Sulfur is in period 3 and has 6 valence electrons. The expected fluoride would be SF2, SF^ a very stable compound is surprisoing. The bonding in SF6 has been described in a number of ways- one is that there is sp3d2 hybridisation and there are 6 equivalent 2 electron 2 center bonds. Other descriptions involve resonance of ionic canonicals where the octet is preserved. Yet another description is "hypervalency" involving 3 centre bonds.
With BeH2 the situation is different, in this there are not enough electrons to form an octet. Some call this electron deficiency. In BeH2 each Be is surrounded by 4 hydrogen atoms, and there 4 BeHBe bonds- 3 center 2 electron. These are similar to bonds in B2H6.
The octet rule is a guideline- it has proved to be remarkably useful- but as someone said ".. in inorganic chemistry the rule is that there are no rules"
Arsenic is a metaloid with variable oxidation states. +/-3 and 5.
Sulfur hexafluoride has covalent bonds.
Anhydrous sodium sulfate has a molar mass of (23+23+32+16+16+16+16) = 142.
The dipole moment is zero in nonpolar molecules and non-zero in polar molecules due to electronegativity. Polar molecules have balanced electronegativity that will cancel one another out, while nonpolar molecules have unbalanced electronegativity causing dipole moments.
hello,all gases are insulators, so if you look at the periodic table on the gas section you would realsile none are solids and none are liquids so they can definatley not be conductors. ooops i was almost going to spell condom hahahafor your information a condom is a very nice tasting rubber thing which should be put on a dick for sex :)AnswerIf the moron who provided the original answer gave some thought to the question, instead of being obsessed with condoms, he would realise that some gases are indeed conductors -otherwise fluorescent tubes and neon tubes wouldn't work, would they? But to answer the question, a gas widely used to insulate high-voltage substation equipment is SF6: sulfur hexafluoride.
One example of a compound where the octet rule is expanded to include 12 electrons is sulfur hexafluoride (SF6). In SF6, the sulfur atom has 12 electrons around it, exceeding the typical octet rule. This expansion allows sulfur to complete its valence shell and achieve stability.
Yes, sulfur hexafluoride (SF6) obeys the octet rule. Sulfur forms 6 covalent bonds with fluorine atoms, allowing it to achieve a full outer shell of 8 electrons (octet).
Yes. In the case of BeCl2 and BF3, there are only 4 and 6 electrons on Be and B respectively and not eight. Similarly, in the case of SF6 and PCl5, there are 12 and 10 electrons on S and P respectively and not eight.
No, AsF6- does not obey the octet rule. Arsenic (As) can expand its valence shell to accommodate more than 8 electrons due to its empty d orbitals, which allows it to have more than 8 electrons around it in the AsF6- ion.
i dont no your level of chemistry, but if you know about orbital you will understand. sulfur is able to disobey the octect rule to form up to 6 bonds tis is due to the presence of d orbital. eg. SF6
Yes, atoms from period 3 and beyond can exceed the octet rule by utilizing d-orbitals to accommodate extra electrons in bonding, known as expanded octet. Examples include sulfur in sulfur hexafluoride (SF6) which has 12 valence electrons around it, surpassing the octet rule.
Sulfur hexafluoride (SF6) is a colorless gas under normal conditions.
The chemical name for compound SF6 is sulfur hexafluoride.
Sulfur hexachloride is an inorganic compound consisting of two different elements. The prefix hexa indicates that there are six chloride atoms. Thus, the formula is SCl6. Note that this compound does not obey the octet rule.
F6S is the formula for Sulfur Hexafluoride.
Sf6 acts as an lewis acid............
Usually in a sealed tank, the switch contacts are in the tank too. The SF6 gas quenches any arcs that form when the switch contacts are opened.