I have to write a X and Y subscript.
If I wanted to put Fe(iron II) charge +2 and N (niterogen) -3 how would that subscript look? Im not use if those would even be able to go together. But if not can you help me fine a +2 and -3 charge is be able to turn into a subscript?
I sometimes type them as
Fe++
and
N---
but
Fe+2 and N-3 is used
Fe3N2 is iron nitride
http://www.endmemo.com/chem/compound/fe3n2.php
Oh ok thank you. I only have one more question then I will post all my answers so someone can check my work.
1. How many liters of carbon are produced at STP when 295g of methane gas (C3H8) is reacted with excess oxygen? The other products is water vapor. Write out a balanced equation.
My answer:
C3H8+O—-> CO3+OH8?
To write the chemical formula with subscripts for Fe(iron II) and N(nitrogen), you need to determine the correct ratio based on the charges of the ions.
The charge of Fe(iron II) is +2, meaning it has lost two electrons, while the charge of N(nitrogen) is -3, indicating it has gained three electrons.
To find the least common multiple of 2 and 3, we need to multiply them together, resulting in 6. This means that the atoms need to exchange six electrons to balance out their charges.
Since the Fe(iron II) ion has a charge of +2, it will need to gain two more electrons to balance its charge to zero.
Therefore, the Fe(iron II) ion with a charge of +2 will be represented as Fe^2+.
On the other hand, the N(nitrogen) ion with a charge of -3 will need to lose three more electrons to balance its charge to zero.
Therefore, the N(nitrogen) ion with a charge of -3 will be represented as N^3-.
The chemical formula with subscripts to represent these ions in a compound would be written as Fe^2+N^3-.