Write an appropriate Lewis structure for each compound. Make certain to distinguish between ionic and molecular compounds. a. BI3 c. HCFO b. K2S d. PBr3

Verified step by step guidance

Step 1: Identify the type of compound (ionic or molecular) for each given formula. BI3, HCFO, and PBr3 are molecular compounds, while K2S is an ionic compound.

Step 2: For molecular compounds (BI3, HCFO, PBr3), determine the total number of valence electrons by adding the valence electrons of each atom in the molecule.

Step 3: Draw the skeletal structure for each molecular compound, placing the least electronegative atom in the center (except hydrogen, which is always terminal). Connect the atoms with single bonds.

Step 4: Distribute the remaining valence electrons around the atoms to satisfy the octet rule (or duet for hydrogen), starting with the outer atoms and then moving to the central atom if needed.

Step 5: For the ionic compound K2S, represent the transfer of electrons from the metal (K) to the non-metal (S), forming K+ and S2- ions. Show the resulting ionic structure with brackets and charges.

Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

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 represent bonds between atoms. Understanding how to draw Lewis structures is essential for visualizing molecular geometry and predicting the behavior of compounds.

Ionic vs. Molecular Compounds

Ionic compounds are formed when electrons are transferred from one atom to another, resulting in the formation of charged ions that attract each other. In contrast, molecular compounds consist of atoms that share electrons through covalent bonds. Distinguishing between these types of compounds is crucial for accurately drawing their Lewis structures and understanding their properties.

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 will bond and interact with others. Knowing the valence electron count for each element in a compound is vital for constructing accurate Lewis structures and predicting molecular behavior.

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