Complete the Lewis structure for each of the following: (6.6)

Verified step by step guidance

1. Identify the central atoms in the structure. In this case, the central atoms are the two carbon (C) atoms.
2. Determine the total number of valence electrons for each atom. Carbon has 4, hydrogen has 1, nitrogen has 5, and oxygen has 6 valence electrons.
3. Connect the atoms with single bonds initially. Each single bond represents 2 electrons. Connect the carbons to each other, and then to hydrogen, nitrogen, and oxygen as shown in the image.
4. Complete the octets for the central atoms (carbon, nitrogen, and oxygen) by adding lone pairs if necessary. Remember that hydrogen only needs 2 electrons to be stable.
5. Check the formal charges on each atom to ensure the most stable structure. Adjust the bonds if necessary to minimize formal charges, ensuring that the total number of electrons used equals the total number of valence electrons calculated.

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 and interpret 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 an atom's reactivity and the types of bonds it can form. In Lewis structures, accurately accounting for valence electrons is vital for ensuring that the structure adheres to the octet rule, where atoms seek to have eight electrons in their outer shell.

Bond Types

There are different types of chemical bonds, including single, double, and triple bonds, which indicate the number of shared electron pairs between atoms. Single bonds involve one pair of shared electrons, while double and triple bonds involve two and three pairs, respectively. Recognizing these bond types is important for constructing accurate Lewis structures and understanding the stability and reactivity of molecules.