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Chapter 10: Problem 132

Briefly describe each of the following ideas: (a) formal charge; (b) resonance; (c) expanded valence shell; (d) bond energy.

Short Answer

Expert verified
Formal charge is the electrical charge difference between the isolated atom and the one in the molecule. Resonance refers to multiple possible structures for a molecule. Expanded valence shell refers to central atoms in period 3 and beyond in the periodic table having more than 8 electrons in their valence shell due to the presence of d orbitals for bonding. Bond energy is the energy required to break a bond under standard conditions.

Step by step solution

01

Formal Charge

Formal charge of an atom in a molecule is the electrical charge difference between the isolated neutral atom and the one in the molecule. It can be calculated as follows: Formal charge = (valence electrons in free atom) - (non-bonding valence electrons) - 1/2(bonding electrons).
02

Resonance

Resonance refers to the capability of certain molecules or ions to be represented more than one Lewis structure. These structures are known as resonance forms. The actual structure of the molecule is a hybrid or blend of these resonance forms.
03

Expanded Valence Shell

The expanded valence shell refers to the concept that central atoms (in period 3 and beyond in the periodic table) can have more than an octet, more than 8 electrons, in their valence shell. This happens due to the presence of d orbital's available for bonding in these elements.
04

Bond Energy

Bond energy or bond dissociation energy is the amount of energy required to break one mole of a bond in a chemical compound under standard conditions. It is often measured in kJ/mol. A high bond energy implies a strong bond.

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Most popular questions from this chapter

Carbon suboxide has the formula \(\mathrm{C}_{3} \mathrm{O}_{2} .\) The carbon- to-carbon bond lengths are \(130 \mathrm{pm}\) and carbon-to-oxygen, \(120 \mathrm{pm} .\) Propose a plausible Lewis structure to account for these bond lengths, and predict the shape of the molecule.

Sodium azide, \(\mathrm{NaN}_{3}\), is the nitrogen gas-forming substance used in automobile air-bag systems. It is an ionic compound containing the azide ion, \(\mathrm{N}_{3}^{-}\). In this ion, the two nitrogen-to-nitrogen bond lengths are \(116 \mathrm{pm} .\) Describe the resonance hybrid Lewis structure of this ion.

What is the VSEPR theory? On what physical basis is the VSEPR theory founded?

Write acceptable Lewis structures for the following molecules: (a) \(\mathrm{H}_{2} \mathrm{NNH}_{2}\); (b) HOClO; (c) (HO) \(_{2}\) SO; (d) HOOH (e) SO \(_{4}^{2-}\).

Estimate the lengths of the following bonds and indicate whether your estimate is likely to be too high or too low: (a) I \(-\mathrm{Cl} ;\) (b) \(\mathrm{C}-\mathrm{F}\).
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