Determine the hybridization about 0 in CH 3 OH.

Question

Want to see more full solutions like this?

Answer 1

Textbook Question

Chapter 7, Problem 1SAQ

Determine the hybridization about 0 in CH₃OH.

Chapter 7, Problem 1SAQ, Determine the hybridization about 0 in CH3OH.

Expert Solution & Answer

Interpretation Introduction

Interpretation:

Find the hybridization of Oxygen (O) in CH3OH.

Concept introduction:

For molecule with two or more than two atoms, the formation of hybrid orbital takes place by the mixing of atomic orbitals of atoms possessing nearly same energy in free state. The mixing of orbitals takes place by the overlapping of orbitals of each atom in the molecule, which result in the formation of bonds. The formed hybrid orbitals possess energies that are different from the energy of atomic orbitals of parent atoms. The hybrid orbitals which possess less energy compared to the atomic orbitals of parent atoms result in formation of sigma molecular orbitals whereas hybrid orbitals which possess more energy compared to the atomic orbitals of parent atoms result in formation of pi molecular orbitals.

Answer to Problem 1SAQ

Option (d) is the correct answer. Because, the Oxygen (O) hybridization of CH3OH is sp3.

Explanation of Solution

Reason for the correct option:

The electronic configuration of O:

1s22s22p4

The oxygen can form two bonds with this electronic configuration.

In CH3OH, this O forms two single bonds one with C atom and one with H. 2py and 2pz are used in this type of the bonding thus, they have 1 electron each. H and C each contribute 1 electron to fill this two half of the p-orbitals of Oxygen(O). So the remaining two pairs of electrons are present in O in the remaining orbitals that is 2px2 and 2s2.

The hybridization of O is sp3 because it forms 2 bonds and has 2 lone pairs. Its 2s and 2p orbitals are involved in the bonding.

Want to see more full solutions like this?

Subscribe now to access step-by-step solutions to millions of textbook problems written by subject matter experts!

Students have asked these similar questions

Part 1 See Periodic Table One resonance structure of CNO¯ is shown. In the first box, add two curved arrows to show the movement of electrons that result in the resonance form with a -1 formal charge on the oxygen atom. In the second box, draw this resonance form with the -1 formal charge on the oxygen atom by adding bonds, lone pairs, and non-zero formal charges. =0% → [N=C=O 1 N-C-0

Draw any major resonance contributor for S2O3, assuming that the S atoms are bonded to each other, and the O atoms are bonded to S atoms. Include all nonbonding electrons and all nonzero formal charges.

Determine which of the following procedures are steps in drawing the resonance structures of pyridine and pyrazine. Check all that apply. Draw the Lewis structure.Consider and draw alternate resonance structures. Calculate the molar mass of the compound. Leave out the lone pairs of electrons. Determine the central atom, if possible. Complete the octets of each atom (dublet for H). Determine the number of covalent bonds in the structure. Check the structure with electron bookkeeping.

Answer 2

Textbook Question

Chapter 7, Problem 1SAQ

Determine the hybridization about 0 in CH₃OH.

Chapter 7, Problem 1SAQ, Determine the hybridization about 0 in CH3OH.

Expert Solution & Answer

Interpretation Introduction

Interpretation:

Find the hybridization of Oxygen (O) in CH3OH.

Concept introduction:

For molecule with two or more than two atoms, the formation of hybrid orbital takes place by the mixing of atomic orbitals of atoms possessing nearly same energy in free state. The mixing of orbitals takes place by the overlapping of orbitals of each atom in the molecule, which result in the formation of bonds. The formed hybrid orbitals possess energies that are different from the energy of atomic orbitals of parent atoms. The hybrid orbitals which possess less energy compared to the atomic orbitals of parent atoms result in formation of sigma molecular orbitals whereas hybrid orbitals which possess more energy compared to the atomic orbitals of parent atoms result in formation of pi molecular orbitals.

Answer to Problem 1SAQ

Option (d) is the correct answer. Because, the Oxygen (O) hybridization of CH3OH is sp3.

Explanation of Solution

Reason for the correct option:

The electronic configuration of O:

1s22s22p4

The oxygen can form two bonds with this electronic configuration.

In CH3OH, this O forms two single bonds one with C atom and one with H. 2py and 2pz are used in this type of the bonding thus, they have 1 electron each. H and C each contribute 1 electron to fill this two half of the p-orbitals of Oxygen(O). So the remaining two pairs of electrons are present in O in the remaining orbitals that is 2px2 and 2s2.

The hybridization of O is sp3 because it forms 2 bonds and has 2 lone pairs. Its 2s and 2p orbitals are involved in the bonding.

Want to see more full solutions like this?

Subscribe now to access step-by-step solutions to millions of textbook problems written by subject matter experts!

Answer 3

Textbook Question

Chapter 7, Problem 1SAQ

Determine the hybridization about 0 in CH₃OH.

Chapter 7, Problem 1SAQ, Determine the hybridization about 0 in CH3OH.

Expert Solution & Answer

Interpretation Introduction

Interpretation:

Find the hybridization of Oxygen (O) in CH3OH.

Concept introduction:

For molecule with two or more than two atoms, the formation of hybrid orbital takes place by the mixing of atomic orbitals of atoms possessing nearly same energy in free state. The mixing of orbitals takes place by the overlapping of orbitals of each atom in the molecule, which result in the formation of bonds. The formed hybrid orbitals possess energies that are different from the energy of atomic orbitals of parent atoms. The hybrid orbitals which possess less energy compared to the atomic orbitals of parent atoms result in formation of sigma molecular orbitals whereas hybrid orbitals which possess more energy compared to the atomic orbitals of parent atoms result in formation of pi molecular orbitals.

Answer to Problem 1SAQ

Option (d) is the correct answer. Because, the Oxygen (O) hybridization of CH3OH is sp3.

Explanation of Solution

Reason for the correct option:

The electronic configuration of O:

1s22s22p4

The oxygen can form two bonds with this electronic configuration.

In CH3OH, this O forms two single bonds one with C atom and one with H. 2py and 2pz are used in this type of the bonding thus, they have 1 electron each. H and C each contribute 1 electron to fill this two half of the p-orbitals of Oxygen(O). So the remaining two pairs of electrons are present in O in the remaining orbitals that is 2px2 and 2s2.

The hybridization of O is sp3 because it forms 2 bonds and has 2 lone pairs. Its 2s and 2p orbitals are involved in the bonding.

Want to see more full solutions like this?

Subscribe now to access step-by-step solutions to millions of textbook problems written by subject matter experts!

Answer 4

Textbook Question

Chapter 7, Problem 1SAQ

Determine the hybridization about 0 in CH₃OH.

Chapter 7, Problem 1SAQ, Determine the hybridization about 0 in CH3OH.

Expert Solution & Answer

Interpretation Introduction

Interpretation:

Find the hybridization of Oxygen (O) in CH3OH.

Concept introduction:

For molecule with two or more than two atoms, the formation of hybrid orbital takes place by the mixing of atomic orbitals of atoms possessing nearly same energy in free state. The mixing of orbitals takes place by the overlapping of orbitals of each atom in the molecule, which result in the formation of bonds. The formed hybrid orbitals possess energies that are different from the energy of atomic orbitals of parent atoms. The hybrid orbitals which possess less energy compared to the atomic orbitals of parent atoms result in formation of sigma molecular orbitals whereas hybrid orbitals which possess more energy compared to the atomic orbitals of parent atoms result in formation of pi molecular orbitals.

Answer to Problem 1SAQ

Option (d) is the correct answer. Because, the Oxygen (O) hybridization of CH3OH is sp3.

Explanation of Solution

Reason for the correct option:

The electronic configuration of O:

1s22s22p4

The oxygen can form two bonds with this electronic configuration.

In CH3OH, this O forms two single bonds one with C atom and one with H. 2py and 2pz are used in this type of the bonding thus, they have 1 electron each. H and C each contribute 1 electron to fill this two half of the p-orbitals of Oxygen(O). So the remaining two pairs of electrons are present in O in the remaining orbitals that is 2px2 and 2s2.

The hybridization of O is sp3 because it forms 2 bonds and has 2 lone pairs. Its 2s and 2p orbitals are involved in the bonding.

Want to see more full solutions like this?

Subscribe now to access step-by-step solutions to millions of textbook problems written by subject matter experts!

Answer 5

Textbook Question

Answer 6

Textbook Question

Answer 7

Expert Solution & Answer

Interpretation Introduction

Interpretation:

Find the hybridization of Oxygen (O) in CH3OH.

Concept introduction:

For molecule with two or more than two atoms, the formation of hybrid orbital takes place by the mixing of atomic orbitals of atoms possessing nearly same energy in free state. The mixing of orbitals takes place by the overlapping of orbitals of each atom in the molecule, which result in the formation of bonds. The formed hybrid orbitals possess energies that are different from the energy of atomic orbitals of parent atoms. The hybrid orbitals which possess less energy compared to the atomic orbitals of parent atoms result in formation of sigma molecular orbitals whereas hybrid orbitals which possess more energy compared to the atomic orbitals of parent atoms result in formation of pi molecular orbitals.

Answer to Problem 1SAQ

Option (d) is the correct answer. Because, the Oxygen (O) hybridization of CH3OH is sp3.

Explanation of Solution

Reason for the correct option:

The electronic configuration of O:

1s22s22p4

The oxygen can form two bonds with this electronic configuration.

In CH3OH, this O forms two single bonds one with C atom and one with H. 2py and 2pz are used in this type of the bonding thus, they have 1 electron each. H and C each contribute 1 electron to fill this two half of the p-orbitals of Oxygen(O). So the remaining two pairs of electrons are present in O in the remaining orbitals that is 2px2 and 2s2.

The hybridization of O is sp3 because it forms 2 bonds and has 2 lone pairs. Its 2s and 2p orbitals are involved in the bonding.

Answer 8

Expert Solution & Answer

Interpretation Introduction

Interpretation:

Find the hybridization of Oxygen (O) in CH3OH.

Concept introduction:

For molecule with two or more than two atoms, the formation of hybrid orbital takes place by the mixing of atomic orbitals of atoms possessing nearly same energy in free state. The mixing of orbitals takes place by the overlapping of orbitals of each atom in the molecule, which result in the formation of bonds. The formed hybrid orbitals possess energies that are different from the energy of atomic orbitals of parent atoms. The hybrid orbitals which possess less energy compared to the atomic orbitals of parent atoms result in formation of sigma molecular orbitals whereas hybrid orbitals which possess more energy compared to the atomic orbitals of parent atoms result in formation of pi molecular orbitals.

Answer to Problem 1SAQ

Option (d) is the correct answer. Because, the Oxygen (O) hybridization of CH3OH is sp3.

Explanation of Solution

Reason for the correct option:

The electronic configuration of O:

1s22s22p4

The oxygen can form two bonds with this electronic configuration.

In CH3OH, this O forms two single bonds one with C atom and one with H. 2py and 2pz are used in this type of the bonding thus, they have 1 electron each. H and C each contribute 1 electron to fill this two half of the p-orbitals of Oxygen(O). So the remaining two pairs of electrons are present in O in the remaining orbitals that is 2px2 and 2s2.

The hybridization of O is sp3 because it forms 2 bonds and has 2 lone pairs. Its 2s and 2p orbitals are involved in the bonding.

Answer 9

Expert Solution & Answer

Answer 10

Expert Solution & Answer

Answer 11

Interpretation Introduction

Interpretation:

Find the hybridization of Oxygen (O) in CH3OH.

Concept introduction:

For molecule with two or more than two atoms, the formation of hybrid orbital takes place by the mixing of atomic orbitals of atoms possessing nearly same energy in free state. The mixing of orbitals takes place by the overlapping of orbitals of each atom in the molecule, which result in the formation of bonds. The formed hybrid orbitals possess energies that are different from the energy of atomic orbitals of parent atoms. The hybrid orbitals which possess less energy compared to the atomic orbitals of parent atoms result in formation of sigma molecular orbitals whereas hybrid orbitals which possess more energy compared to the atomic orbitals of parent atoms result in formation of pi molecular orbitals.

Answer 12

Answer to Problem 1SAQ

Option (d) is the correct answer. Because, the Oxygen (O) hybridization of CH3OH is sp3.

Answer 13

Explanation of Solution

Reason for the correct option:

The electronic configuration of O:

1s22s22p4

The oxygen can form two bonds with this electronic configuration.

In CH3OH, this O forms two single bonds one with C atom and one with H. 2py and 2pz are used in this type of the bonding thus, they have 1 electron each. H and C each contribute 1 electron to fill this two half of the p-orbitals of Oxygen(O). So the remaining two pairs of electrons are present in O in the remaining orbitals that is 2px2 and 2s2.

The hybridization of O is sp3 because it forms 2 bonds and has 2 lone pairs. Its 2s and 2p orbitals are involved in the bonding.

Answer 14

Ch. 7 - Determine the hybridization about 0 in CH3OH.Ch. 7 - Determine the hybridization about C in H2CO.Ch. 7 - According to the valance bond theory, which kind...Ch. 7 - Use molecular orbital theory to determine the bond...Ch. 7 - Use molecular orbital theory to predict which...Ch. 7 - Use molecular orbital theory to determine which...Ch. 7 - Which hybridization scheme occurs about nitrogen...Ch. 7 - Prob. 8SAQ Ch. 7 - Prob. 9SAQ Ch. 7 - Prob. 10SAQ

Determine the hybridization about 0 in CH 3 OH.

Videos

Answer to Problem 1SAQ

Explanation of Solution

Want to see more full solutions like this?

Chapter 7 Solutions