Draw Lewis structures that satisfy the octet rule for the following molecules and ions: d. HCN (H and N are both bonded to C),

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Identify the total number of valence electrons in the molecule. Hydrogen (H) has 1 valence electron, carbon (C) has 4, and nitrogen (N) has 5. Add these together to find the total number of valence electrons available for bonding.

Determine the central atom. In HCN, carbon (C) is the central atom because it can form the most bonds. Hydrogen (H) and nitrogen (N) will be bonded to carbon.

Draw a skeletal structure with single bonds: H-C-N. This uses 2 electrons for each bond, totaling 4 electrons used so far.

Distribute the remaining electrons to satisfy the octet rule. Start by completing the octet for the outer atoms (N in this case), then place any remaining electrons on the central atom (C).

If there are not enough electrons to satisfy the octet rule for all atoms, consider forming double or triple bonds. In HCN, a triple bond between C and N will satisfy the octet rule for both C and N.

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

Octet Rule

The octet rule is a chemical rule of thumb that states 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 arrangement of electrons in molecules and is particularly useful when drawing Lewis structures.

Bonding in HCN

In hydrogen cyanide (HCN), the molecule consists of a hydrogen atom bonded to a carbon atom, which is then triple-bonded to a nitrogen atom. Understanding the specific bonding in HCN is crucial for accurately drawing its Lewis structure, as it involves recognizing the types of bonds (single and triple) and how they satisfy the octet rule for each atom involved.

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Related Practice

Textbook Question

In the following pairs of binary compounds, determine which one is a molecular substance and which one is an ionic substance. Use the appropriate naming convention (for ionic or molecular substances) to assign a name to each compound: (a) TiCl₄ and CaF₂ (b) ClF₃ and VF₃

Draw Lewis structures that satisfy the octet rule for the following molecules and ions: c. SO₃²⁻

Textbook Question

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

Textbook Question

Write Lewis structures that satisfy the octet rule for the following molecules and ions: a. NH4+, b. C2F4 (the two C atoms are bonded to one another), c. COCl2 (the Cl atoms are bonded to C), d. HSO3− (H is bonded to one of the O atoms), e. HNC (H and C are both bonded to N), f. ClO3−.

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.