.

Lewis Structures

Lewis structures are diagrams that represent the bonding between atoms in a molecule and the lone pairs of electrons. They provide a visual way to understand the arrangement of electrons and the connectivity of atoms. Mastery of drawing Lewis structures is fundamental in organic chemistry for predicting molecular behavior and reactivity.

Valence Electrons

Valence electrons are the outermost electrons of an atom and are involved in forming bonds with other atoms. The number of valence electrons determines how an atom can bond and interact with others. Knowing how to count and distribute valence electrons is key to constructing accurate molecular representations.