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
CF4 and XeF4 do not violate the octet rule. In CF4, carbon forms four covalent bonds with fluorine, fulfilling the octet rule. In XeF4, xenon forms four covalent bonds with fluorine and has two lone pairs, also satisfying the octet rule.
BCl3 and BEH2 obey the octet rule because Boron and Beryllium are exceptions to the octet rule and can have stable electron configurations with less than 8 electrons. Cl3CF, NO, and SbF5 do not obey the octet rule because they have incomplete or expanded valence shells.
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 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
CF4 and XeF4 do not violate the octet rule. In CF4, carbon forms four covalent bonds with fluorine, fulfilling the octet rule. In XeF4, xenon forms four covalent bonds with fluorine and has two lone pairs, also satisfying the octet rule.
No chlorine oxides will obey the octet rule.
no it does not follow octet rule
Cs2, NO3, and PO43 do not obey the octet rule because they have an odd number of valence electrons. CI4 and SCI4 do not obey the octet rule because the central atom (Cl or S) exceeds the octet by having more than eight valence electrons.
BCl3 and BEH2 obey the octet rule because Boron and Beryllium are exceptions to the octet rule and can have stable electron configurations with less than 8 electrons. Cl3CF, NO, and SbF5 do not obey the octet rule because they have incomplete or expanded valence shells.
Hydrogen is the atom that doesn't always obey the octet rule. It only needs 2 electrons to have a full outer shell, rather than the 8 electrons typically required by the octet rule. Oxygen and bromine usually follow the 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).
H and l
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 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.
Atoms in the third period or beyond (period 3 and below) can exceed the octet rule due to the availability of d orbitals for expanded valence shells. Examples include sulfur, phosphorus, chlorine, and others in the third row and beyond in the periodic table. Additionally, atoms with an odd number of valence electrons, such as nitrogen and radicals, may also not follow the octet rule.