Question

Explain why o-h has a bond energy of 463 kJ/mol compared to the S-H bond energy...

Explain why o-h has a bond energy of 463 kJ/mol compared to the S-H bond energy of 339 kJ/mol.

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

O- H bond energy is 463 kJ / mol

S-H bond energy is 339 kJ / mol

this means that OH bond energy is more than that of S-H bond energy . it is due to high electronegativity of oxygen atom . because of high electronegativity of O atom compared to S atom , the O atom holds good the hydrogen compared to S. so O-H bond energy is more than S-H

another reason is that small atomic size of O and bigger atomic size of S. due to bigger atomic size S , S cannot overalap with hydrogen . so the S-H bond is very weaker

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
The bond dissociation energy for H-O is 463 kJ/mol. In the stratosphere, water vapor photodissociate as...
The bond dissociation energy for H-O is 463 kJ/mol. In the stratosphere, water vapor photodissociate as follows: H2O + hv --> H(g) + OH (g). calculate the heat of formation of OH(g) given the standard heat of formation of H2O(g) is -242 kj/mol.
The H–Br bond energy is 142 kJ/mol. Therefore the formation of a single bond between atoms...
The H–Br bond energy is 142 kJ/mol. Therefore the formation of a single bond between atoms The H–Br bond energy is 142 kJ/mol. Therefore the formation of a single bond between atoms should require the absorption of 284 kJ per mole of H–Br formed. should result in the release of 142 kJ per mole of H–Br formed. should require the absorption of 142 kJ per mole of H–Br formed. should result in the release of 284 kJ per mole of...
C-F bond energy us 485 KJ/mol and has bond length of 1.35A. Si-F bond energy is...
C-F bond energy us 485 KJ/mol and has bond length of 1.35A. Si-F bond energy is 565 KJ/mol and bond length of 1.6A. A) Explain the difference in bond length B) Rationalize why Si-F is stronger than the C-F bond.
Given the following information: Energy of sublimation of K(s) = 77 kJ/mol Bond energy of HCl...
Given the following information: Energy of sublimation of K(s) = 77 kJ/mol Bond energy of HCl = 427 kJ/mol Ionization energy of K(g) = 419 kJ/mol Electron affinity of Cl(g) = –349 kJ/mol Lattice energy of KCl(s) = –705 kJ/mol Bond energy of H2 = 432 kJ/mol Calculate the net change in energy for the following reaction: 2K(s) + 2HCl(g) → 2KCl(s) + H2(g) ΔE = ______ kJ
Calculate the average C—C bond strength in cyclopropane (in kJ/mol). Its combustion and the experimental enthalpy...
Calculate the average C—C bond strength in cyclopropane (in kJ/mol). Its combustion and the experimental enthalpy of reaction are: C3H6(g) + 4.5O2(g) → 3CO2(g) + 3H2O(g) ΔHºrxn = -1,957.7 kJ/mol Average bond strentgh (kj/mol): O - H = 463 C - H = 414 C - C = 347 O -- O = 498 (DOUBLE BOND) C -- O = 745 (DOUBLE BOND) C -- O (CO2 = 799) Since all reactants and products are in the gaseous state, bond...
Nitric oxide is a diatomic molecule with a bond dissociation energy (626 kJ/mol) in between oxygen...
Nitric oxide is a diatomic molecule with a bond dissociation energy (626 kJ/mol) in between oxygen (498 kJ/mol) and nitrogen (945 kJ/mol). This _______ (is or is not) consistent with the Lewis structure as it shows a bond order of _______ which is _______ (greater, less than, or the same as) the bond order in oxygen and _______ (greater, less than, or the same as) the bond order in nitrogen. Experimentally, nitric acid is found to be paramagnetic. Using a...
Calculate the second ionization energy of the metal M (ΔHion2° in kJ/mol) using the following data:...
Calculate the second ionization energy of the metal M (ΔHion2° in kJ/mol) using the following data: Lattice enthalpy of MO(s), ΔHl° = -2297 kJ/mol Bond dissociation enthalpy of O2(g) = +498 kJ/mol First electron affinity of O = -141 kJ/mol Second electron affinity of O = +744 kJ/mol Enthalpy of sublimation of M = + 102 kJ/mol First ionization energy of M = + 340 kJ/mol Standard enthalpy of formation of MO(s), ΔHf° = -336 kJ/mol Refer to the textbook...
Given the following information: Li(s) → Li(g) enthalpy of sublimation of Li(s) = 166 kJ/mol HF(g)...
Given the following information: Li(s) → Li(g) enthalpy of sublimation of Li(s) = 166 kJ/mol HF(g) → H(g) + F(g) bond energy of HF = 565 kJ/mol Li(g) → Li+(g) + e– ionization energy of Li(g) = 520. kJ/mol F(g) + e– → F–(g) electron affinity of F(g) = -328 kJ/mol Li+(g) + F–(g) → LiF(s) lattice energy of LiF(s) = -1047 kJ/mol H2(g) → 2H(g) bond energy of H2 = 432 kJ/mol Calculate the change in enthalpy for: 2Li(s)...
A reaction proceeds with ∆ H = -80 kJ/mol. The energy of activation of the uncatalyzed...
A reaction proceeds with ∆ H = -80 kJ/mol. The energy of activation of the uncatalyzed reaction is 80 kJ/mol, whereas it is 55 kJ/mol for the catalyzed reaction. How many times faster is the catalyzed reaction than the uncatalyzed reaction at 25°C?
te the lattice energy for LiF(s) given the following: sublimation energy for Li(s) +166 kJ/mol ∆Hf...
te the lattice energy for LiF(s) given the following: sublimation energy for Li(s) +166 kJ/mol ∆Hf for F(g) +77 kJ/mol first ionization energy of Li(g) +520. kJ/mol electron affinity of F(g) –328 kJ/mol enthalpy of formation of LiF(s) –617 kJ/mol A. none of these B. –650. kJ/mol C. 285 kJ/mol D. 800. kJ/mol E. 1052 kJ/mol
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT