calculated below. H-F Bond Energy: 567 kJ/mol example H2 (g) + F2 (g) 2HF AHxn = [energy used for breaking bonds] - [energy formed in making bonds] [436 kJ/mol + 155 kJ/mol] - [2(567 kJ/mol)] = - 543 kJ/mol Average Bond Energies (kJ/mol) 436 kJ/mol 431 kJ/mol H-H С-Н 413 kJ/mol C=C 614 kJ/mol H-CI С-С 348 kJ/mol C=C 839 kJ/mol H-F 567 kJ/mol С-N 293 kJ/mol C=0 799 kJ/mol N-H 391 kJ/mol C-O 358 kJ/mol O=0 495 kJ/mol 201 kJ/mol 463 kJ/mol 146 kJ/mol N-O С-F 485 kJ/mol C=O 1072 kJ/mol O-H C-CI 328 kJ/mol C=N 615 kJ/mol O-0 C-S 259 kJ/mol N=N 418 kJ/mol F-F 155 kJ/mol Cl-CI 242 kJ/mol N=N 941 kJ/mol C=N 891 kJ/mol Estimate the enthalpy change (AHxn) of the following reactions using the bond energies above. II 1. H-H + CI-CI → H-CI + H-CI 4. H-C-CI + O C-CI H-CI CI CI нн H. H 2. O=0 Н-о-н + F-F н-с-с-н 5. H-C-H + → 0=C= + O=0 H-O-H F F H H H 3. Н-с-о-н + Н-с-о-н н-с-о-с-н + H-O-H H H H
calculated below. H-F Bond Energy: 567 kJ/mol example H2 (g) + F2 (g) 2HF AHxn = [energy used for breaking bonds] - [energy formed in making bonds] [436 kJ/mol + 155 kJ/mol] - [2(567 kJ/mol)] = - 543 kJ/mol Average Bond Energies (kJ/mol) 436 kJ/mol 431 kJ/mol H-H С-Н 413 kJ/mol C=C 614 kJ/mol H-CI С-С 348 kJ/mol C=C 839 kJ/mol H-F 567 kJ/mol С-N 293 kJ/mol C=0 799 kJ/mol N-H 391 kJ/mol C-O 358 kJ/mol O=0 495 kJ/mol 201 kJ/mol 463 kJ/mol 146 kJ/mol N-O С-F 485 kJ/mol C=O 1072 kJ/mol O-H C-CI 328 kJ/mol C=N 615 kJ/mol O-0 C-S 259 kJ/mol N=N 418 kJ/mol F-F 155 kJ/mol Cl-CI 242 kJ/mol N=N 941 kJ/mol C=N 891 kJ/mol Estimate the enthalpy change (AHxn) of the following reactions using the bond energies above. II 1. H-H + CI-CI → H-CI + H-CI 4. H-C-CI + O C-CI H-CI CI CI нн H. H 2. O=0 Н-о-н + F-F н-с-с-н 5. H-C-H + → 0=C= + O=0 H-O-H F F H H H 3. Н-с-о-н + Н-с-о-н н-с-о-с-н + H-O-H H H H
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Types of Chemical Bonds
The attractive force which has the ability of holding various constituent elements like atoms, ions, molecules, etc. together in different chemical species is termed as a chemical bond. Chemical compounds are dependent on the strength of chemical bonds between its constituents. Stronger the chemical bond, more will be the stability in the chemical compounds. Hence, it can be said that bonding defines the stability of chemical compounds.
Polarizability In Organic Chemistry
Polarizability refers to the ability of an atom/molecule to distort the electron cloud of neighboring species towards itself and the process of distortion of electron cloud is known as polarization.
Coordinate Covalent Bonds
A coordinate covalent bond is also known as a dative bond, which is a type of covalent bond. It is formed between two atoms, where the two electrons required to form the bond come from the same atom resulting in a semi-polar bond. The study of coordinate covalent bond or dative bond is important to know about the special type of bonding that leads to different properties. Since covalent compounds are non-polar whereas coordinate bonds results always in polar compounds due to charge separation.
Question
Can you explain these questions to me please? thank you
![Bond energy is defined as the amount of energy required to break a bond. These values
are positive, indicating that bond breaking is endothermic. Bond energies are reported in
kilojoules per mole (kJ/mol). The energy for breaking a hydrogen-hydrogen bond is 436
kJ/mol so when a hydrogen-hydrogen bond is formed the process releases 436 kJ/mol.
In a chemical reaction several bonds are broken and formed. For example in the
reaction below a hydrogen-hydrogen bond is broken and a fluorine-fluorine bond is broken.
Two hydrogen-fluorine bonds are formed. The overall energy change for this process is
calculated below.
H-H
Bond energy: 436 kJ/mol
F-F
Bond Energy: 155 kJ/mol
H-F
Bond Energy: 567 kJ/mol
example
H2 (g) + F2 (g)
2HF
AHX0 = [energy used for breaking bonds]- [energy formed in making bonds]
[436 kJ/mol + 155 kJ/mol] - [2(567 kJ/mol)]
=- 543 kJ/mol
Average Bond Energies (kJ/mol)
H-H
436 kJ/mol
С-Н
413 kJ/mol
C=C
614 kJ/mol
H-Cl
431 kJ/mol
C-C
348 kJ/mol
C=C
839 kJ/mol
H-F
567 kJ/mol
С-N
293 kJ/mol
C=0
799 kJ/mol
N-H
391 kJ/mol
C-O
358 kJ/mol
O=0
495 kJ/mol
N-O
201 kJ/mol
С-F
485 kJ/mol
C=0
1072 kJ/mol
O-H
463 kJ/mol
C-Cl
328 kJ/mol
C=N
615 kJ/mol
O-0
146 kJ/mol
C-S
259 kJ/mol
N=N
418 kJ/mol
F-F
155 kJ/mol
Cl-Cl
242 kJ/mol
N=N
941 kJ/mol
C=N
891 kJ/mol
Estimate the enthalpy change (AHxn) of the following reactions using the bond energies above.
II
1.
H-H + CI-CI →
H-CI + H-CI
4.
+ O
C-CI
H-CI
H-C-CI
CI
CI
нн
2. o-
H
O=0
H-O-H
+ F-F -→
н-с-с-н
5.
H-C-H +
O=C=O
H
O=0
H-O-H
F F
H.
H.
H.
3. Н-С-о-н + H-с-о-н — н-с-о-с-н
+ H-O-H
H
H
H
H
O=0-0](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F79e7eefe-8745-42e5-a1d9-5bd5d5e9e0b9%2F1f06f563-8dea-460f-92f0-fb8b87ad906a%2Fg6juz3vo_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Bond energy is defined as the amount of energy required to break a bond. These values
are positive, indicating that bond breaking is endothermic. Bond energies are reported in
kilojoules per mole (kJ/mol). The energy for breaking a hydrogen-hydrogen bond is 436
kJ/mol so when a hydrogen-hydrogen bond is formed the process releases 436 kJ/mol.
In a chemical reaction several bonds are broken and formed. For example in the
reaction below a hydrogen-hydrogen bond is broken and a fluorine-fluorine bond is broken.
Two hydrogen-fluorine bonds are formed. The overall energy change for this process is
calculated below.
H-H
Bond energy: 436 kJ/mol
F-F
Bond Energy: 155 kJ/mol
H-F
Bond Energy: 567 kJ/mol
example
H2 (g) + F2 (g)
2HF
AHX0 = [energy used for breaking bonds]- [energy formed in making bonds]
[436 kJ/mol + 155 kJ/mol] - [2(567 kJ/mol)]
=- 543 kJ/mol
Average Bond Energies (kJ/mol)
H-H
436 kJ/mol
С-Н
413 kJ/mol
C=C
614 kJ/mol
H-Cl
431 kJ/mol
C-C
348 kJ/mol
C=C
839 kJ/mol
H-F
567 kJ/mol
С-N
293 kJ/mol
C=0
799 kJ/mol
N-H
391 kJ/mol
C-O
358 kJ/mol
O=0
495 kJ/mol
N-O
201 kJ/mol
С-F
485 kJ/mol
C=0
1072 kJ/mol
O-H
463 kJ/mol
C-Cl
328 kJ/mol
C=N
615 kJ/mol
O-0
146 kJ/mol
C-S
259 kJ/mol
N=N
418 kJ/mol
F-F
155 kJ/mol
Cl-Cl
242 kJ/mol
N=N
941 kJ/mol
C=N
891 kJ/mol
Estimate the enthalpy change (AHxn) of the following reactions using the bond energies above.
II
1.
H-H + CI-CI →
H-CI + H-CI
4.
+ O
C-CI
H-CI
H-C-CI
CI
CI
нн
2. o-
H
O=0
H-O-H
+ F-F -→
н-с-с-н
5.
H-C-H +
O=C=O
H
O=0
H-O-H
F F
H.
H.
H.
3. Н-С-о-н + H-с-о-н — н-с-о-с-н
+ H-O-H
H
H
H
H
O=0-0
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