No chlorine oxides will obey the octet rule.
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.
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
H and I SCl4 ICl3 SeCI4 F2CCF2
The elements can be described by dot structure. Metals combine with other elements to make its octet complete.
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
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.
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
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).
Yes
because it does
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
No. Some molecules, such as boron triflouride (BF3) and phosphorus pendachloride (PCl5) are octect violators.
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.