12 votes

When would a R-O-R bond be linear?

Oxygen can be bonded with 180° bond angles in perovskite structures, such as silicate minerals formed deep in Earth's mantle (the perovskite form of calcium silicate has been identified at Earth's ...
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  • 38.2k
8 votes

Bond angles of dichlorine and dibromine monoxides

$\ce{F2O}$ Phase Method ∠F−O−F Reference solid (−223.8 °C) powder x-ray diffraction 98.0(1.5)° [1], ICSD-430183 gas microwave spectroscopy 103.07(5)° [2] $\ce{Cl2O}$ Phase Method ∠Cl−O−Cl ...
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  • 34.7k
7 votes

When would a R-O-R bond be linear?

No, bond angles of virtually any $\ce{R-O-R}$ bond will differ from $180^\circ$, so there are no common linear oxygen configurations. Steric hindrance can cause a severe deviation from the ideal ...
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4 votes

Why does methane have 4-different bond dissociation energies?

The dissociation energies are different because bonds don't all break at once Most chemical processes happen step by step. Even in simple molecules like methane where there are only 4 bonds, bond ...
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4 votes
Accepted

Can exact bond angles in cycloalkanes be calculated?

There may be experimental data for the specific cycloalkane in question, for example by a single-crystal diffraction analysis. Beside entries in the primary literature, there are databases with the ...
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4 votes

Why do CCl4 and CH4 have the same bond angle?

In $\ce{NH3}$ and $\ce{NF3}$, $\ce{F}$ having higher electronegativity than $\ce{H}$, $\ce{NF3}$ has a smaller bond angle compared to $\ce{NH3}$. Both of these compounds have a lone pair on the ...
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1 vote

Why do CCl4 and CH4 have the same bond angle?

Welcome to Stack exchange chemistry. Consider for a moment what is known as the isolobal concept, there are a series of atoms and groups which all present the same types of orbitals (or at least close ...
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1 vote

Why is the Br-C-H bond angle in CH3Br smaller than the Cl-C-H bond angle in CH3Cl?

According to VSEPR theory, the bond angles in case of CH3Cl and CH3Br is based on bond pair - bond pair repulsion only as there are no lone pairs in them. The bond pair electrons are spread within the ...
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1 vote

Quantifying location and volume of "lone pairs" for VSEPR

There have been a few efforts to experimentally quantify the polarizability volume of lone pairs, including: "Polarizability of Non-Bonding Electron Pairs" Australian Journal of Chemistry (...
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1 vote

Why does the Lewis structure for NH2 have 4 dots and not 3?

As the compound is negatively charged, there is an extra electron present in the compound. Since the extra electron is held on nitrogen, there is 4 electrons on nitrogen instead of just 3. The extra ...
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