Draw the Lewis structure for each organic compound from its condensed structural formula. a. C₂H₄ b. CH₃NH₂ c. HCHO d. CH₃CH₂OH e. HCOOH

Verified step by step guidance

1. Identify the total number of valence electrons for each compound by adding the valence electrons of each atom present in the formula.
2. For each compound, determine the central atom (usually the least electronegative atom, except hydrogen) and arrange the other atoms around it.
3. Draw single bonds between the central atom and surrounding atoms, using a pair of electrons for each bond.
4. Distribute the remaining valence electrons to satisfy the octet rule for each atom, starting with the outer atoms and then the central atom. Remember that hydrogen only needs two electrons.
5. If any atoms do not have a complete octet, consider forming double or triple bonds by sharing more pairs of electrons between atoms.

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 electrons and lines to represent bonds between atoms. Understanding how to draw Lewis structures is essential for visualizing molecular geometry and predicting reactivity.

Condensed Structural Formulas

Condensed structural formulas provide a shorthand way to represent the structure of a molecule, indicating how atoms are connected without showing all the bonds explicitly. For example, CH3CH2OH indicates that there is an ethyl group (C2H5) attached to a hydroxyl group (OH). Recognizing these formulas is crucial for translating them into Lewis structures.

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 atoms will bond and the overall structure of the molecule. Knowing how to count and distribute valence electrons is vital for accurately drawing Lewis structures.