0
Why are Sulfur-Hydrogen bond lengths longer than Oxygen-Hydrogen bond lengths?
Wiki User
∙ 16y ago
If you take a look at the Periodic Table of Elements, you'll notice that sulfur is directly underneath oxygen. According to trends in the Periodic Table, one knows that the size of the atom of sulfur is larger than that of oxygen because there are more electrons in a higher energy level surrounding the nucleus. The bond between both hydrogen and oxygen and hydrogen and sulfur are covalent. That means that the lone electron around the hydrogen is equally shared between the hydrogen and the sulfur. Simply because sulfur is a larger atom, it will have a larger bond length between anything it bonds with than that if oxygen were to bond with that same atom.
Wiki User
∙ 16y ago
Wiki User
∙ 14y agoOxygen has a much smaller atomic radius compared to sulfur. You can think of bond-lengths as interactions between electrons in the radius of sulfur/oxygen and the radius of hydrogen, so the S-H electron interactions (bonds) must occur over a larger distance than the O-H bonds.
Wiki User
∙ 13y agoBecause a carbon atom is larger than a helium atom. Carbon atoms have a radius of about 77 picometers, while helium atoms have a radius of about 37 picometers. The sum of the two radii usually gives you the bond length between the two elements (between 109 and 114pm for C-H, between 134 and 154pm for C-C.)
Add your answer:
Earn +20 pts
Why are the bond lengths in no3- all identical and shorter than a nitrogen-oxygen single bond?
NO3- has three resonance structure. One double bond between N and O and another two N - O single bond. Since the double bond can be formed between N and any other O it is said that it has a resonance structure. This means that the true structure of NO3- is not any of this structure, but rather a hybrid of all three. Hence all 3 bond lengths would be identical AND shorter than single bond as it is basically an average between single and double bond. It is of course longer than a double bond
Which is longer carbon-carbon single or double bond?
double bonds are shorter because they are stronger so they pull the carbons closer together
Why all carbon-carbon bond lengths in benzene are equal?
This is due to the resonation process that gives the allusion of all bond lengths being equal. In fact the bonds are in a state of constant flux and 'blend' into one. It is much like the apperance of a helicopters rotar blades i.e. in flight it appears as a blurr but whilst stationary it is clear that there are simply two blades -------------- The paragraph above is incorrect. Forget the fan blade and helicopter rotor analogies for resonance. There is NO evidence that bonds are jumping back and forth between a single bond and a double bond. That's just wrong. Resonance structures are simply an attempt at representing with Lewis structures something which really can't be represented with Lewis structures, that of a "partial" double bond. In carbonate ion, all of the carbon-oxygen bonds are identical, and have a length somewhere between that of a single bond and a double bond. The bond order for the carbon-oxygen bond in carbonate is 1.33. The partial double bond comes from delocalized pi bonding. In addition to the single bond between the central carbon and each oxygen, there is a delocalized pi bond between the central carbon and each of the oxygen atoms. There is overlap of the p-orbital on C with each of the p-orbitals on the oxygen atoms, but there are not enough electrons for three double bonds. It is this additional pi bonding which makes each of the carbon-oxygen bonds have a bond order of 1.33, and a bond length and bond strength between those of single and double carbon-oxygen bonds. ----- Pisgahchemist
A chemical bond that occurs when atoms share electrons is a?
This is a covalent bond.
Which is strongest carbon carbon single bond carbon carbon double bond or carbon carbon triple bond?
The strongest chemical bond is the ionic bond. Ionic bond strengths are greater than covalent bond strengths.answer 2it is known that covalent bond is stronger.
What bond length accounts for stronger bonds?
Shorter bond lengths. N2 is very strong with its triple bond.
Does NF3 have unequal bond lengths?
yes it dose
Do oxygen to oxygen bond lengths change in ozone?
yes
Generally are shorter chemical bond lengths stronger?
Yes.
How do you find the lengths of nitrogen-to-nitrogen bond?
The length of nitrogen-to-nitrogen bond is approx. 100 pm.
Which compound contains a longer C-C bond benzene or ethene?
c-c bond length in benzene is 1.397 angston and that of ethene is 1.34 angston structure of benzene is a resonance hybrid, therefore all the c-c bond lengths are equal but different from those in alkanes,alkenes, and alkynes.
Bond Lengths of Nitrogen Oxide?
The length of the bonds in NO is 115 peta metres
A picometer pm is equal to 1 multiplied by 10 to the negative 12 power m. OH bond lengths in water are 95.8 pm while S-H bond lengths in dihydrogen sulfide are 135 pm. Why are S-H bond lengths longer?
A picometer (pm) is equal to 1 x 10^-12 m. The O-H bond lengths in water are 95.8 pm,while S-H bond lengths in dihydrogen sulfide are 135 pm. Why are S-H bonds longer than O-H bonds? Is it because Sulfurs mass is greater than Oxygens mass? Please correct me if I'm wrong. Oxygen = 15.99 Sulfur = 32.06
Why are the bond lengths in no3- all identical and shorter than a nitrogen-oxygen single bond?
NO3- has three resonance structure. One double bond between N and O and another two N - O single bond. Since the double bond can be formed between N and any other O it is said that it has a resonance structure. This means that the true structure of NO3- is not any of this structure, but rather a hybrid of all three. Hence all 3 bond lengths would be identical AND shorter than single bond as it is basically an average between single and double bond. It is of course longer than a double bond
Why do TeO2 bonds have unequal bond lengths unlike SO2?
SO2 contains resonance
Is CO2 molecule has two types of bond lengths?
No, both the bonds in CO2 are identical.
What is the unit used to define bond lengths?
Bond Length is often measured in picometers (pm).
