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Does sulfur break the octet rule?
Yes, sulfur can break the octet rule by expanding its valence shell to accommodate more than eight electrons. This is known as an expanded octet.
Does the element sulfur in SO3 violate the octet rule?
Yes, the element sulfur in SO3 violates the octet rule because it has more than 8 electrons in its valence shell.
Can sulfur exceed the octet rule in chemical bonding?
Yes, sulfur can exceed the octet rule in chemical bonding by expanding its valence shell to accommodate more than eight electrons.
What compound is the octet rule expanded to include 12 electrons?
One example of a compound where the octet rule is expanded to include 12 electrons is sulfur hexafluoride (SF6). In SF6, the sulfur atom has 12 electrons around it, exceeding the typical octet rule. This expansion allows sulfur to complete its valence shell and achieve stability.
Which main-group elements occasionally break the octet rule?
Main-group elements such as boron, beryllium, and sulfur can occasionally break the octet rule by having fewer or more than eight valence electrons in their outermost shell. Boron and beryllium are known to form stable compounds with only six or even four electrons in their valence shell, while sulfur can expand its octet to accommodate more than eight electrons.
Does sulfur break the octet rule?
Yes, sulfur can break the octet rule by expanding its valence shell to accommodate more than eight electrons. This is known as an expanded octet.
Does the element sulfur in SO3 violate the octet rule?
Yes, the element sulfur in SO3 violates the octet rule because it has more than 8 electrons in its valence shell.
Can sulfur exceed the octet rule in chemical bonding?
Yes, sulfur can exceed the octet rule in chemical bonding by expanding its valence shell to accommodate more than eight electrons.
What compound is the octet rule expanded to include 12 electrons?
One example of a compound where the octet rule is expanded to include 12 electrons is sulfur hexafluoride (SF6). In SF6, the sulfur atom has 12 electrons around it, exceeding the typical octet rule. This expansion allows sulfur to complete its valence shell and achieve stability.
Which main-group elements occasionally break the octet rule?
Main-group elements such as boron, beryllium, and sulfur can occasionally break the octet rule by having fewer or more than eight valence electrons in their outermost shell. Boron and beryllium are known to form stable compounds with only six or even four electrons in their valence shell, while sulfur can expand its octet to accommodate more than eight electrons.
Does SF2 obey octet rule?
No, SF6 doesn't. If you draw out the Lewis structure, all 6 fluorine atoms have to connect to the sulfur.
Does H2S follow 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.
Does SO4 2- obey the octet rule?
Yes, SO4 2- can be drawn without violating the octet rule. It is also a resonance structure. Here's an illustration below (ignore the dots, it was the only way it posted correctly!): .......O .......| O -- S -- O ....... .......O Hope this helped!
Which three elements violate the octet rule?
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.
Why does sulfur dioxide have 10 electrons on central atom when that is more than 8. I don't understand how it can violate the rule?
The octet rule is a simplification, not a hard and fast rule. We use it to help students at the start of their studies of bonding. When sulfur forms more bonds, more energy is released. resulting in a more stable situation.
In forming covalent bonds where the octet rule is obeyed sulfur usually forms?
six;seven
Does the CS2 are obeys the octet rule?
No, carbon disulfide (CS2) does not obey the octet rule. In CS2, the central carbon atom has only six electrons in its valence shell, forming double bonds with the sulfur atoms, resulting in a total of 16 valence electrons around the carbon atom.
