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Can oxygen expand its octet in chemical bonding?
Yes, oxygen can expand its octet in chemical bonding by forming more than eight valence electrons in its outer shell.
Can phosphorus expand its octet in chemical bonding?
Yes, phosphorus can expand its octet in chemical bonding by forming more than 8 valence electrons in its outer shell.
Can iodine exceed the octet rule and have an expanded octet?
Yes, iodine can exceed the octet rule and have an expanded octet due to its ability to accommodate more than eight electrons in its valence shell.
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.
Can 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.
Can oxygen expand its octet in chemical bonding?
Yes, oxygen can expand its octet in chemical bonding by forming more than eight valence electrons in its outer shell.
Can phosphorus expand its octet in chemical bonding?
Yes, phosphorus can expand its octet in chemical bonding by forming more than 8 valence electrons in its outer shell.
Does uranium have an octet?
Uranium typically forms compounds where it does not have an octet due to its ability to expand its valence shell beyond eight electrons. Uranium can often exceed the octet rule in its bonding arrangements.
Can iodine exceed the octet rule and have an expanded octet?
Yes, iodine can exceed the octet rule and have an expanded octet due to its ability to accommodate more than eight electrons in its valence shell.
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.
Can 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 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.
Can some atoms exceed the limits of the octet rule in bonding?
The further down the periodic table that you go the more electrons that an element has, also the more orbitals an element has. If you look up general trends in the periodic table ionic size is showen to increase too. The ionic size is directly related to these larger orbital shells that hold more electrons. S orbital = 2 é P orbital = 6é D orbital = 10é You may want to look up these orbitals to get a better understanding of them, each one has a unique shape http://en.wikipedia.org/wiki/Atomic_orbital some atoms can exceed the octet rule by using these unfilled larger orbitals to put electrons into them, so for example they might use the D orbital to place extra electrons into it, causing the octet rule to break down.
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.
In which bonding patterns does X obey the octet rule?
no it does not follow octet rule
Which atom will form a positive ion during ionic bonding sulfur or magnesium?
Magnesium will form a positive ion during ionic bonding. It will lose 2 electrons to achieve a stable octet configuration, resulting in a 2+ ion. Sulfur typically forms a negative ion by gaining 2 electrons to achieve a stable electron configuration.
Elements in the third row of the periodic table or lower can have octets?
Elements in the third row of the periodic table or lower can have octets in their outermost electron shell due to the availability of d orbitals for bonding. This allows them to exceed the usual octet rule of 8 electrons in their valence shell. Examples include elements like sulfur, phosphorus, and chlorine.
