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

Verified step by step guidance

1. Identify the atoms in the molecule that typically have lone pairs. Oxygen is a common atom that carries lone pairs.
2. Recall that oxygen typically has two lone pairs when it forms two bonds, as in a carbonyl group.
3. Examine the structure: the oxygen atom is double-bonded to a carbon atom, indicating it is part of a carbonyl group.
4. Add two lone pairs to the oxygen atom to complete its octet, as it already has two bonds (one double bond) with carbon.
5. Ensure that all other atoms in the structure have the correct number of bonds and no additional lone pairs are needed.

Key Concepts

Lone Pairs

Lone pairs are pairs of valence electrons that are not involved in bonding and are localized on a single atom. In organic chemistry, recognizing lone pairs is crucial for understanding molecular geometry, reactivity, and the overall electronic structure of molecules. They can influence the polarity and hydrogen bonding capabilities of a compound.

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 provide a visual representation of the arrangement of electrons, helping to predict the shape and reactivity of the molecule. Drawing Lewis structures accurately is essential for identifying missing lone pairs and understanding molecular interactions.

Valence Shell Electron Pair Repulsion (VSEPR) Theory

VSEPR theory is a model used to predict the geometry of individual molecules based on the repulsion between electron pairs in the valence shell of the central atom. According to this theory, electron pairs, including lone pairs, will arrange themselves to minimize repulsion, which helps in determining the three-dimensional shape of the molecule. This understanding is vital when drawing structures and identifying lone pairs.