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Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640

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Section
BuyFindarrow_forward

Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640
Chapter 8, Problem 58GQ
Textbook Problem
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In boron compounds, the B atom often is not sur-rounded by four valence electron pairs. Illustrate this with BCl3. Show how the molecule can achieve an octet configuration by forming a coordinate covalent bond with ammonia (NH3).

Interpretation Introduction

Interpretation: The structure of BCl3 has to be illustrated and also has to show how BCl3 will achieve an octet configuration by forming a coordinate covalent bond with ammonia.

Concept Introduction:

  • The Lewis structure is based on the concept of the octet rule so that the electrons shared in each atom should have 8 electrons in its outer shell.
  • According to octet rule an atom is said to be in stable arrangement if its valence shell has 8 electrons and it can be achieved by gaining, losing or sharing of electrons with other atoms.
  • If the valence shell of atom contains 8 electrons, it gets the electronic configuration of noble gas where the outer shell electronic configuration is Chemistry & Chemical Reactivity, Chapter 8, Problem 58GQ .
  • Since the valence shell of noble gases is already filled and has 8 valence electrons, it violates octet rule.
  • Any chemical substance can be classified as an acid or base by using Lewis acid base theory. Further,the acidic and basic nature of the substance can be analyzed through the ability of molecules to accept and donate electrons.
  • According to Lewis acid -base theory,

    An acid is a substance that accepts a pair of electrons.

    A base is a substance that donates a pair of electrons.

Explanation of Solution

There are three outer free electrons for an atomic boron and commonly it forms three bonds.

Consider the molecule BCl3

From the above given figure, it is clear that boron has not been able to complete its octet and there are only six electrons around it.

Thus, BCl3 can be considered as an electron deficient compound and so it can accept electrons from bases

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Chapter 8 Solutions

Chemistry & Chemical Reactivity
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Ch. 8.4 - Draw resonance structures for the bicarbonate ion,...Ch. 8.4 - 1. For which of the following species, SO32−, NO+,...Ch. 8.4 - 2. What are the formal charges on nitrogen and...Ch. 8.5 - Sketch the Lewis structures for CIF2+ and CIF2....Ch. 8.5 - 1. Draw a Lewis structure for HOMO. Are there any...Ch. 8.5 - 2. Draw a Lewis structure for the...Ch. 8.5 - 1. In which of the following sulfur species, SF2,...Ch. 8.5 - 2. How many lone pairs of electrons are on the...Ch. 8.6 - What is the shape of the dichloromethane (CH2C12)...Ch. 8.6 - Give the electron-pair geometry and molecular...Ch. 8.6 - Draw the Lewis structure for lCl2, and then decide...Ch. 8.6 - Use Lewis structures and the VSEPR model to...Ch. 8.6 - Which of the following species has...Ch. 8.6 - What is the molecular geometry of the SbF52 ion?...Ch. 8.6 - What is the approximate ClCCl bond angle in...Ch. 8.6 - 4. What is the molecular geometry of N2O (where...Ch. 8.7 - Draw the resonance structures for SCN. 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Use...Ch. 8 - Draw Lewis structures (and resonance structures...Ch. 8 - Draw resonance structures for the SO2 molecule,...Ch. 8 - What are the orders of the NO bonds in NO2 and...Ch. 8 - Which has the greater ONO bond angle, NO2 or NO2+?...Ch. 8 - Compare the FClF angles in CIF2+ and ClF2. Using...Ch. 8 - Draw an electron dot structure for the cyanide...Ch. 8 - Draw the electron dot structure for the sulfite...Ch. 8 - Dinitrogen monoxide, N2O, can decompose to...Ch. 8 - The equation for the combustion of gaseous...Ch. 8 - The cyanate ion, OCN, has the least...Ch. 8 - Vanillin is the flavoring agent in vanilla extract...Ch. 8 - Explain why (a) XeF2 has a linear molecular...Ch. 8 - The formula for nitryl chloride is ClNO2 (in which...Ch. 8 - Hydroxyproline is a less-common amino acid. 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