Write the Lewis structure for each molecule. a. NF₃ b. HBr c. SBr₂ d. CCl₄

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Determine the total number of valence electrons for each molecule.

For each molecule, identify the central atom (usually the least electronegative, except for hydrogen).

Arrange the remaining atoms around the central atom and connect them with single bonds.

Distribute the remaining valence electrons to satisfy the octet rule (or duet for hydrogen) for each atom.

If any atom lacks an octet, consider forming double or triple bonds as necessary.

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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 molecules.

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 the molecule's reactivity and the types of bonds it can form. Knowing how to count and distribute valence electrons is key to accurately constructing Lewis structures.

Molecular Geometry

Molecular geometry refers to the three-dimensional arrangement of atoms within a molecule. It is influenced by the number of bonding pairs and lone pairs of electrons around the central atom, which can affect the molecule's polarity and reactivity. Understanding molecular geometry helps in predicting the physical and chemical properties of substances.

Write the Lewis structure for each molecule. a. NF3 b. HBr c. SBr2 d. CCl4