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.
No, BCl3 does not follow the octet rule as boron only has 6 valence electrons in this molecule. Boron can form stable compounds with less than an octet due to its electron deficiency.
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
No, NH3 does not follow the octet rule. Nitrogen typically forms 3 bonds in NH3, instead of the expected 4 bonds to fulfill 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.
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.
no it does not follow octet rule
octet rule
No, BCl3 does not follow the octet rule as boron only has 6 valence electrons in this molecule. Boron can form stable compounds with less than an octet due to its electron deficiency.
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
No, NH3 does not follow the octet rule. Nitrogen typically forms 3 bonds in NH3, instead of the expected 4 bonds to fulfill the octet rule.
H2S does follow the octet rule. When you draw the Lewis Structure for H2S, it looks like this: If you count up the lone pairs and sigma bonds (each worth 2), there are 8, thus, H2S follows the octet rule.
The octet rule is a rule in chemistry where elements want to form bonds to attain 8 electrons in their valence shell. An example of this would be sodium chloride. Bonds that don't have 8 electrons in their valence shell don't follow this 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.
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, AlCl3 does not follow the octet rule. Aluminum typically forms compounds where it only has 6 electrons in its outer shell, such as in AlCl3 where it forms 3 bonds with chlorine atoms.
No, xenon does not always follow the octet rule. It is a noble gas and can form stable compounds that have more than eight electrons around the xenon atom, known as expanded octet.