It sure does... or not ! It depends of the molecule you're considering.
Chlorine, in its fundamental state, has 3 doublets of electrons and one spare electron. It *should* thus solely be able to do single bonds (that's enough to satisfy the octet rule), e.g. methyl chloride ClCH3, alcanoyl chlorides ClCO-R or hydrochloric acid H-Cl (which is BTW a gas ; this molecule doesn't exist in water, where it is in the form of two ions : {H+, Cl-}). All these molecules follow the octet rule.
Though chlorine is able to "split" its doublets and spread them onto its 3d vacant orbitals. It can then increase its bonding abilities, breaking the octet rule on the way. For quick example, you can search for chlorine dioxide radical ClO2 with its odd number of electrons (the structure of this molecule has been a conundrum for years) or chloric acid HClO3.
This is the ICl3 Lewis structure. For ICl3, we have 7 valence electrons for Iodine; 7 for Chlorine, but we have three Chlorines; a total of 28 valence electrons. I is the least electronegative, put that in the center, and then Chlorines will go around it. ... The Iodine has an octet, plus some.
No Aluminium be messing that whole gig up
NO
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
because it does
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).
The oxygen atoms in the ion do obey the octet rule. The phosphorus atom has more than eight electrons in its valence shell. It is because of the existence of vacant 3d orbitals.
Yes. Both O-F bonds are single covalent, so all three atoms can claim 8 electrons.
H and I SCl4 ICl3 SeCI4 F2CCF2
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
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).
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
Chlorine Cl : it can have a higher valence (ClO2, HClO3) than predicted by the octet rule. Hydrogen H and oxygen O cannot escape the octet rule.
No. Some molecules, such as boron triflouride (BF3) and phosphorus pendachloride (PCl5) are octect violators.