Bond strength decreases dramatically in the diatomic molecules from N2 (942 kJ mol-1) to O2 (495 kJ mol-1) to F2 (155 kJ...
Bond strength decreases dramatically in the diatomic molecules from N2 (942 kJ mol-1) to O2 (495 kJ mol-1) to F2 (155 kJ mol-1). What accounts for this behavior?
Homework Answers
The bond strength decreases from N2 to F2 as a result of decrease in bond order from 3 to 1. N2 has a bond order of 3, O2 has a bond order of 2 and F2 has a bond order of 1. Bond order is directly proportional to bond strength that implies as the bond order increases bond strength also increases and vice-versa. bond order can be calculated by subtracting the number of anti-bonding electrons present from the number of bonding electrons present, and then dividing the difference by 2 , we get the bond order of the molecule.
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Bond strength decreases dramatically in the diatomic molecules from N2 (942 kJ mol-1) to O2 (495 kJ mol-1) to F2 (155 kJ...
Question 3 1 pts Given the bond dissociation energies (in kJ/mol) for the following diatomic molecules Cl2 (243), F2 (1...
Question 3 1 pts Given the bond dissociation energies (in kJ/mol) for the following diatomic molecules Cl2 (243), F2 (158), H2 (436), O2 (498), N2 (945) choose the one(s) that could be broken by using blue light (=465 nm). F2 and Cl2 o F2 F2, C12, H2, O2 and N2 F2, Cl2 and H2 F2, Cl2, H2 and 02
Part A. Given the bond dissociation energies (in kJ/mol) for the following diatomic molecules Cl2 (243),...
Part A. Given the bond dissociation energies (in kJ/mol) for the following diatomic molecules Cl2 (243), F2 (158), H2 (436), O2 (498), N2 (945) choose the one(s) that could be broken by using blue light (λ=465 nm). Part B. Given the bond energies (in kJ/mol) of the following bonds: F–F (155), F–Cl (193), and Cl–Cl (243), estimate the molar enthalpy of formation of ClF(g), that is find ∆H for the following reaction ½Cl2(g) + ½F2(g) → ClF(g)
Classify these diatomic molecules as diamagnetic or paramagnetic: O2, F2, B2, C2, N2
Classify these diatomic molecules as diamagnetic or paramagnetic: O2, F2, B2, C2, N2
Place the following five diatomic molecules in the first column of the table. For each molecule,...
Place the following five diatomic molecules in the first column of the table. For each molecule, write down its bond order. Li2, H2, C2, O2, N2, Be2 Molecule Bond order Bond length (Å) Dissociation energy (kJ/mol) 0.74 457 1.09 1.21 599 1.21 105 2.72 10.0 942 494 2.67 Number of electrons: H(1), He(2), Li(3), Be(4), C(6), N(7), O(8). Based on the table, draw (on the same plot) the ground state potential energy function of N2, Liz and Be2. Annotate axes....
Given the following: O2 (g) + 2F2 (g)------> 2OF2 (g) delta H=+24.5 kJ/mol Bond dissociation energies:...
Given the following: O2 (g) + 2F2 (g)------> 2OF2 (g) delta H=+24.5 kJ/mol Bond dissociation energies: F2= 159 kJ/mol; O2 (double bond) = 498 kJ/mol Calculate the bond strength of the O-F bonds in OF2.
Question 1) By drawing molecular orbital diagrams for B2, C2, N2, O2, and F2, predict which...
Question 1) By drawing molecular orbital diagrams for B2, C2,
N2, O2, and F2, predict which of these homonuclear diatomic
molecules are magnetic.
Question 2) Based on the molecular orbital diagram for NO, which
of the following electronic configurations and statements are most
correct?
Bond Avg Bond Strength (in kJ/mol) C-C 350 C=O (in CO2) 804 O=O (in O2) 498...
Bond Avg Bond Strength (in kJ/mol) C-C 350 C=O (in CO2) 804 O=O (in O2) 498 O-H 464 C-H 415 The table above gives the average bond strength for a variety of chemical bonds. Use these values to calculate the energy change (in kJ) for the combustion of 24.8 grams of propane? If your answer is positive include no sign, if it is negative, include a negative sign. kJ
4. Diatomic nitrogen and oxygen molecules make up about 99% of all molecules in reasonable "unpolluted”...
4. Diatomic nitrogen and oxygen molecules make up about 99% of all molecules in reasonable "unpolluted” dry air a) Evaluate AGⓇ from the following reaction: N2(g) + O2(g) → NO(g) at 298 K. AG°F (NO(g)) = 86.57 kJ/mol. Is the reaction spontaneous? b) Calculate K, at 25 °C for the equilibrium reaction. What does the K, value you obtained indicates about the equilibrium? Does the reaction occurs (for practical purposes) at 25 °C?
Table 1: Bond Onders and Bond Energies for Selected Molecules Bond Bond Molecule Lewis Structure Bond...
Table 1: Bond Onders and Bond Energies for Selected Molecules Bond Bond Molecule Lewis Structure Bond Energy Order (kJ/mol HF H-8: H-F 1 570 HCI H-C: H-C1 11 432 HBr H-Br 366 НІ H-I 298 Cl2 C1-C1 1 Br-Br I-I 151 H2 Η-Η H-H 436 HO :0-H O-H REF 243 193 B12 498 н HH I H-C-C- H3CCH3 H C-C C-H 376 420 HH HH HCCH C-C C-H 720 444 H-C=C-H CO2 C-O 804 H-C-H H.CO C-O C-H 782 364...
Part A: Draw the Lewis structures of all the molecules involved in the reaction: N2(g)+3H2(g)→2NH3(g) Part B: If the bond energy for the N≡N bond is 946 kJ/mol, how much energy is needed to break all...
Part A: Draw the Lewis structures of all the molecules involved in the reaction: N2(g)+3H2(g)→2NH3(g) Part B: If the bond energy for the N≡N bond is 946 kJ/mol, how much energy is needed to break all the bonds in 3.0 mol of nitrogen molecules? Part C: If the bond energy for the H−H bond is 432 kJ/mol, how much energy is needed to break all the bonds in 9 hydrogen gas? Part D: If the bond energy for the N=H...
Question 3 1 pts Given the bond dissociation energies (in kJ/mol) for the following diatomic molecules Cl2 (243), F2 (158), H2 (436), O2 (498), N2 (945) choose the one(s) that could be broken by using blue light (=465 nm). F2 and Cl2 o F2 F2, C12, H2, O2 and N2 F2, Cl2 and H2 F2, Cl2, H2 and 02
Place the following five diatomic molecules in the first column of the table. For each molecule, write down its bond order. Li2, H2, C2, O2, N2, Be2 Molecule Bond order Bond length (Å) Dissociation energy (kJ/mol) 0.74 457 1.09 1.21 599 1.21 105 2.72 10.0 942 494 2.67 Number of electrons: H(1), He(2), Li(3), Be(4), C(6), N(7), O(8). Based on the table, draw (on the same plot) the ground state potential energy function of N2, Liz and Be2. Annotate axes....
Question 1) By drawing molecular orbital diagrams for B2, C2,
N2, O2, and F2, predict which of these homonuclear diatomic
molecules are magnetic.
Question 2) Based on the molecular orbital diagram for NO, which
of the following electronic configurations and statements are most
correct?
4. Diatomic nitrogen and oxygen molecules make up about 99% of all molecules in reasonable "unpolluted” dry air a) Evaluate AGⓇ from the following reaction: N2(g) + O2(g) → NO(g) at 298 K. AG°F (NO(g)) = 86.57 kJ/mol. Is the reaction spontaneous? b) Calculate K, at 25 °C for the equilibrium reaction. What does the K, value you obtained indicates about the equilibrium? Does the reaction occurs (for practical purposes) at 25 °C?
Table 1: Bond Onders and Bond Energies for Selected Molecules Bond Bond Molecule Lewis Structure Bond Energy Order (kJ/mol HF H-8: H-F 1 570 HCI H-C: H-C1 11 432 HBr H-Br 366 НІ H-I 298 Cl2 C1-C1 1 Br-Br I-I 151 H2 Η-Η H-H 436 HO :0-H O-H REF 243 193 B12 498 н HH I H-C-C- H3CCH3 H C-C C-H 376 420 HH HH HCCH C-C C-H 720 444 H-C=C-H CO2 C-O 804 H-C-H H.CO C-O C-H 782 364...
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