Chapter 10, Problem 10.29P

Interpretation Introduction

(a)

Interpretation:

The structure formula with all valence electrons should be drawn for a carbonyl group.

Concept Introduction:

Lewis structures can be drawn by following some point for any compound as mentioned below:

• Find out number of valence electrons present in the molecule
• The connectivity of atoms need to be understood like which atoms are linked with each other and connect them with covalnet bonds
• The arrangements of electrons in proper manner to achieve complete outer shell

With the help of Lewis model, we can understand the structure formula as well as number of valence electrons of atom present in molecule. Lewis model provide details about the covalent bond present in between atoms like single bond, double bond or triple bond. A covalent bond is formed between the atoms which have electronegativity less than 1.9 and have pairs of electron for sharing.

Answer to Problem 10.29P

Lewis structure for a carbonyl group:

Explanation of Solution

The structure of any atom of prepared with the help of Lewis model which explains guideline for bonding of atom. It guides about the covalent bonds which are formed in various combinations of single, double and triple bonds.

Single covalent bond occurs by sharing one pair of electrons and can be represented by single line in between atoms.

Double and triple bonds are formed when two and three pairs of electrons are shared in between atoms respectively and can be represented by two or three lines in between the atoms.

For several covalent bonds in organic compound containing carbon bonded to hydrogen, nitrogen, chlorine and oxygen shows some important points to be noted for structure are as follow:

1. Carbon forms four covalent bonds while hydrogen form one covalent bond and both has no unshared pair of electrons.
2. Three covalent bonds are formed in nitrogen atom with only one unshared pair of electron left behind.
3. Oxygen can form two covalent bonds and have further more two unshared pair of electron.
4. Iodine, chlorine, bromine and fluorine like halogens can form only one covalent bond like hydrogen but they have three unshared pair of electrons.

To draw Lewis structure for a carbonyl group, following are the steps:

Carbonyl group is generally producing aldehydes when one hydrocarbon and one hydrogen is bonded with its carbon atom and ketone when two hydrocarbon groups bonded to its carbon.

Carbonyl group has double bond between its carbon and oxygen atoms which is completing oxygen’s octet and had two unshared pair of electrons over oxygen symbol.

Carbon can form four bonds from which it has formed double bond with oxygen and two single bonds forms with hydrogen and hydrocarbon or both. This can complete octet of carbon.

Interpretation Introduction

(b)

Interpretation:

The structure formula with all valence electrons should be drawn for a carboxyl group.

Concept Introduction:

Lewis structures can be prepared by following some point for any compound as mentioned below:

• Find out number of valence electrons present in the molecule
• The connectivity o atoms need to be understood like which atoms are linked with each other and connect them with covalnet bonds
• The arrangements of electrons in proper manner to achieve complete outer shell

With the help of Lewis model, we can understand the structure formula as well as number of valence electrons of atom present in molecule. Lewis model provide details about the covalent bond present in between atoms like single bond, double bond or triple bond. A covalent bond is formed between the atoms which have electronegativity less than 1.9 and have pairs of electron for sharing.

Answer to Problem 10.29P

To draw Lewis structure for a carboxyl group:

Explanation of Solution

The structure of any atom of prepared with the help of Lewis model which explains guideline for bonding of atom. It guides about the covalent bonds which are formed in various combinations of single, double and triple bonds.

Single covalent bond occurs by sharing one pair of electrons and can be represented by single line in between atoms.

Double and triple bonds are formed when two and three pairs of electrons are shared in between atoms respectively and can be represented by two or three lines in between the atoms.

For several covalent bonds in organic compound containing carbon bonded to hydrogen, nitrogen, chlorine and oxygen shows some important points to be noted for structure are as follow:

1. Carbon forms four covalent bonds while hydrogen form one covalent bond and both has no unshared pair of electrons.
2. Three covalent bonds are formed in nitrogen atom with only one unshared pair of electron left behind.
3. Oxygen can form two covalent bonds and have further more two unshared pair of electron.
4. Iodine, chlorine, bromine and fluorine like halogens can form only one covalent bond like hydrogen but they have three unshared pair of electrons.

To draw Lewis structure for a carboxyl group, following are the steps:

There are two oxygen atoms present which have formed one single covalent bond with hydrogen atom and one single covalent bond with carbon. There is two valence electron pair of oxygen represented as two dots on symbol of oxygen.

Second oxygen atom has double bond with carbon atom and completes its octet along with two unshared pair of electron on it.

Carbon atom formed double as well as single bond with both oxygen atoms and one single bond with hydrocarbon group or hydrogen atom to complete its octet with no unshared pair of electrons.

R is any hydrocarbon group or hydrogen atoms which bonds with carbon of carboxyl group.

Interpretation Introduction

(c)

Interpretation:

The structure formula with all valence electrons should be drawn for a hydroxyl group.

Concept Introduction:

Lewis structures can be prepared by following some point for any compound as mentioned below:

• Find out number of valence electrons present in the molecule
• The connectivity o atoms need to be understood like which atoms are linked with each other and connect them with covalnet bonds
• The arrangements of electrons in proper manner to achieve complete outer shell

With the help of Lewis model, we can understand the structure formula as well as number of valence electrons of atom present in molecule. Lewis model provide details about the covalent bond present in between atoms like single bond, double bond or triple bond. A covalent bond is formed between the atoms which have electronegativity less than 1.9 and have pairs of electron for sharing.

Answer to Problem 10.29P

To draw Lewis structure for a hydroxyl group:

Explanation of Solution

The structure of any atom of prepared with the help of Lewis model which explains guideline for bonding of atom. It guides about the covalent bonds which are formed in various combinations of single, double and triple bonds.

Single covalent bond occurs by sharing one pair of electrons and can be represented by single line in between atoms.

Double and triple bonds are formed when two and three pairs of electrons are shared in between atoms respectively and can be represented by two or three lines in between the atoms.

For several covalent bonds in organic compound containing carbon bonded to hydrogen, nitrogen, chlorine and oxygen shows some important points to be noted for structure are as follow:

1. Carbon forms four covalent bonds while hydrogen form one covalent bond and both has no unshared pair of electrons.
2. Three covalent bonds are formed in nitrogen atom with only one unshared pair of electron left behind.
3. Oxygen can form two covalent bonds and have further more two unshared pair of electron.
4. Iodine, chlorine, bromine and fluorine like halogens can form only one covalent bond like hydrogen but they have three unshared pair of electrons.

To draw Lewis structure for a hydroxyl group, following are the steps:

As hydroxyl contains two atoms − Oxygen and hydrogen, oxygen only forms one single covalent bond with hydrogen and has three pair of unshed pair of electrons.

Oxygen atoms is not stable because only one covalent is formed, leads to results into formation of hydroxide ion.

Hydrogen atom completes its duet with single bond of oxygen.

Interpretation Introduction

(d)

Interpretation:

The structure formula with all valence electrons should be drawn for a primary amine group.

Concept Introduction:

Lewis structures can be prepared by following some point for any compound as mentioned below:

• Find out number of valence electrons present in the molecule
• The connectivity o atoms need to be understood like which atoms are linked with each other and connect them with covalnet bonds
• The arrangements of electrons in proper manner to achieve complete outer shell

With the help of Lewis model, we can understand the structure formula as well as number of valence electrons of atom present in molecule. Lewis model provide details about the covalent bond present in between atoms like single bond, double bond or triple bond. A covalent bond is formed between the atoms which have electronegativity less than 1.9 and have pairs of electron for sharing.

Answer to Problem 10.29P

To draw Lewis structure for a primary amino group:

Explanation of Solution

The structure of any atom of prepared with the help of Lewis model which explains guideline for bonding of atom. It guides about the covalent bonds which are formed in various combinations of single, double and triple bonds.

Single covalent bond occurs by sharing one pair of electrons and can be represented by single line in between atoms.

Double and triple bonds are formed when two and three pairs of electrons are shared in between atoms respectively and can be represented by two or three lines in between the atoms.

For several covalent bonds in organic compound containing carbon bonded to hydrogen, nitrogen, chlorine and oxygen shows some important points to be noted for structure are as follow:

1. Carbon forms four covalent bonds while hydrogen form one covalent bond and both has no unshared pair of electrons.
2. Three covalent bonds are formed in nitrogen atom with only one unshared pair of electron left behind.
3. Oxygen can form two covalent bonds and have further more two unshared pair of electron.
4. Iodine, chlorine, bromine and fluorine like halogens can form only one covalent bond like hydrogen but they have three unshared pair of electrons.

To draw Lewis structure for a carbonyl group, following are the steps:

In any primary amine group, nitrogen atom is present which carries one unshared pair of electron to bind with any hydrocarbon group or hydrogen atom to forma compound.

Two single covalent bonds of nitrogen are satisfied by hydrogen atoms and both hydrogen atoms also complete its duets by sharing valence electrons with nitrogen atom.

Interpretation Introduction

(e)

Interpretation:

The structure formula with all valence electrons should be drawn for an ester group.

Concept Introduction:

Lewis structures can be prepared by following some point for any compound as mentioned below:

• Find out number of valence electrons present in the molecule
• The connectivity o atoms need to be understood like which atoms are linked with each other and connect them with covalnet bonds
• The arrangements of electrons in proper manner to achieve complete outer shell

With the help of Lewis model, we can understand the structure formula as well as number of valence electrons of atom present in molecule. Lewis model provide details about the covalent bond present in between atoms like single bond, double bond or triple bond. A covalent bond is formed between the atoms which have electronegativity less than 1.9 and have pairs of electron for sharing.

Answer to Problem 10.29P

To draw Lewis structure for an ester group:

Explanation of Solution

The structure of any atom of prepared with the help of Lewis model which explains guideline for bonding of atom. It guides about the covalent bonds which are formed in various combinations of single, double and triple bonds.

Single covalent bond occurs by sharing one pair of electrons and can be represented by single line in between atoms.

Double and triple bonds are formed when two and three pairs of electrons are shared in between atoms respectively and can be represented by two or three lines in between the atoms.

For several covalent bonds in organic compound containing carbon bonded to hydrogen, nitrogen, chlorine and oxygen shows some important points to be noted for structure are as follow:

1. Carbon forms four covalent bonds while hydrogen form one covalent bond and both has no unshared pair of electrons.
2. Three covalent bonds are formed in nitrogen atom with only one unshared pair of electron left behind.
3. Oxygen can form two covalent bonds and have further more two unshared pair of electron.
4. Iodine, chlorine, bromine and fluorine like halogens can form only one covalent bond like hydrogen but they have three unshared pair of electrons.

To draw Lewis structure for an ester group, following are the steps:

There are three atoms present in an ester group − Oxygen, Hydrogen, and Carbon. Carbon forms double bond with oxygen and one single bond with hydrogen by sharing two and one valence electrons respectively. To complete its octet, carbon forms a single bond with any hydrocarbon group or hydrogen atom.

Oxygen carries two valence electron pair and satisfies octet rule by bonding with carbon atom through double covalent bond.

Hydrogen and carbon shares one valence electron pair.