Yes.
To complete the Fluorine octets (6 times) they need to increase from 7- (in fluorine atoms) to 8- (in fluoride ions F-1), so one electron per F atom.
These 6x 1 electrons are ALL donated from the only ONE sulfur atom (which has 6 valence electrons available) thus S becomes S+6
Yes. Carbon tetrafluoride obeys the octet rule.
NF3
CF4 Doesn't violate the Octet Rule, the rest do.
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
Boron trichloride does not follow the octet rule. Boron does not allow the eight required electrons in the outer shell.
No it is not fully obeying the octet rule. Boron has only 6 electrons (3 own + 3 from each F atom), lacking two for the octet. Fluorine is 3x satisfied, each with 8 electrons (each has 7 own plus 1 from boron).
because it does
CF4 Doesn't violate the Octet Rule, the rest do.
No chlorine oxides will obey the octet rule.
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.
no it does not follow 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
Boron trichloride does not follow the octet rule. Boron does not allow the eight required electrons in the outer shell.
because it does
Yes
No it is not fully obeying the octet rule. Boron has only 6 electrons (3 own + 3 from each F atom), lacking two for the octet. Fluorine is 3x satisfied, each with 8 electrons (each has 7 own plus 1 from boron).
H and I SCl4 ICl3 SeCI4 F2CCF2
I know for sure BBr# & PF5 do not obey the octet rule, but i can't remember the rule of isotopes so I can't say for sure whether or not CO3 -2 obeys it or not.
H and l