The number of bonds predicted for nitrogen atom according to valence bond theory should be determined from the given options. Concept introduction: According to valence bond theory , The bonds between atoms are formed by sharing their electrons through the overlap of atomic orbitals between other atoms. The each overlapping atomic orbital must be contained with a single unpaired. The electron carried by each overlapping atomic of must have opposite spins. Formation of a bond between atoms should have lower potential energy as compared to the sum of potential energies of individual atoms. The bond angle of bonds is depends upon the angle between overlapping orbitals and lone pairs of central atom.

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Answer 1

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Definition Definition Theory that explains how individual atomic orbitals with an unpaired electron each, come close to each other and overlap to form a molecular orbital giving a covalent bond. VBT gives a quantum mechanical approach to the formation of covalent bonds with the help of wave functions using attractive and repulsive energies when two atoms are brought from infinity to their internuclear distance.

Chapter 7.4, Problem 7.4.2SR

Interpretation Introduction

Interpretation:

The number of bonds predicted for nitrogen atom according to valence bond theory should be determined from the given options.

Concept introduction:

According to valence bond theory,

The bonds between atoms are formed by sharing their electrons through the overlap of atomic orbitals between other atoms.

The each overlapping atomic orbital must be contained with a single unpaired.

The electron carried by each overlapping atomic of must have opposite spins.

Formation of a bond between atoms should have lower potential energy as compared to the sum of potential energies of individual atoms.

The bond angle of bonds is depends upon the angle between overlapping orbitals and lone pairs of central atom.

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1. Calculate the accurate monoisotopic mass (using all 1H, 12C, 14N, 160 and 35CI) for your product using the table in your lab manual. Don't include the Cl, since you should only have [M+H]*. Compare this to the value you see on the LC-MS printout. How much different are they? 2. There are four isotopic peaks for the [M+H]* ion at m/z 240, 241, 242 and 243. For one point of extra credit, explain what each of these is and why they are present. 3. There is a fragment ion at m/z 184. For one point of extra credit, identify this fragment and confirm by calculating the accurate monoisotopic mass. 4. The UV spectrum is also at the bottom of your printout. For one point of extra credit, look up the UV spectrum of bupropion on Google Images and compare to your spectrum. Do they match? Cite your source. 5. For most of you, there will be a second chromatographic peak whose m/z is 74 (to a round number). For one point of extra credit, see if you can identify this molecule as well and confirm by…

Please draw, not just describe!

can you draw each step on a piece of a paper please this is very confusing to me

Answer 2

Question

Definition Definition Theory that explains how individual atomic orbitals with an unpaired electron each, come close to each other and overlap to form a molecular orbital giving a covalent bond. VBT gives a quantum mechanical approach to the formation of covalent bonds with the help of wave functions using attractive and repulsive energies when two atoms are brought from infinity to their internuclear distance.

Chapter 7.4, Problem 7.4.2SR

Interpretation Introduction

Interpretation:

The number of bonds predicted for nitrogen atom according to valence bond theory should be determined from the given options.

Concept introduction:

According to valence bond theory,

The bonds between atoms are formed by sharing their electrons through the overlap of atomic orbitals between other atoms.

The each overlapping atomic orbital must be contained with a single unpaired.

The electron carried by each overlapping atomic of must have opposite spins.

Formation of a bond between atoms should have lower potential energy as compared to the sum of potential energies of individual atoms.

The bond angle of bonds is depends upon the angle between overlapping orbitals and lone pairs of central atom.

Expert Solution & Answer

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Check out a sample textbook solution

See solution

Answer 3

Question

Definition Definition Theory that explains how individual atomic orbitals with an unpaired electron each, come close to each other and overlap to form a molecular orbital giving a covalent bond. VBT gives a quantum mechanical approach to the formation of covalent bonds with the help of wave functions using attractive and repulsive energies when two atoms are brought from infinity to their internuclear distance.

Chapter 7.4, Problem 7.4.2SR

Interpretation Introduction

Interpretation:

The number of bonds predicted for nitrogen atom according to valence bond theory should be determined from the given options.

Concept introduction:

According to valence bond theory,

The bonds between atoms are formed by sharing their electrons through the overlap of atomic orbitals between other atoms.

The each overlapping atomic orbital must be contained with a single unpaired.

The electron carried by each overlapping atomic of must have opposite spins.

Formation of a bond between atoms should have lower potential energy as compared to the sum of potential energies of individual atoms.

The bond angle of bonds is depends upon the angle between overlapping orbitals and lone pairs of central atom.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 4

Question

Definition Definition Theory that explains how individual atomic orbitals with an unpaired electron each, come close to each other and overlap to form a molecular orbital giving a covalent bond. VBT gives a quantum mechanical approach to the formation of covalent bonds with the help of wave functions using attractive and repulsive energies when two atoms are brought from infinity to their internuclear distance.

Chapter 7.4, Problem 7.4.2SR

Interpretation Introduction