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Ch.10 - Chemical Bonding I: The Lewis Model
All textbooksTro 5th EditionCh.10 - Chemical Bonding I: The Lewis ModelProblem 87b,c,d
Chapter 10, Problem 87b,c,d

Each compound contains both ionic and covalent bonds. Write ionic Lewis structures for each, including the covalent structure for the ion in brackets. Write resonance structures if necessary. b. Ca(OH)2 c. KNO3 d. LiIO

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Identify the ions present in KNO_3. Potassium (K) forms a cation (K^+) and the nitrate ion (NO_3^-) is the anion.
Draw the Lewis structure for the potassium ion (K^+), which is simply K with a positive charge, as it loses one electron.
For the nitrate ion (NO_3^-), start by counting the total number of valence electrons. Nitrogen has 5, each oxygen has 6, and there is an extra electron due to the negative charge, totaling 24 electrons.
Draw the covalent structure for NO_3^-. Place nitrogen in the center, single bond it to each oxygen, and distribute the remaining electrons to satisfy the octet rule. Use double bonds where necessary to minimize formal charges.
Consider resonance structures for NO_3^-. The double bond can be placed between nitrogen and any of the three oxygens, resulting in three equivalent resonance structures. Enclose the nitrate ion structure in brackets with a negative charge outside.

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Key Concepts

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

Ionic Bonds

Ionic bonds are formed through the electrostatic attraction between positively and negatively charged ions. In compounds like KNO3, potassium (K) donates an electron to become K+, while the nitrate ion (NO3-) is formed when nitrogen and oxygen atoms share electrons covalently. Understanding ionic bonds is crucial for drawing accurate Lewis structures, as it helps identify the charge distribution in the compound.
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Covalent Bonds

Covalent bonds occur when two atoms share one or more pairs of electrons, allowing them to achieve a full outer electron shell. In the case of the nitrate ion (NO3-), covalent bonding occurs between nitrogen and oxygen atoms, resulting in a stable structure. Recognizing covalent bonds is essential for constructing Lewis structures, as it determines how atoms are connected within the ion.
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Resonance Structures

Resonance structures are different ways of drawing the same molecule that illustrate the delocalization of electrons. For the nitrate ion (NO3-), resonance structures show that the double bond between nitrogen and one of the oxygen atoms can be represented in multiple ways, reflecting the equal distribution of electron density. This concept is important for accurately depicting the stability and reactivity of the ion in Lewis structures.
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