Yes the sulfur needs to have two more electrons to fill the octet, and chlorine only needs one. So there are two chlorines to give sulfur one electron. The whole molecule is covalently bonded so the electrons are shared between the chlorines and the sulfur so that both the elements octets are filled.
Lewis structure.
.. .. ..
:Cl - S - Cl:
.. .. ..
from there it should be obvious.
Yes, SeCl6 violates the octet rule, since Se has more than 8 electrons in this compound.
No. It obeys the octet rule for the fluorine atoms but not for Se (which has 12 electrons in its valence shell.)
No it does not.
Yes, it does.
yesss !!
i dont
yes
nope
Cl3CF
CF4 Doesn't violate the Octet Rule, the rest do.
Yes
The octet rule does not apply to transition metals.
F2ccf2
nope
Cl3CF
CF4 Doesn't violate the Octet Rule, the rest do.
Yes
The octet rule does not apply to transition metals.
Boron trichloride does not follow the octet rule. Boron does not allow the eight required electrons in the outer shell.
The octet rule cannot be satisfied in molecules whose total number of valence electrons is an odd number.There are also molecules in which an atom has fewer, or more, than an octet of valence electrons.
The octet rule only applies to elements that are heavy enough to have reached the second shell of electrons. In the first shell, the octet rule does not apply because the first shell is completed with only two electrons, not eight. So no, the octet rule does not apply to beryllium hydride.
BCl3 is the formula for Boron Chloride. As a matter of interest it does not obey the octet rule. It is also called a Lewis Acid.
There is ClO2 and ClO2^-. For the chlorite anion (ClO2^-) the Cl will have 10 electrons and will violate the octet rule. For ClO2, all elements will have 8 electrons.
In general, boron will form 3 covalent bonds, using each of its 3 valence shell electrons (sharing them). This will of course violate the octet rule, but obeys the sextet rule, and this is what makes boron stable. It (along with aluminum, eg.) do not obey the octet rule.