menu
bartleby
search
close search
Hit Return to see all results
close solutoin list

Vitamin B 6 is an organic compound whose deficiency in the human body can cause apathy, irritability, and an increased susceptibility to infections. Below is an incomplete Lewis structure for vitamin B 6 . Complete the Lewis structure and answer the following questions. Hint: Vitamin B 6 can be classified as an organic compound (a compound based on carbon atoms). The majority of Lewis structures for simple organic compounds have all atoms with a formal charge of zero. Therefore, add lone pairs and multiple bonds to the structure below to give each atom a formal charge of zero. a. How many σ bonds and π bonds exist in vitamin B 6 ? b. Give approximate values for the bond angles marked a through g in the structure. c. How many carbon atoms are sp 2 hybridized? d. How many carbon, oxygen, and nitrogen atoms are sp 3 hybridized? e. Does vitamin B 6 exhibit delocalized π bonding? Explain.

BuyFindarrow_forward

Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243

Solutions

Chapter
Section
BuyFindarrow_forward

Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243
Chapter 4, Problem 84AE
Textbook Problem
294 views

Vitamin B6 is an organic compound whose deficiency in the human body can cause apathy, irritability, and an increased susceptibility to infections. Below is an incomplete Lewis structure for vitamin B6. Complete the Lewis structure and answer the following questions. Hint: Vitamin B6 can be classified as an organic compound (a compound based on carbon atoms). The majority of Lewis structures for simple organic compounds have all atoms with a formal charge of zero. Therefore, add lone pairs and multiple bonds to the structure below to give each atom a formal charge of zero.

Chapter 4, Problem 84AE, Vitamin B6 is an organic compound whose deficiency in the human body can cause apathy, irritability,

a. How many σ bonds and π bonds exist in vitamin B6?

b. Give approximate values for the bond angles marked a through g in the structure.

c. How many carbon atoms are sp2 hybridized?

d. How many carbon, oxygen, and nitrogen atoms are sp3 hybridized?

e. Does vitamin B6 exhibit delocalized π bonding? Explain.

(I)

Interpretation Introduction

Interpretation:

The structure of vitamin B6 has been given and the Lewis structure for Vitamin B6 has to be drawn.

Concept Introduction:

The hybridization of an atom can be obtained by finding its steric number. The sum of the numbers of atoms bonded to the required atom and the number of lone pairs the atom has is known as the steric number.

If the steric number is 4, the atom is sp3 hybridized.

If the steric number is 3, the atom is sp2 hybridized.

If the steric number is 2, the atom is sp hybridized.

Sigma bonds are the single bonds present between atoms in a compound. The second bonding that occurs between the atoms is known as the pi bonding.

Explanation of Solution

For vitamin B6

The electronic configuration of the elements present is,

  H=1s1C=1s22s22p2N=1s22s22p3O=1s22s22p4

Hydrogen has only one electron. The number of valence electrons in carbon is four, in nitrogen is five and in oxygen is six

(a)

Interpretation Introduction

Interpretation:

The total number of pi bonds and sigma bonds present in the Vitamin B6 has to be given.

Concept Introduction:

The hybridization of an atom can be obtained by finding its steric number. The sum of the numbers of atoms bonded to the required atom and the number of lone pairs the atom has is known as the steric number.

If the steric number is 4, the atom is sp3 hybridized.

If the steric number is 3, the atom is sp2 hybridized.

If the steric number is 2, the atom is sp hybridized.

Sigma bonds are the single bonds present between atoms in a compound. The second bonding that occurs between the atoms is known as the pi bonding.

(b)

Interpretation Introduction

Interpretation:

In the Lewis structure of Vitamin B6, the approximate value of bond angles from a to g has to be given.

(c)

Interpretation Introduction

Interpretation:

The total number of carbon atoms that are sp2 hybridized has to be given.

Concept Introduction:

The hybridization of an atom can be obtained by finding its steric number. The sum of the numbers of atoms bonded to the required atom and the number of lone pairs the atom has is known as the steric number.

If the steric number is 4, the atom is sp3 hybridized.

If the steric number is 3, the atom is sp2 hybridized.

If the steric number is 2, the atom is sp hybridized.

Sigma bonds are the single bonds present between atoms in a compound. The second bonding that occurs between the atoms is known as the pi bonding.

(d)

Interpretation Introduction

Interpretation:

The number of carbon, oxygen, and nitrogen atoms that are sp3 hybridized has to be given.

Concept Introduction:

The hybridization of an atom can be obtained by finding its steric number. The sum of the numbers of atoms bonded to the required atom and the number of lone pairs the atom has is known as the steric number.

If the steric number is 4, the atom is sp3 hybridized.

If the steric number is 3, the atom is sp2 hybridized.

If the steric number is 2, the atom is sp hybridized.

Sigma bonds are the single bonds present between atoms in a compound.  The second bonding that occurs between the atoms is known as the pi bonding.

(e)

Interpretation Introduction

Interpretation:

Delocalized pi bonding is present in Vitamin B6 or not has to be explained.

Concept Introduction:

The hybridization of an atom can be obtained by finding its steric number. The sum of the numbers of atoms bonded to the required atom and the number of lone pairs the atom has is known as the steric number.

If the steric number is 4, the atom is sp3 hybridized.

If the steric number is 3, the atom is sp2 hybridized.

If the steric number is 2, the atom is sp hybridized.

Sigma bonds are the single bonds present between atoms in a compound. The second bonding that occurs between the atoms is known as the pi bonding.

Still sussing out bartleby?

Check out a sample textbook solution.

See a sample solution

The Solution to Your Study Problems

Bartleby provides explanations to thousands of textbook problems written by our experts, many with advanced degrees!

Get Started

Chapter 4 Solutions

Chemistry: An Atoms First Approach
Show all chapter solutions
add
Ch. 4 - Which of the following would you expect to be more...Ch. 4 - Arrange the following molecules from most to least...Ch. 4 - Which is the more correct statement: The methane...Ch. 4 - Compare and contrast the MO model with the local...Ch. 4 - What are the relationships among bond order, bond...Ch. 4 - Which of the following statements is/are true?...Ch. 4 - Give one example of a compound having a linear...Ch. 4 - In the hybrid orbital model, compare and contrast ...Ch. 4 - Give the expected hybridization for the molecular...Ch. 4 - In the molecular orbital mode l, compare and...Ch. 4 - Why are d orbitals sometimes used to form hybrid...Ch. 4 - The atoms in a single bond can rotate about the...Ch. 4 - Compare and contrast bonding molecular orbitals...Ch. 4 - What modification to the molecular orbital model...Ch. 4 - Why does the molecular orbital model do a better...Ch. 4 - The three NO bonds in NO3 are all equivalent in...Ch. 4 - Predict the molecular structure (including bond...Ch. 4 - Predict the molecular structure (including bond...Ch. 4 - Predict the molecular structure and bond angles...Ch. 4 - Predict the molecular structure and bond angles...Ch. 4 - There are several molecular structures based on...Ch. 4 - Two variations of the octahedral geometry (see...Ch. 4 - Predict the molecular structure (including bond...Ch. 4 - Predict the molecular structure (including bond...Ch. 4 - State whether or not each of the following has a...Ch. 4 - The following electrostatic potential diagrams...Ch. 4 - Which of the molecules in Exercises 21 and 22 have...Ch. 4 - Which of the molecules in Exercises 27 and 28 have...Ch. 4 - Write Lewis structures and predict the molecular...Ch. 4 - Write Lewis structures and predict whether each of...Ch. 4 - Consider the following Lewis structure where E is...Ch. 4 - Consider the following Lewis structure where E is...Ch. 4 - The molecules BF3, CF4, CO2, PF5, and SF6 are all...Ch. 4 - Two different compounds have the formula XeF2Cl2....Ch. 4 - Use the localized electron model to describe the...Ch. 4 - Use the localized electron model to describe the...Ch. 4 - Use the localized electron model to describe the...Ch. 4 - Use the localized electron model to describe the...Ch. 4 - The space-filling models of ethane and ethanol are...Ch. 4 - The space-filling models of hydrogen cyanide and...Ch. 4 - Give the expected hybridization of the central...Ch. 4 - Give the expected hybridization of the central...Ch. 4 - Give the expected hybridization of the central...Ch. 4 - Give the expected hybridization of the central...Ch. 4 - For each of the following molecules, write the...Ch. 4 - For each of the following molecules or ions that...Ch. 4 - Why must all six atoms in C2H4 lie in the same...Ch. 4 - The allene molecule has the following Lewis...Ch. 4 - Indigo is the dye used in coloring blue jeans. The...Ch. 4 - Urea, a compound formed in the liver, is one of...Ch. 4 - Biacetyl and acetoin are added to margarine to...Ch. 4 - Many important compounds in the chemical industry...Ch. 4 - Two molecules used in the polymer industry are...Ch. 4 - Hot and spicy foods contain molecules that...Ch. 4 - One of the first drugs to be approved for use in...Ch. 4 - The antibiotic thiarubin-A was discovered by...Ch. 4 - Consider the following molecular orbitals formed...Ch. 4 - Sketch the molecular orbital and label its type (...Ch. 4 - Which of the following are predicted by the...Ch. 4 - Which of the following are predicted by the...Ch. 4 - Using the molecular orbital model, write electron...Ch. 4 - Consider the following electron configuration:...Ch. 4 - Using molecular orbital theory, explain why the...Ch. 4 - Using the molecular orbital model to describe the...Ch. 4 - The transport of O2 in the blood is carried out by...Ch. 4 - A Lewis structure obeying the octet rule can be...Ch. 4 - Using the molecular orbital model, write electron...Ch. 4 - Using the molecular orbital model, write electron...Ch. 4 - In which of the following diatomic molecules would...Ch. 4 - In terms of the molecular orbital model, which...Ch. 4 - Show how two 2p atomic orbitals can combine to...Ch. 4 - Show how a hydrogen 1s atomic orbital and a...Ch. 4 - Use Figs. 4-54 and 4-55 to answer the following...Ch. 4 - The diatomic molecule OH exists in the gas phase....Ch. 4 - Acetylene (C2H2) can be produced from the reaction...Ch. 4 - Describe the bonding in NO+, NO, and NO, using...Ch. 4 - Describe the bonding in the O3 molecule and the...Ch. 4 - Describe the bonding in the CO32 ion using the...Ch. 4 - Draw the Lewis structures, predict the molecular...Ch. 4 - Vitamin B6 is an organic compound whose deficiency...Ch. 4 - Two structures can be drawn for cyanuric acid: a....Ch. 4 - What do each of the following sets of...Ch. 4 - What do each of the following sets of...Ch. 4 - Aspartame is an artificial sweetener marketed...Ch. 4 - Using bond energies from Table 3-3, estimate the...Ch. 4 - The three most stable oxides of carbon are carbon...Ch. 4 - Refer back to the formal charge Exercises 99 and...Ch. 4 - Which of the following molecules have net dipole...Ch. 4 - The strucrure of TeF5 is Draw a complete Lewis...Ch. 4 - Complete the following resonance structures for...Ch. 4 - The N2O molecule is linear and polar. a. On the...Ch. 4 - Describe the bonding in the first excited state of...Ch. 4 - Using an MO energy-level diagram, would you expect...Ch. 4 - Show how a dxz. atomic orbital and a pz, atomic...Ch. 4 - What type of molecular orbital would result from...Ch. 4 - Consider three molecules: A, B, and C. Molecule A...Ch. 4 - The formulas of several chemical substances are...Ch. 4 - Predict the molecular structure, bond angles, and...Ch. 4 - Draw the Lewis structures for SO2, PCl3, NNO, COS,...Ch. 4 - Draw the Lewis structures for TeCl4, ICl5, PCl5,...Ch. 4 - A variety of chlorine oxide fluorides and related...Ch. 4 - Pelargondin is the molecule responsible for the...Ch. 4 - Complete a Lewis structure for the compound shown...Ch. 4 - Which of the following statements concerning SO2...Ch. 4 - Consider the molecular orbital electron...Ch. 4 - Place the species B2+ , B2, and B2 in order of...Ch. 4 - The compound NF3 is quite stable, but NCl3 is very...Ch. 4 - Predict the molecular structure for each of the...Ch. 4 - Consider the following computer-generated model of...Ch. 4 - Cholesterol (C27liu;O) has the following...Ch. 4 - Cyanamide (H2NCN), an important industrial...Ch. 4 - As compared with CO and O2, CS and S2 are very...Ch. 4 - Values of measured bond energies may vary greatly...Ch. 4 - Use the MO model to explain the bonding in BeH2....Ch. 4 - Bond energy has been defined in the text as the...Ch. 4 - Arrange the following from lowest to highest...Ch. 4 - Use the MO model to determine which of the...Ch. 4 - Given that the ionization energy of F2 is 290...Ch. 4 - Carbon monoxide (CO) forms bonds to a variety of...Ch. 4 - The space-filling model for benzoic acid, a food...Ch. 4 - As the bead engineer of your starship in charge of...Ch. 4 - A flask containing gaseous N2 is irradiated with...Ch. 4 - Determine the molecular structure and...

Additional Science Textbook Solutions

Find more solutions based on key concepts
Show solutions add
Insufficient dietary protein can cause slowed protein synthesis. hepatitis. accelerated growth in children. all...

Nutrition: Concepts and Controversies - Standalone book (MindTap Course List)

Describe the physical properties of gases.

Chemistry for Engineering Students

A block slides down a frictionless plane having an inclination of 15.0. The block starts from rest at the top...

Physics for Scientists and Engineers, Technology Update (No access codes included)

Of what commercial importance are marine algae and plants?

Oceanography: An Invitation To Marine Science, Loose-leaf Versin