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The oxidant number is the number of electrons gained or lost by an atom to comply with the octet rule
As it forms the I- ion froming an octet its most likely oxidation number is -1
The oxidation number of Neon is 0. It does not want to gain or lose any electrons. It already has a full octet, therefore it remains at 0.
The number of Covalent Bonds is equal to eight minus the group number.
The oxidation number of Neon is 0. It does not want to gain or lose any electrons. It already has a full octet, therefore it remains at 0.
-1. Fluorine has an atomic number of 9. It has seven valence electrons (in the 2d shell) so it gains one electron to achieve th octet- hence it has an oxidation number of -1
The oxidant number is the number of electrons gained or lost by an atom to comply with the octet rule
As it forms the I- ion froming an octet its most likely oxidation number is -1
The oxidation number of Neon is 0. It does not want to gain or lose any electrons. It already has a full octet, therefore it remains at 0.
Protons (the number of ..) determine the 'kind' of element,and the electrons in the outmost valency orbital determine the properties(the number of electron; and 'octet' rule: "make it eight preferably').
The number of Covalent Bonds is equal to eight minus the group number.
No, oxygen will never have a -3 oxidation number. If it had a -3 oxidation number, it would not have a full octet. It would have a +1 charge, therefore making it not happy.
The oxidation number of Neon is 0. It does not want to gain or lose any electrons. It already has a full octet, therefore it remains at 0.
The oxidation number of Neon is 0. It does not want to gain or lose any electrons. It already has a full octet, therefore it remains at 0.
Because they require one electron to complete their octet
8 so then it is an Octet.
The clue for knowing the number of lines in an octet is that in a Lewis structure a line represents two electrons. This means that an element with four lines attached to other elements has an octet.