For each of the following ions of nitrogen and oxygen, write a single Lewis structure that obeys the octet rule, and calculate the oxidation numbers and formal charges on all the atoms: c. NO2+.

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Step 1: Determine the total number of valence electrons.

Step 2: Draw a skeletal structure for NO2+.

Step 3: Distribute the remaining electrons to satisfy the octet rule.

Step 4: Calculate the formal charges for each atom.

Step 5: Determine the oxidation numbers for nitrogen and oxygen.

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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 are essential for visualizing how atoms share or transfer electrons to achieve stable electron configurations, typically following the octet rule, which states that atoms tend to bond in such a way that they each have eight electrons in their valence shell.

Octet Rule

The octet rule is a chemical rule of thumb that reflects the tendency of atoms to prefer having eight electrons in their valence shell, leading to greater stability. This rule is particularly applicable to main group elements and guides the formation of covalent bonds, as atoms will share, gain, or lose electrons to achieve a full outer shell, often resulting in the formation of ions or molecules.

Oxidation Numbers and Formal Charges

Oxidation numbers are assigned to atoms in a molecule to indicate the degree of oxidation or reduction, reflecting the number of electrons lost or gained. Formal charge, on the other hand, is a theoretical charge assigned to an atom in a molecule, calculated based on the number of valence electrons, the number of bonds, and the number of lone electrons. Both concepts are crucial for understanding the distribution of electrons in a molecule and ensuring that the Lewis structure accurately represents the molecule's electronic structure.

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Formal Charge

Related Practice

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.

Textbook Question

(b) With what allotrope of oxygen is it isoelectronic?

Textbook Question

Consider the formate ion, HCO₂^-, which is the anion formed when formic acid loses an H⁺ ion. The H and the two O atoms are bonded to the central C atom. (b) Are resonance structures needed to describe the structure?

Textbook Question

Predict the ordering, from shortest to longest, of the bond lengths in CO, CO₂, and CO₃^2- .