(a) Interpretation: Whether the bond in H − I is polarized or not is to be stated. If polarized bond is present in the corresponding molecule, then the resulting charge distribution in molecule is to be shown. Concept introduction: Electronegativity is defined as the tendency of an atom to attract electrons towards it. Polarized bonds are a result of the electronegativity difference between bonding atoms. If the electronegativity difference is 0 , the bond is known as nonpolar covalent bond, if it’s between 0 to 2.1 , the bond is known as polar covalent bond and if its more than 2.1 , the bond is known as ionic bond.

Question

Want to see the full answer?

Answer 1

Question

Chapter 4, Problem 4.56E

Interpretation Introduction

(a)

Interpretation:

Whether the bond in H−I is polarized or not is to be stated. If polarized bond is present in the corresponding molecule, then the resulting charge distribution in molecule is to be shown.

Concept introduction:

Electronegativity is defined as the tendency of an atom to attract electrons towards it. Polarized bonds are a result of the electronegativity difference between bonding atoms. If the electronegativity difference is 0, the bond is known as nonpolar covalent bond, if it’s between 0 to 2.1, the bond is known as polar covalent bond and if its more than 2.1, the bond is known as ionic bond.

Interpretation Introduction

(b)

Interpretation:

Whether the bond in SO2 is polarized or not is to be stated. If polarized bond is present in the corresponding molecule, then the resulting charge distribution in molecule is to be shown.

Concept introduction:

Electronegativity is defined as the tendency of an atom to attract electrons towards it. Polarized bonds are a result of the electronegativity difference between bonding atoms. If the electronegativity difference is 0, the bond is known as nonpolar covalent bond, if it’s between 0 to 2.1, the bond is known as polar covalent bond and if its more than 2.1, the bond is known as ionic bond.

Interpretation Introduction

(c)

Interpretation:

Whether the bond in O3 is polarized or not is to be stated. If polarized bond is present in the corresponding molecule, then the resulting charge distribution in molecule is to be shown.

Concept introduction:

Electronegativity is defined as the tendency of an atom to attract electrons towards it. Polarized bonds are a result of the electronegativity difference between bonding atoms. If the electronegativity difference is 0, the bond is known as nonpolar covalent bond, if it’s between 0 to 2.1, the bond is known as polar covalent bond and if its more than 2.1, the bond is known as ionic bond.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Students have asked these similar questions

1. How many valence electrons does each of the following elements have? a. Helium: b. Calcium: C. Sulfur: d. Aluminum: 2. Define electronegativity: 3. How many electrons must an oxygen atom gain to achieve a stable configuration? 4. How many electrons must a sodium atom lose to achieve a stable configuration? 5. What characteristic of metals causes them to readily conduct heat and electricity? 6. Indicate whether you expect the bond in each of the following pairs of atoms to be ionic, polar covalent, nonpolar covalent, or metallic. a. Cs bonding with Cl b. Cl bonding with Cl c. Mg bonding with O d. O bonding with N

Indicate whether each statement below is true or false. a. The core electrons are called valence electrons. b. lonic bonds are formed by the attraction between cations and anions. c. Ionic bonds are formed from atoms by a transfer of electrons. d. In a Lewis symbol, the chemical symbol represents the nucleus of the atom. e. An ion written as a Lewis symbol has brackets outside the electrons. f. Two electrons involved in a bond produce a double bond. g. If the AEN value is very large the bond is polar covalent. h. The central atom is typically the atom with the highest electronegativity. i. An expanded octet has larger electron clouds. j. A nonpolar molecule can have polar bonds.

1. A bond in which an electron pair is shared unequally is called a(n) a. ionic bond b. covalent bond c. polar covalent bond d. co-ordinate covalent bond 2. A measure of an atom's ability to attract electrons in a covalent bond is called a. electron affinity b. electropositivity c. electronegativity d. valence activity 3. Electrons that are found in the outermost shell of an atom are called a. lone pair electrons b. Lewis electrons C. active electrons d. valence electrons 4. An atom that possesses more electrons than protons is called a(n) a. proton b. anion C. cation d. polyatomic ion A compound that, when dissolved in water, produces a solution that conducts electricity is called a(n) 5. a. covalent compound b. electrolyte c. polar covalent compound d. molecule 6. Which of the following compounds contain(s) ionic bonds? a. b. CH, С. СО. d. CaCl, Use the following choices for questions 7 to 12 a. synthesis b. decomposition c. single displacement d. double displacement 7. CaO ) + CO2…

Answer 2

Question

Chapter 4, Problem 4.56E

Interpretation Introduction

(a)

Interpretation:

Whether the bond in H−I is polarized or not is to be stated. If polarized bond is present in the corresponding molecule, then the resulting charge distribution in molecule is to be shown.

Concept introduction:

Electronegativity is defined as the tendency of an atom to attract electrons towards it. Polarized bonds are a result of the electronegativity difference between bonding atoms. If the electronegativity difference is 0, the bond is known as nonpolar covalent bond, if it’s between 0 to 2.1, the bond is known as polar covalent bond and if its more than 2.1, the bond is known as ionic bond.

Interpretation Introduction

(b)

Interpretation:

Whether the bond in SO2 is polarized or not is to be stated. If polarized bond is present in the corresponding molecule, then the resulting charge distribution in molecule is to be shown.

Concept introduction:

Electronegativity is defined as the tendency of an atom to attract electrons towards it. Polarized bonds are a result of the electronegativity difference between bonding atoms. If the electronegativity difference is 0, the bond is known as nonpolar covalent bond, if it’s between 0 to 2.1, the bond is known as polar covalent bond and if its more than 2.1, the bond is known as ionic bond.

Interpretation Introduction

(c)

Interpretation:

Whether the bond in O3 is polarized or not is to be stated. If polarized bond is present in the corresponding molecule, then the resulting charge distribution in molecule is to be shown.

Concept introduction:

Electronegativity is defined as the tendency of an atom to attract electrons towards it. Polarized bonds are a result of the electronegativity difference between bonding atoms. If the electronegativity difference is 0, the bond is known as nonpolar covalent bond, if it’s between 0 to 2.1, the bond is known as polar covalent bond and if its more than 2.1, the bond is known as ionic bond.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 3

Question

Chapter 4, Problem 4.56E

Interpretation Introduction

(a)

Interpretation:

Whether the bond in H−I is polarized or not is to be stated. If polarized bond is present in the corresponding molecule, then the resulting charge distribution in molecule is to be shown.

Concept introduction:

Electronegativity is defined as the tendency of an atom to attract electrons towards it. Polarized bonds are a result of the electronegativity difference between bonding atoms. If the electronegativity difference is 0, the bond is known as nonpolar covalent bond, if it’s between 0 to 2.1, the bond is known as polar covalent bond and if its more than 2.1, the bond is known as ionic bond.

Interpretation Introduction

(b)

Interpretation:

Whether the bond in SO2 is polarized or not is to be stated. If polarized bond is present in the corresponding molecule, then the resulting charge distribution in molecule is to be shown.

Concept introduction:

Electronegativity is defined as the tendency of an atom to attract electrons towards it. Polarized bonds are a result of the electronegativity difference between bonding atoms. If the electronegativity difference is 0, the bond is known as nonpolar covalent bond, if it’s between 0 to 2.1, the bond is known as polar covalent bond and if its more than 2.1, the bond is known as ionic bond.

Interpretation Introduction

(c)

Interpretation:

Whether the bond in O3 is polarized or not is to be stated. If polarized bond is present in the corresponding molecule, then the resulting charge distribution in molecule is to be shown.

Concept introduction:

Electronegativity is defined as the tendency of an atom to attract electrons towards it. Polarized bonds are a result of the electronegativity difference between bonding atoms. If the electronegativity difference is 0, the bond is known as nonpolar covalent bond, if it’s between 0 to 2.1, the bond is known as polar covalent bond and if its more than 2.1, the bond is known as ionic bond.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 4

Question

Chapter 4, Problem 4.56E

Interpretation Introduction

(a)

Interpretation:

Whether the bond in H−I is polarized or not is to be stated. If polarized bond is present in the corresponding molecule, then the resulting charge distribution in molecule is to be shown.

Concept introduction:

Electronegativity is defined as the tendency of an atom to attract electrons towards it. Polarized bonds are a result of the electronegativity difference between bonding atoms. If the electronegativity difference is 0, the bond is known as nonpolar covalent bond, if it’s between 0 to 2.1, the bond is known as polar covalent bond and if its more than 2.1, the bond is known as ionic bond.

Interpretation Introduction

(b)

Interpretation:

Whether the bond in SO2 is polarized or not is to be stated. If polarized bond is present in the corresponding molecule, then the resulting charge distribution in molecule is to be shown.

Concept introduction:

Electronegativity is defined as the tendency of an atom to attract electrons towards it. Polarized bonds are a result of the electronegativity difference between bonding atoms. If the electronegativity difference is 0, the bond is known as nonpolar covalent bond, if it’s between 0 to 2.1, the bond is known as polar covalent bond and if its more than 2.1, the bond is known as ionic bond.

Interpretation Introduction

(c)

Interpretation:

Whether the bond in O3 is polarized or not is to be stated. If polarized bond is present in the corresponding molecule, then the resulting charge distribution in molecule is to be shown.

Concept introduction:

Electronegativity is defined as the tendency of an atom to attract electrons towards it. Polarized bonds are a result of the electronegativity difference between bonding atoms. If the electronegativity difference is 0, the bond is known as nonpolar covalent bond, if it’s between 0 to 2.1, the bond is known as polar covalent bond and if its more than 2.1, the bond is known as ionic bond.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 5

Chapter 4, Problem 4.56E

Interpretation Introduction

(a)

Interpretation:

Whether the bond in H−I is polarized or not is to be stated. If polarized bond is present in the corresponding molecule, then the resulting charge distribution in molecule is to be shown.

Concept introduction:

Electronegativity is defined as the tendency of an atom to attract electrons towards it. Polarized bonds are a result of the electronegativity difference between bonding atoms. If the electronegativity difference is 0, the bond is known as nonpolar covalent bond, if it’s between 0 to 2.1, the bond is known as polar covalent bond and if its more than 2.1, the bond is known as ionic bond.

Interpretation Introduction

(b)

Interpretation:

Whether the bond in SO2 is polarized or not is to be stated. If polarized bond is present in the corresponding molecule, then the resulting charge distribution in molecule is to be shown.

Concept introduction:

Electronegativity is defined as the tendency of an atom to attract electrons towards it. Polarized bonds are a result of the electronegativity difference between bonding atoms. If the electronegativity difference is 0, the bond is known as nonpolar covalent bond, if it’s between 0 to 2.1, the bond is known as polar covalent bond and if its more than 2.1, the bond is known as ionic bond.

Interpretation Introduction

(c)

Interpretation:

Whether the bond in O3 is polarized or not is to be stated. If polarized bond is present in the corresponding molecule, then the resulting charge distribution in molecule is to be shown.

Concept introduction:

Electronegativity is defined as the tendency of an atom to attract electrons towards it. Polarized bonds are a result of the electronegativity difference between bonding atoms. If the electronegativity difference is 0, the bond is known as nonpolar covalent bond, if it’s between 0 to 2.1, the bond is known as polar covalent bond and if its more than 2.1, the bond is known as ionic bond.

Answer 6

Chapter 4, Problem 4.56E

Interpretation Introduction

(a)

Interpretation:

Whether the bond in H−I is polarized or not is to be stated. If polarized bond is present in the corresponding molecule, then the resulting charge distribution in molecule is to be shown.

Concept introduction:

Electronegativity is defined as the tendency of an atom to attract electrons towards it. Polarized bonds are a result of the electronegativity difference between bonding atoms. If the electronegativity difference is 0, the bond is known as nonpolar covalent bond, if it’s between 0 to 2.1, the bond is known as polar covalent bond and if its more than 2.1, the bond is known as ionic bond.

Answer 7

Chapter 4, Problem 4.56E

Interpretation Introduction

(a)

Interpretation:

Whether the bond in H−I is polarized or not is to be stated. If polarized bond is present in the corresponding molecule, then the resulting charge distribution in molecule is to be shown.

Concept introduction:

Electronegativity is defined as the tendency of an atom to attract electrons towards it. Polarized bonds are a result of the electronegativity difference between bonding atoms. If the electronegativity difference is 0, the bond is known as nonpolar covalent bond, if it’s between 0 to 2.1, the bond is known as polar covalent bond and if its more than 2.1, the bond is known as ionic bond.

Answer 8

Interpretation Introduction

(b)

Interpretation:

Whether the bond in SO2 is polarized or not is to be stated. If polarized bond is present in the corresponding molecule, then the resulting charge distribution in molecule is to be shown.

Concept introduction:

Electronegativity is defined as the tendency of an atom to attract electrons towards it. Polarized bonds are a result of the electronegativity difference between bonding atoms. If the electronegativity difference is 0, the bond is known as nonpolar covalent bond, if it’s between 0 to 2.1, the bond is known as polar covalent bond and if its more than 2.1, the bond is known as ionic bond.

Answer 9

Interpretation Introduction

(b)

Interpretation:

Whether the bond in SO2 is polarized or not is to be stated. If polarized bond is present in the corresponding molecule, then the resulting charge distribution in molecule is to be shown.

Concept introduction:

Electronegativity is defined as the tendency of an atom to attract electrons towards it. Polarized bonds are a result of the electronegativity difference between bonding atoms. If the electronegativity difference is 0, the bond is known as nonpolar covalent bond, if it’s between 0 to 2.1, the bond is known as polar covalent bond and if its more than 2.1, the bond is known as ionic bond.

Answer 10

Interpretation Introduction

(c)

Interpretation:

Whether the bond in O3 is polarized or not is to be stated. If polarized bond is present in the corresponding molecule, then the resulting charge distribution in molecule is to be shown.

Concept introduction:

Electronegativity is defined as the tendency of an atom to attract electrons towards it. Polarized bonds are a result of the electronegativity difference between bonding atoms. If the electronegativity difference is 0, the bond is known as nonpolar covalent bond, if it’s between 0 to 2.1, the bond is known as polar covalent bond and if its more than 2.1, the bond is known as ionic bond.

Answer 11

Interpretation Introduction

(c)

Interpretation:

Whether the bond in O3 is polarized or not is to be stated. If polarized bond is present in the corresponding molecule, then the resulting charge distribution in molecule is to be shown.

Concept introduction:

Electronegativity is defined as the tendency of an atom to attract electrons towards it. Polarized bonds are a result of the electronegativity difference between bonding atoms. If the electronegativity difference is 0, the bond is known as nonpolar covalent bond, if it’s between 0 to 2.1, the bond is known as polar covalent bond and if its more than 2.1, the bond is known as ionic bond.

Answer 12

Expert Solution & Answer

Answer 13

Expert Solution & Answer

Answer 14

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 15

Ch. 4 - Refer to the group numbers of the periodic table...Ch. 4 - Prob. 4.2E Ch. 4 - Write abbreviated electronic configurations for...Ch. 4 - Write abbreviated electronic configurations for...Ch. 4 - Draw Lewis structure for the elements given in...Ch. 4 - Draw Lewis structures for the elements given in...Ch. 4 - Prob. 4.7E Ch. 4 - Prob. 4.8E Ch. 4 - Prob. 4.9E Ch. 4 - Prob. 4.10E

Solution Summary: The author explains that polarized bonds are a result of the electronegativity difference between bonding atoms.

Concept explainers

Videos

Want to see the full answer?

Chapter 4 Solutions