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Answered 2010-07-27 20:28:42

Yes, SiH4 obeys the octet rule


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No chlorine oxides will obey the octet rule.

no it does not follow octet rule

Yes both of carbon and oxygen obey the octet rule in CO2

No, Beryllium is an exception to the octet rule.

No, IF5 does not obey the octet rule. I has more than 8 valence electrons, so it has an expanded octet.

Hydrogen does not obey the octet rule. Boron does not always obey the octet rule and in fact forms Lewis acids such as BF3 which only has 6 electrons.

Yes. Carbon tetrafluoride obeys the octet rule.

SO42-, ClO4- and SeCl4 do not obey octet rule.

yes PCl3 obey octet rule there are 5 electrons in the valence shell of phosphorous it need 3 electron to complete its octet so it form bond with 3 chlorine after bond formation there are 8 electron in its octet it obey octet rule

Beryllium does not obey the octet rule, as it is one of the exceptions. Other exceptions include: H, He, Li, and B

The atoms in the compound share electrons to form covalent (molecular) bonds and thus obey the octet rule.

Yes. Si (silicon) usually obeys the octet rule.

There is no chemical by the formula BF6. BF3 exists, but it doesn't obey octet rule

P certainly obeys the octet rule in phosphides: PH3, Na3P etc.

No. It obeys the octet rule for the fluorine atoms but not for Se (which has 12 electrons in its valence shell.)

No, SF6 does not obey the octet rule, since sulfur has more than 8 electrons.

Cs2 and Co3 2 obey the octet rule. the others don't

They don't have enough electrons

Molecules that do not follow the octet rule are usually more reactive than ones that do. Free radicals do not follow the octet rule. They have at least one unpaired electron.

Most molecules will obey the octet rule. It does not matter how many shells the element has. An element with 3 shells is electrically stable with both 8 or 18 electrons in its valence shell. Some molecules which obey this rule include oxygen and chlorine gas.

Elements that are exceptions to the Octet Rule are Helium , Hydroen, Lithium that obey the Duet Rule. Some reactive groups such as the Carbines. Some compounds that are good Lewis Acids that react well with Lewis Bases. Free Radicals such as Chlorine. The Transition Metals that obey the Dodectet Rule

No Aluminium be messing that whole gig up

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