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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
The octet rule states that atoms tend to gain, lose, or share electrons in order to achieve a full outer shell of eight electrons (except for hydrogen and helium, which follow the duet rule and only need two electrons). Hydrogen is an exception to the octet rule because it only needs two electrons to achieve a full outer shell. Hydrogen can either gain an electron to mimic helium or lose an electron to have an empty outer shell, making it an exception to the octet rule.
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Which obeys the octet rule PF5 Cs2 BBr3 CO3 2?
PF5 obeys the octet rule as it has 5 bonding pairs of electrons around the central phosphorus atom, satisfying the octet. Cs2 does not follow the octet rule as Cs is in Group 1 and can only form ionic bonds. BBr3 is an exception to the octet rule as boron has only 6 electrons around it due to the empty d orbital. CO3 2- also obeys the octet rule as each oxygen atom has a complete octet.
How does the octet rule influence Lewis dot structures?
Lewis dot structures are influenced by octet rule, when the electrons increase or decrease to fit into noble gas. Hence the chemical bonding in Lewis structure change.
What is the Lewis dot structure for Hydrogen Sulfide?
The Lewis dot structure for hydrogen sulfide (H2S) has a central sulfur atom bonded to two hydrogen atoms. The sulfur atom has 6 valence electrons, and each hydrogen atom contributes 1 valence electron, giving a total of 8 valence electrons in the structure.
Does the formula for potassium iodide illustrate the octet rule?
Yes, it does.
How many hydrogen atoms would a boron atom need to form covalent bond with it so that the boron is stable?
A boron atom would need 3 hydrogen atoms to form covalent bonds with it in order to achieve stability. This would allow boron to have a full octet of electrons in its outer shell, satisfying the octet rule.
Is water an exception to the octet rule?
It is one of many, many exceptions to the octet rule. Hydrogen does NOT require 8 electrons.
Which of the atoms don't always obey the octet rule H O Br?
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.
What is the octet rule in terms of lewis structures?
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).
Is NH3 an exception to the octet rule?
NH3 is not an exception to the octet rule. Nitrogen (N) in NH3 has a total of 8 valence electrons (5 from nitrogen and 3 from hydrogen), fulfilling the octet rule. Nitrogen has 3 bonded pairs and 1 lone pair of electrons, following the octet rule.
A molecule with bonding that follow the octet rule?
An example of a molecule that follows the octet rule is methane (CH4). In methane, carbon forms four covalent bonds with hydrogen, allowing each atom to achieve a full outer shell of electrons (octet) and satisfy the octet rule.
Why octet rule is not obeyed in the formation of h2 molecule?
In the formation of an H2 molecule, each hydrogen atom shares one electron with the other, creating a covalent bond. This bond satisfies the duet rule, which states that the stable electron configuration for hydrogen is to have two electrons in their outer shell, rather than the octet rule commonly observed in other elements. Therefore, the octet rule does not apply to hydrogen atoms when they form a molecule.
Why can a hydrogen atom form a covalent bond without fulfilling the octet rule?
A hydrogen atom can form a covalent bond without fulfilling the octet rule because it only needs two electrons to achieve a stable electron configuration, which is a duet rule for hydrogen. This allows hydrogen to share electrons with another atom to complete its valence shell and achieve a more stable state.
How many does the atoms electrons in their outer shells does the Octet Rule state they need?
The Octet Rule states that atoms are most stable when they have 8 electrons in their outer shell, except for hydrogen and helium, which are stable with 2 electrons in their outer shell.
What do you mean by octet and duplet?
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.
Which one doesn't follow the octet rule nh3 cf4 bcl3 ash3 hcl?
HCl doesn't follow the octet rule because hydrogen can only have 2 valence electrons and doesn't need a full octet to achieve a stable configuration.
Give example of octet rule?
Az important rule: any octet has to have eight parts, otherwise it is not an octet.
Octet rule for diatomic elements?
In diatomic elements, such as hydrogen (H2) or oxygen (O2), each atom follows the octet rule by sharing electrons to achieve a stable electron configuration. This results in a full outer shell of electrons with a total of 8 electrons, satisfying the octet rule. The sharing of electrons allows the diatomic molecule to be stable.
