Draw Lewis structures that satisfy the octet rule for the following molecules and ions: f. HOCl

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Identify the total number of valence electrons in the molecule. Hydrogen (H) has 1 valence electron, oxygen (O) has 6 valence electrons, and chlorine (Cl) has 7 valence electrons.

Add up the valence electrons: 1 (H) + 6 (O) + 7 (Cl) = 14 valence electrons.

Determine the central atom. In this case, oxygen (O) is typically the central atom because it can form more bonds than hydrogen.

Connect the atoms with single bonds: H-O-Cl. This uses 2 electrons for each bond, totaling 4 electrons.

Distribute the remaining electrons to satisfy the octet rule, starting with the outer atoms (Cl and O) and then placing any remaining electrons on the central atom (O). Ensure that each atom (except H) has 8 electrons around it.

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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 in chemical reactions.

Octet Rule

The octet rule is a chemical rule of thumb that states that atoms tend to bond in such a way that they each have eight electrons in their valence shell, achieving a stable electron configuration similar to that of noble gases. This rule helps predict the types of bonds that will form between atoms, particularly in covalent compounds, and is crucial for understanding the stability of molecules like HOCl.

Polar Covalent Bonds

Polar covalent bonds occur when two atoms with different electronegativities share electrons unequally, resulting in a molecule with a partial positive charge on one end and a partial negative charge on the other. In the case of HOCl, the bond between hydrogen and oxygen, as well as between oxygen and chlorine, exhibits polarity, which affects the molecule's properties and reactivity.

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Textbook Question

Which one of these statements about formal charge is true? (a) Formal charge is the same as oxidation number. (b) To draw the best Lewis structure, you should minimize formal charge. (c) Formal charge takes into account the different electronegativities of the atoms in a molecule. (d) Formal charge is most useful for ionic compounds. (e) Formal charge is used in calculating the dipole moment of a diatomic molecule.