Questions: Give the systematic name for the following: Part 1 of 2 CuF= Part 2 of 2 Fe2 S3=

Transcript text: Give the systematic name for the following: Part 1 of 2 \[ \mathrm{CuF}= \] $\square$ Part 2 of 2 \[ \mathrm{Fe}_{2} \mathrm{~S}_{3}= \] $\square$

Solution

Solution Steps

Step 1: Identify the elements and their oxidation states

For $\mathrm{CuF}$:
- Copper (Cu) can have oxidation states of +1 or +2.
- Fluorine (F) has an oxidation state of -1.

Step 2: Determine the correct oxidation state for copper

Since there is only one fluorine atom, the oxidation state of copper must be +1 to balance the -1 charge of fluorine.

Step 3: Write the systematic name for $\mathrm{CuF}$

The systematic name is Copper(I) fluoride.

Step 4: Identify the elements and their oxidation states

For $\mathrm{Fe}_{2} \mathrm{~S}_{3}$:
- Iron (Fe) can have oxidation states of +2 or +3.
- Sulfur (S) has an oxidation state of -2.

Step 5: Determine the correct oxidation state for iron

There are 3 sulfur atoms, each with a -2 charge, giving a total of -6.
To balance this, the 2 iron atoms must have a total charge of +6, so each iron atom has an oxidation state of +3.

Step 6: Write the systematic name for $\mathrm{Fe}_{2} \mathrm{~S}_{3}$