The octet rule is a simple rule of thumb that states that atoms tend to combine in such a way that they each have eight electrons in their valence shells, giving them the same electron configuration as a noble gas. The rule is applicable to the main-group elements.
In simple terms, molecules or ions tend to be most stable when the outermost electron shells of their constituent atoms contain eight electrons.
Hydrogen as you know only has one electron, this electron sits in the S orbital which is represented in 3d as a sphere. These S orbitals can only hold 2 electrons at most. So to get a configuration of the next nobel gas(helium) the hydrogen must have 1 electron applied to it. To this end the Hydrogen may bond with another Hydrogen to provide a stable(ish) configuration of 2S(i.e. 2 electrons in the s orbital) or the hdrogen may bind to another element that need a single electron to get a stable octet, in this case hydrogen may bond with any of the nobel gases e.g.: HF HCl etc....
Hydrogen is not confined to just the halogens though, since it provides one electron it may bond to several different elements to give them a stable octet e.g: H2O, H2S, NH3, CH4, B2H6
But hydrogen will not try and form compounds like LiH7 as the energy of formation of these compounds is far too high and they are too unstable
.. H - S - H (please see explanation below)*** .. *****The valence electron pairs are suppose to be on top and on bottom of the sulfur, instead of the hydrogen. This follows the octet rule for the sulfur and the duet rule for the hydrogen.
Hydrogen is different because it is the only element to not contain a neutron. It also does not follow the octet rule, and can be"happy" with two electrons like Helium. I hope that covers it!
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.
Flourins has 2s2 and 2p5 configuration and total 9 electrons in outermost shell. There are two possibilities for fluorine i.e. either to complete the outermost shell or to follow the octet rule. If it follow the octet rule there will remain 4 electrons in 2p. Hence its reactivity towards metals or other compounds will differ which is against its nature.Thats why flourine shows restrictions towards octet rule
Neon obeys the octet rule by not reacting and not forming ionic compounds as it already has a stable outer shell of eight electrons.
It is one of many, many exceptions to the octet rule. Hydrogen does NOT require 8 electrons.
Octet rule states that each electron wants to complete its octet ( 8 electrons in the outermost shell) or a duplet (in case of hydrogen and helium).
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.
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 atoms have only one shell( K-shell) which can accommodate only two electrons. Therefore each hydrogen atom in hydrogen moleculecontributes one electron forming a pair which is shared between the two atoms. Thus in hydrogen molecule duplet rule is followed and not the octet rule.
In chemistry, the octet and duplet rules are part of electronic configuration. The octet rule is when the outermost shell has 8 valence electrons. The duplet rule is when the outermost shell has 2 valence electrons, e.g. Helium and Hydrogen.
\helium (He) and hydrogen (H)
Hydrogen, helium and the transition metals
It does follow the octet rule!
I know Hydrogen and Helium for sure, not sure about the other elements. The noble gases.
Az important rule: any octet has to have eight parts, otherwise it is not an octet.
No, CH4 follows the octet rule.