To determine the name of the compound [tex]\( FeCl_3 \)[/tex], we need to utilize our understanding of chemical nomenclature, specifically for ionic compounds involving transition metals.
1. Identify the elements involved:
- [tex]\( Fe \)[/tex] is the chemical symbol for Iron.
- [tex]\( Cl \)[/tex] is the chemical symbol for Chlorine.
2. Determine the type of compound:
- The compound consists of a metal (Iron) and a non-metal (Chlorine), so this is an ionic compound.
3. Consider the oxidation state of the metal:
- Iron is a transition metal, and transition metals can have multiple oxidation states.
- Chlorine typically has an oxidation state of [tex]\(-1\)[/tex].
4. Determine the total charge contribution from chlorine:
- There are three chlorine atoms in [tex]\( FeCl_3 \)[/tex].
- Each chlorine atom has a charge of [tex]\(-1\)[/tex], contributing a total of [tex]\( -3 \)[/tex] to the compound ([tex]\( 3 \times -1 = -3 \)[/tex]).
5. Identify the charge of the iron ion:
- For the compound to be neutral, the charge on the iron ion must balance the charge from the chlorine ions.
- Therefore, the iron ion must have a charge of [tex]\( +3 \)[/tex] to counterbalance the [tex]\( -3 \)[/tex] from the three chlorines.
6. Determine the correct naming convention:
- The cation (metal) is named first, followed by the anion (non-metal).
- For transition metals, the oxidation state of the metal is indicated in Roman numerals in parentheses immediately following the name of the metal.
7. Name the compound:
- The name of the anion [tex]\( Cl \)[/tex] is derived from chlorine, and in ionic compounds, it typically ends in “-ide,” so it is called chloride.
- Since iron in this compound has a [tex]\( +3 \)[/tex] oxidation state, it is named Iron(III).
Hence, the name of the compound [tex]\( FeCl_3 \)[/tex] is Iron(III) chloride.
