0 in N2
Zero
Oxidation numbers are defined for atoms, not molecules such as N2. The oxidation number of both atoms in a divalent elemental molecule is specified to be 0, as is the oxidation number of an atom of an element for which one atom constitutes a molecular unit.
zero for each nitrogen
The oxidation state (or number) is zero. This is true for any element in any of its allotropic elemental forms.
0 in N2
Zero
Oxidation numbers are defined for atoms, not molecules such as N2. The oxidation number of both atoms in a divalent elemental molecule is specified to be 0, as is the oxidation number of an atom of an element for which one atom constitutes a molecular unit.
zero for each nitrogen
The oxidation state (or number) is zero. This is true for any element in any of its allotropic elemental forms.
It is zero since it is a free element and it does not react with anything
It reacts with it. The reaction is a redx reaction. Nitrogen is reduced (its oxidation number goes from 0 to -3) and hydrogen is oxidised (its oxidation number goes from 0 to +1)
Nitrogen has an oxidation number of -3. Since it is in group 15, it has 5 valence electrons. It wants to have eight, so it will gain three electrons. Electrons are negative, that's why the oxidation number is negative.
The oxidation number of an element in its elemental form is always zero. Chemical compounds forming diatomic molecules may have elements in non zero oxidation number e.g. in HCl, H is +1 and Cl is -1.
the oxidation number of nitrogen is 5
The oxidation number of N, or Nitrogen, is N-3. Nitrogen is in group five, meaning it has five valence electrons. It needs to get eight to be stable. So it will gain 3 electrons to be stable. If you gain electrons, that makes it a negative number since electrons are negative in charge.
oxidation number of I is -1. oxidation number of F is +1.